REVIEWER FOR FINALS in CHM 11-3

Multiple ChoiceIdentify the choice that best completes the statement or answers the question.

____ 1. Name the molecular compound, SO3.a. sulfur oxideb. sulfurous acidc. sulfur trioxided. sulfuric acide. none of the above

____ 2. The molecular formula for a compound is CX4. If 2.819 g of this compound contains 0.102 g of carbon, what is the atomic weight of X?a. 320b. 160c. 35.5d. 79.9e. 39.9

____ 3. How many atoms are in 1.00 mole of water?a. 6.02 1023

b. 1.20 1024

c. 1.81 1024

d. 2.41 1024

e. 3.01 1023

____ 4. How many grams of CaCl2 equal 4.26 moles of CaCl2?a. 26.1 gb. 170 gc. 302 gd. 473 ge. 322 g

____ 5. Which of the following is not a correct description of 16.0 grams of methane, CH4?a. It is one mole of methane.b. It is the amount of methane that contains 12.0 g of carbon.c. It is 16.0 6.02 1023 molecules of methane.d. It is the amount of methane that contains 4.0 grams of hydrogen.e. It is the amount of methane that contains 4 6.02 1023 hydrogen atoms.

____ 6. A compound is known to contain only carbon, hydrogen, and oxygen. If the complete combustion of a 0.150-g sample of this compound produces 0.225 g of CO2 and 0.0614 g of H2O, what is the empirical formula of this compound?a. C3H4

b. CH4Oc. C3HO3

d. C3H4O3

e. C5H7O5

____ 7. Balance the following equation with the smallest whole number coefficients. What is the coefficient for H2O in the balanced equation?

     Al(OH)3 HCl AlCl3 H2Oa. 1b. 2c. 3d. 14e. 5

____ 8. What is the coefficient for HBr when the following equation is balanced with the smallest whole number coefficients?     Br2 H2O HBr HBrO3

a. 5b. 7c. 8d. 3e. 6

____ 9. Balance the following equation with the smallest whole number coefficients. Choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one".     RbOH H3PO4 Rb3PO4 H2Oa. 8b. 10c. 12d. 4e. 6

____ 10. Balance the following equation with the smallest whole number coefficients. Choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one".     CuSO4 NH3 H2O (NH4)2SO4 Cu(NH3)4(OH)2

a. 8b. 9c. 11d. 12e. 14

____ 11. Ammonium nitrate fertilizer is sometimes used as an explosive. How many moles of water can be formed from the decomposition of 13.2 moles of ammonium nitrate?     2NH4NO3 2N2 O2 4H2Oa. 6.60b. 14.0c. 26.4d. 13.2e. 18.0

____ 12. How many grams of magnesium are required to produce 5.000 kg of Si?     SiCl4 2Mg Si 2MgCl2

a. 7595 gb. 7581 gc. 4327 gd. 9999 ge. 2164 g

____ 13. The following statements apply to the interpretation of chemical equations. Not all of the statements are true. Which statement is false?a. The number of grams of the reactants must equal the number of grams of products in a

balanced equation.

b. There will always be some of the excess reagent left at the completion of the reaction.c. The following equation for the reaction involving hypothetical substances, A, B, C, and D,

implies that the products C and D are always produced in a three to one mole ratio. A  2B  3C  D

d. The equation A 2B 3C D implies that in any reaction involving A and B as reactants, A must be the limiting reactant.

e. The total number of atoms in the reactants that react must always equal the total number of atoms in the products produced by the reaction.

____ 14. If 20.0 g of each reactant were used in performing the following reaction, which would be the limiting reactant?     2MnO2 4KOH O2 Cl2 2KMnO4 2KCl 2H2Oa. MnO2

b. KOHc. O2

d. Cl2

e. KMnO4

____ 15. What mass of water is contained in 200. grams of 15.0% KCl solution?a. 11.3 gb. 170. gc. 174. gd. 30.0 ge. 25.5 g

