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Chemistry Final Review 1) The difference between a scientific theory and a 11) Which of the following is a true statement about scientific law is that _____ . compounds? A) a law only summarizes observations; a theory A) They are pure substances. attempts to explain observations B) They can be physically separated into their B) a theory only summarizes observations; a law constituent elements. attempts to explain observations C) They have properties similar to those of their C) There is no difference. constituent elements. 2) An important characteristic of an accepted D) They have variable compositions. scientific theory is that _____ . 12) One difference between a mixture and a A) it is agreed upon by all scientists. compound is that B) it can be proven true. A) a compound is made up of more than one C) it cannot be modified. phase. D) it can be disproved at any time. B) a mixture must be uniform in composition. 3) Matter is defined as anything that _____ . C) a mixture can only be separated into its A) has a fixed volume and weight components by chemical means. B) has mass and takes up space D) a compound can only be separated into its C) can be weighed on a balance components by chemical means. D) has a definite volume 13) The chemical formula of a compound indicates 4) A vapor is which state of matter? the _____. A) plasma B) gas A) three-dimensional structure of the compound C) liquid D) solid B) relative proportions of the elements in the 5) Which state of matter is characterized by having an compound indefinite shape, but a definite volume? C) type and arrangement of the bonds in the A) plasma B) gas C) solid D) liquid compound 6) Which of the following materials is a pure D) identity of the elements in the compound only substance? 14) Consider the chemical reaction in which carbon A) diamond B) air reacts with oxygen to produce carbon dioxide. What C) brass D) tea mass of carbon dioxide would be produced if 24 E) gasoline grams of carbon reacted completely with 64 grams of 7) All of the following are physical properties of oxygen? matter EXCEPT A) 64 g B) 48 g C) 40 g A) color B) explosiveness D)130 g E) 88 g C) hardness D) mass 15) Which of the following is a chemical property of E) melting point an antacid tablet? 8) All of the following are physical properties of a A) tart taste B) lack of color substance in the liquid state EXCEPT _____. C) ability to neutralize acid D) white color A) definite mass 16) The diameter of a carbon atom is 0.000 000 000 B) indefinite shape 154 m. What is this number expressed in scientific C) virtual incompressibility notation? D) indefinite volume A) 1.54 x 1010 m B) 1.54 x 10-12 m 9) Which of the following does NOT involve a C) 1.54 x 1012 m D) 1.54 x 10-10 m physical change? 17) What is 5928 km expressed in scientific notation? A) melting B) grinding A) 5.928 x 10-3 B) 5.928 x 102 C) mixing D) tarnishing C) 5.928 x 100 D) 5.928 x 103 10) Which of the following is a homogeneous 18) How many significant figures are there in the mixture? measurement 40 500 mg? A) beef stew B) raisin bread A) four B) five C) three C) soil D) sand and water D) two E) This cannot be determined. E) brine Page 1 of 9 19) What is the quantity 7896 millimeters expressed in meters? A) 7.896 m B) 789 600 m C) 78.96 m D) 789.6 m E) 7 896 000 m 20) Which of the following equalities is NOT correct? A) 1 cm3 = 1 mL B) 1000 kg = 1 g C) 1000 mm = 1 m D) 100 cg = 1 g 21) What is the density of an object having a mass of 8.0 g and a volume of 25 cm3? A) 2.0 g/cm3 B) 3.1 g/cm3 C) 200 g/cm3 3 D) 0.32 g/cm E) none of the above 22) What is the volume of 45.6 g of silver if the density of silver is 10.5 g/mL? A) 4.34 mL B) 0.23 mL C) 479 mL D) none of the above 23) How are the numerator and denominator in a conversion factor related? A) They each have the same units. B) One is greater than or less than the other. C) Both equal the value 1. D) They are equal. 