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Regents Chemistry REVIEW - 2 *Questions from NYS Chemistry Regents exams Kenneth E. Schnobrich Just a Note • The questions in Review-2 generally do not involve reference to a major diagram. • All questions are taken from Regents Exams, parts A and B-1. • In most cases, it will help to have your “Reference Tables for Physical Setting/CHEMISTRY” available. 2 1/07-1 • Which subatomic particles are located in the nucleus of a neon atom? (1) Electrons and positrons (2) Electrons and neutrons (3) Protons and neutrons (4) Protons and electrons 3 1/07-1 • Which subatomic particles are located in the nucleus of a neon atom? (1) Electrons and positrons (2) Electrons and neutrons (3) Protons and neutrons (4) Protons and electrons correct 4 1/07-2 • The total mass of the protons in an atom of gold-198 is approximately (1) 79 atomic mass units (2) 119 atomic mass units (3) 198 atomic mass units (4) 277 atomic mass units 5 1/07-2 • The total mass of the protons in an atom of gold-198 is approximately (1) 79 atomic mass units (3) 198 atomic mass units correct (2) 119 atomic mass units (4) 277 atomic mass units 6 1/07-3 • In a calcium atom in the ground state, the electrons that possess the least amount of energy are located in the (1) First electron shell (2) Second electron shell (3) Third electron shell (4) Fourth electron shell 7 1/07-3 • In a calcium atom in the ground state, the electrons that possess the least amount of energy are located in the (1) First electron shell (3) Third electron shell correct (2) Second electron shell (4) Fourth electron shell 8 1/07-4 • Which group of atomic models is listed in historical order from the earliest to the most recent? (1) hard-sphere model, wave-mechanical model, electron-shell model (2) hard-sphere model, electron-shell model, wave-mechanical model (3) electron-shell model, wavemechanical model, hard-sphere model (4) electron-shell model, hard-sphere model, wave-mechanical model 9 1/07-4 • Which group of atomic models is listed in historical order from the earliest to the most recent? (1) hard-sphere model, wave-mechanical model, electron-shell model (2) hard-sphere model, electron-shell model, wave-mechanical model correct (3) electron-shell model, wavemechanical model, hard-sphere model (4) electron-shell model, hard-sphere model, wave-mechanical model 10 1/07-5 • Which isotopic notation represents an atom of carbon-14? (1) 8C6 (2) 6C8 (3) 14C8 (4) 6C14 11 1/07-5 • Which isotopic notation represents an atom of carbon-14? (1) 8C6 (2) 6C8 (3) 14C8 (4) 6C14 correct 12 1/07-6 • An atom of argon rarely bonds to an atom of another element because an argon atom has (1) 8 valence electrons (2) 2 valence electrons (3) 3 valence electrons (4) 22 valence electrons 13 1/07-6 • An atom of argon rarely bonds to an atom of another element because an argon atom has (1) 8 valence electrons (3) 3 valence electrons correct (2) 2 valence electrons (4) 22 valence electrons 14 1/07-7 • The elements on the Periodic Table are arranged in order of increasing (1) Boiling point (2) electronegativity (3) Atomic number (4) Atomic mass 15 1/07-7 • The elements on the Periodic Table are arranged in order of increasing (1) Boiling point (3) Atomic number (2) electronegativity correct (4) Atomic mass 16 1/07-8 • Which element is classified as a nonmetal? (1) Be (2) Al (3) Si (4) Cl 17 1/07-8 • Which element is classified as a nonmetal? (1) Be (2) Al (3) Si (4) Cl correct 18 1/07-9 • Solid samples of the element phosphorous can be white, black, or red in color. The variations in the color are due to different (1) Atomic masses (2) Molecular structures (3) Ionization energies (4) Nuclear charges 19 1/07-9 • Solid samples of the element phosphorous can be white, black, or red in color. The variations in the color are due to different (1) Atomic masses (2) Molecular structures (3) Ionization energies (4) Nuclear charges correct 20 1/07-10 • Given the balanced equation representing a reaction between propane and oxygen: C3H8 + 5O2 -> 3CO2 + 4H2O According to this equation, which ratio of oxygen to propane is correct? (1) 5 grams O2/1 gram of C3H8 (2) 10 grams O2/11 grams C3H8 (3) 5 moles O2/1 mole C3H8 (4) 10 moles O2/11 moles C3H8 21 1/07-10 • Given the balanced equation representing a reaction between propane and oxygen: C3H8 + 5O2 -> 3CO2 + 4H2O According to this equation, which ratio of oxygen to propane is correct? (1) 5 grams O2/1 gram of C3H8 (3) 5 moles O2/1 mole C3H8 (2) 10 grams O2/11 grams C3H8 correct (4) 10 moles O2/11 moles C3H8 22 1/07-11 • Lithium and potassium have similar chemical properties because the atoms of both elements have the same (1) Mass number (2) Atomic number (3) Number of electron shells (4) Number of valence electrons 23 1/07-11 • Lithium and potassium have similar chemical properties because the atoms of both elements have the same (1) Mass number (2) Atomic number (3) Number of electron shells (4) Number of valence electrons correct 24 1/07-12 • Which two substances are covalent compounds? (1) C6H12O6(s) and KI(s) (2) C6H12O6(s) and HCl(g) (3) KI(s) and NaCl(s) (4) NaCl(s) and HCl(g) 25 1/07-12 • Which two substances are covalent compounds? (1) C6H12O6(s) and KI(s) (2) C6H12O6(s) and HCl(g) (3) KI(s) and NaCl(s) (4) NaCl(s) and HCl(g) correct 26 1/07-13 • which substance when dissolved in water, forms a solution that conducts and electric current? (1) C2H5OH (2) C6H12O6 (3) C12H22O11 (4) CH3COOH 27 1/07-13 • Which substance when dissolved in water, forms a solution that conducts and electric current? (1) C2H5OH (2) C6H12O6 (3) C12H22O11 (4) CH3COOH correct 28 1/07-15 • Compared to a phosphorous atom, a P3- ion has (1) More electrons and a larger radius (2) More electrons and a smaller radius (3) Fewer electrons and a larger radius (4) Fewer electrons and a smaller radius 29 1/07-15 • Compared to a phosphorous atom, a P3- ion has (1) More electrons and a larger radius (2) More electrons and a smaller radius (3) Fewer electrons and a larger radius (4) Fewer electrons and a smaller radius correct 30 1/07-16 • The balanced equation below represents a molecule of bromine separating into two bromine atoms. Br2 -> Br + Br What occurs during the change? (1) Energy is absorbed and a bond is formed (2) Energy is absorbed and a bond is broken (3) energy is released and a bond is formed (4) Energy is released and a bond is broken 31 1/07-16 • The balanced equation below represents a molecule of bromine separating into two bromine atoms. Br2 -> Br + Br What occurs during the change? (1) Energy is absorbed and a bond is formed (2) Energy is absorbed and a bond is correct broken (3) energy is released and a bond is formed (4) Energy is released and a bond is broken 32 1/07-17 • Which substance can be decomposed by chemical means? (1) tungsten (2) antimony (3) krypton (4) methane 33 1/07-17 • Which substance can be decomposed by chemical means? (1) tungsten (2) antimony (3) krypton (4) methane correct 34 1/07-18 • Bronze contains 90 to 95% copper and 5 to 10% tin. Because these percentages can vary, bronze is classified as (1) A compound (2) An element (3) A mixture (4) A substance 35 1/07-18 • Bronze contains 90 to 95% copper and 5 to 10% tin. Because these percentages can vary, bronze is classified as (1) A compound (3) A mixture (2) An element correct (4) A substance 36 1/07-19 • Compared to a 2.0 M aqueous solution of NaCl at 1 atmosphere, a 3.0 M aqueous solution of NaCl at 1 atmosphere has a (1) Lower boiling point and a higher freezing point (2) Lower boiling point and a lower freezing point (3) Higher boiling point and a higher freezing point (4) Higher boiling point and lower freezing point 37 1/07-19 • Compared to a 2.0 M aqueous solution of NaCl at 1 atmosphere, a 3.0 M aqueous solution of NaCl at 1 atmosphere has a (1) Lower boiling point and a higher freezing point (2) Lower boiling point and a lower freezing point (3) Higher boiling point and a higher freezing point (4) Higher boiling point and lower freezing correct point 38 1/07-20 • In which reaction are the electrons transferred from one reactant to another? (1) 2Ca(s) + O2(g) -> 2CaO(s) (2) AgNO3(aq) + KCl(aq) -> AgCl(s) + KNO3 (3) HCl(aq) + NaOH(aq) -> NaCl(aq) + H2O(l) (4) H3O+(aq) + OH-(aq) -> 2H2O(l) 39 1/07-20 • In which reaction are the electrons transferred from one reactant to another? (1) 2Ca(s) + O2(g) -> 2CaO(s) correct (3) HCl(aq) + NaOH(aq) -> NaCl(aq) + H2O(l) (2) AgNO3(aq) + KCl(aq) -> AgCl(s) + KNO3 (4) H3O+(aq) + OH-(aq) -> 2H2O(l) 40 1/07-21 • Which statement must be true for any chemical reaction at equilibrium? (1) The concentration of the products is greater than the concentration of the reactants. (2) The concentration of the products is less than the concentration of the reactants. (3) The concentration of the products and the concentration of the reactants are equal. (4) The concentration of the products and the concentration of the reactants are constant. 41 1/07-21 • Which statement must be true for any chemical reaction at equilibrium? (1) The concentration of the products is greater than the concentration of the reactants. (2) The concentration of the products is less than the concentration of the reactants. (3) The concentration of the products and the concentration of the reactants are equal. (4) The concentration of the products and the concentration of the reactants are correct constant. 42 1/07-24 • Which group of emissions is listed in order of increasing charge? (1) Alpha particle, beta particle, gamma radiation (2) Gamma radiation, alpha particle, beta particle (3) positron, alpha particle, neutron (4) neutron, positron, alpha particle 43 1/07-25 • Two substances have different physical and chemical properties. Both substances have molecules that contain two carbon atoms, one oxygen atom, and six hydrogen atoms. These two substances must be (1) Isomers of each other (2) Isotopes of each other (3) The same compound (4) The same hydrocarbon 44 1/07-25 • Two substances have different physical and chemical properties. Both substances have molecules that contain two carbon atoms, one oxygen atom, and six hydrogen atoms. These two substances must be (1) Isomers of each other (3) The same compound correct (2) Isotopes of each other (4) The same hydrocarbon 45 1/07-26 • Given the balanced equation representing a reaction: CH3CH2CH3 + Br2 -> CH3CH2CH2Br + HBr This organic reaction is best classified as (1) An addition reaction (2) An esterification reaction (3) A polymerization reaction (4) A substitution reaction 46 1/07-26 • Given the balanced equation representing a reaction: CH3CH2CH3 + Br2 -> CH3CH2CH2Br + HBr This organic reaction is best classified as (1) An addition reaction (2) An esterification reaction (3) A polymerization reaction (4) A substitution reaction correct 47 1/07-27 • In terms of energy and entropy, systems in nature tend to undergo changes toward (1) Higher energy and higher entropy (2) Higher energy and lower entropy (3) Lower energy and higher entropy (4) Lower energy and lower entropy 48 1/07-27 • In terms of energy and entropy, systems in nature tend to undergo changes toward (1) Higher energy and higher entropy (2) Higher energy and lower entropy (3) Lower energy and higher entropy (4) Lower energy and lower entropy correct 49 1/07-29 • Which compound has hydrogen bonding between its molecules? (1) CH4 (2) KH (3) CaH2 (4) NH3 50 1/07-29 • Which compound has hydrogen bonding between its molecules? (1) CH4 (2) KH (3) CaH2 (4) NH3 correct 51 1/07-30 • Which ion is the only negative ion produced by an Arrhenius base in water? (1) NO3- (2) Cl- (3) OH- (4) H- 52 1/07-30 • Which ion is the only negative ion produced by an Arrhenius base in water? (1) NO3(3) OH- (2) Cl- correct (4) H- 53 1/07-31 • When the elements in Group 1 are considered in order from top to bottom, each successive element at standard pressure has (1) A higher melting point and a higher boiling point (2) A higher melting point and a lower boiling point (3) A lower melting point and a higher boiling point (4) A lower melting point and a lower boiling point 54 1/07-31 • When the elements in Group 1 are considered in order from top to bottom, each successive element at standard pressure has (1) A higher melting point and a higher boiling point (2) A higher melting point and a lower boiling point (3) A lower melting point and a higher boiling point (4) A lower melting point and a lower correct boiling point 55 1/07-32 • Which isotopic notation identifies a metalloid that is matched with the corresponding number of protons in each of its atoms (1) 24Mg and 12 protons (3) 75As and 75 protons (2) 28Si and 14 protons (4) 80Br and 80 protons 56 1/07-32 • Which isotopic notation identifies a metalloid that is matched with the corresponding number of protons in each of its atoms (1) 24Mg and 12 protons (3) 75As and 75 protons (2) 28Si and 14 protons correct (4) 80Br and 80 protons 57 1/07-33 • At STP, which list of elements contains a solid, liquid, and a gas? (1) Hf, Hg, He (2) Cr, Cl2, C (3) Ba, Br2, B (4) Se, Sn, Sr 58 1/07-33 • At STP, which list of elements contains a solid, liquid, and a gas? (1) Hf, Hg, He (2) Cr, Cl2, C (3) Ba, Br2, B (4) Se, Sn, Sr 59 1/07-33 • At STP, which list of elements contains a solid, liquid, and a gas? (1) Hf, Hg, He (3) Ba, Br2, B correct (2) Cr, Cl2, C (4) Se, Sn, Sr 60 1/07-34 • Element X reacts with iron to form two different compounds with the formulas FeX and Fe2X3. To which group on the Periodic Table does element X belong? (1) Group 8 (2) Group 2 (3) Group 13 (4) Group 16 61 1/07-34 • Element X reacts with iron to form two different compounds with the formulas FeX and Fe2X3. To which group on the Periodic Table does element X belong? (1) Group 8 (2) Group 2 (3) Group 13 (4) Group 16 correct 62 1/07-35 • The molar mass of Ba(OH)2 is (1) 154.3 g (2) 155.3 g (3) 171.3 g (4) 308.6 g 63 1/07-35 • The molar mass of Ba(OH)2 is (1) 154.3 g (3) 171.3 g (2) 155.3 g correct (4) 308.6 g 64 1/07-36 • Given the balanced equation representing a reaction: 4NH3 + 5O2 -> 4NO + 6H2O What is the minimum number of moles of O2 that are needed to completely react 1ith 16 moles of NH3? (1) 16 mol (2) 20. mol (3) 64 mol (4) 80. mol 65 1/07-36 • Given the balanced equation representing a reaction: 4NH3 + 5O2 -> 4NO + 6H2O What is the minimum number of moles of O2 that are needed to completely react 1ith 16 moles of NH3? (1) 16 mol (2) 20. mol (3) 64 mol (4) 80. mol correct 66 1/07-38 • A 10.0-gram sample of which element has the smallest volume at STP? (1) aluminum (2) magnesium (3) titanium (4) zinc 67 1/07-38 • A 10.0-gram sample of which element has the smallest volume at STP? (1) aluminum (2) magnesium (3) titanium (4) zinc correct 68 1/07-39 • A which temperature would atoms of a He(g) sample have the greatest average kinetic energy? (1) 25°C (2) 37°C (3) 273 K (4) 298 K 69 1/07-39 • A which temperature would atoms of a He(g) sample have the greatest average kinetic energy? (1) 25°C (2) 37°C (3) 273 K (4) 298 K correct 70 1/07-41 • At room temperature, a mixture of sand and water can be separated by (1) ionization (2) combustion (3) filtration (4) sublimation 71 1/07-41 • At room temperature, a mixture of sand and water can be separated by (1) ionization (3) filtration (2) combustion correct (4) sublimation 72 1/07-42 • Given a balanced equation representing a reaction at 101.3 kPa and 298 K: N2(g) + 3H2(g) -> 2NH3(g) + 91.8 kJ Which statement is true about this reaction? (1) It is exothermic and the ∆H equals 91.8 kJ (2) It is exothermic and the ∆H equals +91.8 kJ (3) it is endothermic and the ∆H equals 91.8 kJ (4) It is endothermic and the ∆H equals +91.8 kJ 73 1/07-42 • Given a balanced equation representing a reaction at 101.3 kPa and 298 K: N2(g) + 3H2(g) -> 2NH3(g) + 91.8 kJ Which statement is true about this reaction? (1) It is exothermic and the ∆H equals correct 91.8 kJ (2) It is exothermic and the ∆H equals +91.8 kJ (3) it is endothermic and the ∆H equals 