____ 16. Silver nitrate, AgNO3, reacts with sodium chloride as indicated by the following equation. What mass of NaCl would be required to react with 200. mL of 0.200 M AgNO3 solution?     AgNO3 NaCl AgCl NaNO3

a. 0.117 gb. 1.17 gc. 2.34 gd. 4.68 ge. 3.06 g

____ 17. Which element and group are not correctly matched?

Element Periodic Group or Classification

a. Sb metalloidb. Kr noble gasc. Al alkali metald. F halogene. Ca alkaline earth metal

____ 18. To which classification does strontium belong?a. alkali metalb. halogenc. alkaline earth metald. noble gase. metalloid

____ 19. Which one of the following salts is insoluble in water?a. K2Sb. NaClOc. Mg(NO3)2

d. Rb2CO3

e. Ba3(PO4)2

____ 20. Determine the oxidation number of the underlined element in Li2SO4.a. 6b. 2c. 3d. 4e. 5

____ 21. Determine the oxidation number of the underlined element in H2P2O7.a. 6b. 7c. 3d. 4e. 5

____ 22. Which of the following matched pairs of name and formula has an error?

Formula Name

a. Al(NO2)3 aluminum nitrateb. BaSO3 barium sulfitec. Cr(SCN)3 chromium(III) thiocyanated. N2O3 dinitrogen trioxidee. Sb4O6 tetraantimony hexoxide

____ 23. When two nonmetals combine, ____.a. they form a binary ionic compound.b. they form a binary covalent compound.c. they release hydrogen gas.d. they form two or more products.e. they neutralize the acid formed in the reaction.

____ 24. Which of the following reactions is not a decomposition reaction?a. 2HgO(s) 2Hg( ) O2(g)b. H2(g) Cl2(g) 2HCl(g)c. NH4NO3(s) N2O(g) 2H2O(g)d. Mg(OH)2(s) MgO(s) H2O(g)e. 2H2O2(aq) 2H2O( ) O2(g)

____ 25. What salt is formed when aqueous calcium hydroxide is mixed with phosphoric acid?a. CaPO4

b. Ca(OH)2

c. Ca3(PO4)2

d. P(OH)3

e. no salt formation occurs

____ 26. Which of the following is not a metathesis reaction?a. CH4(g) 2O2(g) CO2(g) 2H2O( )b. FeS(s) 2HCl(aq) FeCl2(aq) H2S(g)c. CaCl2(aq) K2CO3(aq) CaCO3(s) 2KCl(aq)d. 2HCl(aq) Ba(OH)2(aq) BaCl2(aq) 2H2O( )e. AgNO3(aq) NaBr(aq) AgBr(s) NaNO3(aq)

____ 27. Classify the following reaction by giving the reaction type that applies.

     2NiS(s) 3O2(g) 2NiO(s) 2SO2(g)a. redoxb. combinationc. decompositiond. displacemente. metathesis

____ 28. What is a vertical column on the periodic table called?a. a groupb. a periodc. a cland. the metals

____ 29. Which one of the following salts is the most soluble?a. iron(II) chloride, FeCl2

b. silver carbonate, Ag2CO3

c. silver chloride, AgCld. iron(III) phosphate, FePO4

____ 30. In the Rutherford gold foil experiment, the fact that most of the alpha particles were not deflected as they passed through the gold foil indicates thata. the nucleus is positively charged.b. the atom is mostly empty space.c. atoms are solid spheres touching each other in the solid state.d. gold is very dense.e. none of the above is correct.

____ 31. The atomic number of an atom is the number of ____ in the atom.a. protons plus the number of electronsb. neutronsc. protonsd. protons plus the number of neutronse. electrons plus the number of neutrons

____ 32. What is the symbol for a species composed of 35 protons, 44 neutrons, and 36 electrons?a.

b.

c.

d.

e.

____ 33. What is the symbol for a species composed of 20 protons, 20 neutrons, and 18 electrons?a. 40Cab. 40Arc. 34S2

d. 39K

e. 40Ca2

____ 34. An atom of the 40Ar isotope contains ____ protons.a. 18b. 20c. 22d. 40e. 19

____ 35. These three species 80Se, 81Br and 82Kr havea. the same atomic mass.b. the same number of protons.c. the same number of neutrons.d. the same mass number.e. the same number of electrons.