24) Which of the following conversion can be used to change centimeters to kilometers? A) ( 1 m/100 cm) x ( 1000 m/1 km) B) ( 100 cm/1 m) x ( 1 km/1000 m) C) ( 100 cm/1 m) x ( 1000 m/1 km) D) ( 1 m/100 cm) x ( 1 km/1000 m) 25) If 20 gits equal 1 erb, and 1 futz equals 2 hews, and 10 erbs equal 1 futz, how many gits equal 5 hews? A) 500 gits B) 50 gits C) 100 gits D) 1000 gits 26) What is the smallest particle of an element that retains the properties of that element? A) an atom B) a proton C) an electron D) a molecule E) a neutron 27) Dalton's atomic theory included which idea? A) Atoms of different elements always combine in one-to-one ratios. B) When an atom of an element changes into another element, a chemical reaction takes place. C) Individual atoms can be seen with a microscope. D) Atoms of the same element are always identical. E) All atoms of all elements are the same size. 28) Why did J. J. Thomson reason that electrons must be a part of the atoms of all elements? A) Cathode rays were always accompanied by anode rays. B) Cathode rays can be deflected by magnets. C) Cathode rays are always made of electrons, regardless of the gas used. D) Cathode rays are negatively-charged particles. E) An electron is 2000 times lighter than a hydrogen atom. 29) As a consequence of the discovery of the nucleus by Rutherford, which model of the atoms is believed to be true? A) A model in which the nucleus is made of protons, electrons, and neutrons B) A model in which the nucleus is made of neutrons only C) A model in which the nucleus is made of electrons and protons. D) A model in which the protons, electrons, and neutrons are evenly distributed throughout the volume of the atom E) A model in which the region outside the nucleus is largely empty space in which the electrons are situated 30) In which of the following sets are the symbol of the element, the number of protons, and the number of electrons given correctly? A) In, 49 protons, 49 electrons B) Cs, 55 protons, 132.9 electrons C) Zn, 30 protons, 60 electrons D) He, 4 protons, 4 electrons E) F, 19 protons, 19 electrons 31) Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope with a mass number of 20 is 25% abundant; the isotope with a mass number of 22 is 75% abundant. What is the average atomic mass for element Z? A) 42.0 g B) 2.0 g C) 21.0 g D) 21.5 g E) 20.5 g 32) Which subatomic particle plays the greatest part in determining the physical and chemical properties of an element? A) electron B) neutron C) proton D) quark E) muon 33) In which of the following is the symbol for the ion and the number of electrons it contains correct? A) Br- has 34 electrons. B) Al3+ has 16 electrons. C) Ca2+ has 18 electrons. D) S2- has 2 electrons. + E) H has 1 electron. Page 2 of 9 34) Which of the following statements is true concerning the composition of ionic compounds? A) They are formed from two or more nonmetallic elements. B) They are formed from two or more metallic elements. C) They are composed of anions only. D) They are composed of cations only. E) They are composed of anions and cations. 