Question 1

The lattice energy of large ions is greater in magnitude than that of small ions of the same charge.

Accepted Answer

A) True 
 B)False  False

Question 2

Using the bond energies provided below, calculate ΔH° for the reaction CH4(g) + 4Cl2(g) → CCl4(g) + 4HCl(g)
Bond energies: C-H = 413 kJ/mol, Cl-Cl = 243 kJ/mol, C-Cl = 339 kJ/mol, H-Cl = 427 kJ/mol

Accepted Answer

A) 1422 kJ 
B) 440 kJ 
C) 110 kJ 
D) −110 kJ 
E) −440 kJ 
A) 1422 kJ 
B) 440 kJ 
C) 110 kJ 
D) −110 kJ 
E) −440 kJ E

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 D

Question 4

Select the compound with the lowest (i.e., least negative) lattice energy.

Accepted Answer

A) CsBr( s) 
B) NaCl( s) 
C) SrO( s) 
D) CaO( s) 
E) KBr( s) 
A) CsBr( s) 
B) NaCl( s) 
C) SrO( s) 
D) CaO( s) 
E) KBr( s)

Question 5

In covalent bond formation, the potential energy reaches a maximum when the internuclear distance is equal to the bond length.

Accepted Answer

A) True 
 B)False

Question 6

Select the most polar bond amongst the following.

Accepted Answer

A) C-O 
B) Si-F 
C) Cl-F 
D) C-F 
E) C-I 
A) C-O 
B) Si-F 
C) Cl-F 
D) C-F 
E) C-I

Question 7

Which one of the following properties is least characteristic of typical metals?

Accepted Answer

A) Moderately high melting point 
B) High boiling point 
C) Brittleness 
D) Good electrical conductor when solid 
E) Good electrical conductor when molten 
A) Moderately high melting point 
B) High boiling point 
C) Brittleness 
D) Good electrical conductor when solid 
E) Good electrical conductor when molten

Question 8

Which of the following contains ionic bonding?

Accepted Answer

A) CO 
B) SrF 2 
C) Al 
D) OCl 2 
E) HCl 
A) CO 
B) SrF 2 
C) Al 
D) OCl 2 
E) HCl

Question 9

Select the compound with the highest lattice energy.

Accepted Answer

A) CaS( s) 
B) BaO( s) 
C) NaI( s) 
D) LiBr( s) 
E) MgO( s) 
A) CaS( s) 
B) BaO( s) 
C) NaI( s) 
D) LiBr( s) 
E) MgO( s)

Question 10

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

Accepted Answer

A) CO 2 
B) Si 
C) Br 2 
D) S 8 
E) Cr 
A) CO 2 
B) Si 
C) Br 2 
D) S 8 
E) Cr

Question 11

Acetone can be easily converted to isopropyl alcohol by addition of hydrogen to the carbon-oxygen double bond. Calculate the enthalpy of reaction using the bond energies given.

Accepted Answer

A) −484 kJ 
B) −366 kJ 
C) −61 kJ 
D) +61 kJ 
E) +366 kJ 
A) −484 kJ 
B) −366 kJ 
C) −61 kJ 
D) +61 kJ 
E) +366 kJ

Question 12

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

Accepted Answer

A) NO 2 
B) CO 2 
C) H 2O 
D) HF 
E) NH 3 
A) NO 2 
B) CO 2 
C) H 2O 
D) HF 
E) NH 3

Question 13

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

Accepted Answer

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

Question 14

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 15

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

Accepted Answer

A) C 6H 14 
B) C 5H 12 
C) C 6H 14O 
D) C 6H 12O 
E) C 6H 10O 3 
A) C 6H 14 
B) C 5H 12 
C) C 6H 14O 
D) C 6H 12O 
E) C 6H 10O 3

Question 16

Which of the following is a covalent compound?

Accepted Answer

A) Na 2O 
B) CaCl 2 
C) Cl 2O 
D) CsCl 
E) Al 2O 3 
A) Na 2O 
B) CaCl 2 
C) Cl 2O 
D) CsCl 
E) Al 2O 3

Question 17

Which of the following elements is the most electronegative?

Accepted Answer

A) Ne 
B) Rb 
C) P 
D) I 
E) Cl 
A) Ne 
B) Rb 
C) P 
D) I 
E) Cl

Question 18

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

Accepted Answer

A) True 
 B)False

Question 19

The lattice energy for ionic crystals increases as the charge on the ions __________ and the size of the ions __________.

Accepted Answer

A) increases; increases 
B) increases; decreases 
C) decreases; increases 
D) decreases; decreases 
E) None of these choices are correct. 
A) increases; increases 
B) increases; decreases 
C) decreases; increases 
D) decreases; decreases 
E) None of these choices are correct.

Question 20

Which of the following is an ionic compound?

Accepted Answer

A) H 2S 
B) NH 3 
C) I 2 
D) KI 
E) CCl 4 
A) H 2S 
B) NH 3 
C) I 2 
D) KI 
E) CCl 4

Exam 9: Models of Chemical Bonding

The lattice energy of large ions is greater in magnitude than that of small ions of the same charge.

Using the bond energies provided below, calculate ΔH° for the reaction CH4(g) + 4Cl2(g) → CCl4(g) + 4HCl(g) Bond energies: C-H = 413 kJ/mol, Cl-Cl = 243 kJ/mol, C-Cl = 339 kJ/mol, H-Cl = 427 kJ/mol

Select the strongest bond in the following group.

Select the compound with the lowest (i.e., least negative) lattice energy.

In covalent bond formation, the potential energy reaches a maximum when the internuclear distance is equal to the bond length.

Select the most polar bond amongst the following.

Which one of the following properties is least characteristic of typical metals?

Which of the following contains ionic bonding?

Select the compound with the highest lattice energy.

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

Acetone can be easily converted to isopropyl alcohol by addition of hydrogen to the carbon-oxygen double bond. Calculate the enthalpy of reaction using the bond energies given.

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

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

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

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

Which of the following is a covalent compound?

Which of the following elements is the most electronegative?

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

The lattice energy for ionic crystals increases as the charge on the ions __________ and the size of the ions __________.

Which of the following is an ionic compound?

Keys to the Study of 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

Using the bond energies provided below, calculate ΔH° for the reaction CH₄(g) + 4Cl₂(g) → CCl₄(g) + 4HCl(g) Bond energies: C-H = 413 kJ/mol, Cl-Cl = 243 kJ/mol, C-Cl = 339 kJ/mol, H-Cl = 427 kJ/mol

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

The lattice energy for ionic crystals increases as the charge on the ions and the size of the ions .