____ 36. What is the atomic weight of a hypothetical element consisting of two isotopes, one with mass 64.23 amu (26.00%), and one with mass 65.32 amu?a. 65.16 amub. 64.37 amuc. 64.96 amud. 65.04 amue. 64.80 amu

____ 37. A hypothetical element consists of the following naturally occurring isotopes. What is the atomic weight of the element?

Isotopes Mass Abundance1 46.041 amu 26.00%2 47.038 amu 58.00%3 49.034 amu 16.00%

a. 46.78 amub. 46.89 amuc. 47.02 amud. 47.10 amue. 47.24 amu

Chapter 5 Values

Some of the following values may be useful for solving some of the problems.

speed of light 3.00 108 m/s 1 joule 1 kg•m2/s2Planck's constant 6.63 1034 J•s 1 Ångstrom 1 1010 m

____ 38. What is the energy in joules of a photon of light of wavelength 3.75 103 Å?a. 3.30 1013 Jb. 5.30 1019 Jc. 1.10 1017 Jd. 1.38 1014 Je. 2.22 1011 J

____ 39. The principal quantum number of an orbital is n 1. This must be a(an) ____ orbital.a. sb. pc. dd. fe. g

____ 40. Which response includes all the following statements that are true, and no false statements?

I. Each set of d orbitals contains 7 orbitals.II. Each set of d orbitals can hold a maximum of 14 electrons.III. The first energy level contains only s and p orbitals.IV. The s orbital in any shell is always spherically symmetrical.

a. I and IIb. I, III, and IVc. IVd. II and IVe. III

____ 41. What is the value of the angular momentum quantum number, l , for the following orbital?

a.

b. 1c. 0d. 1e. 2

____ 42. No two electrons in the same atom can have the same set of four quantum numbers is a statement of ____.a. the Aufbau Principleb. the Pauli Exclusion Principlec. Dalton's Theoryd. Hund's Rulee. the Heisenberg Uncertainty Principle

____ 43. The total number of electrons in s orbitals in a germanium atom (Z 32) is ____.a. 18b. 15c. 8d. 20e. 6

____ 44. An element has the following outer electron configuration in its ground state, where n represents the highest occupied energy level: (n 1)d10ns1. Which of the elements listed below could it be?a. Kb. Agc. Ged. Gae. Cd

____ 45. An element that has four electrons in its outer shell in its ground state is ____.a. Nbb. Crc. Snd. Tie. O

____ 46. Of the following, which element does not match its designation?a. Sr representative metalb. In representative nonmetalc. Si metalloidd. W d-transition metale. Th f-transition metal

____ 47. ____ is a noble gas.a. Tib. Moc. Tld. Kre. U

____ 48. ____ is an actinide.a. Tib. Moc. Tld. Kre. U

____ 49. Arrange the following elements in order of decreasing first ionization energy.     Be, Ca, Cs, Mg, Ka. Mg > Be > Ca > K > Csb. Be > Mg > Ca > K > Csc. Cs > K > Ca > Be > Mgd. Ca > Mg > Be > Cs > Ke. Ca > Mg > Be > K > Cs

____ 50. Which of the following elements has the most negative electron affinity?a. Sib. Pc. Sd. See. Te

____ 51. A property that measures the ability of an atom to attract electrons in a chemical bond isa. binding energy.b. mass defect.c. electron affinity.d. ionization energy.e. electronegativity.

____ 52. Which element has the highest electronegativity?a. Bb. Gec. Cad. Oe. At

____ 53. Which one of the following is a molecular hydride?a. RbHb. SrHc. NaHd. PHe. CaH

____ 54. Write the balanced formula unit equation for the reaction of magnesium with hydrochloric acid. What is the sum of the coefficients? Don't forget coefficients of one. Use the smallest whole number coefficients.a. 5b. 6c. 3d. 4e. none of these

____ 55. Magnesium hydride is ____.a. basicb. neutralc. acidicd. inerte. non-reactive with water

____ 56. Which of the following statements about oxygen is false?a. The most common form of oxygen is a diatomic molecule.b. Ozone is an allotrope of oxygen.c. Both ozone and oxygen are oxidizing agents.d. Oxygen forms binary compounds with nonmetals called acid anhydrides.e. Oxygen forms basic nonmetal oxides.