35) Which of the following formulas represents an ionic compound? A) Kr B) BaI2 C) PCl3 D) N2O4 E) CS2 36) In which of the following groups of ions are the charges all shown correctly? A) Ca2+, Al3+, BrB) Be2+, Cl2-, Sr2+ C) Li-, O2-, S2+ D) Na+, I-, RbE) K2-, F-, Mg2+ 37) In which of the following are the symbol and name for the ion given correctly? A) PO33- phosphate; PO34-phosphite B) NH4+ ammonia; H+: hydride C) C2H3O2- acetate; CO32- carbonite D) OH- : hydroxide; O2-: oxide E) HSO4- hydrogen sulfate; HSO32- hydrogen sulfite 38) What is the ionic charge on the zirconium ion in the ionic compound zirconium oxide, ZrO2? A) 2B) 4+ C) 2+ D) 0 E) 439) Which of the following compounds contains the Mn3+ ion? A) MnO B) MnS C) Mn3O2 D) MnBr2 E) Mn2O3 40) Which set of chemical name and chemical formula for the same compound is correct? A) iron(III) phosphate, FePO4 B) potassium chlorine, K2Cl2 C) ammonium sulfite, (NH4)2S D) magnesium dichromate, MgCrO4 E) lithium carbonate, LiCO3 41) Which of the following shows both the correct formula and correct name of an acid? A) H2CO3, bicarbonic acid B) HNO2, hydronitrous acid C) HClO2, chloric acid D) HI, iodic acid E) H3PO4, phosphoric acid 42) How many moles of silver atoms are there in 1.8 x 1020 atoms of silver? A) 1.1 x 1044 B) 3.0 x 10-4 C) 3.0 x 102 D) 3.3 x 10-3 43) How many molecules are there in 2.10 mol CO2? A) 1.05 x 10-23 B) 3.49 x 10-24 24 C) 1.26 x 10 D) 3.79 x 1024 E) 2.53 x 1024 44) How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C3H7O? A) 5 x (6.02 x 1023) B) 35 x (6.02 x 1023) C) 5 D) 35 45) What is the mass, in grams, of 0.450 moles of Sb? A) 0.450 g B) 2.71 x 1023 C) 2.02 x 101 D) 3.55 x 101 E) 5.48 x 101 46) A large weather balloon filled with helium has a volume of 7.00 x 102 L at STP. Which expression should be used to find the mass of helium in the balloon? A) 22.4 L/mol/7.00 x 10-2 L x 4 g He/mol B) 7.0 x 102/L x 4 g He/mol C) 22.4 L/mol x 4 g He/mol D) 7.00 x 102 L/22.4 L/mol x 4 g He/mol 47) What is the volume, in liters, of 6.8 mol of Kr gas at STP? A) 25 L B) 13 000 L C) 0.30 L D) 3.3 L E) 150 L 48) If 20.0 grams of Ca combines completely with 16.0 grams of S to form a compound, what is the percent composition of Ca in the compound? A) 20.0% B) 55.6% C) 44.4% D) 80.0% E) 1.25% 49) Which of the following compounds have the same empirical formula? A) C4H10 and C10H4 B) CO2 and SO2 C) C7H14 and C10H20 D) NO and NO2 E) C6H12 and C6H14 50) What are the missing coefficients for the skeleton equation below? Cr(s) + Fe(NO3)2(aq) → Fe(s) + Cr(NO3)3(aq) A) 2,3,3,2 B) 4,6,6,2 C) 2,3,1,2 D) 2,3,2,3 E) 1,3,3,1 Page 3 of 9 51) Which of the following is the correct skeleton equation for the reaction that takes place when solid phosphorus combines with oxygen gas to form diphosphorus pentoxide? A) P(s) + O(g) → P5O2(g) B) P2O5 → P2(s) + O2(g) C) P(s) + O2(g) → P2O5 D) P(s) + O2(g) → PO2(g) E) P2(s) + O5(g) → P2O5(g) 52) Aluminum chloride and bubbles of hydrogen gas are produced when metallic aluminum is placed in hydrochloric acid. What is the balanced equation for this reaction? A) Al + HCl3 → AlCl3 + H B) H2 + AlCl3 → Al + 2HCl C) H + AlCl → Al + HCl D) Al + 2HCl → AlCl2 + H2 E) 2Al + 6HCl → 2AlCl3 + 3H2 53) The equation H3PO4 + 3KOH → K3PO4 + 3H2O is an example of which type of reaction? A) combination B) decomposition C) single-replacement D) double-replacement 54) A double-replacement reaction takes place when aqueous Na2CO3 reacts with aqueous Sn(NO3)2. You would expect one of the products of this reaction to be _____. A) CNO3 B) Sn(CO3)2 C) NaNO3 D) NaSn 55) What is conserved in the reaction shown below? N2(g) + 3F2(g) → 2NF3(g) A) only atoms B) only mass C) only moles D) only mass and atoms E) only mass, atoms, moles, and molecules 56) Hydrogen gas can be produced by reacting aluminum with sulfuric acid. How many moles of sulfuric acid are needed to completely react with 15.0 mol of aluminum? 