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Unit 1: Sig. Figs, Compounds, Elements, Homo/Hetero mixtures, density 1. Materials made from a single type of atom that cannot be broken down any further are called a. substances. b. elements. c. molecules. d. solutions. e. compounds. 2. Which group of substances contains only elements? a. hydrogen, plastics, carbon b. salt, copper, aluminum c. gold, silver, limestone d. steel, carbon, oxygen e. calcium, carbon, helium 3. Carbon dioxide, water (H2O), and nitrous oxide are best characterized as a. atoms b. elements c. mixtures d. all chemicals e. molecules 4. Sand, air, and powdered iced tea are best characterized as a. atoms b. elements c. mixtures d. solutions e. molecules 5. The main difference between compounds and mixtures is a. compounds cost more than mixtures. b. all mixtures include some of the heavy metals. c. mixtures are formed from the elements in specific proportions. d. most compounds are highly reactive. e. mixtures are not chemically bonded. 6. A material that has a definite shape and volume, and which is rigid enough to counteract a force imposed on it is a. a solid b. a liquid c. a gas. d. a plasma. e. all of the above at one time or another 7. A material that maintains a constant volume, but assumes the shape of its container is a. a gas. b. a solid. c. a liquid. d. a polymer. e. a and c both 8. In order of the least to the greatest, rank these phases of matter according to their kinetic energy. a. solid liquid gas b. gas liquid solid c. liquid gas solid d. solid gas liquid Unit 1: Sig. Figs, Compounds, Elements, Homo/Hetero mixtures, density 9. A change of phase of matter a. usually involves a change in the chemical identity of the individual atoms as part of the process of transformation. b. can in some cases involve a change from a solid directly to a gas without the appearance of a liquid. c. is only on rare occasion related to the energy of the individual atoms in the substance. d. all of the above e. none of the above 10. The fundamental building block for all matter; the smallest representative sample of a substance that maintains chemical identity. a. atom b. mixture c. molecule d. compound 11. The atmosphere of the Earth is best described as a/an a. Compound b. Element c. Mixture d. Molecule Use the three tables below to answer questions twelve and thirteen. Table One (Substance One) Table Two (Substance Two) Density of Substances Mass Volume Mass Volume Substance Density 5g 10 mL 5g 5 mL H2O 1 g/mL 10 g 20 mL 10 g 10 mL NaOH 2.1 g/mL 15 g 30 mL 15 g 15 mL HCl (aq) 1.15 g/mL 20 g 40 mL 20 g 20 mL NH3 0.76 g/mL 25 g 50 mL 25 g 25 mL 12. From the data in tables two and three, sample two is most likely: a. HCl b. NaOH c. H2O d. NH3 13. Use the tables to compare the two substances and determine which of the following statements is true. a. Substance one will float on substance two b. Substance two will float on substance one c. Substance one will dissolve in substance two d. The two substances are the same 14. A cup of water is added to a quart of Kool-aid. The resulting mixture is: a. A heterogeneous mixture, formed by a physical change b. A homogeneous mixture, formed by a physical change c. A single pure substance, formed by a chemical change d. A new compound, formed by a chemical change Unit 1: Sig. Figs, Compounds, Elements, Homo/Hetero mixtures, density 15. Which one of the following is an example of a physical change? a. Iron rusting b. Steak cooking c. Sugar dissolving in water d. A candle burning 16. A physical change means that no new substance is formed a. True b. False 17. Breaking water up by separating it into hydrogen and oxygen is an example of a a. Physical change b. Chemical change 18. Melting and oiling causes a a. Physical change b. Chemical change 19. A change in size or shape is a a. Physical change b. Chemical change 20. A chemical change means that a new substance with new properties is formed. a. True b. False 21. The fact that sugar is white is a a. Physical property