____ 57. Which one of the following will not react with oxygen to form a peroxide?a. Beb. Cac. Srd. Bae. all form peroxides

____ 58. Which response includes all of the following oxides that are acid anhydrides?

I. COII. CaOIII. ClOIV. Tl O

a. I and IIIb. II and IVc. I and IVd. II, III, and IVe. I

____ 59. The acid formed by dissolving Cl O in water is ____.a. HClOb. HClOc. HClOd. HClOe. HCl

____ 60. Write the balanced formula unit equation for the reaction of nitrogen oxide with oxygen. What is the sum of the coefficients?a. 3b. 6c. 8d. 4e. 5

____ 61. Which one of the elements listed below has the largest atomic radius?a. magnesium, Mgb. potassium, Kc. rubidium, Rbd. calcium, Ca

____ 62. What is the charge formed by alkaline earth metals when they react with nonmetals?a. +1b. -1c. +2d. -2e. +3

____ 63. Magnesium and nitrogen react to form Mg N an ionic compound. The magnesium ion, Mg , has ____ electrons in its highest occupied energy level.a. 8b. 2c. 10d. 4e. 5

____ 64. The internuclear distance at which the attractive and repulsive forces balance in a covalent bond is called the ____.a. bond lengthb. bond energyc. stabilization lengthd. single bonde. none of these

____ 65. What is the correct Lewis dot formula for H CO ?a.

b.

c.

d.

e.

____ 66. Assign a formal charge to each atom of .a. As = 5+, Cl = 1-b. As = 5-, Cl = 7+c. As = 0, Cl = 0d. As = 4+, Cl = 1-e. As = 6+, Cl = 2-

____ 67. Which of the following molecules has the least polar bonds?a. BrIb. HIc. H2Od. HFe. NH3

____ 68. Which of the following compounds does not contain both ionic and covalent bonding?a. Na SOb. NH NOc. NH Cld. KCle. KClO

____ 69. What are the Lewis formulas for the chlorides of phosphorus, PCl3 and PCl5?a.

b.

c.

d.

____ 70. An ionic bond is most likely to be formed betweena. a metal of low ionization energy and a nonmetal of low (very positive) electron affinity.b. a metal of high ionization energy and a nonmetal of high (very negative) electron affinity.c. a metal of high ionization energy and a nonmetal of low (very positive) electron affinity.d. a metal of low ionization energy and a nonmetal of high (very negative) electron affinity.

____ 71. Which of the following is not one of the basic ideas of the VSEPR theory?a. Each electron group in the valence shell of a central atom is significant.b. The groups of valence shell electrons on the central atom repel one another.c. The groups of valence shell electrons are arranged about the central atom so that the

repulsions among them are as small as possible.d. The electron groups have maximum separation about the central atom.e. The number of electron groups is determined by counting the number of lone pairs and the

total number of bonds.____ 72. CH4 is a nonpolar molecule. Which of the following similar molecules is also nonpolar?

a. CH3Clb. CH2Cl2

c. SiH3Cld. SiH4

e. SiH2Cl2

____ 73. Which response contains all the following statements that are true, and no others?

I. A set of sp2 orbitals can be thought of as one s orbital one-third of the time and two p orbitals two-thirds of the time.

II. A set of sp orbitals can accommodate a maximum of six electrons.III. The orbitals resulting from sp3d2 hybridization are directed toward the corners of an

octahedron.IV. A set of sp3 orbitals results from the mixing of one s orbital and three p orbitals.

