Question 1

Using the table of bond dissociation energies, the ΔH for the following gas-phase reaction is ________ kJ.

Accepted Answer

A) 291 
B) 2017 
C) -57 
D) -356 
E) -291 
A) 291 
B) 2017 
C) -57 
D) -356 
E) -291 C

Question 2

Ni2+ ions are represented by the electron configuration ________.

Accepted Answer

A) [Ar]3d8 
B) [Ar]3d10 
C) [Ar]3d6 
D) [Ar]4s23d6 
E) [Kr]4d8 
A) [Ar]3d8 
B) [Ar]3d10 
C) [Ar]3d6 
D) [Ar]4s23d6 
E) [Kr]4d8 A

Question 3

Of the bonds C-C, C   C, and C≡C, the C-C bond is ________.

Accepted Answer

A) strongest/shortest 
B) strongest/longest 
C) weakest/longest 
D) weakest/shortest 
E) intermediate in both strength and length 
A) strongest/shortest 
B) strongest/longest 
C) weakest/longest 
D) weakest/shortest 
E) intermediate in both strength and length C

Question 4

Atoms surrounded by eight valence electrons tend to lose electrons.

Accepted Answer

A) True 
 B)False

Question 5

Based on the octet rule, magnesium most likely forms a ________ ion.

Accepted Answer

A) Mg2+ 
B) Mg2- 
C) Mg6- 
D) Mg6+ 
E) Mg- 
A) Mg2+ 
B) Mg2- 
C) Mg6- 
D) Mg6+ 
E) Mg-

Question 6

The Lewis structure of AsH3 shows ________ nonbonding electron pair(s)on As.

Accepted Answer

A) 0 
B) 1 
C) 2 
D) 3 
E) This cannot be determined from the data given. 
A) 0 
B) 1 
C) 2 
D) 3 
E) This cannot be determined from the data given.

Question 7

In ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion charges _______ and the radii ________.

Accepted Answer

A) increases, decrease, increase 
B) increases, increase, increase 
C) decreases, increase, increase 
D) increases, increase, decrease 
E) increases, decrease, decrease 
A) increases, decrease, increase 
B) increases, increase, increase 
C) decreases, increase, increase 
D) increases, increase, decrease 
E) increases, decrease, decrease

Question 8

The Lewis structure of HCN (H bonded toC)shows that ________ has ________ nonbonding electron pair(s).

Accepted Answer

A) C, 1 
B) N, 1 
C) H, 1 
D) N, 2 
A) C, 1 
B) N, 1 
C) H, 1 
D) N, 2

Question 9

Which of the following does not have eight valence electrons?

Accepted Answer

A) Cl- 
B) Xe 
C) Ti+4 
D) Rb+ 
E) Sr+ 
A) Cl- 
B) Xe 
C) Ti+4 
D) Rb+ 
E) Sr+

Question 10

There are ________ valence electrons in the Lewis structure of CH3Cl.

Accepted Answer

A) 14 
B) 16 
C) 18 
D) 20 
E) 22 
A) 14 
B) 16 
C) 18 
D) 20 
E) 22

Question 11

The strength of a covalent bond is measured by its ________.

Accepted Answer

The answer of The strength of a covalent bond is...

Question 12

The bond length in an HI molecule is 1.61 Å and the measured dipole moment is 0.44 D. What is the magnitude (in units of e)of the negative charge on I in HI? (1 debye = 3.34 × 10-30 coulomb-meters; e = 1.6 × 10-19 coulombs)

Accepted Answer

A) 1.6 × 10-19 
B) 0.057 
C) 9.1 
D) 1 
E) 0.22 
A) 1.6 × 10-19 
B) 0.057 
C) 9.1 
D) 1 
E) 0.22

Question 13

Benzene is a(n)________ compound with ________ equivalent Lewis structures.

Accepted Answer

The answer of Benzene is a(n)________ compound with ________ equivalent...

Question 14

How many hydrogen atoms must bond to silicon to give it an octet of valence electrons?

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 4 
E) 5 
A) 1 
B) 2 
C) 3 
D) 4 
E) 5

Question 15

Give the electron configuration of Cu2+.

Accepted Answer

Question 16

The reaction below is used to produce methanol:
CO (g) + 2H2 (g) → CH3OH (l)△Hrxn = -128 kJ
(a) Calculate the C-H bond energy given the following data:   (b) The tabulated value of the (C-H)bond energy is 413 kJ/mol. Explain why there is a difference between the number you have calculated in (a)and the tabulated value.

