Question 1

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.F) A) and E)
G) A) and B)

Question 2

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

Accepted Answer

A) True 
 B)False

Question 3

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

Accepted Answer

A) True 
 B)False

Question 4

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.F) A) and E)
G) C) and D)

Question 5

Which of the following contains covalent bonds?

Accepted Answer

A)   BaO
B)   IBr
C)   Mg
D)   LiBr
E)   CuF) B) and C)
G) A) and D)

Question 6

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.F) D) and E)
G) C) and D)

Question 7

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.F) A) and D)
G) B) and C)

Question 8

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 9

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)   S8F) A) and B)
G) C) and E)

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)   C6H10O3F) A) and E)
G) A) and B)

Question 11

Select the element whose Lewis symbol is correct.

Accepted Answer

A)   
B)   
C)   
D)   
E)   F) C) and E)
G) A) and B)

Question 12

Select the strongest bond in the following group.

Accepted Answer

A)   C-S
B)   C-O
C)   C=C
D)   C≡N
E)   C-FF) D) and E)
G) A) and B)

Question 13

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

Accepted Answer

A)   NO2
B)   CO2
C)   H2O
D)   HF
E)   NH3F) A) and E)
G) A) and C)

Question 14

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 15

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.F) C) and D)
G) B) and C)

Question 16

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 moltenF) A) and D)
G) B) and E)

Question 17

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 kJF) C) and E)
G) A) and C)

Question 18

Which of the following elements is the most electronegative?

Accepted Answer

A)   S
B)   Ru
C)   Si
D)   Te
E)   CsF) A) and B)
G) B) and D)

Question 19

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

Accepted Answer

A) True 
 B)False

Question 20

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 pmF) A) and D)
G) B) and D)

Exam 9: Models of Chemical Bonding

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

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Which of the following elements is the most electronegative?

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

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

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

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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

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

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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?

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

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

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Which of the following contains covalent bonds?

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

Correct AnswerverifiedShow Answer

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

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

Correct AnswerverifiedShow Answer

Electronegativity is a measure of

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Select the strongest bond in the following group.

Correct AnswerverifiedShow Answer

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

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

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Select the element whose Lewis symbol is correct.

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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

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

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