2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g) A) 10.0 mol B) 22.5 mol C) 2710 mol D) 0.100 mol E) 15.0 mol 57) How many grams of chromium are needed to react with an excess of CuSO4 to produce 27.0 g Cu? 2Cr(s) + 3CuSO4(aq) → Cr2(SO4)3(aq) + 3Cu(s) A) 14.7 g B) 33.2 g C) 81.5 g D) 0.005 48 g E) 18.0 g 58) How many liters of chlorine gas can be produced when 0.98 L of HCl react with excess O2, at STP? 4HCl(g) + O2(g) → 2Cl2(g) + 2H2O(g) A) 0.49 L B) 0.98 L C) 2.0 L D) 3.9 L E) 0.25 L 59) The reagent present in the smallest amount is _____ the limiting reagent. A) never B) always C) sometimes 60) Methane and hydrogen sulfide form when hydrogen reacts with carbon disulfide. Identify the excess reagent and calculate how much remains after 36 L of H2 reacts with 12 L of CS2. 4H2(g) + CS2(g) → CH4(g) + 2H2S(g) A) 9 L CS2 B) 12 L H2 C) 24 L H2 D) 3 L CS2 E) 6 L CS2 61) What happens to the average kinetic energy of the particles in a sample of matter as the temperature of the sample is increased? A) It decreases. B) It does not change. C) It increases. 62) What is the volume occupied by 2.20 mol of hydrogen at STP? A) 49.3 L B) 24.6 L C) 98.6 L D) 2.60 L E) 2.20 L 63) Equal volumes of nitrogen and oxygen, at the same temperature and pressure, would _____. A) have different average kinetic energies B) contain the same number of particles C) contain different numbers of particles D) have the same mass 64) If a liquid is sealed in a container and kept at constant temperature, how does its vapor pressure change over time? A) It rises at first, then falls. B) It rises continuously. C) It rises at first, then remains constant. 65) Water could be made to boil at 105°C instead of 100°C by A) increasing the air pressure on the water B) applying a great deal of heat C) decreasing the pressure on the water D) decreasing the air pressure above the water 66) How many kilocalories of heat are required to raise the temperature of 225 g of aluminum from 20°C to 100°C? (specific heat of Al = 0.21 cal/g x °C) A) 0.59 kcal B) 85 kcal C) 3.8 kcal D) none of the above Page 4 of 9 67) What is the specific heat of olive oil if it takes approximately 420 J of heat to raise the temperature of 7 g of olive oil by 30°C? A) less than the specific heat of water B) equal to the specific heat of water C) greater than the specific heat of water D) Not enough information given. 68) Which of the following equations correctly represents an endothermic reaction? A) A + B + heat → C + D B) A + B → C + D + heat 69) What is the standard heat of reaction for this reaction: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) (∆Hf° for Cu2+ = +64.4 kJ/mol; ∆Hf° for Zn2+ = 152.4 kJ/mol) A) 88.0 kJ created per mole B) 88.0 kJ absorbed per mole C) 216.8 kJ absorbed per mole D) 216.8 kJ created per mole 70) When heat is added to boiling water, its temperature _____. A) depends on the amount of water B) decreases C) increases D) stays the same 71) For ammonia, (NH3), ∆Hf° = -46 kJ/mol. This means that A) 46 kJ is released when 1 mole of ammonia is formed from nitrogen and hydrogen B) it takes 46 kJ to form 1 mole of ammonia from nitrogen and hydrogen C) it takes 46 kJ to vaporize 1 mole of liquid ammonia D) 46 kJ of heat is released when 1 mole of ammonia gas condenses 72) Why does the pressure inside a container of gas increase if more gas is added to the container? A) because there is a corresponding decrease in volume B) because there is a corresponding increase in the temperature C) because there is a corresponding increase in the number of particles striking an area of the wall of the container per unit time D) because there is a corresponding increase in the force of the collisions between the particles and the walls of the container 73) What happens to the pressure of a gas inside a container if the temperature of the gas is lowered? A) The pressure decreases. B) The pressure does not change. C) The pressure increases. 74) If the volume of a container holding a gas is reduced, what will happen to the pressure within the container? A) The pressure will decrease. B) The pressure will not change. C) The pressure will increase. 