a. II and IVb. I, II, and IVc. II, III, and IVd. III and IVe. all are true

____ 74. The bond angles associated with sp3d2 hybridization are ____.a. 90° and 180°

b. 120°c. 109°d. 90° and 120°e. 109° and 120°

____ 75. The central atom in a molecule is sharing a total of 12 electrons. What type of hybrid orbitals are formed by the central atom?a. spb. sp2

c. sp3

d. sp3de. sp3d2

____ 76. Which of the following molecules has 120° bond angles?a. BF4

-

b. CF4

c. H2Od. BI3

e. NH4+

____ 77. Which one of the following molecules is polar?a. BCl3

b. CdI2

c. CCl4

d. NCl3

e. Br2

____ 78. What is the hybridization of the sulfur atom in SO32-?

a. spb. sp2

c. sp3

d. sp3de. sp3d2

____ 79. For AsF3, the electronic geometry is ____ and the molecular geometry is ____.a. tetrahedral, trigonal planarb. trigonal planar, tetrahedralc. tetrahedral, tetrahedrald. trigonal planar, trigonal planare. trigonal planar, linear

____ 80. The electronic geometry of the central atom in PCl3 is ____.a. pyramidalb. trigonal planarc. tetrahedrald. octahedrale. trigonal bipyramidal

____ 81. Which response contains all of the following molecules that can be described as bent or angular molecules and none that have other shapes?     BeI2, SO2, H2S, PF3, CO2

a. SO2, H2Sb. BeI2, SO2

c. BeI2, PF3, CO2

d. PF3, CO2

e. another combination

____ 82. What is the hybridization at the sulfur atom in SF6?a. spb. sp2

c. sp3

d. sp3de. sp3d2

____ 83. What is the geometry of a carbon atom involved in one double bond?a. linearb. trigonal planarc. tetrahedrald. trigonal bipyramidale. octahedral

____ 84. Which of the following statements regarding a carbon atom involved in 2 double bonds is false?a. The geometry is linear.b. The hybridization is sp.c. There are 2 sigma and two pi bonds.d. The C atom has two unhybridized p atomic orbitals.e. The C atom can make one more bond to complete its octet.

____ 85. What is the hybridization of a carbon atom involved in a triple bond?a. spb. sp2

c. sp3

d. sp3de. sp3d2

____ 86. Which molecule is incorrectly matched with the molecular geometry?

Molecule Molecular Geometry

a. CCl4 tetrahedralb. PH3 pyramidalc. BeCl2 lineard. BBr3 trigonal planare. SO2 linear

____ 87. Which, if any, of the compounds listed are not sp3d hybridized at the central atom?

I. BF3

II. AsI5

III. SF4

IV. BrF5

V. XeF4

a. III and IVb. I, II, and IIIc. I, IV, and Vd. III and Ve. all are sp3d hybridized

____ 88. Each molecule of boron trifluoride, BF3, is trigonal planar. The boron atom is in the center, with the three fluorine atoms around it. Each fluorine atom is bonded only to the boron atom. Draw a picture of this molecule.

What is the angle between any two boron-fluorine bonds?a. 60b. 90c. 120d. 180

____ 89. Ultra-pure Si is required to produce semi-conductors. The first step in this process is combining silicon dioxide with carbon and chlorine. Choose the answer that represents the sum of all the coefficients when this equation is balanced using the smallest whole number coefficients.     SiO2 C Cl2 CO SiCl4

a. 5b. 6c. 16d. 7e. 8

____ 90. Propane (C3H8) burns in oxygen to form CO2 and H2O according to the following equation. How many grams of O2 are required to burn 3.01 1023 propane molecules?     C3H8 5O2 3CO2 4H2Oa. 80.0 gb. 40.0 gc. 160 gd. 16.0 ge. 64.0 g

____ 91. How many moles of H2O will be produced from the complete combustion of 2.4 grams of CH4?     CH4 2O2 CO2 2H2Oa. 0.15b. 0.30c. 1.5d. 3.0e. 6.0

____ 92. If 25.0 g of each reactant were used in performing the following reaction, which would be the limiting reactant?     3PbO2 Cr2(SO4)3 K2SO4 H2O 3PbSO4 K2Cr2O7 H2SO4

a. PbO2

b. H2Oc. K2SO4

d. PbSO4

e. Cr2(SO4)3

____ 93. How many moles of carbon dioxide could be produced if 10 moles of octane, C8H18, are combined with 20 moles of oxygen?     C8H18 25O2 16CO2 18H2Oa. 40 molb. 8.0 molc. 12.8 mold. 62.5 mole. 20 mol

____ 94. What is the percent yield of CO2 if the reaction of 10.0 grams of CO with excess O2 produces 12.8 grams of CO2?     2CO(g) O2(g) 2CO2(g)a. 76.4%b. 78.1%

c. 81.5%d. 84.4%e. 88.9%

____ 95. Salicylic acid reacts with acetic anhydride to form aspirin, acetylsalicylic acid. If the percent yield in this reaction is 78.5%, what mass of salicylic acid is required to produce 150. g aspirin?