b. Chemical property 22. Iron rust when exposed to air. This is a a. Physical property b. Chemical property 23. Which one of the following is not a physical property of hydrogen? a. It is a gas b. It is explosive c. It is colorless d. It has no smell 24. Which one of the following is not a physical change? a. Clothes drying in the dryer b. Making a cup of coffee c. Chopping wood d. Boiling an egg 25. How many significant figures are in 0.040930? a. 7 b. 5 c. 6 d. 4 26. How many significant figures are in 5.010 × 103? a. 3 b. 1 c. 4 d. 7 Unit 1: Sig. Figs, Compounds, Elements, Homo/Hetero mixtures, density 27. Perform the indicated operation and give an answer with the proper number of significant figures: 48.2 m + 3.87 m + 48.4394 m a. 100.51 b. 101 c. 100.5 d. 100.5094 28. Perform the indicated operation and give an answer with the proper number of significant figures: 451 g – 15.46 g a. 435.5 b. 435 c. 436 d. 435.54 29. Perform the indicated operation and give an answer with the proper number of significant figures: (33.58 × 1.007) / 0.00705 a. 4796.4624 b. 4800 c. 4796 d. 4.80 × 103 30. What is the density of a salt solution if 50.3 mL has a mass of 57.35 grams, using the correct number of significant figures? a. 1.140 g/mL b. 1.14 g/mL c. 1.1 g/mL d. 1.1401591 g/mL 31. What is the volume of 5.78 grams of gold? Report your answer to the correct number of significant figures. a. 0.3 cm3 b. 0.299 cm3 c. 0.30 cm3 d. 0.29 cm3 32. Identify the following pictures as a mixture or substance. If the picture represents a substance, state whether it is a compound or element. If the picture represents a mixture, state whether it is homogeneous or heterogeneous. a. b. c. d. Unit 2: Atoms, experiments, p+, n0, e-, ions, isotopes, nuclear equations 1. What is the name of Dalton’s model of the atom? a. Plum pudding model b. Quantum mechanical model c. Nuclear model d. Solid sphere model 2. What is the name of J.J. Thompson’s model of the atom? a. Plum pudding model b. Quantum mechanical model c. Nuclear model d. Solid sphere model 3. What is the name of Schrodinger’s model of the atom? a. Plum pudding model b. Quantum mechanical model c. Nuclear model d. Solid sphere model 4. What is the name of Rutherford’s model of the atom? a. Plum pudding model b. Quantum mechanical model c. Nuclear model d. Solid sphere model 5. Which of the following are results of Rutherford’s model of the atom? a. Dense positively charged nucleus, a lot of empty space b. Dense negatively charged nucleus, no empty space c. Dense positively charged nucleus, no empty space d. Dense negatively charged nucleus, a lot of empty space 6. Which of the following shows the order of correct charge, mass, and location of a proton in an atom? a. +1, 0, outside the nucleus b. +1, 1, outside the nucleus c. +1, 1, inside the nucleus d. +1, 0, inside the nucleus 7. Which of the following shows the order of correct charge, mass, and location of an electron in an atom? a. -1, 0, outside the nucleus b. -1, 1, outside the nucleus c. -1, 1, inside the nucleus d. -1, 0, inside the nucleus 8. How many electrons, protons, and neutrons does a neutral atom of strontium – 89 have? a. e- = 38, p+= 38, n0= 41 b. e- = 38, p+= 41, n0= 41 c. e- = 41, p+= 38, n0= 41 d. e- = 38, p+= 41, n0= 38 9. How many electrons, protons, and neutrons does a neutral atom of fluorine – 19 have? a. e- = 19, p+= 19, n0= 10 b. e- = 19, p+= 9, n0= 9 c. e- = 9, p+= 9, n0= 10 d. e- = 10, p+= 10, n0= 9 10. How many electrons, protons, and neutrons does an ion of 9 Be have? a. e- = 2, p+= 4, n0= 9 Unit 2: Atoms, experiments, p+, n0, e-, ions, isotopes, nuclear equations b. e- = 2, p+= 4, n0= 5 c. e- = 4, p+= 4, n0= 5 d. e- = 4, p+= 2, n0= 5 11. How many electrons, protons, and neutrons does an ion of 32 P have? a. e- = 15, p+= 15, n0= 17 b. e- = 15, p+= 17, n0= 15 c. e- = 18, p+= 15, n0= 16 d. e- = 18, p+= 15, n0= 17 12. When an atom of gallium forms a gallium ion, its charge becomes ______ because it _______ electron(s). a. -3, loses b. +3, gains c. +3, loses