91.8 kJ (4) It is endothermic and the ∆H equals +91.8 kJ 74 1/07-43 • Which balanced equation represents a phase equilibrium? (1) 1 (2) 2 (3) 3 (4) 4 75 1/07-43 • Which balanced equation represents a phase equilibrium? (1) 1 (3) 3 (2) 2 correct (4) 4 76 1/07-44 • Given the system at equilibrium: 2POCl(g) + Energy = 2PCl3(g) + O2(g) Which changes occur when O2(g) is added to the system? (1) The equilibrium shifts to the right and the concentration of PCl3(g) increases (2) The equilibrium shifts to the right and the concentration of PCl3(g) decreases (3) The equilibrium shifts to the left and the concentration of PCl3(g) increases (4) The equilibrium shifts to left and the concentration fo PCl3(g) decreases 77 1/07-44 • Given the system at equilibrium: 2POCl(g) + Energy = 2PCl3(g) + O2(g) Which changes occur when O2(g) is added to the system? (1) The equilibrium shifts to the right and the concentration of PCl3(g) increases (2) The equilibrium shifts to the right and the concentration of PCl3(g) decreases (3) The equilibrium shifts to the left and correct the concentration of PCl3(g) increases (4) The equilibrium shifts to left and the concentration fo PCl3(g) decreases 78 1/07-45 • What is the oxidation number of chromium in the chromate ion, CrO42-? (1) +6 (2) +2 (3) +3 (4) +8 79 1/07-45 • What is the oxidation number of chromium in the chromate ion, CrO42-? (1) +6 (3) +3 correct (2) +2 (4) +8 80 1/07-46 • Given the balanced equation representing a reaction: Which type of reaction is represented by this equation? (1) decomposition (2) neutralization (3) single replacement (4) synthesis 81 1/07-46 • Given the balanced equation representing a reaction: Which type of reaction is represented by this equation? (1) decomposition (2) neutralization (3) single replacement (4) synthesis correct 82 1/07-47 • In which 0.01 M solution is phenolphthalein pink? (1) CH3OH(aq) (2) Ca(OH)2(aq) (3) CH3COOH(aq) (4) HNO3(aq) 83 1/07-47 • In which 0.01 M solution is phenolphthalein pink? (1) CH3OH(aq) (2) Ca(OH)2(aq) (3) CH3COOH(aq) (4) HNO3(aq) correct 84 1/07-48 • As the pH of a solution is changed from 3 to 6, the concentration of the hydronium ions (1) Increases by a factor of 3 (2) Increases by a factor of 1000 (3) Decreases by a factor of 3 (4) Decreases by a factor of 1000 85 1/07-48 • As the pH of a solution is changed from 3 to 6, the concentration of the hydronium ions (1) Increases by a factor of 3 (2) Increases by a factor of 1000 (3) Decreases by a factor of 3 (4) Decreases by a factor of 1000 correct 86 1/07-49 • If 1/8 of an original sample of krypton-74 remains unchanged after 34.5 minutes, what is the half-life of krypton-74? (1) 11.5 min (2) 23.0 min (3) 34.5 min (4) 46.0 min 87 1/07-49 • If 1/8 of an original sample of krypton-74 remains unchanged after 34.5 minutes, what is the half-life of krypton-74? (1) 11.5 min (3) 34.5 min correct (2) 23.0 min (4) 46.0 min 88 1/07-50 • Given the nuclear equation: •Which particle is represented by X? (1) 2He4 (2) -1e0 (3) 0n1 (4) +1e0 89 1/07-50 • Given the nuclear equation: •Which particle is represented by X? (1) 2He4 (3) 0n1 correct (2) -1e0 (4) +1e0 90 6/07-1 • According to the wave-mechanical model of the atom, electrons in an atom (1) Travel in defined circles (2) Are most likely found in an excited state (3) Have a positive charge (4) Are located in orbitals outside the nucleus 91 6/07-1 • According to the wave-mechanical model of the atom, electrons in an atom (1) Travel in defined circles (2) Are most likely found in an excited state (3) Have a positive charge (4) Are located in orbitals outside the correct nucleus 92 6/07-2 • What is the total charge of the nucleus of a carbon atom? (1) -6 (2) 0 (3) +6 (4) +12 93 6/07-2 • What is the total charge of the nucleus of a carbon atom? (1) -6 (2) 0 (3) +6 (4) +12 correct 94 6/07-3 • A sample composed only of atoms having the same atomic number is classified as (1) A compound (2) A solution (3) An element (4) An isomer 95 6/07-3 • A sample composed only of atoms having the same atomic number is classified as (1) A compound (3) An element (2) A solution correct (4) An isomer 96 6/07-4 • Which two particles each have a mass approximately equal to one atomic mass unit? (1) Electron and neutron (2) Electron and positron (3) Proton and electron (4) Proton and neutron 97 6/07-4 • Which two particles each have a mass approximately equal to one atomic mass unit? (1) Electron and neutron (2) Electron and positron (3) Proton and electron (4) Proton and neutron correct 98 6/07-5 • Which two characteristics are associated with metals? (1) Low first ionization energy and low electronegativity (2) Low first ionization energy and high electronegativity (3) High first ionization energy and low electronegativity (4) Low first ionization energy and high electronegativity 99 6/07-5 • Which two characteristics are associated with metals? (1) Low first ionization energy and low correct electronegativity (2) Low first ionization energy and high electronegativity (3) High first ionization energy and low electronegativity (4) Low first ionization energy and high electronegativity 100 6/07-6 • Which element is most chemically similar to chlorine? (1) Ar (2) F (3) Fr (4) S 101 6/07-6 • Which element is most chemically similar to chlorine? (1) Ar (2) F (3) Fr (4) S correct 102 6/07-7 • Which substance can be decomposed by chemical means? (1) ammonia (2) oxygen (3) phosphorous (4) silicon 103 6/07-7 • Which substance can be decomposed by chemical means? (1) ammonia (3) phosphorous correct (2) oxygen (4) silicon 104 6/07-8 • When an atom loses one or more electrons, this atom becomes a (1) Positive ion with a radius smaller than the radius of this atom (2) Positive ion with a radius larger than the radius of this atom (3) Negative ion with a radius smaller than (4) Negative ion with a radius larger than the radius of this atom the radius of this atom 105 6/07-8 • When an atom loses one or more electrons, this atom becomes a (1) Positive ion with a radius smaller than correct the radius of this atom (2) Positive ion with a radius larger than the radius of this atom (3) Negative ion with a radius smaller than (4) Negative ion with a radius larger than the radius of this atom the radius of this atom 106 6/07-9 • What is the name of the polyatomic ion in the compound Na2O2? (1) hydroxide (2) oxalate (3) oxide (4) peroxide 107 6/07-9 • What is the name of the polyatomic ion in the compound Na2O2? (1) hydroxide (2) oxalate (3) oxide (4) peroxide correct 108 6/07-10 • Given the balanced equation: I + I -> I2 Which statement describes the process represented by this equation? (1) A bond is formed and energy is absorbed (2) A bond is formed and energy is released (3) A bond is broken and energy is absorbed (4) A bond is broken and energy is released 109 6/07-10 • Given the balanced equation: I + I -> I2 Which statement describes the process represented by this equation? (1) A bond is formed and energy is correct absorbed (2) A bond is formed and energy is released (3) A bond is broken and energy is absorbed (4) A bond is broken and energy is released 110 6/07-11 • An oxygen molecule contains a double bond because two atoms of oxygen share a total of (1) 1 electron (2) 2 electrons (3) 3 electrons (4) 4 electrons 111 6/07-11 • An oxygen molecule contains a double bond because two atoms of oxygen share a total of (1) 1 electron (2) 2 electrons (3) 3 electrons (4) 4 electrons correct 112 6/07-12 • Which term is defined as a measure of the average kinetic energy of the particles in a sample? (1) temperature (2) pressure (3) thermal energy (4) chemical energy 113 6/07-12 • Which term is defined as a measure of the average kinetic energy of the particles in a sample? (1) temperature (3) thermal energy correct (2) pressure (4) chemical energy 114 6/07-13 • A 3.0 M HCl(aq) solution contains a total of (1) 3.0 grams of HCl per liter of water (2) 3.0 grams of HCl per mole of solution (3) 3.0 moles of HCl per liter of solution (4) 3.0 moles of HCl per mole of water 115 6/07-13 • A 3.0 M HCl(aq) solution contains a total of (1) 3.0 grams of HCl per liter of water (2) 3.0 grams of HCl per mole of solution (3) 3.0 moles of HCl per liter of solution (4) 3.0 moles of HCl per mole of water correct 116 6/07-14 • A dilute, aqueous potassium nitrate solution is best classified as a (1) Homogeneous compound (2) Homogeneous mixture (3) Heterogeneous compound (4) Heterogeneous mixture 117 6/07-14 • A dilute, aqueous potassium nitrate solution is best classified as a (1) Homogeneous compound (2) Homogeneous mixture correct (3) Heterogeneous compound (4) Heterogeneous mixture 118 6/07-15 • Given the equation representing a phase change at equilibrium: C2H5OH(l) = C2H5OH(g) Which statement is true? (1) The forward process proceeds faster than the reverse process (2) The reverse process proceeds faster than the forward process (3) The forward and reverse processes proceed at the same rate (4) The forward and reverse processes both stop 119 6/07-15 • Given the equation representing a phase change at equilibrium: C2H5OH(l) = C2H5OH(g) Which statement is true? (1) The forward process proceeds faster than the reverse process (2) The reverse process proceeds faster than the forward process (3) The forward and reverse processes correct proceed at the same rate (4) The forward and reverse processes both stop 120 6/07-16 • A 5.0-gram sample of zinc and a 50. –milliliter sample of hydrochloric acid are used in a chemical reaction. Which combination of these samples has the fastest reaction rate? (1) A zinc strip and 1.0 M HCl(aq) (2) A zinc strip and 3.0 M HCl(aq) (3) Zinc powder and 1.0 M HCl(aq) (4) Zinc powder and 3.0 M HCl(aq) 121 6/07-16 • A 5.0-gram sample of zinc and a 50. –milliliter sample of hydrochloric acid are used in a chemical reaction. Which combination of these samples has the fastest reaction rate? (1) A zinc strip and 1.0 M HCl(aq) (2) A zinc strip and 3.0 M HCl(aq) (3) Zinc powder and 1.0 M HCl(aq) (4) Zinc powder and 3.0 M HCl(aq) correct 122 6/07-17 • For a given reaction, adding a catalyst increases the rate of the reaction by (1) Providing an alternate reaction pathway that has a higher activation energy (2) Providing an alternate reaction pathway that has a lower activation energy (3) Using the same reaction pathway and increasing the activation energy (4) Using the same reaction pathway and decreasing the activation energy 123 6/07-17 • For a given reaction, adding a catalyst increases the rate of the reaction by (1) Providing an alternate reaction pathway that has a higher activation energy (2) Providing an alternate reaction pathway that has a lower activation correct energy (3) Using the same reaction pathway and increasing the activation energy (4) Using the same reaction pathway and decreasing the activation energy 124 6/07-18 • Which reaction releases the greatest amount of energy per 2 moles of product? (1) 1 (2) 2 (3) 3 (4) 4 125 6/07-18 • Which reaction releases the greatest amount of energy per 2 moles of product? (1) 1 (2) 2 (3) 3 (4) 4 correct 126 6/07-19 • What is the total number of carbon atoms in a molecule of ethanoic acid? (1) 1 (2) 2 (3) 3 (4) 4 127 6/07-19 • What is the total number of carbon atoms in a molecule of ethanoic acid? (1) 1 (2) 2 (3) 3 (4) 4 correct 128 6/07-21 • A double carbon-carbon bond is found in a molecule of (1) pentane (2) pentene (3) pentyne (4) pentanol 129 6/07-21 • A double carbon-carbon bond is found in a molecule of (1) pentane (2) pentene (3) pentyne (4) pentanol correct 130 6/07-22 • Which changes occur when Pt2+ is reduced? (1) The Pt2+ gains electrons and its oxidation number increases (2) The Pt2+ gains electrons and its oxidation number decreases (3) The Pt2+ loses electrons and its oxidation number increases (4) The Pt2+ loses electrons and its oxidation number decreases 131 6/07-22 • Which changes occur when Pt2+ is reduced? (1) The Pt2+ gains electrons and its oxidation number increases (2) The Pt2+ gains electrons and its oxidation number decreases correct (3) The Pt2+ loses electrons and its oxidation number increases (4) The Pt2+ loses electrons and its oxidation number decreases 132 6/07-23 • Which balanced equation represents an oxidation-reduction reaction? (1) 1 (2) 2 (3) 3 (4) 4 133 6/07-23 • Which balanced equation represents an oxidation-reduction reaction? (1) 1 (2) 2 (3) 3 (4) 4 correct 134 6/07-24 • Which energy conversion occurs during the operation of a voltaic cell? (1) Chemical energy is spontaneously converted to electrical energy (2) Chemical energy is converted to electrical energy only when an external power source is provided (3) Electrical energy is spontaneously converted to chemical energy (4) Electrical energy is converted to chemical energy only when an external power source is provided 135 6/07-24 • Which energy conversion occurs during the operation of a voltaic cell? (1) Chemical energy is spontaneously converted to electrical energy correct (2) Chemical energy is converted to electrical energy only when an external power source is provided (3) Electrical energy is spontaneously converted to chemical energy (4) Electrical energy is converted to chemical energy only when an external power source is provided 136 6/07-25 • An Arrhenius base yields which ion as the only negative ion in an aqueous solution? (1) Hydride ion (2) Hydrogen ion (3) Hydronium ion (4) Hydroxide ion 137 6/07-25 • An Arrhenius base yields which ion as the only negative ion in an aqueous solution? (1) Hydride ion (2) Hydrogen ion (3) Hydronium ion (4) Hydroxide ion correct 138 6/07-26 • According to the acid-base theory, a water molecule acts as an acid when the water molecule (1) Accepts H- (2) Accepts OH- (3) Donates a H+ (4) Donates an OH- 139 6/07-26 • According to the acid-base theory, a water molecule acts as an acid when the water molecule (1) Accepts H(3) Donates a H+ (2) Accepts OH- correct (4) Donates an OH- 140 6/07-27 • Which list of radioisotopes contains an alpha emitter, a beta emitter, and a positron emitter? (1) C-14, N-16, P-32 (2) Cs-137, Fr-220, Tc-99 (3) Kr-85, Ne-19, Rn-222 (4) Pu-239, Th-232, U-238 141 6/07-27 • Which list of radioisotopes contains an alpha emitter, a beta emitter, and a positron emitter? (1) C-14, N-16, P-32 (3) Kr-85, Ne-19, Rn-222 (2) Cs-137, Fr-220, Tc-99 correct (4) Pu-239, Th-232, U-238 142 6/07-28 • Which nuclear decay emission consists of energy, only? (1) alpha particle (2) Beta particle (3) gamma radiation (4) positron 143 6/07-28 • Which nuclear decay emission consists of energy, only? (1) alpha particle (3) gamma radiation (2) Beta particle correct (4) positron 144 6/07-29 • Which balanced equation represents nuclear fusion? (1) 1 (2) 2 (3) 3 (4) 4 145 6/07-29 • Which balanced equation represents nuclear fusion? (1) 1 (2) 2 (3) 3 (4) 4 correct 146 6/07-30 • The energy released by a nuclear reaction results primarily from the (1) Breaking of bonds between atoms (2) Formation of bonds between atoms (3) Conversion of mass into energy (4) Conversion of energy into mass 147 6/07-30 • The energy released by a nuclear reaction results primarily from the (1) Breaking of bonds between atoms (2) Formation of bonds between atoms (3) Conversion of mass into energy (4) Conversion of energy into mass correct 148 6/07-33 • What is the total number of neutrons in an atom of 26Fe57? (1) 26 (2) 31 (3) 57 (4) 83 149 6/07-33 • What is the total number of neutrons in an atom of 26Fe57? (1) 26 (2) 31 (3) 57 (4) 83 correct 150 6/07-34 • At STP, which element is brittle and not a conductor of electricity? (1) S (2) K (3) Na (4) Ar 151 6/07-34 • At STP, which element is brittle and not a conductor of electricity? (1) S (3) Na correct (2) K (4) Ar 152 6/07-35 • What is the total number of electrons in a Mg2+ ion? (1) 10 (2) 12 (3) 14 (4) 24 153 6/07-35 • What is the total number of electrons in a Mg2+ ion? (1) 10 (3) 14 correct (2) 12 (4) 24 154 6/07-36 • Which formula represents lead(II) chromate? (1) PbCrO4 (2) Pb(CrO4)2 (3) Pb2CrO4 (4) Pb2(CrO4)3 155 6/07-36 • Which formula represents lead(II) chromate? (1) PbCrO4 (3) Pb2CrO4 correct (2) Pb(CrO4)2 (4) Pb2(CrO4)3 156 6/07-37 • Compared to an electron in the first electron shell of an atom, an electron in the third shell of the same atom has (1) Less mass (2) Less energy (3) More mass (4) More energy 157 6/07-37 • Compared to an electron in the first electron shell of an atom, an electron in the third shell of the same atom has (1) Less mass (2) Less energy (3) More mass (4) More energy correct 158 6/07-38 • Which pair consists of a molecular formula and its corresponding empirical formula? (1) C2H2 and CH3CH3 (2) C6H6 and C2H2 (3) P4O10 and P2O5 (4) SO2 and SO3 159 6/07-38 • Which pair consists of a molecular formula and its corresponding empirical formula? (1) C2H2 and CH3CH3 (3) P4O10 and P2O5 (2) C6H6 and C2H2 correct (4) SO2 and SO3 160 6/07-41 • At STP, fluorine is a gas and bromine is a liquid because, compared to fluorine, bromine has (1) Stronger covalent bonds (2) Stronger intermolecular forces (3) Weaker covalent bonds (4) Weaker intermolecular forces 161 6/07-41 • At STP, fluorine is a gas and bromine is a liquid because, compared to fluorine, bromine has (1) Stronger covalent bonds (2) Stronger intermolecular forces correct (3) Weaker covalent bonds (4) Weaker intermolecular forces 162 6/07-41 • At STP, fluorine is a gas and bromine is a liquid because, compared to fluorine, bromine has (1) Stronger covalent bonds (2) Stronger intermolecular forces correct (3) Weaker covalent bonds (4) Weaker intermolecular forces 163 6/07-42 • The boiling point of a liquid is the temperature at which the vapoir pressure of the liquid is equal to the pressure on the surface of the liquid. What is the boiling point of propanone if the pressure on its surface is 48 kilopascals? (1) 25°C (2) 30.