2 C7H6O3 C4H6O3 2 C9H8O4 H2Osalicylic acid acetic anhydride aspirin

a. 292 gb. 146 gc. 90.0 gd. 73.0 ge. 191 g

Prefinals for Chm 11-3

Answer

MULTIPLE CHOICE

1. ANS: C PTS: 1 TOP: Chemical Formulas2. ANS: D PTS: 1 DIF: * Harder Question

TOP: Atomic Weights3. ANS: C PTS: 1 TOP: The Mole4. ANS: D PTS: 1 TOP: Formula Weights, Molecular Weights, and Moles5. ANS: C PTS: 1 TOP: Formula Weights, Molecular Weights, and Moles6. ANS: D PTS: 1 TOP: Derivation of Formulas from Elemental Composition7. ANS: C PTS: 1 TOP: Chemical Equations8. ANS: A PTS: 1 TOP: Chemical Equations9. ANS: A PTS: 1 TOP: Chemical Equations

10. ANS: C PTS: 1 TOP: Chemical Equations11. ANS: C PTS: 1 TOP: Calculations Based on Chemical Equations12. ANS: A PTS: 1 TOP: Calculations Based on Chemical Equations13. ANS: D PTS: 1 TOP: The Limiting Reactant Concept14. ANS: B PTS: 1 TOP: The Limiting Reactant Concept15. ANS: B PTS: 1 TOP: Concentrations of Solutions16. ANS: C PTS: 1 TOP: Using Solutions in Chemical Reactions17. ANS: C PTS: 1 TOP: The Periodic Table: Metals, Nonmetals, and Metalloids18. ANS: C PTS: 1 TOP: The Periodic Table: Metals, Nonmetals, and Metalloids19. ANS: E PTS: 1 TOP: Aqueous Solutions--An Introduction20. ANS: A PTS: 1 TOP: Oxidation Numbers21. ANS: A PTS: 1 TOP: Oxidation Numbers22. ANS: A PTS: 1 TOP: Naming Ternary Acids and Their Salts23. ANS: B PTS: 1 TOP: Combination Reactions24. ANS: B PTS: 1 TOP: Decomposition Reactions25. ANS: C PTS: 1 TOP: Metathesis (Acid--Base) Reactions26. ANS: A PTS: 1 TOP: Gas-Formation Reactions27. ANS: A PTS: 1 TOP: Summary of Reaction Types28. ANS: A PTS: 1 TOP: Additional Questions29. ANS: A PTS: 1 TOP: Additional Questions30. ANS: B PTS: 1 TOP: Rutherford and the Nuclear Atom31. ANS: C PTS: 1 TOP: Mass Number and Isotopes32. ANS: E PTS: 1 TOP: Mass Number and Isotopes33. ANS: E PTS: 1 TOP: Mass Number and Isotopes34. ANS: A PTS: 1 TOP: Mass Number and Isotopes35. ANS: C PTS: 1 TOP: Mass Number and Isotopes36. ANS: D PTS: 1 TOP: The Atomic Weight Scale and Atomic Weights37. ANS: D PTS: 1 TOP: The Atomic Weight Scale and Atomic Weights38. ANS: B PTS: 1 TOP: Electromagnetic Radiation39. ANS: A PTS: 1 TOP: Quantum Numbers40. ANS: C PTS: 1 TOP: Atomic Orbitals41. ANS: E PTS: 1 TOP: Atomic Orbitals

42. ANS: B PTS: 1 TOP: Electron Configurations43. ANS: C PTS: 1 TOP: The Periodic Table and Electron Configurations44. ANS: B PTS: 1 DIF: * Harder Question