75) When the pressure and number of particles are kept constant for a sample of gas, which of the following is also constant for the sample? A) the difference of the volume and temperature (in kelvins) B) the product of the volume and temperature (in kelvins) C) the sum of the volume and temperature (in kelvins) D) the quotient of the volume and temperature (in kelvins) 76) Which of the following gases will effuse the most rapidly? A) hydrogen B) chlorine C) argon D) bromine E) ammonia 77) What is the maximum number of electrons in the second principal energy level? A) 32 B) 8 C)18 D) 2 78) In Bohr's model of the atom, where are the electrons and protons located? A) The electrons orbit the protons, which are at the center of the atom. B) The electrons and protons are located throughout the atom, but they are not free to move. C) The electrons occupy fixed positions around the protons, which are at the center of the atom. D) The electrons and protons move throughout the atom. 79) What did Rutherford's experiment demonstrate? A) that most of an atom's mass is concentrated in a relatively small portion of the atom's entire volume B) that all neutrons are located in the nucleus C) that electrons orbit the nucleus D) that atoms are made of positively and negatively charged particles Page 5 of 9 80) What is the electron configuration of potassium? A) 1s22s23s23p63d1 B) 1s22s22p23s23p24s1 C) 1s22s22p103s23p3 D) 1s22s22p63s23p64s1 81) The atomic emission spectra of a sodium atom on earth and of a sodium atom in the sun would be _____. A) different from each other B) the same as each other only in the ultraviolet range C) the same as those of several other elements D) the same 82) What is the approximate frequency of a photon having an energy 5 x 10-24 J? (h = 6.6 x 10-34 J s) A) 1 x 10-11 Hz B) 1 x 10-10 Hz C) 7 x 109 Hz D) 3 x 10-58 Hz -57 E) 3 x 10 Hz 83) Emission of light from an atom occurs when the electron A) jumps from a lower to a higher energy level B) moves within its atomic orbital C) falls into the nucleus D) drops from a higher to a lower energy level 84) What element has the electron configuration 1s22s22p63s23p2? A) silver B) selenium C) silicon D) nitrogen 85) Which of the following groupings contains only representative elements? A) Hg, Cr, Ag B) Ni, Fe, Zn C) Cu, Co, Cd D) Al, Mg, Li 86) Which group of the periodic table has the highest electronegativity? A) 3A B) 6A C) 1A D) 2A E) 7A 87) Atomic size generally _____. A) increases as you move from left to right across a period B) remains constant within a period C) decreases as you move down a group D) decreases as you move from left to right across a period 88) As you move from left to right across the second period of the periodic table _____. A) the atomic mass decreases B) the atomic radii increase C) the ionization energy increases D) the electron affinity decreases 89) Which of the following increases with increasing atomic number in Group 2A? A) electron affinity B) first ionization energy C) atomic radius D) number of outermost electrons 90) How many valence electrons are there in an atom of magnesium? A) 4 B) 6 C) 5 D) 3 E) 2 91) What is the electron configuration of the gallium ion? A) 1s22s22p63s23p54s1 B) 1s22s22p63s23p3 C) 1s22s22p63s23p6 D) 1s22s22p63s23p63d10 E) 1s22s22p63s23p64s24p6 92) What is the formula of the ion formed when phosphorus achieves a noble-gas electron configuration? A) PB) P3+ C) P3- D) P2+ E) P293) How does oxygen obey the octet rule when reacting to form compounds? A) It gives up electrons. B) It does not change its number of electrons. C) It gains electrons. 