°C (3) 35°C (4) 40.°C 164 6/07-42 • The boiling point of a liquid is the temperature at which the vapoir pressure of the liquid is equal to the pressure on the surface of the liquid. What is the boiling point of propanone if the pressure on its surface is 48 kilopascals? (1) 25°C (3) 35°C (2) 30.°C correct (4) 40.°C 165 6/07-42 • The boiling point of a liquid is the temperature at which the vapoir pressure of the liquid is equal to the pressure on the surface of the liquid. What is the boiling point of propanone if the pressure on its surface is 48 kilopascals? (1) 25°C (3) 35°C (2) 30.°C correct (4) 40.°C 166 6/07-43 • At which Celsius temperature does lead change from a solid to a liquid? (1) 874°C (2) 601°C (3) 328°C (4) 0°C 167 6/07-43 • At which Celsius temperature does lead change from a solid to a liquid? (1) 874°C (3) 328°C (2) 601°C correct (4) 0°C 168 6/07-44 • Given the equation representing a reaction at equilibrium: N2(g) + 3H2(g) = 2NH3(g) + energy Which change causes the equilibrium to shift to the right? (1) Decreasing the concentration of H2(g) (2) Decreasing the pressure (3) Increasing the concentration of N2(g) (4) Increasing the temperature 169 6/07-44 • Given the equation representing a reaction at equilibrium: N2(g) + 3H2(g) = 2NH3(g) + energy Which change causes the equilibrium to shift to the right? (1) Decreasing the concentration of H2(g) (2) Decreasing the pressure (3) Increasing the concentration of N2(g) (4) Increasing the temperature correct 170 6/07-45 • Which compound is an unsaturated hydrocarbon? (1) hexanal (2) hexane (3) Hexanoic acid (4) hexyne 171 6/07-45 • Which compound is an unsaturated hydrocarbon? (1) hexanal (2) hexane (3) Hexanoic acid (4) hexyne correct 172 6/07-46 • The organic compound represented by the condensed structural formula CH3CH2CH2CHO is classified as an (1) alcohol (2) aldehyde (3) ester (4) ether 173 6/07-46 • The organic compound represented by the condensed structural formula CH3CH2CH2CHO is classified as an (1) alcohol (2) aldehyde (3) ester (4) ether correct 174 6/07-47 • (1) Al to Mg2+ (2) Al3+ to Mg (3) Mg to Al3+ (4) Mg2+ to Al 175 6/07-47 • (1) Al to Mg2+ (3) Mg to Al3+ (2) Al3+ to Mg correct (4) Mg2+ to Al 176 6/07-48 • Which two formulas represent Arrhenius acids? (1) 1 (2) 2 (3) 3 (4) 4 177 6/07-48 • Which two formulas represent Arrhenius acids? (1) 1 (2) 2 (3) 3 (4) 4 178 6/07-49 • Information about a titration experiment is given in the balanced equation and table below. correct Based on the equation and results, what is the concentration of H2SO4(aq)? (1) 0.12 M (2) 0.24 M (3) 0.16 M (4) 0.96 M 179 6/07-49 • Information about a titration experiment is given in the balanced equation and table below. correct Based on the equation and results, what is the concentration of H2SO4(aq)? (1) 0.12 M (2) 0.24 M (3) 0.16 M (4) 0.96 M correct 180 6/07-50 • Which radioisotope is used in medicine to treat thyroid disorders? (1) cobalt-60 (2) iodine-131 (3) phosphorous-32 (4) uranium-238 181 6/07-50 • Which radioisotope is used in medicine to treat thyroid disorders? (1) cobalt-60 (2) iodine-131 (3) phosphorous-32 (4) uranium-238 correct 182 8/07-1 • What was concluded about the structure of the atom as a result of the gold foil experiment? (1) A positively charged nucleus was surrounded by positively charged particles (2) A positively charged nucleus was surrounded by mostly empty space (3) A negatively charged nucleus is surrounded by positively charged particles (4) A negatively charged nucleus is surrounded by mostly empty space 183 8/07-1 • What was concluded about the structure of the atom as a result of the gold foil experiment? (1) A positively charged nucleus was surrounded by positively charged particles (2) A positively charged nucleus was surrounded by mostly empty space (3) A negatively charged nucleus is surrounded by positively charged particles (4) A negatively charged nucleus is surrounded by mostly empty space correct 184 8/07-2 • An atom is electrically neutral because (1) Number of protons equals number of electrons (2) Number of protons equals number of neutrons (3) Ratio of the number of neutrons to the (4) Ratio of the number of neutrons to the number electrons is 1:1 number of protons is 2:1 185 8/07-2 • An atom is electrically neutral because (1) Number of protons equals number of correct electrons (2) Number of protons equals number of neutrons (3) Ratio of the number of neutrons to the (4) Ratio of the number of neutrons to the number electrons is 1:1 number of protons is 2:1 186 8/07-3 • How do energy and the most probable location of an electron in the third shell of an atom compare to the energy and most probable location of an electron in the first shell of the same atom? (1) In the third shell, the electron has more energy and is closer to the nucleus (2) In the third shell, an electron has more energy and is farther from the nucleus (3) In the third shell, an electron has less energy and is closer to the nucleus (4) In the third shell, an electron has less energy and is farther from the nucleus 187 8/07-3 • How do energy and the most probable location of an electron in the third shell of an atom compare to the energy and most probable location of an electron in the first shell of the same atom? (1) In the third shell, the electron has more energy and is closer to the nucleus (2) In the third shell, an electron has more energy and is farther from the nucleus (3) In the third shell, an electron has less energy and is closer to the nucleus (4) In the third shell, an electron has less energy and is farther from the nucleus correct 188 8/07-4 • Which element is a solid at STP and a good conductor of electricity? (1) iodine (2) mercury (3) nickel (4) sulfur 189 8/07-4 • Which element is a solid at STP and a good conductor of electricity? (1) iodine (3) nickel (2) mercury correct (4) sulfur 190 8/07-5 • Which element has both metallic and nonmetallic properties? (1) Rb (2) Rn (3) Si (4) Sr 191 8/07-5 • Which element has both metallic and nonmetallic properties? (1) Rb (3) Si (2) Rn correct (4) Sr 192 8/07-6 • The carbon atoms in graphite and the carbon atoms in diamond have different (1) Atomic numbers (2) Atomic masses (3) electronegativities (4) Structural arrangements 193 8/07-6 • The carbon atoms in graphite and the carbon atoms in diamond have different (1) Atomic numbers (2) Atomic masses (3) electronegativities (4) Structural arrangements correct 194 8/07-7 • Which element has the greatest tendency to gain electrons? (1) bromine (2) chlorine (3) fluorine (4) iodine 195 8/07-7 • Which element has the greatest tendency to gain electrons? (1) bromine (3) fluorine (2) chlorine correct (4) iodine 196 8/07-8 • Which statement describes a chemical property of the element magnesium? (1) Magnesium is malleable (2) Magnesium conducts electricity (3) Magnesium reacts with an acid (4) Magnesium has a high boiling point 197 8/07-8 • Which statement describes a chemical property of the element magnesium? (1) Magnesium is malleable (2) Magnesium conducts electricity (3) Magnesium reacts with an acid (4) Magnesium has a high boiling point correct 198 8/07-9 • Matter that is composed of two or more different elements chemically combined in a fixed proportion is classified as (1) A compound (2) An isotope (3) A mixture (4) A solution 199 8/07-9 • Matter that is composed of two or more different elements chemically combined in a fixed proportion is classified as (1) A compound (2) An isotope (3) A mixture (4) A solution correct 200 8/07-10 • Given the balanced equation representing a reaction: 2CO(g) + O2(g) -> 2CO2(g) What is the mole ratio of CO(g) to CO2(g) in this reaction? (1) 1:1 (2) 1:2 (3) 2:1 (4) 3:2 201 8/07-10 • Given the balanced equation representing a reaction: 2CO(g) + O2(g) -> 2CO2(g) What is the mole ratio of CO(g) to CO2(g) in this reaction? (1) 1:1 (3) 2:1 correct (2) 1:2 (4) 3:2 202 8/07-11 • Given the balanced equation representing a reaction: H+(aq) OH-(aq) -> H2O(l) + 58 kJ In this reaction there is conservation of (1) Mass, only (2) Mass and charge, only (3) Mass and energy, only (4) mass, charge, and energy 203 8/07-11 • Given the balanced equation representing a reaction: H+(aq) OH-(aq) -> H2O(l) + 58 kJ In this reaction there is conservation of (1) Mass, only (2) Mass and charge, only (3) Mass and energy, only (4) mass, charge, and energy correct 204 8/07-12 • Which polyatomic ion contains the greatest number of oxygen atoms? (1) acetate (2) carbonate (3) hydroxide (4) peroxide 205 8/07-12 • Which polyatomic ion contains the greatest number of oxygen atoms? (1) acetate (2) carbonate (3) hydroxide (4) peroxide correct 206 8/07-13 • Which formula represents an ionic compound? (1) H2 (2) CH4 (3) CH3OH (4) NH4Cl 207 8/07-13 • Which formula represents an ionic compound? (1) H2 (2) CH4 (3) CH3OH (4) NH4Cl correct 208 8/07-14 • An ion of which element has a larger radius than an atom of the same element? (1) aluminum (2) chlorine (3) magnesium (4) sodium 209 8/07-14 • An ion of which element has a larger radius than an atom of the same element? (1) aluminum (2) chlorine (3) magnesium (4) sodium correct 210 8/07-15 • Which statement must be true when solution equilibrium occurs? (1) The solution is at STP (2) The solution is supersaturated (3) The concentration of the solution remains constant (4) The masses of the dissolved solute and the undissolved solute are equal 211 8/07-15 • Which statement must be true when solution equilibrium occurs? (1) The solution is at STP (2) The solution is supersaturated (3) The concentration of the solution correct remains constant (4) The masses of the dissolved solute and the undissolved solute are equal 212 8/07-16 • Which liquid has the highest vapor pressure at 75°C? (1) ethanoic acid (2) ethanol (3) propanone (4) water 213 8/07-16 • Which liquid has the highest vapor pressure at 75°C? (1) ethanoic acid (2) ethanol (3) propanone (4) water correct 214 8/07-17 • What is the total number of different elements present in NH4NO3? (1) 7 (2) 9 (3) 3 (4) 4 215 8/07-17 • What is the total number of different elements present in NH4NO3? (1) 7 (2) 9 (3) 3 (4) 4 correct 216 8/07-18 • Which sample of matter is a single substance? (1) Air (2) Ammonia gas (3) Hydrochloric acid (4) Salt water 217 8/07-18 • Which sample of matter is a single substance? (1) Air (2) Ammonia gas (3) Hydrochloric acid (4) Salt water correct 218 8/07-19 • At STP, which sample contains the same number of molecules as 11.2 liters of CO2(g) at STP (1) 5.6 liters of NO(g) (2) 11.2 liters of N2(g) (3) 7.5 liters of H2(g) (4) 22.4 liters of CO(g) 219 8/07-19 • At STP, which sample contains the same number of molecules as 11.2 liters of CO2(g) at STP (1) 5.6 liters of NO(g) (2) 11.2 liters of N2(g) (3) 7.5 liters of H2(g) (4) 22.4 liters of CO(g) correct 220 8/07-20 • A sample of gas is held at a constant pressure. Increasing the Kelvin temperature of this gas sample causes the average kinetic energy of its molecules to (1) Decrease and the volume of the gas sample to decrease (2) Decrease and the volume of the gas sample to increase (3) Increase and the volume of this gas sample to decrease (4) Increase and the volume of this gas sample to increase 221 8/07-20 • A sample of gas is held at a constant pressure. Increasing the Kelvin temperature of this gas sample causes the average kinetic energy of its molecules to (1) Decrease and the volume of the gas sample to decrease (2) Decrease and the volume of the gas sample to increase (3) Increase and the volume of this gas sample to decrease (4) Increase and the volume of this gas correct sample to increase 222 8/07-21 • Given the balanced equation representing a reaction: Cl2(g) -> Cl(g) + Cl(g) What occurs during this change? (1) Energy is absorbed and a bond is broken (2) Energy is absorbed and a bond is formed (3) Energy is released and a bond is broken (4) Energy is released and a bond if formed 223 8/07-21 • Given the balanced equation representing a reaction: Cl2(g) -> Cl(g) + Cl(g) What occurs during this change? (1) Energy is absorbed and a bond is correct broken (2) Energy is absorbed and a bond is formed (3) Energy is released and a bond is broken (4) Energy is released and a bond if formed 224 8/07-22 • A molecule of butane and a molecule of 2-butene both have the same total number of (1) Carbon atoms (2) Hydrogen atoms (3) Single bonds (4) Double bonds 225 8/07-22 • A molecule of butane and a molecule of 2-butene both have the same total number of (1) Carbon atoms (2) Hydrogen atoms correct (3) Single bonds (4) Double bonds 226 8/07-23 • Which general formula represents the homologous series of hydrocarbons that includes the compound 1-heptyne? (1) CnH2n-6 (2) CnH2n-2 (3) CnH2n (4) CnH2n+2 227 8/07-23 • Which general formula represents the homologous series of hydrocarbons that includes the compound 1-heptyne? (1) CnH2n-6 (2) CnH2n-2 correct (3) CnH2n (4) CnH2n+2 228 8/07-24 • Which two compounds are isomers of each other? (1) 1 (2) 2 (3) 3 (4) 4 229 8/07-24 • Which two compounds are isomers of each other? (1) 1 (2) 2 correct (3) 3 (4) 4 230 8/07-26 • Which formula represents the hydronium ion? (1) H3O+ (2) NH4+ (3) OH- (4) HCO3- 231 8/07-26 • Which formula represents the hydronium ion? (1) H3O+ (3) OH- correct (2) NH4+ (4) HCO3- 232 8/07-27 • Which compound is an Arrhenius acid? (1) H2SO4 (2) KCl (3) NaOH (4) NH3 233 8/07-27 • Which compound is an Arrhenius acid? (1) H2SO4 (3) NaOH correct (2) KCl (4) NH3 234 8/07-28 • What is the decay mode of 37K? (1) beta (2) positron (3) gamma (4) alpha 235 8/07-28 • What is the decay mode of 37K? (1) beta (2) positron (3) gamma (4) alpha correct 236 8/07-29 • Which nuclear emission has the greatest penetrating power? (1) Alpha particle (2) Beta particle (3) Gamma radiation (4) Positron 237 8/07-29 • Which nuclear emission has the greatest penetrating power? (1) Alpha particle (3) Gamma radiation (2) Beta particle correct (4) Positron 238 8/07-30 • What is the mass number of an alpha particle? (1) 1 (2) 2 (3) 0 (4) 4 239 8/07-30 • What is the mass number of an alpha particle? (1) 1 (2) 2 (3) 0 (4) 4 correct 240 8/07-31 • What is the net charge on an ion that has 9 protons, 11 neutrons, and 10 electrons? (1) 1+ (2) 2+ (3) 1- (4) 2- 241 8/07-31 • What is the net charge on an ion that has 9 protons, 11 neutrons, and 10 electrons? (1) 1+ (3) 1- (2) 2+ correct (4) 2- 242 8/07-32 • Which two particles make up most of the mass of a hydrogen-2 atom? (1) Electron and neutron (2) Electron and proton (3) Proton and neutron (4) Proton and positron 243 8/07-32 • Which two particles make up most of the mass of a hydrogen-2 atom? (1) Electron and neutron (3) Proton and neutron (2) Electron and proton correct (4) Proton and positron 244 8/07-33 • Which statement explains why sulfur is classified as a Group 16 element? (1) A sulfur atom has 6 valence electrons (2) A sulfur atom has 16 neutrons (3) Sulfur is a yellow solid at STP (4) Sulfur reacts with most metals 245 8/07-33 • Which statement explains why sulfur is classified as a Group 16 element? (1) A sulfur atom has 6 valence electrons (2) A sulfur atom has 16 neutrons (3) Sulfur is a yellow solid at STP (4) Sulfur reacts with most metals correct 246 8/07-34 • How do the atomic radius and metallic properties of sodium compare to the atomic radius and metallic properties of phosphorous? (1) Sodium has a larger atomic radius and is more metallic (2) Sodium has a larger atomic radius and is less metallic (3) Sodium has a smaller atomic radius and is more metallic (4) Sodium has a smaller atomic radius and is less metallic 247 8/07-34 • How do the atomic radius and metallic properties of sodium compare to the atomic radius and metallic properties of phosphorous? (1) Sodium has a larger atomic radius and correct is more metallic (2) Sodium has a larger atomic radius and is less metallic (3) Sodium has a smaller atomic radius and is more metallic (4) Sodium has a smaller atomic radius and is less metallic 248 8/07-35 • A compound has a molar mass of 90. grams per mole and the empirical formula CH2O. What is the molecular formula for this compound? (1) CH2O (2) C2H4O2 (3) C3H6O3 (4) C4H8O4 249 8/07-35 • A compound has a molar mass of 90. grams per mole and the empirical formula CH2O. What is the molecular formula for this compound? (1) CH2O (3) C3H6O3 (2) C2H4O2 correct (4) C4H8O4 250 8/07-36 • At standard pressure, a certain compound has a low boiling point and is insoluble in water. At STP, this compound most likely exists as (1) Ionic crystals (2) Metallic crystals (3) Nonpolar molecules (4) Polar molecules 251 8/07-36 • At standard pressure, a certain compound has a low boiling point and is insoluble in water. At STP, this compound most likely exists as (1) Ionic crystals (3) Nonpolar molecules (2) Metallic crystals correct (4) Polar molecules 252 8/07-38 • Which group on the Periodic Table of the Elements contains elements that react with oxygen to form compounds with the general formula X2O? (1) Group 1 (2) Group 2 (3) Group 14 (4) Group 18 253 8/07-38 • Which group on the Periodic Table of the Elements contains elements that react with oxygen to form compounds with the general formula X2O? (1) Group 1 (3) Group 14 correct (2) Group 2 (4) Group 18 254 8/07-39 • A unsaturated solution is formed when 80. grams of a salt is dissolved in 100 grams of water at 40.°C. This salt could be (1) KCl (2) KNO3 (3) NaCl (4) NaNO3 255 8/07-39 • A unsaturated solution is formed when 80. grams of a salt is dissolved in 100 grams of water at 40.°C. This salt could be (1) KCl (2) KNO3 (3) NaCl (4) NaNO3 correct 256 8/07-40 • Which Kelvin temperature is equal to 56°C? (1) -329 K (2) -217 K (3) 217 K (4) 329 K 257 8/07-40 • Which Kelvin temperature is equal to 56°C? (1) -329 K (2) -217 K (3) 217 K (4) 329 K correct 258 8/07-42 • Given the balanced equation representing the reaction occuring in a voltaic cell: Zn(s) + Pb2+(aq) -> Zn2+(aq) + Pb(s) In the completed external circuit, the electrons flow from (1) 1 (2) 2 (3) 3 (4) 4 259 8/07-42 • Given the balanced equation representing the reaction occuring in a voltaic cell: Zn(s) + Pb2+(aq) -> Zn2+(aq) + Pb(s) In the completed external circuit, the electrons flow from (1) 1 (3) 3 (2) 2 correct (4) 4 260 8/07-43 • Which balanced equation represents a redox reaction? (1) 1 (2) 2 (3) 3 (4) 4 261 8/07-43 • Which balanced equation represents a redox reaction? (1) 1 (2) 2 (3) 3 (4) 4 correct 262 8/07-44 • Given the unbalanced ionic equation: 3Mg + ____Fe3+ -> 3Mg2+ + ____Fe When this equation is balanced, both Fe3+ and Fe have a coefficient of (1) 1, because a total of 6 electrons is transferred (2) 2, because a total of 6 electrons is transferred (3) 1, because a total of 3 electrons is transferred (4) 2, because a total of 3 electrons is tranferred 263 8/07-44 • Given the unbalanced ionic equation: 3Mg + ____Fe3+ -> 3Mg2+ + ____Fe When this equation is balanced, both Fe3+ and Fe have a coefficient of (1) 1, because a total of 6 electrons is transferred (2) 2, because a total of 6 electrons is correct transferred (3) 1, because a total of 3 electrons is transferred (4) 2, because a total of 3 electrons is tranferred 264 8/07-45 • A student collects the materials and equipment below to construct a voltaic cell •Two 250-mL beakers •Wire and a switch •One strip of magnesium •One strip of copper •125 mL of 0.20 M Mg(NO3)2(aq) •125 mL of 0.20 M Cu(NO3)2(aq) Which additional item is required for the construction of the voltaic cell? (1) An anode (2) A battery (3) A cathode (4) A salt bridge 265 8/07-45 • A student collects the materials and equipment below to construct a voltaic cell •Two 250-mL beakers •Wire and a switch •One strip of magnesium •One strip of copper •125 mL of 0.20 M Mg(NO3)2(aq) •125 mL of 0.20 M Cu(NO3)2(aq) Which additional item is required for the construction of the voltaic cell? (1) An anode (2) A battery (3) A cathode (4) A salt bridge correct 266 8/07-48 • What is the pH of a solution that has hydronium ion concentration 100 times greater than a solution with a pH of 4? (1) 5 (2) 2 (3) 3 (4) 6 267 8/07-48 • What is the pH of a solution that has hydronium ion concentration 100 times greater than a solution with a pH of 4? (1) 5 (2) 2 (3) 3 (4) 6 correct 268 8/07-49 • Which nuclear equation represents a natural transmutation? (1) 1 (2) 2 (3) 3 (4) 4 269 8/07-49 • Which nuclear equation represents a natural transmutation? (1) 1 (2) 2 (3) 3 (4) 4 correct 270 8/07-50 • A nuclear fission reaction and a nuclear fusion reaction are similar because both reactions (1) Form heavy nuclides from light nuclides (2) Form light nuclides from heavy nuclides (3) Release a large amount of energy (4) Absorb a large amount of energy 271 8/07-50 • A nuclear fission reaction and a nuclear fusion reaction are similar because both reactions (1) Form heavy nuclides from light nuclides (2) Form light nuclides from heavy nuclides (3) Release a large amount of energy (4) Absorb a large amount of energy correct 272 1/09-1 • On the modern Periodic Table, the elements are arranged in order of increasing (1) atomic mass (2) mass number (3) atomic number (4) oxidation number 273 1/09-1 • On the modern Periodic Table, the elements are arranged in order of increasing (1) atomic mass (2) mass number (3) atomic number (4) oxidation number correct 274 1/09-2 • Which particle has a mass that is approximately the same as the mass of a proton? (1) an alpha particle (2) a neutron (3) a beta particle (4) a positron 275 1/09-2 • Which particle has a mass that is approximately the same as the mass of a proton? (1) an alpha particle (2) a neutron (3) a beta particle (4) a positron correct 276 1/09-3 • An atom of an element forms a 2+ ion. In which group on the Periodic Table could this element be located? (1) 1 (2) 13 (3) 2 (4) 14 277 1/09-3 • An atom of an element forms a 2+ ion. In which group on the Periodic Table could this element be located? (1) 1 (3) 2 (2) 13 correct (4) 14 278 1/09-4 • Which statement describes the relative energy of the electrons in the shells of a calcium atom? (1) An electron in the first shell has more energy than an electron in the second shell. (2) An electron in the first shell has the same amount of energy as an electron in the second shell. (3) An electron in the third shell has more energy than an electron in the second shell. (4) An electron in the third shell has less energy than an electron in second shell. 279 1/09-4 • Which statement describes the relative energy of the electrons in the shells of a calcium atom? (1) An electron in the first shell has more energy than an electron in the second shell. (2) An electron in the first shell has the same amount of energy as an electron in the second shell. (3) An electron in the third shell has more energy than an electron in the second correct shell. (4) An electron in the third shell has less energy than an electron in second shell. 280 1/09-5 • According to the electron-cloud model of the atom, an orbital is a (1) circular path traveled by an electron around the nucleus (2) spiral path traveled by the electron toward the nucleus (3) region of the most probable proton location (4) region of the most probable electron location 281 1/09-5 • According to the electron-cloud model of the atom, an orbital is a (1) circular path traveled by an electron around the nucleus (2) spiral path traveled by the electron toward the nucleus (3) region of the most probable proton location (4) region of the most probable electron correct location 282 1/09-6 • What can be determined if only the atomic number of an atom is known? (1) the total number of neutrons in the atom, only (2) the total number of protons in the atom, only (3) the total number of protons and the total number of neutrons in the atom (4) the total number of protons and the total number of electrons in the atom 283 1/09-6 • What can be determined if only the atomic number of an atom is known? (1) the total number of neutrons in the atom, only (2) the total number of protons in the atom, only (3) the total number of protons and the total number of neutrons in the atom (4) the total number of protons and the total number of electrons in the atom correct 284 1/09-7 • The most common isotope of chromium has a mass number of 52. Which notation represents a different isotope of chromium? 52 24Cr (2) 24Cr54 (3) 54Cr24 (4) 52Cr24 (1) 285 1/09-7 • The most common isotope of chromium has a mass number of 52. Which notation represents a different isotope of chromium? 52 24Cr (2) 24Cr54 (3) 54Cr24 (4) 52Cr24 (1) correct 286 1/09-8 • Which Group 14 element is a metalloid? (1) tin (2) silicon (3) lead (4) carbon 287 1/09-8 • Which Group 14 element is a metalloid? (1) tin (2) silicon (3) lead (4) carbon correct 288 1/09-9 • Samples of four Group 15 elements, antimony, arsenic, bismuth, and phosphorous, are in the gaseous phase. An atom in the ground state of which element requires the least amount of energy to remove its most loosely held electron? (1) As (2) Bi (3) P (4) Sb 289 1/09-9 • Samples of four Group 15 elements, antimony, arsenic, bismuth, and phosphorous, are in the gaseous phase. An atom in the ground state of which element requires the least amount of energy to remove its most loosely held electron? (1) As (2) Bi (3) P (4) Sb correct 290 1/09-10 • Which substance cab be broken down by chemical means? (1) CO (2) Ce (3) Ca (4) Cu 291 1/09-10 • Which substance cab be broken down by chemical means? (1) CO (3) Ca correct (2) Ce (4) Cu 292 1/09-11 • During all chemical reactions, mass, energy, and charge are (1) absorbed (2) conserved (3) formed (4) released 293 1/09-11 • During all chemical reactions, mass, energy, and charge are (1) absorbed (2) conserved (3) formed (4) released correct 294 1/09-12 • Which formula represents a molecular compound? (1) Kr (2) LiOH (3) N2O4 (4) NaI 295 1/09-12 • Which formula represents a molecular compound? (1) Kr (3) N2O4 (2) LiOH correct (4) NaI 296 1/09-13 • The bonds in BaO are best described as (1) covalent, because valence electrons are shared (2) covalent, because valence electrons are transferred (3) ionic, because valence electrons are shared (4) ionic, because valence electrons are transferred 297 1/09-13 • The bonds in BaO are best described as (1) covalent, because valence electrons are shared (2) covalent, because valence electrons are transferred (3) ionic, because valence electrons are shared (4) ionic, because valence electrons are correct transferred 298 1/09-14 • In which sample of water do the water molecules have the highest average kinetic energy? (1) 20. mL at 100°C (2) 40. mL at 80°C (3) 60. mL at 60°C (4) 80. mL at 40°C 299 1/09-14 • In which sample of water do the water molecules have the highest average kinetic energy? (1) 20. mL at 100°C (3) 60. mL at 60°C correct (2) 40. mL at 80°C (4) 80. mL at 40°C 300 1/09-15 • Which compound is insoluble in water? (1) calcium bromide (2) potassium bromide (3) silver bromide (4) sodium bromide 301 1/09-15 • Which compound is insoluble in water? (1) calcium bromide (3) silver bromide (2) potassium bromide correct (4) sodium bromide 302 1/09-16 • Which element is a brittle solid with low conductivity at STP? (1) sulfur (2) sodium (3) argon (4) aluminum 303 1/09-16 • Which element is a brittle solid with low conductivity at STP? (1) sulfur (3) argon correct (2) sodium (4) aluminum 304 1/09-17 • Which two samples of gas at STP contain the same total number of molecules? (1) 1 L of CO(g) and 0.5L of N2(g) (2) 2 L of CO(g) and 0.5L of NH3(g) (3) 1 L of H2(g) and 2 L of Cl2(g) (4) 2 L of H2(g) and 2 L of Cl2(g) 305 1/09-17 • Which two samples of gas at STP contain the same total number of molecules? (1) 1 L of CO(g) and 0.5L of N2(g) (2) 2 L of CO(g) and 0.5L of NH3(g) (3) 1 L of H2(g) and 2 L of Cl2(g) (4) 2 L of H2(g) and 2 L of Cl2(g) correct 306 1/09-18 • A reaction is most likely to occur when reactant particles collide with (1) proper energy, only (2) proper orientation, only (3) both proper energy and proper orientation (4) neither proper energy nor proper orientation 307 1/09-18 • A reaction is most likely to occur when reactant particles collide with (1) proper energy, only (2) proper orientation, only (3) both proper energy and proper correct orientation (4) neither proper energy nor proper orientation 308 1/09-19 • The net energy released or absorbed during a reversible chemical reaction is equal to (1) the activation energy of the endothermic reaction (2) the activation energy of the exothermic reaction (3) the difference between the potential energy of the reactants and the potential energy of the products (4) the sum of the potential energy of the reactants and the potential energy of the products 309 1/09-19 • The net energy released or absorbed during a reversible chemical reaction is equal to (1) the activation energy of the endothermic reaction (2) the activation energy of the exothermic reaction (3) the difference between the potential energy of the reactants and the potential correct energy of the products (4) the sum of the potential energy of the reactants and the potential energy of the products 310 1/09-20 • A catalyst lowers the activation energy of a reaction by (1) providing an alternate energy pathway (2) decreasing the heat of reaction (3) increasing the mass of the reactants (4) changing the mole ratio of the reaction 311 1/09-21 • Which element is present in every organic compound? (1) carbon (2) fluorine (3) nitrogen (4) oxygen 312 1/09-21 • Which element is present in every organic compound? (1) carbon (3) nitrogen correct (2) fluorine (4) oxygen 313 1/09-22 • Given the balanced equation representing a reaction: 2Fe + 3Cu2+ -> 2Fe3+ + 3Cu When the iron atoms lose six moles of electrons, how many moles of electrons are gained by the copper ions? (1) 12 moles (2) 2 moles (3) 3 moles (4) 6 moles 314 1/09-22 • Given the balanced equation representing a reaction: 2Fe + 3Cu2+ -> 2Fe3+ + 3Cu When the iron atoms lose six moles of electrons, how many moles of electrons are gained by the copper ions? (1) 12 moles (2) 2 moles (3) 3 moles (4) 6 moles correct 315 1/09-23 • Which