TOP: The Periodic Table and Electron Configurations45. ANS: C PTS: 1 TOP: The Periodic Table and Electron Configurations46. ANS: B PTS: 1 TOP: More About the Periodic Table47. ANS: D PTS: 1 TOP: More About the Periodic Table48. ANS: E PTS: 1 TOP: More About the Periodic Table49. ANS: B PTS: 1 TOP: Ionization Energy50. ANS: C PTS: 1 TOP: Electron Affinity51. ANS: E PTS: 1 TOP: Electronegativity52. ANS: D PTS: 1 TOP: Electronegativity53. ANS: D PTS: 1 TOP: Hydrogen and the Hydrides54. ANS: A PTS: 1 TOP: Hydrogen and the Hydrides55. ANS: A PTS: 1 TOP: Hydrogen and the Hydrides56. ANS: E PTS: 1 TOP: Oxygen and the Oxides57. ANS: A PTS: 1 TOP: Oxygen and the Oxides58. ANS: A PTS: 1 TOP: Oxygen and the Oxides59. ANS: D PTS: 1 TOP: Oxygen and the Oxides60. ANS: E PTS: 1 TOP: Oxygen and the Oxides61. ANS: C PTS: 1 TOP: Additional Questions62. ANS: C PTS: 1 TOP: Formation of Ionic Compounds63. ANS: A PTS: 1 TOP: Formation of Ionic Compounds64. ANS: A PTS: 1 TOP: Bond Lengths and Bond Energies65. ANS: C PTS: 1 TOP: Writing Lewis Formulas: The Octet Rule66. ANS: C PTS: 1 TOP: Formal Charge67. ANS: A PTS: 1 TOP: Polar and Nonpolar Covalent Bonds68. ANS: D PTS: 1 TOP: The Continuous Range of Bonding Types69. ANS: B PTS: 1 TOP: Additional Questions70. ANS: D PTS: 1 TOP: Additional Questions71. ANS: E PTS: 1 TOP: Valence Shell Electron Pair Repulsion (VSEPR) Theory72. ANS: D PTS: 1 TOP: Polar Molecules: The Influence of Molecular Geometry73. ANS: D PTS: 1 TOP: Valence Bond (VB) Theory74. ANS: A PTS: 1 TOP: Valence Bond (VB) Theory75. ANS: E PTS: 1 TOP: Valence Bond (VB) Theory76. ANS: D PTS: 1 TOP: Trigonal Planar Electronic Geometry77. ANS: D PTS: 1 TOP: Tetrahedral Electronic Geometry: AB4 Species78. ANS: C PTS: 1 TOP: Tetrahedral Electronic Geometry: AB3U Species79. ANS: A PTS: 1 TOP: Tetrahedral Electronic Geometry: AB3U Species80. ANS: C PTS: 1 TOP: Tetrahedral Electronic Geometry: AB3U Species81. ANS: A PTS: 1 TOP: Tetrahedral Electronic Geometry: AB2U2 Species82. ANS: E PTS: 1

TOP: Octahedral Electronic Geometry: AB6, AB5U, and AB4U283. ANS: B PTS: 1 TOP: Compounds Containing Double or Triple Bonds84. ANS: E PTS: 1 TOP: Compounds Containing Triple Bonds85. ANS: A PTS: 1 TOP: Compounds Containing Triple Bonds86. ANS: E PTS: 1 TOP: A Summary of Electronic and Molecular Geometries

87. ANS: C PTS: 1 TOP: A Summary of Electronic and Molecular Geometries88. ANS: C PTS: 1 TOP: Additional Questions89. ANS: E PTS: 1 TOP: Chemical Equations90. ANS: A PTS: 1 TOP: Calculations Based on Chemical Equations91. ANS: B PTS: 1 TOP: Calculations Based on Chemical Equations92. ANS: A PTS: 1 TOP: The Limiting Reactant Concept93. ANS: C PTS: 1 TOP: The Limiting Reactant Concept94. ANS: C PTS: 1 TOP: Percent Yields from Chemical Reactions95. ANS: B PTS: 1 TOP: Percent Yields from Chemical Reactions