Question 1

The stronger the bonds in a fuel, the more energy it will yield.

Accepted Answer

A) True 
 B)False

Question 2

As a measure of the strength of metallic bonding, the boiling point of a metal is a better indicator than its melting point.

Accepted Answer

A) True 
 B)False

Question 3

Select the strongest bond in the following group.

Accepted Answer

A)  C-S 
B)  C-O 
C)  C=C 
D)  C≡N 
E)  C-F 
A)  C-S 
B)  C-O 
C)  C=C 
D)  C≡N 
E)  C-F

Question 4

Bond energy increases as bond order increases, for bonding between a given pair of atoms.

Accepted Answer

A) True 
 B)False

Question 5

Hydrogenation of double and triple bonds is an important industrial process. Calculate (in kJ) the standard enthalpy change ΔH° for the hydrogenation of ethyne (acetylene) to ethane. H-C≡C-H(g) + 2H2(g) → H3C-CH3(g)
Bond: C-C C≡C C-H H-H
Bond energy (kJ/mol): 347 839 413 432

Accepted Answer

A)  -296 kJ 
B)  -51 kJ 
C)  51 kJ 
D)  296 kJ 
E)  381 kJ 
A)  -296 kJ 
B)  -51 kJ 
C)  51 kJ 
D)  296 kJ 
E)  381 kJ

Question 6

A single covalent bond consists of a single delocalized electron pair.

Accepted Answer

A) True 
 B)False

Question 7

Which of the following contains covalent bonds?

Accepted Answer

A)  BaO 
B)  IBr 
C)  Mg 
D)  LiBr 
E)  Cu 
A)  BaO 
B)  IBr 
C)  Mg 
D)  LiBr 
E)  Cu

Question 8

Combustion of a fat will release more energy than combustion of an equal mass of carbohydrate because

Accepted Answer

A)  fats contain more bonds to oxygen than carbohydrates. 
B)  fats contain fewer bonds to oxygen than carbohydrates. 
C)  the total energy of the carbon-carbon and carbon-hydrogen bonds in fats is greater than the energy content of the carbon-oxygen and oxygen-hydrogen bonds in the reaction products (carbon dioxide and water). 
D)  the total energy of the carbon-carbon and carbon-hydrogen bonds in fats is greater than the energy content of the bonds in carbohydrates. 
E)  fats have higher molar masses than carbohydrates. 
A)  fats contain more bonds to oxygen than carbohydrates. 
B)  fats contain fewer bonds to oxygen than carbohydrates. 
C)  the total energy of the carbon-carbon and carbon-hydrogen bonds in fats is greater than the energy content of the carbon-oxygen and oxygen-hydrogen bonds in the reaction products (carbon dioxide and water). 
D)  the total energy of the carbon-carbon and carbon-hydrogen bonds in fats is greater than the energy content of the bonds in carbohydrates. 
E)  fats have higher molar masses than carbohydrates.

Question 9

The lattice energy of CaF2 is the energy change for which one, if any, of the following processes?

Accepted Answer

A)  Ca2+(s) + 2F-(g) → CaF2(g) 
B)  CaF2(g) → CaF2(s) 
C)  Ca(g) + 2F(g) → CaF2(s) 
D)  CaF2(aq) → CaF2(s) 
E)  None of these choices are correct. 
A)  Ca2+(s) + 2F-(g) → CaF2(g) 
B)  CaF2(g) → CaF2(s) 
C)  Ca(g) + 2F(g) → CaF2(s) 
D)  CaF2(aq) → CaF2(s) 
E)  None of these choices are correct.

Question 10

When one mole of each of the following liquids is burned, which will produce the most heat energy?

Accepted Answer

A)  C6H14 
B)  C5H12 
C)  C6H14O 
D)  C6H12O 
E)  C6H10O3 
A)  C6H14 
B)  C5H12 
C)  C6H14O 
D)  C6H12O 
E)  C6H10O3

Question 11

Select the element whose Lewis symbol is correct.

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 12

In which of these substances are the atoms held together by polar covalent bonding?

Accepted Answer

A)  SrCl2 
B)  CsCl 
C)  ClF 
D)  TiF2 
E)  S8 
A)  SrCl2 
B)  CsCl 
C)  ClF 
D)  TiF2 
E)  S8

Question 13

Which one of the following properties is least characteristic of substances composed of small, covalently-bonded molecules?

Accepted Answer

A)  low melting point 
B)  low boiling point 
C)  weak bonds 
D)  poor electrical conductor when solid 
E)  poor electrical conductor when molten 
A)  low melting point 
B)  low boiling point 
C)  weak bonds 
D)  poor electrical conductor when solid 
E)  poor electrical conductor when molten

Question 14

A Born-Haber cycle applied to the formation reaction of an ionic solid

Accepted Answer

A)  is normally used to calculate ionization energy. 
B)  is normally used to calculate electron affinity. 
C)  is normally used to calculate bond energy. 
D)  is normally used to determine the overall enthalpy change. 
E)  is an application of Hess's Law. 
A)  is normally used to calculate ionization energy. 
B)  is normally used to calculate electron affinity. 
C)  is normally used to calculate bond energy. 
D)  is normally used to determine the overall enthalpy change. 
E)  is an application of Hess's Law.