d. -3, gains 13. When an atom of bromine forms a bromine ion, its charge becomes _______ because it _______ electron(s). a. -1, gain b. -1, lose c. +1, gain d. +1, lose 14. Which of the following is not a property of a metal? a. Conducts electricity in the solid state b. High melting/boiling point c. Malleable and ductile d. Conducts electricity when dissolved in water 15. Which of the following is not a property of a nonmetal? a. Most solids at room temperature b. Low melting/boiling point c. Brittle solids at room temperature d. Right of the metalloid (semi-metal) “staircase” line 16. Which of the following is a correctly balanced nuclear equation? a. 23892U 23490Th + 42He b. 146C 147N + 42He c. 146C 147N + 0-1 Mg d. 23892U 23490Th + 42β 17. Which of the following represents alpha decay of radon – 222? a. 22286Rn 21884Po + 42He b. 86222Rn 82220Th + 42He c. 22688Ra 22286Rn + 42He d. 22286Rn 22287Fr + 0-1β Unit 3: Electrons, Quantum Mechanical model, energy levels, electron configurations 1. What element has the noble gas configuration [Ne]3s23p1? __________________ 2. What element has the electron configuration notation 1s22s22p63s1? ___________ 3. Which of the following is the correct noble-gas notation for the element strontium? a. [Kr]5s1 b. [Xe]5s2 c. [Kr]6s2 d. [Kr]5s2 4. The above orbital notation is used to represent which element? a. Boron b. Sulfur c. Oxygen d. fluorine 5. The above orbital notation is used to represent which element? a. Phosphorus b. Arsenic c. Nitrogen d. Silicon 6. Which of the following is the correct configuration notation for the element titanium (Ti)? a. 1s22s22p63s23p64s23d2 b. 1s22s22p63s23p63d24s2 c. 1s22s22p63s23p64s24d2 d. 1s22s22p63s23p64s21d2 7. Which of the following is the correct electron configuration notation for the element nitrogen, N? a. 1s22s2 b. 1s22s22p6 c. 1s22s22p3 d. 1s22s21p3 8. Which of the following is the correct electron configuration for an aluminum ion? a. 1s22s22p63s23p1 b. 1s22s22p63s23p6 c. 1s22s22p6 d. 1s22s22p63s2 Unit 3: Electrons, Quantum Mechanical model, energy levels, electron configurations 9. Which of the following electron dot notations is correct for the element phosphorus when it is in the ground state? a. I b. II c. V d. III 10. Which of the following electron dot notations is correct for the element oxygen when it is in the ground state? a. I b. II c. III d. V 11. Which of the following elements has the same number of valence electrons as the element sodium? a. Ar b. Cs c. Ca d. Mg 12. Which of the following elements has the same number of valence electrons as the element selenium? a. Fe b. K c. P d. O 13. Which of the following elements will have similar physical and chemical properties as lithium? a. Rubidium b. Carbon c. Nitrogen d. neon 14. Which of the following elements will have similar physical and chemical properties as Iodine? a. Te b. Xe c. F d. Po Unit 3: Electrons, Quantum Mechanical model, energy levels, electron configurations 15. When an electron gets excited and goes up an energy level, it has ____________ energy and when an electron goes down an energy level, it has ____________ energy. a. Absorbed, released b. Released, absorbed c. Ground, excited d. Excited, absorbed 16. When an electron transitions from n = 3 to n = 4, it has ____________. a. Absorbed energy b. Released energy c. Excited state d. Ground state 17. When an electron transitions from n = 6 to n = 2, it has ___________. a. Absorbed energy b. Released energy c. Ultraviolet radiation d. Infrared radiation 18. What color light is produced when an electron transitions from the n = 6 to n = 2 energy level? a. Blue b. Red c. No color d. violet 19. Given the representation of a chlorine atom, which circle might represent an atom of bromine? a. Circle B b. Circle D c. None of these d. Circle C Unit 3: Electrons, Quantum Mechanical model, energy levels, electron configurations 20. Given the representation of a chlorine atom, which circle might represent an atom of sulfur? a. None of these b. Circle B c. Circle D