Accepted Answer

(a)△H_rxn = D(C≡O)+ 2 D(H-H)- [3 D(C-H)+ D(C

Question 17

The Lewis structure of PF3 shows that the central phosphorus atom has ________ nonbonding and ________ bonding electron pair(s).

Accepted Answer

A) 2, 2 
B) 1, 3 
C) 3, 1 
D) 1, 2 
E) 3, 3 
A) 2, 2 
B) 1, 3 
C) 3, 1 
D) 1, 2 
E) 3, 3

Question 18

A valid Lewis structure of ________ cannot be drawn without violating the octet rule.

Accepted Answer

A) NF3 
B) BeH2 
C) SO2 
D) CF4 
E) SO32- 
A) NF3 
B) BeH2 
C) SO2 
D) CF4 
E) SO32-

Question 19

Using the table of bond dissociation energies, the ΔH for the following reaction is ________ kJ. 2HCl (g) + F2 (g) → 2HF (g) + Cl2 (g)

Accepted Answer

A) -359 
B) -223 
C) 359 
D) 223 
E) 208 
A) -359 
B) -223 
C) 359 
D) 223 
E) 208

Question 20

What is the maximum number of double bonds that a carbon atom can form?

Accepted Answer

A) 4 
B) 1 
C) 0 
D) 2 
E) 3 
A) 4 
B) 1 
C) 0 
D) 2 
E) 3

Exam 8: Basic Concepts of Chemical Bonding

Using the table of bond dissociation energies, the ΔH for the following gas-phase reaction is ________ kJ.

Ni2+ ions are represented by the electron configuration ________.

Of the bonds C-C, C C, and C≡C, the C-C bond is ________.

Atoms surrounded by eight valence electrons tend to lose electrons.

Based on the octet rule, magnesium most likely forms a ________ ion.

The Lewis structure of AsH3 shows ________ nonbonding electron pair(s)on As.

In ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion charges _______ and the radii ________.

The Lewis structure of HCN (H bonded toC)shows that ________ has ________ nonbonding electron pair(s).

Which of the following does not have eight valence electrons?

There are ________ valence electrons in the Lewis structure of CH3Cl.

The strength of a covalent bond is measured by its ________.

The bond length in an HI molecule is 1.61 Å and the measured dipole moment is 0.44 D. What is the magnitude (in units of e)of the negative charge on I in HI? (1 debye = 3.34 × 10-30 coulomb-meters; e = 1.6 × 10-19 coulombs)

Benzene is a(n)________ compound with ________ equivalent Lewis structures.

How many hydrogen atoms must bond to silicon to give it an octet of valence electrons?

Give the electron configuration of Cu2+.

The Lewis structure of PF3 shows that the central phosphorus atom has ________ nonbonding and ________ bonding electron pair(s).

A valid Lewis structure of ________ cannot be drawn without violating the octet rule.

Using the table of bond dissociation energies, the ΔH for the following reaction is ________ kJ. 2HCl (g) + F2 (g) → 2HF (g) + Cl2 (g)

What is the maximum number of double bonds that a carbon atom can form?

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

Ni²⁺ ions are represented by the electron configuration ________.

The Lewis structure of AsH₃ shows ________ nonbonding electron pair(s)on As.

In ionic bond formation, the lattice energy of ions ____ as the magnitude of the ion charges _ and the radii ______.

The Lewis structure of HCN (H bonded toC)shows that has nonbonding electron pair(s).

There are ________ valence electrons in the Lewis structure of CH₃Cl.

The bond length in an HI molecule is 1.61 Å and the measured dipole moment is 0.44 D. What is the magnitude (in units of e)of the negative charge on I in HI? (1 debye = 3.34 × 10^-30 coulomb-meters; e = 1.6 × 10^-19 coulombs)

Benzene is a(n) compound with equivalent Lewis structures.

Give the electron configuration of Cu²⁺.

The Lewis structure of PF₃ shows that the central phosphorus atom has nonbonding and bonding electron pair(s).

Using the table of bond dissociation energies, the ΔH for the following reaction is ________ kJ. 2HCl (g) + F₂ (g) → 2HF (g) + Cl₂ (g)