94) What is the name of the ionic compound formed from strontium and phosphorus? A) strontium phosphorus B) strontium phosphate C) strontide phosphate D) strontium phosphoride E) strontium phosphide 95) Under what conditions can potassium bromide conduct electricity? A) only when melted, or dissolved in water B) only when melted C) only when dissolved D) only when it is in crystal form E) all of the above 96) Which of the following particles are free to drift in metals? A) protons B) neutrons C) electrons D) cations E) pions 97) How many unshared pairs of electrons does the nitrogen atom in ammonia possess? A) 4 B) 5 C) 2 D) 1 E) 3 98) How many electrons does carbon need to gain to obtain a noble-gas electron configuration? A) 4 B) 8 C) 2 D) 1 E) 3 99) Which of the following diatomic molecules is joined by a double covalent bond? A) O2 B) Cl2 C) N2 D) H2 Page 6 of 9 100) According to VSEPR theory, molecules adjust their shapes A) an emulsion B) supersaturated C) unsaturated D) saturated 114) What is the molarity of a solution containing 9.0 moles of solute in 500.0 mL of solution? A) 0.18M B) 4.5M C) 18M D) 1.8M E) 0.45M 115) What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution? A) 3M B) 6M C) 7M D) 12M 116) Which of the following operations yields the number of moles of solute? A) moles of solution ÷ volume of solution B) molarity x mass of solution C) molarity x moles of solution D) molarity x volume of solution E) mass of solution ÷ volume of solution 117) What is the molality of a solution containing 9.0 moles of solute in 2.4 kg of solvent? A) 3.8m B) 22m C) 0.38m D) 2.4m 118) What is the boiling point of a solution that contains 3 moles of KBr in 2000 g of water? (Kb = 0.512°C/m; gram formula mass of water = 18 g) A) 99.7°C B) 97°C C) 100°C D) 101.5°C E) 103°C 119) Activation energy is _____. A) the energy given off when reactants collide B) an energy barrier between reactants and products C) generally very high for a reaction that takes place rapidly D) the heat released in a reaction 120) Why does a higher concentration make a reaction faster? A) There are more collisions per second and the collisions are of greater energy. B) Collisions occur with greater energy. C) There are more collisions per second only. 121) Why does a small particle size generally cause a reaction to proceed faster? A) There are more collisions per second and the collisions are of greater energy. B) The collisions occur with greater energy. C) There are more collisions per second only. 122) The rate of a chemical reaction normally _____. A) increases as reactant concentration increases B) is slowed down by a catalyst C) decreases as temperature increases D) decreases as reactant concentration increases Page 7 of 9 Problems 158) When a mixture of sulfur and metallic silver is 142) What is the density of an object having a mass of heated, silver sulfide is produced. What mass of 4.0 g and a volume of 39.0 cubic centimeters? silver sulfide is produced from a mixture of 3.0 g 143) What is the temperature 198 K expressed in Ag and 3.0 g S8? degrees Celsius? 16Ag(s) + S8(s) → 8Ag2S(s) 144) What is the volume of 500.0 g of ice if the 159) How many molecules are present in 33.0 L of density of ice is 0.92 g/mL? nitrogen gas at STP? 145) Convert 0.0349 mm to meters. 160) A 55.0 g piece of copper wire is heated, and the 146) List the number of protons, neutrons, and temperature of the wire changes from 19.0°C to electrons in each of the following atoms. 86.0°C. The amount of heat absorbed is 343 cal. What is the specific heat of copper? 161) If 500 g of iron absorbs 22 000 cal of heat, what will be the change in temperature? (specific heat of iron = 0.11 cal/(g x °C)) 162) A gas has a volume of 590 mL at a temperature of -55.0°C. What volume will the gas occupy at 30.0°C? 163) A gas has a pressure of 710 mm Hg at 227°C. What will its pressure be at 27°C, if the volume 147) Name the following compounds: CoCl2, N2O5, does not change? and K2Cr2O7. 