d. Circle C 21. As one moves from left to right ( → ) within a period across the periodic table, the electronegativity of the elements encountered tends to: a. stay the same b. increase c. decrease 22. The elements with the largest atomic radii are found in the: a. lower right-hand corner of the periodic table b. lower left-hand corner of the periodic table c. upper right-hand corner of the periodic table d. upper left-hand corner of the periodic table Unit 3: Electrons, Quantum Mechanical model, energy levels, electron configurations 23. Of the following elements, which one would have the largest radius? a. Cesium (Cs, atomic #55) b. Potassium (K, atomic #19) c. Hydrogen (H, atomic #1) d. Sodium (Na, atomic #11) 24. The energy required to remove an electron from an atom is known as: a. radioactivity b. electron affinity c. ionization energy d. electronegativity 25. Of the following elements, which one would have the largest ionization energy? a. Cesium (Cs, atomic #55) b. Hydrogen (H, atomic #1) c. Sodium (Na, atomic #11) d. Potassium (K, atomic #19) Unit 4: Bond types, lewis structures, polarity of molecules 1. Which of the following gases does not exist in nature as a diatomic molecule? a. Nitrogen b. Helium c. Hydrogen d. oxygen 2. Ionic compounds generally form: a. Liquids b. Gases c. Crystals d. molecules 3. In metallic bonding, the valence electrons of all atoms are shared in: a. A nonpolar covalent bond b. An electron sea c. A polar covalent bond d. Transferred to metallic ions 4. The metalloids possess properties of metals and nonmetals and are also known as a. Semimetals b. Halogens c. Gases d. Liquids 5. The seven elements that occur as diatomic elements are a. H2,N2,O2,He2,Ne2,C2,Na2 b. H2,N2,O2,He2,Ne2,Cl2,Br2 c. H2,N2,O2,F2,I2,Cl2,Br2 d. Fe2,Rn2,O2,He2,Ne2,C2,Br2 6. The bond between sodium and oxygen is expected to be a. Gaseous b. Nonpolar covalent c. Ionic d. Polar covalent 7. When compared to single bonds, double bonds are generally a. Shorter and stronger b. Longer and stronger c. Longer and weaker d. Shorter and weaker 8. The bond between lithium and fluorine is a. Polar covalent b. Ionic c. Nonpolar covalent d. metallic 9. In the ionic compound magnesium fluoride, what is the ratio of the two elements necessary so that each element obtains its octet from the transfer of electrons? a. 3 magnesium: 1 fluorine b. 1 magnesium: 1 fluorine c. 2 magnesium: 1 fluorine d. 1 magnesium: 2 fluorine 10. In the correct Lewis structure for water, how many unshared pairs of electrons will oxygen have? a. 1 b. 3 c. 4 d. 2 Unit 4: Bond types, lewis structures, polarity of molecules 11. In the correct Lewis structure for the methane molecule, how many unshared electron pairs surround the carbon? a. 2 b. 0 c. 8 d. 4 12. In nonpolar covalent bonds, valence electrons are a. Equally shared b. Unequally shared c. Destroyed d. transferred 13. Which of the following is an acceptable Lewis structure for chloromethane (CH3Cl)? a. b. c. d. 14. In a diatomic molecule of an element, the bond between the atoms must be a. Nonpolar covalent b. Polar covalent c. Metallic d. ionic 15. In polar covalent bonds, valence electrons are a. transferred b. unequally shared c. destroyed d. equally shared Unit 4: Bond types, lewis structures, polarity of molecules 16. In ionic bonds, valence electrons are a. Equally shared b. Transferred c. Unequally shared d. destroyed 17. How many atoms are needed to provide the electrons necessary to complete the valence octet of an oxygen atom? a. Three sodium atoms b. Two sodium atoms c. Four sodium atoms d. One sodium atom 18. The measure of the attraction that an atom has for electrons involved in chemical bonds is known as a. Ionization energy b. Radioactivity c. Electronegativity d. Electron affinity 19. Which of the following is the correct Lewis structure for ammonia? a. b. c. d. 20. In drawing Lewis structures, a single line (single bond) between two elements represents a. An octet of electrons b. An unshared pair of electrons c. A shared electron