statement describes electrolysis? (1) chemical energy is used to produce an electrical change (2) chemical energy is used to produce a thermal change (3) electrical energy is used to produce a chemical change (4) thermal energy is used to produce a chemical change 316 1/09-23 • Which statement describes electrolysis? (1) chemical energy is used to produce an electrical change (2) chemical energy is used to produce a thermal change (3) electrical energy is used to produce a correct chemical change (4) thermal energy is used to produce a chemical change 317 1/09-24 • During which process does the atom gain one or more electrons? (1) transmutation (2) reduction (3) oxidation (4) neutralization 318 1/09-24 • During which process does the atom gain one or more electrons? (1) transmutation (2) reduction (3) oxidation (4) neutralization correct 319 1/09-25 • Which substance is an Arrhenius base? (1) CH3OH (2) CH3Cl (3) LiOH (4) LiCl 320 1/09-25 • Which substance is an Arrhenius base? (1) CH3OH (3) LiOH (2) CH3Cl correct (4) LiCl 321 1/09-26 • Which statement describes an alternate theory of acids and bases? (1) Acids and bases are both H+ acceptors (2) Acids and bases are both H+ donors (3) Acids are H+ acceptors and bases are H+ donors (4) Acids are H+ donors and bases are H+ acceptors 322 1/09-26 • Which statement describes an alternate theory of acids and bases? (1) Acids and bases are both H+ acceptors (2) Acids and bases are both H+ donors (3) Acids are H+ acceptors and bases are H+ donors (4) Acids are H+ donors and bases are H+ correct acceptors 323 1/09-27 • Which two compounds are electrolytes? (1) C6H12O6 and CH3CH2OH (2) C6H12O6 and HCl (3) NaOH and HCl (4) NaOH and CH3CH2OH 324 1/09-27 • Which two compounds are electrolytes? (1) C6H12O6 and CH3CH2OH (3) NaOH and HCl (2) C6H12O6 and HCl correct (4) NaOH and CH3CH2OH 325 1/09-28 • The only positive ion found in H2SO4(aq) is the (1) ammonium ion (2) hydronium ion (3) hydroxide ion (4) sulfate ion 326 1/09-28 • The only positive ion found in H2SO4(aq) is the (1) ammonium ion (2) hydronium ion (3) hydroxide ion (4) sulfate ion correct 327 1/09-29 • Which risk is associated with using nuclear fission to produce energy in a power plant? (1) depletion of hydrocarbon (2) depletion of atmospheric oxygen (3) exposure of workers to radiation (4) exposure of workers to sulfur dioxide 328 1/09-29 • Which risk is associated with using nuclear fission to produce energy in a power plant? (1) depletion of hydrocarbon (2) depletion of atmospheric oxygen (3) exposure of workers to radiation (4) exposure of workers to sulfur dioxide correct 329 1/09-30 • An unstable nucleus loses most mass if the nucleus emits (1) an alpha particle (2) a beta particle (3) a positron (4) a gamma ray 330 1/09-30 • An unstable nucleus loses most mass if the nucleus emits (1) an alpha particle (3) a positron correct (2) a beta particle (4) a gamma ray 331 1/09-33 • What is the total number of valence electrons in an atom of germanium in the ground state? (1) 8 (2) 2 (3) 14 (4) 4 332 1/09-33 • What is the total number of valence electrons in an atom of germanium in the ground state? (1) 8 (2) 2 (3) 14 (4) 4 correct 333 1/09-34 • In the formula X2O5, the symbol X could represent an element in Group (1) 1 (2) 2 (3) 15 (4) 18 334 1/09-35 • A 50.0-gram block of copper at 10.0°C is carefully lowered into 100.0 grams of water at 90.0°C in an insulated container. Which statement describes the transfer of heat in this system? (1) The water loses heat to the block until both are at 10.0°C. (2) The block gains heat from the water until both are at 90.0°C. (3) The water loses heat and the block gains heat until both are at the same temperature that is between 10.0°C and 90.0°C. (4) The water gains heat and the block loses heat until both are at the same temperature that is between 10.0°C and 90.0°C. 335 1/09-35 • A 50.0-gram block of copper at 10.0°C is carefully lowered into 100.0 grams of water at 90.0°C in an insulated container. Which statement describes the transfer of heat in this system? (1) The water loses heat to the block until both are at 10.0°C. (2) The block gains heat from the water until both are at 90.0°C. (3) The water loses heat and the block gains heat until both are at the same temperature that is between 10.0°C and correct 90.0°C. (4) The water gains heat and the block loses heat until both are at the same temperature that is between 10.0°C and 90.0°C. 336 1/09-36 • The compounds C2H4 and C4H8 have the same (1) freezing point at standard pressure (2) boiling point at standard pressure (3) molecular formula (4) empirical formula 337 1/09-36 • The compounds C2H4 and C4H8 have the same (1) freezing point at standard pressure (2) boiling point at standard pressure (3) molecular formula (4) empirical formula correct 338 1/09-37 • The chemical bond between which two atoms is most polar? (1) C-N (2) H-H (3) S-Cl (4) Si-O 339 1/09-37 • The chemical bond between which two atoms is most polar? (1) C-N (2) H-H (3) S-Cl (4) Si-O correct 340 1/09-38 • What is the total amount of heat absorbed by 100.0 grams of water when the temperature of the water is increased from 30.0°C to 45.0°C? (1) 418 J (2) 6270 J (3) 12,500 J (4) 18,800 J 341 1/09-38 • What is the total amount of heat absorbed by 100.0 grams of water when the temperature of the water is increased from 30.0°C to 45.0°C? (1) 418 J (2) 6270 J (3) 12,500 J (4) 18,800 J correct 342 1/09-39 • Which process is exothermic? (1) boiling water (2) melting copper (3) condensing of ethanol vapor (4) sublimation of iodine 343 1/09-39 • Which process is exothermic? (1) boiling water (2) melting copper (3) condensing of ethanol vapor (4) sublimation of iodine correct 344 1/09-40 • Which sample, when dissolved in 1.0 liter of water, produces a solution with the lowest freezing point? (1) 0.1 mol of C2H5OH (2) 0.1 mol of LiBr (3) 0.2 mol of C6H12O6 (4) 0.2 mol of CaCl2 345 1/09-40 • Which sample, when dissolved in 1.0 liter of water, produces a solution with the lowest freezing point? (1) 0.1 mol of C2H5OH (2) 0.1 mol of LiBr (3) 0.2 mol of C6H12O6 (4) 0.2 mol of CaCl2 correct 346 1/09-43 • Which compound is an alkyne? (1) C2H2 (2) C2H4 (3) C4H8 (4) C4H10 347 1/09-43 • Which compound is an alkyne? (1) C2H2 (3) C4H8 correct (2) C2H4 (4) C4H10 348 1/09-44 • What is the oxidation state of sulfur in Na2S2O3? (1) -1 (2) +2 (3) +6 (4) +4 349 1/09-44 • What is the oxidation state of sulfur in Na2S2O3? (1) -1 (2) +2 (3) +6 (4) +4 correct 350 1/09-47 • A 25.0-milliliter sample of HNO3(aq) is neutralized by 32.1 milliliters of 0.150 M KOH(aq). What is the molarity of the HNO3(aq)? (1) 0.117 M (2) 0.150 M (3) 0.193 M (4) 0.300 M 351 1/09-47 • A 25.0-milliliter sample of HNO3(aq) is neutralized by 32.1 milliliters of 0.150 M KOH(aq). What is the molarity of the HNO3(aq)? (1) 0.117 M (3) 0.193 M (2) 0.150 M correct (4) 0.300 M 352 1/09-48 • Which nuclide has a half-life that is less than one minute? (1) cesium-137 (2) francium-220 (3) phosphorous-32 (4) strontium-90 353 1/09-48 • Which nuclide has a half-life that is less than one minute? (1) cesium-137 (2) francium-220 (3) phosphorous-32 (4) strontium-90 correct 354 1/09-50 • Cobalt-60 and iodine-131 are radioactive isotopes that are used in (1) dating geologic formations (2) industrial measurements (3) medical procedures (4) nuclear power 355 1/09-50 • Cobalt-60 and iodine-131 are radioactive isotopes that are used in (1) dating geologic formations (2) industrial measurements (3) medical procedures (4) nuclear power correct 356 1/08-1 • Which quantity indentifies an element? (1) atomic number (2) mass number (3) total number of neutrons in an atom of an element (4) total number of valence electrons in an atom of an element 357 1/08-1 • Which quantity indentifies an element? (1) atomic number correct (3) total number of neutrons in an atom of an element (2) mass number (4) total number of valence electrons in an atom of an element 358 1/08-2 • Which atom in the ground state has a partially filled second electron shell? (1) hydrogen atom (2) lithium atom (3) potassium atom (4) sodium atom 359 1/08-2 • Which atom in the ground state has a partially filled second electron shell? (1) hydrogen atom (2) lithium atom (3) potassium atom (4) sodium atom correct 360 1/08-3 • What is the total charge of the nucleus of a nitrogen atom? (1) +5 (2) +2 (3) +7 (4) +14 361 1/08-3 • What is the total charge of the nucleus of a nitrogen atom? (1) +5 (3) +7 (2) +2 correct (4) +14 362 1/08-4 • Which value of an element is calculated using both the mass and the relative abundance of each of the naturally occurring isotopes of this element? (1) atomic number (2) atomic mass (3) half-life (4) molar volume 363 1/08-4 • Which value of an element is calculated using both the mass and the relative abundance of each of the naturally occurring isotopes of this element? (1) atomic number (2) atomic mass (3) half-life (4) molar volume correct 364 1/08-5 • The mass of 12 protons is approximately equal to (1) 1 atomic mass unit (2) 12 atomic mass units (3) the mass of 1 electron (4) the mass of 12 electrons 365 1/08-5 • The mass of 12 protons is approximately equal to (1) 1 atomic mass unit (2) 12 atomic mass units (3) the mass of 1 electron (4) the mass of 12 electrons correct 366 1/08-6 • Sodium atoms, potassium atoms, and cesium atoms have the same (1) atomic radius (2) first ionization energy (3) total number of protons (4) oxidation state 367 1/08-6 • Sodium atoms, potassium atoms, and cesium atoms have the same (1) atomic radius (2) first ionization energy (3) total number of protons (4) oxidation state correct 368 1/08-7 • Which statement describes a chemical property of hydrogen gas? (1) hydrogen burns in air (2) hydrogen gas is colorless (3) hydrogen gas has a density of 0.00009 g/cm3 (4) hydrogen gas has a boiling point of 20. K at standard pressure. 369 1/08-7 • Which statement describes a chemical property of hydrogen gas? (1) hydrogen burns in air (2) hydrogen gas is colorless (3) hydrogen gas has a density of 0.00009 g/cm3 (4) hydrogen gas has a boiling point of 20. K at standard pressure. correct 370 1/08-8 • Which element has the greatest density at STP? (1) calcium (2) carbon (3) chlorine (4) copper 371 1/08-8 • Which element has the greatest density at STP? (1) calcium (2) carbon (3) chlorine (4) copper correct 372 1/08-9 • Which equation shows conservation of atoms? (1) H2 + O2 -> H2O (2) H2 + O2 -> 2H2O (3) 2H2 + O2 -> 2H2O (4) 2H2 + 2O2 -> 2H2O 373 1/08-9 • Which equation shows conservation of atoms? (1) H2 + O2 -> H2O (3) 2H2 + O2 -> 2H2O (2) H2 + O2 -> 2H2O correct (4) 2H2 + 2O2 -> 2H2O 374 1/08-10 • Which term indicates how strongly an atom attracts the electrons in a chemical bond? (1) alkalinity (2) atomic mass (3) electronegativity (4) activation energy 375 1/08-10 • Which term indicates how strongly an atom attracts the electrons in a chemical bond? (1) alkalinity (3) electronegativity (2) atomic mass correct (4) activation energy 376 1/08-11 • A solid substance is an excellent conductor of electricity. The chemical bonds in this substance are most likely (1) ionic, because the valence electrons are shared between atoms (2) ionic, because the valence electrons are mobile (3) electronegativity (4) activation energy 377 1/08-11 • A solid substance is an excellent conductor of electricity. The chemical bonds in this substance are most likely (1) ionic, because the valence electrons are shared between atoms (2) ionic, because the valence electrons are mobile (3) electronegativity (4) activation energy correct 378 1/08-12 • Magnesium nitrate contains chemical bonds that are (1) covalent, only (2) ionic, only (3) both covalent and ionic (4) neither covalent nor ionic 379 1/08-12 • Magnesium nitrate contains chemical bonds that are (1) covalent, only (3) both covalent and ionic (2) ionic, only correct (4) neither covalent nor ionic 380 1/08-13 • Which substance can be broken down by a chemical change? (1) antimony (2) carbon (3) hexane (4) sulfur 381 1/08-13 • Which substance can be broken down by a chemical change? (1) antimony (3) hexane (2) carbon correct (4) sulfur 382 1/08-14 • Which barium salt is insoluble in water? (1) BaCO3 (2) BaCl2 (3) Ba(ClO4)2 (4) Ba(NO3)2 383 1/08-14 • Which barium salt is insoluble in water? (1) BaCO3 (3) Ba(ClO4)2 correct (2) BaCl2 (4) Ba(NO3)2 384 1/08-16 • Under which conditions of temperature and pressure is a gas most soluble in water? (1) high temperature and low pressure (2) high temperature and high pressure (3) low temperature and low pressure (4) low temperature and high pressure 385 1/08-16 • Under which conditions of temperature and pressure is a gas most soluble in water? (1) high temperature and low pressure (2) high temperature and high pressure (3) low temperature and low pressure (4) low temperature and high pressure correct 386 1/08-15 • Which unit can be used to express solution concentration? (1) J/mol (2) L/mol (3) mol/L (4) mol/s 387 1/08-15 • Which unit can be used to express solution concentration? (1) J/mol (3) mol/L (2) L/mol correct (4) mol/s 388 1/08-17 • Given the equation representing a system at equilibrium: H2O(s) = H2O(l) At which temperature does the equilibrium exist at 101.3 kPa? (1) 0 K (2) 0°C (3) 32 K (4) 273°C 389 1/08-17 • Given the equation representing a system at equilibrium: H2O(s) = H2O(l) At which temperature does the equilibrium exist at 101.3 kPa? (1) 0 K (2) 0°C (3) 32 K (4) 273°C correct 390 1/08-18 • In a redox reaction, the total number of electrons lost is (1) less than the total number of electrons (2) greater than the total number of gained electrons gained (3) equal to the total number of electrons gained (4) equal to the total number of protons gained 391 1/08-18 • In a redox reaction, the total number of electrons lost is (1) less than the total number of electrons (2) greater than the total number of gained electrons gained (3) equal to the total number of electrons correct gained (4) equal to the total number of protons gained 392 1/08-19 • Which formula represents and alkene? (1) C2H6 (2) C3H6 (3) C4H10 (4) C5H12 393 1/08-19 • Which formula represents and alkene? (1) C2H6 (2) C3H6 (3) C4H10 (4) C5H12 correct 394 1/08-20 • Which term refers to the difference between the potential energy of the products and the potential energy of the reactants for any chemical change? (1) heat of decomposition (2) heat of fusion (3) heat of reaction (4) heat of vaporization 395 1/08-20 • Which term refers to the difference between the potential energy of the products and the potential energy of the reactants for any chemical change? (1) heat of decomposition (3) heat of reaction (2) heat of fusion correct (4) heat of vaporization 396 1/08-21 • Which energy conversion occurs in a voltaic cell? (1) chemical energy to electrical energy (2) chemical energy to nuclear energy (3) electrical energy to chemical energy (4) nuclear energy to electrical energy 397 1/08-21 • Which energy conversion occurs in a voltaic cell? (1) chemical energy to electrical energy (2) chemical energy to nuclear energy (3) electrical energy to chemical energy (4) nuclear energy to electrical energy correct 398 1/08-22 • Which metal is more active than Ni and less active than Zn? (1) Cu (2) Cr (3) Mg (4) Pb 399 1/08-22 • Which metal is more active than Ni and less active than Zn? (1) Cu (2) Cr (3) Mg (4) Pb correct 400 1/08-23 • As water is added to a 0.10 M NaCl aqueous solution, the conductivity of the resulting solution (1) decreases because the concentration of the ions decreases (2) decreases, but the concentration of ions remains the same (3) increases because the concentration of ions decreases (4) increases, but the concentration of ions remains the same 401 1/08-23 • As water is added to a 0.10 M NaCl aqueous solution, the conductivity of the resulting solution (1) decreases because the concentration correct of the ions decreases (2) decreases, but the concentration of ions remains the same (3) increases