Question 15

Electronegativity is a measure of

Accepted Answer

A)  the energy needed to remove an electron from an atom. 
B)  the energy released when an electron is added to an atom. 
C)  the magnitude of the negative charge on an electron. 
D)  the attraction by an atom for electrons in a chemical bond. 
E)  the magnitude of the negative charge on a molecule. 
A)  the energy needed to remove an electron from an atom. 
B)  the energy released when an electron is added to an atom. 
C)  the magnitude of the negative charge on an electron. 
D)  the attraction by an atom for electrons in a chemical bond. 
E)  the magnitude of the negative charge on a molecule.

Question 16

The lattice energy is the energy released when separated ions in the gas phase combine to form ionic molecules in the gas phase.

Accepted Answer

A) True 
 B)False

Question 17

Arrange calcium, rubidium, sulfur, and arsenic in order of decreasing electronegativity.

Accepted Answer

A)  S > As > Rb > Ca 
B)  S > As > Ca > Rb 
C)  As > S > Rb > Ca 
D)  As > S > Ca > Rb 
E)  None of these choices are correct. 
A)  S > As > Rb > Ca 
B)  S > As > Ca > Rb 
C)  As > S > Rb > Ca 
D)  As > S > Ca > Rb 
E)  None of these choices are correct.

Question 18

Which of the following elements is the most electronegative?

Accepted Answer

A)  S 
B)  Ru 
C)  Si 
D)  Te 
E)  Cs 
A)  S 
B)  Ru 
C)  Si 
D)  Te 
E)  Cs

Question 19

The diameter of a chloride ion is 362 pm, and the diameter of a potassium ion is 276 pm. What is the distance between the nuclei of adjacent chloride and potassium ions in solid potassium chloride?

Accepted Answer

A)  1276 pm 
B)  638 pm 
C)  319 pm 
D)  181 pm 
E)  138 pm 
A)  1276 pm 
B)  638 pm 
C)  319 pm 
D)  181 pm 
E)  138 pm

Question 20

Which of the following compounds displays the greatest ionic character in its bonds?

Accepted Answer

A)  NO2 
B)  CO2 
C)  H2O 
D)  HF 
E)  NH3 
A)  NO2 
B)  CO2 
C)  H2O 
D)  HF 
E)  NH3

Exam 9: Models of Chemical Bonding

The stronger the bonds in a fuel, the more energy it will yield.

As a measure of the strength of metallic bonding, the boiling point of a metal is a better indicator than its melting point.

Select the strongest bond in the following group.

Bond energy increases as bond order increases, for bonding between a given pair of atoms.

Hydrogenation of double and triple bonds is an important industrial process. Calculate (in kJ) the standard enthalpy change ΔH° for the hydrogenation of ethyne (acetylene) to ethane. H-C≡C-H(g) + 2H2(g) → H3C-CH3(g) Bond: C-C C≡C C-H H-H Bond energy (kJ/mol): 347 839 413 432

A single covalent bond consists of a single delocalized electron pair.

Which of the following contains covalent bonds?

Combustion of a fat will release more energy than combustion of an equal mass of carbohydrate because

The lattice energy of CaF2 is the energy change for which one, if any, of the following processes?

When one mole of each of the following liquids is burned, which will produce the most heat energy?

Select the element whose Lewis symbol is correct.

In which of these substances are the atoms held together by polar covalent bonding?

Which one of the following properties is least characteristic of substances composed of small, covalently-bonded molecules?

A Born-Haber cycle applied to the formation reaction of an ionic solid

Electronegativity is a measure of

The lattice energy is the energy released when separated ions in the gas phase combine to form ionic molecules in the gas phase.

Arrange calcium, rubidium, sulfur, and arsenic in order of decreasing electronegativity.

Which of the following elements is the most electronegative?

The diameter of a chloride ion is 362 pm, and the diameter of a potassium ion is 276 pm. What is the distance between the nuclei of adjacent chloride and potassium ions in solid potassium chloride?

Which of the following compounds displays the greatest ionic character in its bonds?

Keys to Studying Chemistry Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces Liquids, Solids, and Phase Changes

The Properties of Mixtures Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics Rates and Mechanisms of Chemical Reactions

Equilibrium the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics Entropy, Free Energy, and Reaction Direction

Electrochemistry Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Hydrogenation of double and triple bonds is an important industrial process. Calculate (in kJ) the standard enthalpy change ΔH° for the hydrogenation of ethyne (acetylene) to ethane. H-C≡C-H(g) + 2H₂(g) → H₃C-CH₃(g) Bond: C-C C≡C C-H H-H Bond energy (kJ/mol): 347 839 413 432

The lattice energy of CaF₂ is the energy change for which one, if any, of the following processes?