d. A shared pair of electrons 21. Which of the following is a correct Lewis structure for hydrogen cyanide, HCN? a. b. c. d. Unit 4: Bond types, lewis structures, polarity of molecules 22. Which of the following is the correct Lewis structure for formaldehyde, CH2O a. b. c. d. 23. Which of the following is the correct Lewis structure for phosphorus tribromide? a. b. c. d. 24. Which of the diatomic elements has a double bond between its atoms? a. Fluorine b. Nitrogen c. Oxygen d. Hydrogen Unit 5: Moles, molar mass, number of particles/atoms/ions/molecules 1. What is the mass of 2 moles of propane gas, C3H8? a. 11 grams b. 44 grams c. 22 grams d. 88 grams 2. How many moles of propane gas, C3H8, are contained in 11 grams of C3H8? a. 11 × 1023 moles b. 4 moles c. 1.5 × 1023 moles d. 0.25 moles 3. What is the mass in grams of 3 moles of water molecules, H2O? a. 54 grams b. 0.166 grams c. 6 grams d. 21 grams 4. How many moles of water molecules, H2O, are present in a 27 gram sample of water? a. 9 × 1023 moles b. 1.5 moles c. 2 moles d. 2/3 mole 5. What is the mass of 10 moles of ammonia, NH3? a. 1.7 grams b. 27 grams c. 170 grams d. 0.587 grams 6. How many moles of methane, CH4, are in 80 grams of methane? a. 6.022 × 1080 moles b. 5 moles c. 80 × 1023 moles d. 0.201 moles 7. How many molecules are contained in 3 moles of water, H2O? a. 6 molecules b. 54 molecules c. 1.8 × 1024 molecules d. 3 × 1023 molecules 8. A sample of carbon dioxide gas (CO2) contains 6.022× 1023 molecules. How many moles of carbon dioxide does this represent? a. 1 mole b. 440 moles c. 44 moles d. 10 moles 9. How many molecules of ethane gas, C2H6, are in 15 grams of the compound? a. 0.5 moles b. 2 moles c. 3 × 1023 moles Unit 5: Moles, molar mass, number of particles/atoms/ions/molecules d. 45 moles 10. What is the mass, in grams, of 3 × 1023 atoms of helium? a. 2 grams b. 1.2 × 1024 grams c. 3 × 1023 grams d. 8 grams 11. Approximately how many atoms of carbon are present in a 120 gram sample of carbon? a. 10 atoms b. 6 × 1022 atoms c. 6 × 1024 d. 1440 atoms 1 mole of a compound/element = _________________________ particles 1 mole of a compound/element = _________________________ in grams Molar mass of a compound = 6.022× 1023 particles Unit 6: Naming Ionic and Covalent Compounds, % composition, empirical and molecular formulas 1. What is the mass of 2 moles of propane gas, C3H8? a. 11 grams b. 44 grams c. 22 grams d. 88 grams 2. How many moles of propane gas, C3H8, are contained in 11 grams of C3H8? a. 11 × 1023 moles b. 4 moles c. 1.5 × 1023 moles d. 0.25 moles 3. What is the mass in grams of 3 moles of water molecules, H2O? a. 54 grams b. 0.166 grams c. 6 grams d. 21 grams 4. How many moles of water molecules, H2O, are present in a 27 gram sample of water? a. 9 × 1023 moles b. 1.5 moles c. 2 moles d. 2/3 mole 5. What is the mass of 10 moles of ammonia, NH3? a. 1.7 grams b. 27 grams c. 170 grams d. 0.587 grams 6. How many moles of methane, CH4, are in 80 grams of methane? a. 6.022 × 1080 moles b. 5 moles c. 80 × 1023 moles d. 0.201 moles 7. How many molecules are contained in 3 moles of water, H2O? a. 6 molecules b. 54 molecules c. 1.8 × 1024 molecules d. 3 × 1023 molecules 8. A sample of carbon dioxide gas (CO2) contains 6.022× 1023 molecules. How many moles of carbon dioxide does this represent? a. 1 mole b. 440 moles c. 44 moles d. 10 moles 9. How many molecules of ethane gas, C2H6, are in 15 grams of the compound? a. 0.5 moles b. 2 moles c. 3 × 1023 moles Unit 6: Naming Ionic and Covalent Compounds, % composition, empirical and molecular formulas d. 45 moles 10. What is the mass, in grams, of 3 × 1023 atoms of helium? a. 2 grams b. 1.2 × 1024 grams c. 3 × 1023 grams d. 8 grams 11. Approximately how many atoms of carbon are present in a 120 gram sample of carbon? a. 10 atoms b. 6 × 1022 atoms c. 6 × 1024 d. 1440 atoms 1 mole of a compound/element = _________________________ particles 1 mole of a compound/element = _________________________ in grams Molar mass of a compound = 6.022× 1023 particles