because the concentration of ions decreases (4) increases, but the concentration of ions remains the same 402 1/08-24 • Which substance is an Arrhenius acid? (1) Ba(OH)2 (2) CH3COOCH3 (3) H3PO4 (4) NaCl 403 1/08-24 • Which substance is an Arrhenius acid? (1) Ba(OH)2 (3) H3PO4 (2) CH3COOCH3 correct (4) NaCl 404 1/08-25 • Which compound releases hydroxide ions in an aqueous solution? (1) CH3COOH (2) CH3OH (3) HCl (4) KOH 405 1/08-25 • Which compound releases hydroxide ions in an aqueous solution? (1) CH3COOH (2) CH3OH (3) HCl (4) KOH correct 406 1/08-26 • Which reaction converts an atom of one element to an atom of another element? (1) combustion (2) polymerization (3) saponification (4) transmutation 407 1/08-26 • Which reaction converts an atom of one element to an atom of another element? (1) combustion (2) polymerization (3) saponification (4) transmutation correct 408 1/08-27 • Which nuclear emission has the greatest mass? (1) alpha particle (2) beta particle (3) gamma ray (4) positron 409 1/08-27 • Which nuclear emission has the greatest mass? (1) alpha particle (3) gamma ray correct (2) beta particle (4) positron 410 1/08-28 • Which two isotopes have the same decay mode? (1) 37Ca and 53Fe (2) 220Fr and 60Co (3) 37K and 42K (4) 99Tc and 19Ne 411 1/08-28 • Which two isotopes have the same decay mode? (1) 37Ca and 53Fe (3) 37K and 42K correct (2) 220Fr and 60Co (4) 99Tc and 19Ne 412 1/08-29 • Which list of nuclear emissions is arranged in order from the least penetrating power to the greatest penetrating power? (1) alpha particle, beta particle, gamma ray (2) alpha particle, gamma ray, beta particle (3) gamma ray, beta particle, alpha particle (4) beta particle, alpha particle, gamma ray 413 1/08-29 • Which list of nuclear emissions is arranged in order from the least penetrating power to the greatest penetrating power? (1) alpha particle, beta particle, gamma correct ray (2) alpha particle, gamma ray, beta particle (3) gamma ray, beta particle, alpha particle (4) beta particle, alpha particle, gamma ray 414 1/08-30 • One benefit of nuclear fission reactions is (1) nuclear reactor meltdowns (2) storage of waste materials (3) biological exposure (4) production of energy 415 1/08-30 • One benefit of nuclear fission reactions is (1) nuclear reactor meltdowns (2) storage of waste materials (3) biological exposure (4) production of energy correct 416 1/08-31 • Which list of elements consists of metalloids only? (1) B, Al, Ga (2) C, N, P (3) O, S, Se (4) Si, Ge, As 417 1/08-31 • Which list of elements consists of metalloids only? (1) B, Al, Ga (2) C, N, P (3) O, S, Se (4) Si, Ge, As correct 418 1/08-32 • Which two notations represent different isotopes of the same element? (1) 4Be6 and 4Be9 (2) 3Li7 and 3Li7 (3) 7N14 and 6C14 (4) 15P32 and 16S32 419 1/08-32 • Which two notations represent different isotopes of the same element? (1) 4Be6 and 4Be9 (3) 7N14 and 6C14 correct (2) 3Li7 and 3Li7 (4) 15P32 and 16S32 420 1/08-33 • Which general trend is found in Period 2 on the Periodic Table as the elements are considered in order of increasing atomic number? (1) decreasing atomic mass (2) decreasing electronegativity (3) increasing atomic radius (4) increasing first ionization energy 421 1/08-33 • Which general trend is found in Period 2 on the Periodic Table as the elements are considered in order of increasing atomic number? (1) decreasing atomic mass (2) decreasing electronegativity (3) increasing atomic radius (4) increasing first ionization energy correct 422 1/08-34 • What is the gram-formula mass of Ca3(PO4)2? (1) 248 g/mol (2) 263 g/mol (3) 279 g/mol (4) 310. g/mol 423 1/08-34 • What is the gram-formula mass of Ca3(PO4)2? (1) 248 g/mol (2) 263 g/mol (3) 279 g/mol (4) 310. g/mol correct 424 1/08-36 • When sodium and fluorine combine to produce the compound NaF, the ions formed have the same electron configuration as atoms of (1) argon, only (2) neon, only (3) both argon and neon (4) neither argon nor neon 425 1/08-36 • When sodium and fluorine combine to produce the compound NaF, the ions formed have the same electron configuration as atoms of (1) argon, only (2) neon, only (3) both argon and neon (4) neither argon nor neon correct 426 1/08-35 • What is the total number of pairs of electrons shared between the carbon atom and the oxygen atom in a molecule of methanal? (1) 1 (2) 2 (3) 3 (4) 4 427 1/08-35 • What is the total number of pairs of electrons shared between the carbon atom and the oxygen atom in a molecule of methanal? (1) 1 (2) 2 (3) 3 (4) 4 correct 428 1/08-37 • In which compound is the ratio of metal ions to nonmetal ions 1 to 2? (1) calcium bromide (2) calcium oxide (3) calcium phosphide (4) calcium sulfide 429 1/08-37 • In which compound is the ratio of metal ions to nonmetal ions 1 to 2? (1) calcium bromide (3) calcium phosphide correct (2) calcium oxide (4) calcium sulfide 430 1/08-38 • What is the concentration of O2(g), in parts per million, in a solution that contains 0.008 gram of O2(g) dissolved in 1000. grams of H2O(l)? (1) 0.8 ppm (2) 8 ppm (3) 80 ppm (4) 800 ppm 431 1/08-38 • What is the concentration of O2(g), in parts per million, in a solution that contains 0.008 gram of O2(g) dissolved in 1000. grams of H2O(l)? (1) 0.8 ppm (2) 8 ppm (3) 80 ppm (4) 800 ppm correct 432 1/08-40 • At which temperature is the vapor pressure of ethanol equal to the vapor pressure of propanone at 35°C? (1) 35°C (2) 60.°C (3) 82°C (4) 95°C correct 433 1/08-41 • A rigid cylinder with a moveable piston contains a 2.0-Liter sample of neon gas at STP. What is the volume of this sample of neon gas when its temperature is increased to 30.°C while its pressure is decreased to 90. kilopascals? (1) 2.5 L (2) 2.0 L (3) 1.6 L (4) 0.22 L 434 1/08-41 • A rigid cylinder with a moveable piston contains a 2.0-Liter sample of neon gas at STP. What is the volume of this sample of neon gas when its temperature is increased to 30.°C while its pressure is decreased to 90. kilopascals? (1) 2.5 L (3) 1.6 L correct (2) 2.0 L (4) 0.22 L 435 1/08-42 • Which compound is a saturated hydrocarbon? (1) CH2CH2 (2) CH3CHO (3) CH3CH3 (4) CH3CH2OH 436 1/08-42 • Which compound is a saturated hydrocarbon? (1) CH2CH2 (3) CH3CH3 (2) CH3CHO correct (4) CH3CH2OH 437 1/08-43 • A molecule of a compound contains a total of 10 hydrogen atoms and has the general formula CnH2n+2. Which prefix is used in the name of this compound? (1) but- (2) dec- (3) oct- (4) pent- 438 1/08-43 • A molecule of a compound contains a total of 10 hydrogen atoms and has the general formula CnH2n+2. Which prefix is used in the name of this compound? (1) but(3) oct- correct (2) dec(4) pent- 439 1/08-44 • Reduction occurs at the cathode in (1) electrolytic cells, only (2) voltaic cells, only (3) both electrolytic cells and voltaic cells (4) neither electrolytic cells nor voltaic cells 440 1/08-44 • Reduction occurs at the cathode in (1) electrolytic cells, only (2) voltaic cells, only (3) both electrolytic cells and voltaic cells (4) neither electrolytic cells nor voltaic cells correct 441 1/08-45 • Which are the products of a reaction between KOH(aq) and HCl(aq)? (1) H2 and KClO3 (2) H2O and KCl (3) KH and HClO (4) KOH and HCl 442 1/08-45 • Which are the products of a reaction between KOH(aq) and HCl(aq)? (1) H2 and KClO3 (2) H2O and KCl (3) KH and HClO (4) KOH and HCl correct 443 1/08-46 • Which volume of 0.10 M NaOH(aq) exactly neutralizes 15.0 millimliters of 0.20 M HNO3(aq)? (1) 1.5 mL (2) 7.5 mL (3) 3.0 mL (4) 30. mL 444 1/08-47 • Which indicator, when added to a solution, changes color from yellow to blue as the pH of the solution in changed from 5.5 to 8.0? (1) bromcresol green (2) bromthymol blue (3) litmus (4) methyl orange 445 1/08-47 • Which indicator, when added to a solution, changes color from yellow to blue as the pH of the solution in changed from 5.5 to 8.0? (1) bromcresol green (2) bromthymol blue (3) litmus (4) methyl orange correct 446 1/08-48 • The pH of an aqueous solution changes from 4 to 3 when hydrogen ion concentration in the solution is (1) decreased by a factor of 3/4 (2) decreased by a factor of 10 (3) increased by a factor of 4/3 (4) increased by a factor of 10 447 1/08-48 • The pH of an aqueous solution changes from 4 to 3 when hydrogen ion concentration in the solution is (1) decreased by a factor of 3/4 (2) decreased by a factor of 10 (3) increased by a factor of 4/3 (4) increased by a factor of 10 correct 448 1/08-49 • Which fraction of an original 20.00-gram sample of nitrogen-16 remains unchanged after 36.0 seconds? (1) 1/5 (2) 1/8 (3) 1/16 (4) 1/32 449 1/08-49 • Which fraction of an original 20.00-gram sample of nitrogen-16 remains unchanged after 36.0 seconds? (1) 1/5 (2) 1/8 (3) 1/16 (4) 1/32 correct 450 1/08-50 • Which radioactive isotope is used in treating cancer? (1) carbon-14 (2) cobalt-60 (3) lead-206 (4) uranium-238 451 1/08-50 • Which radioactive isotope is used in treating cancer? (1) carbon-14 (3) lead-206 (2) cobalt-60 correct (4) uranium-238 452 6/08-1 • An atom in the ground state has seven valence electrons. This atom could be an atom of which element? (1) calcium (2) fluorine (3) oxygen (4) sodium 453 6/08-1 • An atom in the ground state has seven valence electrons. This atom could be an atom of which element? (1) calcium (2) fluorine (3) oxygen (4) sodium correct 454 6/08-2 • What is the total number of electrons in an atom of potassium?? (1) 18 (2) 19 (3) 20 (4) 39 455 6/08-2 • What is the total number of electrons in an atom of potassium?? (1) 18 (2) 19 (3) 20 (4) 39 correct 456 6/08-3 • A proton has a charge that is opposite the charge of (1) an alpha particle (2) a neutron (3) an electron (4) a positron 457 6/08-3 • A proton has a charge that is opposite the charge of (1) an alpha particle (3) an electron (2) a neutron correct (4) a positron 458 6/08-4 • Which conclusion was a direct result of the gold foil experiment? (1) An atom is mostly empty space with a dense, positively charged nucleus. (2) An atom is composed of at least three types of subatomic particles. (3) An electron has a positive charge and is located inside the nucleus. (4) An electron has properties of both waves and particles. 459 6/08-4 • Which conclusion was a direct result of the gold foil experiment? (1) An atom is mostly empty space with a dense, positively charged nucleus. (2) An atom is composed of at least three types of subatomic particles. (3) An electron has a positive charge and is located inside the nucleus. (4) An electron has properties of both waves and particles. correct 460 6/08-5 • Which statement identifies the element arsenic? (1) Arsenic has an atomic number of 33. (2) Arsenic has a melting point of 84 K. (3) An atom of arsenic in the ground state has eight valence electrons. (4) An atom of arsenic in the ground state has a radius of 146 pm. 461 6/08-5 • Which statement identifies the element arsenic? (1) Arsenic has an atomic number of 33. (2) Arsenic has a melting point of 84 K. correct (3) An atom of arsenic in the ground state has eight valence electrons. (4) An atom of arsenic in the ground state has a radius of 146 pm. 462 6/08-6 • Which element has an atom with the greatest attraction for electrons in a chemical bond? (1) As (2) Bi (3) N (4) P 463 6/08-6 • Which element has an atom with the greatest attraction for electrons in a chemical bond? (1) As (3) N (2) Bi correct (4) P 464 6/08-7 • Given the balanced equation representing a reaction: H+(aq) + OH-(aq) -> H2O(l) + energy In this reaction there is a conservation of (1) mass, only (2) mass and charge, only (3) charge and energy, only (4) charge , energy, and mass 465 6/08-7 • Given the balanced equation representing a reaction: H+(aq) + OH-(aq) -> H2O(l) + energy In this reaction there is a conservation of (1) mass, only (2) mass and charge, only (3) charge and energy, only (4) charge , energy, and mass correct 466 6/08-8 • Which statement describes the composition of potassium chlorate, KClO3? (1) The proportion by mass of elements combined in potassium chlorate is fixed. (2) The proportion by mass of elements combined in potassium chlorate varies. (3) Potassium chlorate is composed of four elements. (4) Potassium chlorate is composed of five elements. 467 6/08-8 • Which statement describes the composition of potassium chlorate, KClO3? (1) The proportion by mass of elements combined in potassium chlorate is correct fixed. (2) The proportion by mass of elements combined in potassium chlorate varies. (3) Potassium chlorate is composed of four elements. (4) Potassium chlorate is composed of five elements. 468 6/08-9 • As a bond between a hydrogen atom and a sulfur atom is formed, electrons are (1) shared to form an ionic bond (2) shared to form a covalent bond (3) transferred to form an ionic bond (4) transferred to form a covalent bond 469 6/08-9 • As a bond between a hydrogen atom and a sulfur atom is formed, electrons are (1) shared to form an ionic bond (2) shared to form a covalent bond correct (3) transferred to form an ionic bond (4) transferred to form a covalent bond 470 6/08-10 • Atoms of which element can bond to each other to form chains, rings, and networks? (1) carbon (2) fluorine (3) hydrogen (4) oxygen 471 6/08-10 • Atoms of which element can bond to each other to form chains, rings, and networks? (1) carbon (3) hydrogen correct (2) fluorine (4) oxygen 472 6/08-11 • Which formula represents a polar molecule? (1) Br2 (2) CO2 (3) CH4 (4) NH3 473 6/08-11 • Which formula represents a polar molecule? (1) Br2 (2) CO2 (3) CH4 (4) NH3 correct 474 6/08-12 • Two solid sample each contain sulfur, oxygen, and sodium atoms, only. These samples have the same color, melting point, density, and reaction with an aqueous solution of barium chloride solution. It can be concluded that the two samples are the same (1) compound (2) element (3) mixture (4) solution 475 6/08-12 • Two solid sample each contain sulfur, oxygen, and sodium atoms, only. These samples have the same color, melting point, density, and reaction with an aqueous solution of barium chloride solution. It can be concluded that the two samples are the same (1) compound (3) mixture correct (2) element (4) solution 476 6/08-13 • Which equation represents a physical change? (1) 1 (2) 2 (3) 3 (4) 4 477 6/08-13 • Which equation represents a physical change? (1) 1 (3) 3 correct (2) 2 (4) 4 478 6/08-14 • Which liquid has the lowest vapor pressure at 65°C? (1) ethanoic acid (2) propanone (3) ethanol (4) water 479 6/08-14 • Which liquid has the lowest vapor pressure at 65°C? (1) ethanoic acid (3) ethanol correct (2) propanone (4) water 480 6/08-15 • Which substance cannot be broken down by a chemical reaction? (1) ammonia (2) argon (3) methane (4) water 481 6/08-15 • Which substance cannot be broken down by a chemical reaction? (1) ammonia (2) argon (3) methane (4) water correct 482 6/08-16 • In which sample is the average kinetic energy of the particles greatest? (1) 10. mL of HCl(aq) at 25°C (2) 15 mL of HCl(aq) at 20.°C (3) 10. mL of H2O at 35°C (4) 15 mL of H2O at 30.°C 483 6/08-16 • In which sample is the average kinetic energy of the particles greatest? (1) 10. mL of HCl(aq) at 25°C (2) 15 mL of HCl(aq) at 20.°C (3) 10. mL of H2O at 35°C (4) 15 mL of H2O at 30.°C correct 484 6/08-17 • A thermometer is in a beaker of water. Which statement best explains why the thermometer reading initially increases when LiBr(s) is dissolved in the water. (1) The entropy of the LiBr(aq) is greater than the entropy of the water. (2) The entropy of the LiBr(aq) is less than the entropy of the water. (3) The dissolving of the LiBr(s) in water is an endothermic process. (4) The dissolving of LiBr(s) in water is an exothermic process. 