164) What is the pressure exerted by 32 g of O2 in a 148) Write the formulas for the following compounds: 22.0-L container at 30.0°C? barium cyanide, sulfur hexafluoride, and 165) How many electrons are in the highest occupied mercury(II) chloride. energy level of a neutral strontium atom? 149) Find the mass in grams of 2.20 x 1023 166) What is the wavelength of light with a frequency molecules of F2. of 1.0 x 1020 Hz? (c = 3.0 x 108 m/s) 150) What is the empirical formula of a compound 167) What is the energy of a photon of light with that is 40.7% carbon, 54.2% oxygen, and 5.1% frequency hydrogen? 1.0 x 1012 Hz? (h = 6.6 x 10-34 J s) 151) Find the number of moles of argon in 481 g of 168) What is the electron configuration of oxygen? argon. 169) Which element in the second principal energy 152) Balance the following equation. Complete the level has the greatest atomic radius? equation first, if necessary. 170) Give the electron configurations for sulfur and C3H6 + O2 → CO2 + H2O its 2- ion. 153) Balance the following equation. Complete the 171) Give the electron configurations for iodine and equation first, if necessary. its 1- ion. Al + Cl2 → 172) How many electrons does a gallium atom give up when it becomes an ion? 154) Balance the following equation. Complete the 173) Give the electron configuration for the lithium equation first, if necessary. ion. Fe2(SO4)3 + Ba(OH)2→ 174) Write the formula for the compound, aluminum 155) How many liters of O2 are needed to react iodide. completely with 45.0 L of H2S at STP? 175) How many calories are required to heat 354 2H2S(g) + 3O2(g) → 2SO2(g) + 2H2O(g) grams of water from 19°C to 87°C? 156) How many liters of O2 are needed to react 176) How many calories are released when 15 grams completely with 47.0 L of H2S at STP? of steam at 100°C condense to 15 grams of water at 100°C? 2H2S(g) + 3O2(g) → 2SO2(g) + 2H2O(g) 157) For the reaction 2Na + Cl2 → 2NaCl, how many grams of NaCl could be produced from 103.0 g of Na and 13.0 L of Cl2 (at STP)? Page 8 of 9 Answers 1) A 2) D 3) B 4) B 5) D 6) A 7) B 8) D 9) D 10) E 11) A 12) D 13) B 14) E 15) C 16) D 17) D 18) C 19) A 20) B 21) D 22) A 23) D 24) D 25) A 26) A 27) D 28) C 29) E 30) A 31) D 32) A 33) C 34) E 35) B 36) A 37) D 38) B 39) E 40) A 41) E 42) B 43) C 44) D 45) E 46) D 47) E 48) B 49) C 50) A 51) C 52) E 53) D 54) C 55) D 56) B 57) A 58) A 59) C 60) D 61) C 62) A 63) B 64) C 65) A 66) C 67) A 68) A 69) D 70) D 71) A 72) C 73) A 74) C 75) D 76) A 77) B 78) A 79) A 80) D 81) D 82) C 83) D 84) C 85) D 86) E 87) D 88) C 89) C 90) E 91) D 92) C 93) C 94) E 95) A 96) C 97) D 98) A 99) A 100) A 101) C 102) D 103) B 104) A 105) B 106) A 107) D 108) D 109) A 110) C 111) A 112) B 113) B 114) C 115) A 116) D 117) A 118) D 119) B 120) C 121) C 142) 0.10 g/cm3 143) -75°C 144) 540 mL 145) 0.0000349 m 146) Protons: 6, 7, 10, 5, 4 Neutrons: 7, 8, 10, 6, 5 Electrons: 6, 7, 10, 5, 4 147) cobalt(II) chloride, dinitrogen pentoxide, potassium dichromate 148) Ba(CN)2 SF6 HgCl2 149) 13.9 g F2 150) Empirical formula = C2H3O2 151) 12.1 mol Ar 152) C3H6 + 3O2 →3CO + 3H2O 153) 2Al + 3Cl2 → 2AlCl3 154) Fe2(SO4)3 + 3Ba(OH)2 → 2Fe(OH)3 + 3BaSO4 155) 67.5 L O2 156) 70.5 L O2 157) Cl2 is limiting reagent: 67.3 g NaCl 158) Answer: Limiting reagent is silver: 3.72 g Ag2S 159) 8.87 x 1023 molecules Page 9 of 9 160) 9.31 x 10-2 cal/(g x °C) 161) 400°C 162) 820 mL 163) 470 mmHg 164) 1.13 atm or 860 mmHg 165) 2 166) 3.0 x 10-12 m 167) 6.6 x 10-22 J 168) 1s22s22p4 169) lithium 170) S 1s22s22p63s23p4 S2- 1s22s22p63s23p6 171) I 1s22s22p63s23p63d104s24p64d 104f145s25p5 I1s22s22p63s23p63d104s24p64d 104f145s25p6 172) 3 173) 1s2 174) AlI3 175) 2.4 x 104 cal 176) 8.1 x 103cal