485 6/08-17 • A thermometer is in a beaker of water. Which statement best explains why the thermometer reading initially increases when LiBr(s) is dissolved in the water. (1) The entropy of the LiBr(aq) is greater than the entropy of the water. (2) The entropy of the LiBr(aq) is less than the entropy of the water. (3) The dissolving of the LiBr(s) in water is an endothermic process. (4) The dissolving of LiBr(s) in water is an exothermic process. correct 486 6/08-18 • Which process increases the potential energy of the particles in a sample? (1) condensation (2) deposition (3) solidification (4) vaporization 487 6/08-18 • Which process increases the potential energy of the particles in a sample? (1) condensation (2) deposition (3) solidification (4) vaporization correct 488 6/08-19 • Which sample at STP has the same number of molecules as 5 Liters of NO2(g) at STP? (1) 5 grams of H2(g) (2) 5 liters of CH4(g) (3) 5 moles of O2(g) (4) 5 x 1023 molecules of CO2(g) 489 6/08-19 • Which sample at STP has the same number of molecules as 5 Liters of NO2(g) at STP? (1) 5 grams of H2(g) (2) 5 liters of CH4(g) (3) 5 moles of O2(g) (4) 5 x 1023 molecules of CO2(g) correct 490 6/08-20 • Under which conditions of temperature and pressure does oxygen gas behave least like an ideal gas? (1) low temperature and low pressure (2) low temperature and high pressure (3) high temperature and low pressure (4) high temperature and high pressure 491 6/08-20 • Under which conditions of temperature and pressure does oxygen gas behave least like an ideal gas? (1) low temperature and low pressure (2) low temperature and high pressure (3) high temperature and low pressure (4) high temperature and high pressure correct 492 6/08-21 • How is a chemical reaction affected by the addition of a catalyst? (1) The activation energy decreases. (2) The heat of reaction increases. (3) The number of collisions between particles increases. (4) The potential energy of the reactants increases. 493 6/08-21 • How is a chemical reaction affected by the addition of a catalyst? (1) The activation energy decreases. (2) The heat of reaction increases. (3) The number of collisions between particles increases. (4) The potential energy of the reactants increases. correct 494 6/08-22 • Systems in nature tend to undergo changes toward (1) lower energy and lower disorder (2) lower energy and more disorder (3) higher energy and less disorder (4) higher energy and more disorder 495 6/08-22 • Systems in nature tend to undergo changes toward (1) lower energy and lower disorder (2) lower energy and more disorder (3) higher energy and less disorder (4) higher energy and more disorder correct 496 6/08-23 • What can be concluded if an ion of an element is smaller than an atom of the same element? (1) The ion is negatively charged because it has fewer electrons than the atom. (2) The ion is negatively charged because it has more electrons than the atom. (3) The ion is positively charged because it (4) The ion is positively charged because it has fewer electrons than the atom. has more electrons than the atom. 497 6/08-23 • What can be concluded if an ion of an element is smaller than an atom of the same element? (1) The ion is negatively charged because it has fewer electrons than the atom. (2) The ion is negatively charged because it has more electrons than the atom. (3) The ion is positively charged because it (4) The ion is positively charged because it has fewer electrons than the atom.correct has more electrons than the atom. 498 6/08-24 • Which class of compounds has molecules that contain nitrogen atoms? (1) alcohol (2) amine (3) ether (4) ketone 499 6/08-24 • Which class of compounds has molecules that contain nitrogen atoms? (1) alcohol (2) amine (3) ether (4) ketone correct 500 6/08-25 • Which two compounds have the same molecular formula but different chemical and physical properties? (1) CH3CH2Cl and CH3CH2Br (2) CH3CHCH2 and CH3CH2CH3 (3) CH3CHO and CH3COCH3 (4) CH3CH2OH and CH3OCH3 501 6/08-25 • Which two compounds have the same molecular formula but different chemical and physical properties? (1) CH3CH2Cl and CH3CH2Br (2) CH3CHCH2 and CH3CH2CH3 (3) CH3CHO and CH3COCH3 (4) CH3CH2OH and CH3OCH3 correct 502 6/08-26 • Which half reaction equation represents the reduction of a potassium ion? (1) K+ + e- -> K (2) K + e- -> K+ (3) K+ -> K + e- (4) K -> K+ + e- 503 6/08-26 • Which half reaction equation represents the reduction of a potassium ion? (1) K+ + e- -> K (3) K+ -> K + e- correct (2) K + e- -> K+ (4) K -> K+ + e- 504 6/08-27 • According to the Arrhenius theory, an acid is a substance that (1) changes litmus from red to blue (2) changes phenolphthalein from colorless to pink (3) produces hydronium ions as the only positive ions in an aqueous solution (4) produces hydroxide ions as the only negative ion in an aqueous solution 505 6/08-27 • According to the Arrhenius theory, an acid is a substance that (1) changes litmus from red to blue (2) changes phenolphthalein from colorless to pink (3) produces hydronium ions as the only correct positive ions in an aqueous solution (4) produces hydroxide ions as the only negative ion in an aqueous solution 506 6/08-28 • Which type of reaction occurs when a high-energy particle collides with the nucleus of an atom, converting that atom to an atom of a different element? (1) addition (2) neutralization (3) substitution (4) transmutation 507 6/08-28 • Which type of reaction occurs when a high-energy particle collides with the nucleus of an atom, converting that atom to an atom of a different element? (1) addition (2) neutralization (3) substitution (4) transmutation correct 508 6/08-29 • Which particle is emitted when an atom of 85Kr spontaneously decays? (1) an alpha particle (2) a beta particle (3) a neutron (4) a proton 509 6/08-29 • Which particle is emitted when an atom of 85Kr spontaneously decays? (1) an alpha particle (2) a beta particle (3) a neutron (4) a proton correct 510 6/08-30 • What is a problem commonly associated with nuclear power facilities? (1) A small quantity of energy is produced. (2) Reaction products contribute to acid rain. (3) It is impossible to control nuclear fission. (4) It is difficult to dispose of waste. 511 6/08-30 • What is a problem commonly associated with nuclear power facilities? (1) A small quantity of energy is produced. (2) Reaction products contribute to acid rain. (3) It is impossible to control nuclear fission. (4) It is difficult to dispose of waste. correct 512 6/08-31 • The wave-mechanical model of the atom is required to explain the (1) mass number and atomic number of an atom (2) organization of atoms in crystals (3) radioactive nature of some atoms (4) spectra of elements in multielectron atoms 513 6/08-31 • The wave-mechanical model of the atom is required to explain the (1) mass number and atomic number of an atom (2) organization of atoms in crystals (3) radioactive nature of some atoms (4) spectra of elements in multielectron correct atoms 514 6/08-32 • Magnesium and calcium have similar chemical properties because an atom of each element has the same total number of (1) electron shells (2) valence electrons (3) neutrons (4) protons 515 6/08-32 • Magnesium and calcium have similar chemical properties because an atom of each element has the same total number of (1) electron shells (2) valence electrons (3) neutrons (4) protons correct 516 6/08-34 • A barium atom attains a stable electron configuration when it bonds with (1) one chlorine atom (2) two chlorine atoms (3) one sodium atom (4) two sodium atoms 517 6/08-34 • A barium atom attains a stable electron configuration when it bonds with (1) one chlorine atom (2) two chlorine atoms (3) one sodium atom (4) two sodium atoms correct 518 6/08-35 • A student measures the mass and volume of a piece of aluminum. The measurements are 25.6 grams and 9.1 cubic centimeters. The student calculates the density of the aluminum. What is the percent error of the student’s calculated density of aluminum? (1) 1% (2) 2% (3) 3% (4) 4% 519 6/08-35 • A student measures the mass and volume of a piece of aluminum. The measurements are 25.6 grams and 9.1 cubic centimeters. The student calculates the density of the aluminum. What is the percent error of the student’s calculated density of aluminum? (1) 1% (2) 2% (3) 3% (4) 4% correct 520 6/08-36 • Given the balanced equation representing a reaction: 2H2 + O2 -> 2H2O What is the total mass of water formed when 8 grams of hydrogen reacts completely with 64 grams of oxygen? (1) 18 g (2) 36 g (3) 56 g (4) 72 g 521 6/08-36 • Given the balanced equation representing a reaction: 2H2 + O2 -> 2H2O What is the total mass of water formed when 8 grams of hydrogen reacts completely with 64 grams of oxygen? (1) 18 g (2) 36 g (3) 56 g (4) 72 g correct 522 6/08-37 • Which compound contains both ionic and covalent bonds? (1) ammonia (2) methane (3) sodium nitrate (4) potassium chloride 523 6/08-37 • Which compound contains both ionic and covalent bonds? (1) ammonia (3) sodium nitrate (2) methane correct (4) potassium chloride 524 6/08-38 • An iron bar at 325 K is placed in a sample of water. The iron bar gains energy from the water if the temperature of the water is (1) 65 K (2) 45 K (3) 65°C (4) 45°C 525 6/08-38 • An iron bar at 325 K is placed in a sample of water. The iron bar gains energy from the water if the temperature of the water is (1) 65 K (3) 65°C (2) 45 K correct (4) 45°C 526 6/08-40 • Given the balanced equation representing a reaction: Cu + S -> CuS + energy Which statement explains why the energy term is written to the right of the arrow? (1) The compound CuS is composed of two metals. (2) The compound CuS is composed of two nonmetals. (3) Energy is absorbed as the bonds in CuS (4) Energy is released as the bonds in CuS form. form. 527 6/08-40 • Given the balanced equation representing a reaction: Cu + S -> CuS + energy Which statement explains why the energy term is written to the right of the arrow? (1) The compound CuS is composed of two metals. (2) The compound CuS is composed of two nonmetals. (3) Energy is absorbed as the bonds in CuS (4) Energy is released as the bonds in CuS correct form. form. 528 6/08-41 • A 1.0-liter sample of which element will uniformly fill a closed 2.0-liter container at STP? (1) Antimony (2) sulfur (3) tellurium (4) xenon 529 6/08-41 • A 1.0-liter sample of which element will uniformly fill a closed 2.0-liter container at STP? (1) Antimony (2) sulfur (3) tellurium (4) xenon correct 530 6/08-42 • Given the balanced equation representing a reaction: C3H8(g) + 5O2(g) -> 3CO2(g) + 4H2O(g) What is the total number of moles of O2(g) required for the complete combustion of 1.5 moles of C3H8(g)? (1) 0.30 mol (2) 1.5 mol (3) 4.5 mol (4) 7.5 mol 531 6/08-42 • Given the balanced equation representing a reaction: C3H8(g) + 5O2(g) -> 3CO2(g) + 4H2O(g) What is the total number of moles of O2(g) required for the complete combustion of 1.5 moles of C3H8(g)? (1) 0.30 mol (2) 1.5 mol (3) 4.5 mol (4) 7.5 mol correct 532 6/08-43 • A sample of gas occupies a volume of 50.0 milliliters in a cylinder with a movable piston. The pressure of the sample is 0.90 atmosphere and the temperature is 298 K. What is the volume of the sample at STP? (1) 41 mL (2) 49 mL (3) 51 mL (4) 55 mL 533 6/08-43 • A sample of gas occupies a volume of 50.0 milliliters in a cylinder with a movable piston. The pressure of the sample is 0.90 atmosphere and the temperature is 298 K. What is the volume of the sample at STP? (1) 41 mL (3) 51 mL correct (2) 49 mL (4) 55 mL 534 6/08-44 • Which solution has the lowest freezing point? (1) 10. g of KI dissolved in 100. g of water (2) 20. g of KI dissolved in 200 g of water (3) 30. g of KI dissolved in 100. g of water (4) 40. g of KI dissolved in 200. g of water 535 6/08-44 • Which solution has the lowest freezing point? (1) 10. g of KI dissolved in 100. g of water (2) 20. g of KI dissolved in 200 g of water (3) 30. g of KI dissolved in 100. g of water (4) 40. g of KI dissolved in 200. g of water correct 536 6/08-45 • Which 1-mole sample has the lowest entropy? (1) Br2(s) at 266 K (2) Br2(l) at 266 K (3) Br2(l) at 332 K (4) Br2(g) at 332 K 537 6/08-45 • Which 1-mole sample has the least entropy? (1) Br2(s) at 266 K (2) Br2(l) at 266 K (3) Br2(l) at 332 K (4) Br2(g) at 332 K 538 6/08-46 • At 20.°C, a 1.2-gram sample of Mg ribbon reacts rapidly with 10.0 milliliters of 1.0 M HCl(aq). Which change in conditions would have caused the reaction to proceed more slowly? (1) increasing the initial temperature to 25°C (2) decreasing the concentration of HCl(aq) to 0.1 M (3) using 1.2 g of powdered Mg (4) using 2.4 g of Mg ribbon 539 6/08-46 • At 20.°C, a 1.2-gram sample of Mg ribbon reacts rapidly with 10.0 milliliters of 1.0 M HCl(aq). Which change in conditions would have caused the reaction to proceed more slowly? (1) increasing the initial temperature to 25°C (2) decreasing the concentration of correct HCl(aq) to 0.1 M (3) using 1.2 g of powdered Mg (4) using 2.4 g of Mg ribbon 540 6/08-47 • Which general formula represents the compound CH3CH2CCH? (1) CnHn (2) CnH2n (3) CnH2n-2 (4) CnH2n+2 541 6/08-47 • Which general formula represents the compound CH3CH2CCH? (1) CnHn (3) CnH2n-2 (2) CnH2n correct (4) CnH2n+2 542 6/08-48 • Which compound dissolves in water to form an aqueous solution that can conduct an electric current? (1) CCl4 (2) C2H5OH (3) CH3COOH (4) CH4 543 6/08-48 • Which compound dissolves in water to form an aqueous solution that can conduct an electric current? (1) CCl4 (3) CH3COOH (2) C2H5OH correct (4) CH4 544 6/08-50 • An original sample of K-40 has a mass 0f 25.00 grams. After 3.9 x 109 years, 3.125 grams of the original sample remains unchanged. What is the half-life of K-40? (1) 1.3 x 109 y (2) 2.6 x 109 y (3) 3.9 x 109 y (4) 1.2 x 1010 y 545 6/08-50 • An original sample of K-40 has a mass 0f 25.00 grams. After 3.9 x 109 years, 3.125 grams of the original sample remains unchanged. What is the half-life of K-40? (1) 1.3 x 109 y (3) 3.9 x 109 y correct (2) 2.6 x 109 y (4) 1.2 x 1010 y 546 6/08-49 • Given the equation representing a reaction at equilibrium: NH3(g) + H2O(l) = NH4+(aq) + OH-(aq) The H+ acceptor for the forward reaction is (1) H2O(l) (2) NH3(g) (3) NH4+(aq) (4) OH-(aq) 547 6/08-49 • Given the equation representing a reaction at equilibrium: NH3(g) + H2O(l) = NH4+(aq) + OH-(aq) The H+ acceptor for the forward reaction is (1) H2O(l) (2) NH3(g) (3) NH4+(aq) (4) OH-(aq) correct 548 8/08-1 • In the wave-mechanical model of the atom, orbitals are regions of the most probable locations of (1) protons (2) positrons (3) neutrons (4) electrons 549 8/08-1 • In the wave-mechanical model of the atom, orbitals are regions of the most probable locations of (1) protons (2) positrons (3) neutrons (4) electrons correct 550 8/08-2 • Which phrase describes an atom? (1) a positively charged electron cloud surrounding a positively charged nucleus (2) a positively charged electron cloud surrounding a negative charged nucleus (3) a negative charged electron cloud surrounding a positively charged nucleus (4) a negatively charged electron cloud surrounding a negatively charged nucleus 551 8/08-2 • Which phrase describes an atom? (1) a positively charged electron cloud surrounding a positively charged nucleus (2) a positively charged electron cloud surrounding a negative charged nucleus (3) a negative charged electron cloud surrounding a positively charged nucleus (4) a negatively charged electron cloud surrounding a negatively charged nucleus correct 552 8/08-3 • Which total mass is the smallest? (1) the mass of two electrons (2) the mass of two neutrons (3) the mass of one electron plus the mass of one proton (4) the mass of one neutron plus the mass of one proton 553 8/08-3 • Which total mass is the smallest? (1) the mass of two electrons (2) the mass of two neutrons (3) the mass of one electron plus the mass of one proton (4) the mass of one neutron plus the mass of one proton correct 554 8/08-4 • Elements on the modern Periodic Table are arranged in order of increasing (1) atomic mass (2) atomic number (3) number of neutrons (4) number of valence electrons 555 8/08-4 • Elements on the modern Periodic Table are arranged in order of increasing (1) atomic mass (2) atomic number (3) number of neutrons (4) number of valence electrons correct 556 8/08-5 • As the elements of Group 17 are considered in order of increasing atomic number, there is an increase in (1) atomic radius (2) electronegativity (3) first ionization energy (4) number of electrons in the first shell 557 8/08-5 • As the elements of Group 17 are considered in order of increasing atomic number, there is an increase in (1) atomic radius (3) first ionization energy correct (2) electronegativity (4) number of electrons in the first shell 558 8/08-6 • Chlorine-37 can be represented as (1) 35Cl17 (2) 37Cl20 (3) 20Cl35 (4) 17Cl37 559 8/08-6 • Chlorine-37 can be represented as (1) 35Cl17 (2) 37Cl20 (3) 20Cl35 (4) 17Cl37 correct 560 8/08-7 • Which element is a metal that is in the liquid phase at STP? (1) bromine (2) cobalt (3) hydrogen (4) mercury 561 8/08-7 • Which element is a metal that is in the liquid phase at STP? (1) bromine (2) cobalt (3) hydrogen (4) mercury correct 562 8/08-8 • Which list of formulas represents compounds, only? (1) CO2, H2O, NH3 (2) H2, N2, O2 (3) H2, Ne, NaCl (4) MgO, NaCl, O2 563 8/08-8 • Which list of formulas represents compounds, only? (1) CO2, H2O, NH3 (3) H2, Ne, NaCl correct (2) H2, N2, O2 (4) MgO, NaCl, O2 564 8/08-9 • What is the chemical formula for iron(III) oxide? (1) FeO (2) Fe2O3 (3) Fe3O (4) Fe3O2 565 8/08-9 • What is the chemical formula for iron(III) oxide? (1) FeO (2) Fe2O3 (3) Fe3O (4) Fe3O2 correct 566 8/08-10 • An atom of which element has the greatest attraction for the electrons in a bond with the hydrogen atom? (1) chlorine (2) phosphorous (3) silicon (4) sulfur 567 8/08-10 • An atom of which element has the greatest attraction for the electrons in a bond with the hydrogen atom? (1) chlorine (3) silicon correct (2) phosphorous (4) sulfur 568 8/08-11 • Which property could be used to identify a compound in the laboratory? (1) mass (2) melting point (3) temperature (4) volume 569 8/08-11 • Which property could be used to identify a compound in the laboratory? (1) mass (2) melting point (3) temperature (4) volume correct 570 8/08-12 • Which statement describes what occurs as two atoms of bromine combine to form a molecule of bromine? (1) Energy is absorbed as a bond is formed. (2) Energy is absorbed as a bond is broken. (3) Energy is released as a bond is formed. (4) Energy is absorbed as a bond is broken. 571 8/08-12 • Which statement describes what occurs as two atoms of bromine combine to form a molecule of bromine? (1) Energy is absorbed as a bond is formed. (2) Energy is absorbed as a bond is broken. (3) Energy is released as a bond is formed. (4) Energy is absorbed as a bond is correct broken. 572 8/08-14 • Solid ZnCl2 and liquid ZnCl2 have different (1) empirical formulas (2) formula masses (3) ion ratios (4) physical properties 573 8/08-14 • Solid ZnCl2 and liquid ZnCl2 have different (1) empirical formulas (2) formula masses (3) ion ratios (4) physical properties correct 574 8/08-15 • Which phrase describes the molarity of a solution? (1) liters of solute per mole of solution (2) liters of solution per mole of solution (3) moles of solute per liter of solution (4) moles of solution per liter of solution 575 8/08-15 • Which phrase describes the molarity of a solution? (1) liters of solute per mole of solution (2) liters of solution per mole of solution (3) moles of solute per liter of solution (4) moles of solution per liter of solution correct 576 8/08-16 • Which substance cannot be decomposed by a chemical change? (1) AlCl3 (2) H2O (3) HI (4) Cu 577 8/08-16 • Which substance cannot be decomposed by a chemical change? (1) AlCl3 (2) H2O (3) HI (4) Cu correct 578 8/08-17 • Tetrachloromethane, CCl4, is classified as a (1) compound because the atoms of the elements are combined in a fixed proportion (2) compound because the atoms of the elements are combined in a proportion that varies (3) mixture because the atoms of the elements are combined in a fixed proportion (4) mixture because the atoms of the elements are combined in a proportion that varies 579 8/08-17 • Tetrachloromethane, CCl4, is classified as a (1) compound because the atoms of the elements are combined in a fixed correct proportion (2) compound because the atoms of the elements are combined in a proportion that varies (3) mixture because the atoms of the elements are combined in a fixed proportion (4) mixture because the atoms of the elements are combined in a proportion that varies 580 8/08-18 • Which formulas represent two polar molecules? (1) CO2 and HCl (2) CO2 and CH4 (3) H2O and HCl (4) H2O and CH4 581 8/08-18 • Which formulas represent two polar molecules? (1) CO2 and HCl (3) H2O and HCl (2) CO2 and CH4 correct (4) H2O and CH4 582 8/08-19 • Hydrocarbons are compounds that contain (1) carbon, only (2) carbon and hydrogen, only (3) carbon, hydrogen, and oxygen, only (4) carbon, hydrogen, oxygen, and nitrogen, only 583 8/08-19 • Hydrocarbons are compounds that contain (1) carbon, only (2) carbon and hydrogen, only correct (3) carbon, hydrogen, and oxygen, only (4) carbon, hydrogen, oxygen, and nitrogen, only 584 8/08-20 • The reaction that joins thousands of small, identical molecules to form one very long molecule is called (1) esterification (2) fermentation (3) polymerization (4) substitution 585 8/08-20 • The reaction that joins thousands of small, identical molecules to form one very long molecule is called (1) esterification (3) polymerization (2) fermentation correct (4) substitution 586 8/08-22 • A voltaic cell spontaneously converts chemical energy to (1) electrical energy (2) geothermal energy (3) mechanical energy (4) nuclear energy 587 8/08-22 • A voltaic cell spontaneously converts chemical energy to (1) electrical energy (3) mechanical energy correct (2) geothermal energy (4) nuclear energy 588 8/08-23 • Given the balanced equation representing a reaction: Mg(s) + Ni+2(aq) -> Mg+2(aq) + Ni(s) What is the total number of moles of electrons lost by Mg(s) when 2.0 moles of electrons are gained by Ni+2(aq)? (1) 1.0 mol (2) 2.0 mol (3) 3.0 mol (4) 4.0 mol 589 8/08-23 • Given the balanced equation representing a reaction: Mg(s) + Ni+2(aq) -> Mg+2(aq) + Ni(s) What is the total number of moles of electrons lost by Mg(s) when 2.0 moles of electrons are gained by Ni+2(aq)? (1) 1.0 mol (2) 2.0 mol (3) 3.0 mol (4) 4.0 mol correct 590 8/08-24 • Which half reaction correctly represents reduction? (1) Mn4+-> Mn3++ e- (2) Mn4+-> Mn7++ 3e- (3) Mn4++ e- -> Mn3+ (4) Mn4+ + 3e- -> Mn7+ 591 8/08-24 • Which half reaction correctly represents reduction? (1) Mn4+-> Mn3++ e- (2) Mn4+-> Mn7++ 3e- (3) Mn4++ e- -> Mn3+ (4) Mn4+ + 3e- -> Mn7+ correct 592 8/08-25 • Which indicator is blue in a solution that has a pH of 5.6? (1) bromcresol green (2) bromthymol blue (3) methyl orange (4) thymol blue 593 8/08-25 • Which indicator is blue in a solution that has a pH of 5.6? (1) bromcresol green (3) methyl orange correct (2) bromthymol blue (4) thymol blue 594 8/08-26 • The Arrhenius theory explains the behavior of (1) acids and bases (2) alcohols and amines (3) isomers and isotopes (4) metals and nonmetals 595 8/08-26 • The Arrhenius theory explains the behavior of (1) acids and bases (3) isomers and isotopes correct (2) alcohols and amines (4) metals and nonmetals 596 8/08-27 • In which laboratory process could a student use 0.10 M NaOH(aq) to determine the concentration of an aqueous solution of HBr? (1) chromatography (2) decomposition of the solute (3) evaporation of the solvent (4) titration 597 8/08-27 • In which laboratory process could a student use 0.10 M NaOH(aq) to determine the concentration of an aqueous solution of HBr? (1) chromatography (2) decomposition of the solute (3) evaporation of the solvent (4) titration correct 598 8/08-28 • A nuclear reaction in which two light nuclei combine to form a more massive nucleus is called (1) addition (2) fission (3) fusion (4) substitution 599 8/08-28 • A nuclear reaction in which two light nuclei combine to form a more massive nucleus is called (1) addition (3) fusion (2) fission correct (4) substitution 600 8/08-29 • The nucleus of a radium-226 atom is unstable, which causes the nucleus to spontaneously (1) absorb electrons (2) absorb protons (3) decay (4) oxidize 601 8/08-29 • The nucleus of a radium-226 atom is unstable, which causes the nucleus to spontaneously (1) absorb electrons (3) decay (2) absorb protons correct (4) oxidize 602 8/08-30 • A serious risk factor associated with the operation of a nuclear power plant is the production of (1) acid rain (2) helium gas (3) greenhouse gases, such as CO2 (4) radioisotopes with long half-lives 603 8/08-30 • A serious risk factor associated with the operation of a nuclear power plant is the production of (1) acid rain (2) helium gas (3) greenhouse gases, such as CO2 (4) radioisotopes with long half-lives correct 604 8/08-31 • What is the total number of protons in an atom with the electron configuration 2-8-28-32-18-1? (1) 69 (2) 79 (3) 118 (4) 197 605 8/08-31 • What is the total number of protons in an atom with the electron configuration 2-8-28-32-18-1? (1) 69 (2) 79 (3) 118 (4) 197 correct 606 8/08-32 • Which two elements have the most similar chemical properties? (1) Be and Mg (2) Ca and Br (3) Cl and Ar (4) Na and P 607 8/08-32 • Which two elements have the most similar chemical properties? (1) Be and Mg (3) Cl and Ar correct (2) Ca and Br (4) Na and P 608 8/08-33 • In the ground state, each atom of an element has two valence electrons. The element has a lower first ionization energy than calcium. Where is this element located on the Periodic Table? (1) Group 1, Period 4 (2) Group 2, Period 5 (3) Group 2, Period 3 (4) Group 3, Period 4 609 8/08-33 • In the ground state, each atom of an element has two valence electrons. The element has a lower first ionization energy than calcium. Where is this element located on the Periodic Table? (1) Group 1, Period 4 (2) Group 2, Period 5 (3) Group 2, Period 3 (4) Group 3, Period 4 correct 610 8/08-34 • Which equation shows conservation of mass and charge? (1) 1 (2) 2 (3) 3 (4) 4 611 8/08-34 • Which equation shows conservation of mass and charge? (1) 1 (2) 2 (3) 3 (4) 4 correct 612 8/08-35 • What is the percent composition by mass of hydrogen in NH4HCO3 (gram formula mass = 79 grams/mole)? (1) 5.1% (2) 6.3% (3) 10.% (4) 50.% 613 8/08-35 • What is the percent composition by mass of hydrogen in NH4HCO3 (gram formula mass = 79 grams/mole)? (1) 5.1% (2) 6.3% correct (3) 10.% (4) 50.% 614 8/08-36 • What is the total number of valence electrons in a sulfide ion in the ground state? (1) 8 (2) 2 (3) 16 (4) 18 615 8/08-36 • What is the total number of valence electrons in a sulfide ion in the ground state? (1) 8 (2) 2 correct (3) 16 (4) 18 616 8/08-37 • A temperature of 37°C is equivalent to a temperature of (1) 98.6 K (2) 236 K (3) 310. K (4) 371 K 617 8/08-37 • A temperature of 37°C is equivalent to a temperature of (1) 98.6 K (3) 310. K (2) 236 K correct (4) 371 K 618 8/08-38 • Which balanced equation represents a chemical change? (1) 1 (2) 2 (3) 3 (4) 4 619 8/08-38 • Which balanced equation represents a chemical change? (1) 1 (2) 2 (3) 3 (4) 4 correct 620 8/08-39 • When 5 grams of KCl are dissolved in 50. grams of water at 25°C, the resulting mixture can be described as (1) heterogeneous and unsaturated (2) heterogeneous and supersaturated (3) homogeneous and unsaturated (4) homogeneous and supersaturated 621 8/08-39 • When 5 grams of KCl are dissolved in 50. grams of water at 25°C, the resulting mixture can be described as (1) heterogeneous and unsaturated (2) heterogeneous and supersaturated (3) homogeneous and unsaturated (4) homogeneous and supersaturated correct 622 8/08-40 • Which aqueous solution of KI freezes at the lowest temperature? (1) 1 mol of KI in 500. grams of water (2) 2 mol of KI in 500. grams of water (3) 1 mol of KI in 1000. grams of water (4) 2 mol of KI in 1000. grams of water 623 8/08-40 • Which aqueous solution of KI freezes at the lowest temperature? (1) 1 mol of KI in 500. grams of water (2) 2 mol of KI in 500. grams of water correct (3) 1 mol of KI in 1000. grams of water (4) 2 mol of KI in 1000. grams of water 624 8/08-41 • Which compound is a member of the same homologous series as C3H8? (1) CH4 (2) C4H8 (3) C5H8 (4) C5H10 625 8/08-41 • Which compound is a member of the same homologous series as C3H8? (1) CH4 (3) C5H8 correct (2) C4H8 (4) C5H10 626 8/08-42 • Which equation represents an oxidation-reduction reaction? (1) 1 (2) 2 (3) 3 (4) 4 627 8/08-42 • Which equation represents an oxidation-reduction reaction? (1) 1 (3) 3 correct (2) 2 (4) 4 628 8/08-43 • Given the balanced equation representing a reaction: 2KClO3(s) -> 2KCl(s) + 3O2(g) The oxidation state of chlorine in this reaction changes from (1) -1 to +1 (2) -1 to +5 (3) +1 to -1 (4) +5 to -1 629 8/08-43 • Given the balanced equation representing a reaction: 2KClO3(s) -> 2KCl(s) + 3O2(g) The oxidation state of chlorine in this reaction changes from (1) -1 to +1 (2) -1 to +5 (3) +1 to -1 (4) +5 to -1 correct 630 8/08-45 • Given the balanced equation representing a reaction occuring in an electrolytic cell: 2NaCl(l) -> 2Na(l) + Cl2(g) Where is Na(l) produced in the cell? (1) at the anode, where oxidation occurs (2) at the anode, where reduction occurs (3) at the cathode, where oxidation occurs (4) at the cathode, where reduction occurs 631 8/08-45 • Given the balanced equation representing a reaction occuring in an electrolytic cell: 2NaCl(l) -> 2Na(l) + Cl2(g) Where is Na(l) produced in the cell? (1) at the anode, where oxidation occurs (2) at the anode, where reduction occurs (3) at the cathode, where oxidation occurs (4) at the cathode, where reduction correct occurs 632 8/08-46 • Given the balanced equation representing a reaction: NH3(g) + H2O(l) -> NH4+(aq) + OH-(aq) According to one acid-base theory, the NH3(g) molecules act as (1) an acid because they accept H+ ions (2) an acid because they donate H+ ions (3) a base because they accept H+ ions (4) a base because the donate H+ ions 633 8/08-46 • Given the balanced equation representing a reaction: NH3(g) + H2O(l) -> NH4+(aq) + OH-(aq) According to one acid-base theory, the NH3(g) molecules act as (1) an acid because they accept H+ ions (2) an acid because they donate H+ ions (3) a base because they accept H+ ions (4) a base because the donate H+ ions correct 634 8/08-47 • What volume of 0.120 M HNO3(aq) is needed to completely neutralize 150.0 milliliters of 0.100 M NaOH(aq)? (1) 62.5 mL (2) 125 mL (3) 180.mL (4) 360. mL 635 8/08-47 • What volume of 0.120 M HNO3(aq) is needed to completely neutralize 150.0 milliliters of 0.100 M NaOH(aq)? (1) 62.5 mL (2) 125 mL (3) 180.mL (4) 360. mL correct 636 8/08-49 • An original sample of a radioisotope fluorine-21 had a mass of 80.0 milligrams. Only 20.0 milligrams of this original sample remain unchanged after 8.32 seconds. What is the half-life of fluorine-21 (1) 1.04 s (2) 2.08 s (3) 4.16 s (4) 8.32 s 637 8/08-49 • An original sample of a radioisotope fluorine-21 had a mass of 80.0 milligrams. Only 20.0 milligrams of this original sample remain unchanged after 8.32 seconds. What is the half-life of fluorine-21 (1) 1.04 s (2) 2.08 s (3) 4.16 s (4) 8.32 s 638 8/08-48 • Given the balanced equation representing a reaction: Which particle is represented by X? (1) electron (2) proton (3) alpha particle (4) neutron 639 8/08-48 • Given the balanced equation representing a reaction: Which particle is represented by X? (1) electron (2) proton (3) alpha particle (4) neutron correct 640 8/08-50 • Which nuclide is paired with a specific use of that nuclide? (1) carbon-14, treatment of cancer (2) cobalt-60, dating of rock formations (3) iodine-131, treatment of thyroid disorders (4) uranium-238, dating of once-living organisms 641 8/08-50 • Which nuclide is paired with a specific use of that nuclide? (1) carbon-14, treatment of cancer (2) cobalt-60, dating of rock formations (3) iodine-131, treatment of thyroid correct disorders (4) uranium-238, dating of once-living organisms 642