Question 1

What is the maximum number of triple 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

Question 2

Alternative but equivalent Lewis structures are called __________.

Accepted Answer

resonance

Question 3

Using the table of average bond energies below, the ΔH for the reaction is __________ kJ. H-C≡C-H (g)+ H-I (g)→ H2C-CHI (g)
Bond: C≡C C=C H-I C-I C-H
D (kJ/mol): 839 614 299 240 413

Accepted Answer

A) +506 
B) -931 
C) -506 
D) -129 
E) +129 
A) +506 
B) -931 
C) -506 
D) -129 
E) +129

Question 4

As electronegativity difference increases, bond length will decrease.

Accepted Answer

A) True 
 B)False

Question 5

The ion NO- has __________ valence electrons.

Accepted Answer

A) 15 
B) 14 
C) 16 
D) 10 
E) 12 
A) 15 
B) 14 
C) 16 
D) 10 
E) 12

Question 6

What is the electron configuration for the Fe3+ ion?

Accepted Answer

A) [Ar]4s13d6 
B) [Ar]4s03d7 
C) [Ar]4s03d5 
D) [Ar]4s23d9 
E) [Ne]3s23p10 
A) [Ar]4s13d6 
B) [Ar]4s03d7 
C) [Ar]4s03d5 
D) [Ar]4s23d9 
E) [Ne]3s23p10

Question 7

Dynamite consists of nitroglycerine mixed with __________.

Accepted Answer

A) potassium nitrate 
B) damp KOH 
C) TNT 
D) diatomaceous earth or cellulose 
E) solid carbon 
A) potassium nitrate 
B) damp KOH 
C) TNT 
D) diatomaceous earth or cellulose 
E) solid carbon

Question 8

Which of the following does not have eight valence electrons?

Accepted Answer

A) Cl- 
B) Xe 
C) Ti+4 
D) Rb+1 
E) Sr+1 
A) Cl- 
B) Xe 
C) Ti+4 
D) Rb+1 
E) Sr+1

Question 9

The electron configuration of the S2- ion is __________.

Accepted Answer

A) [Ar]3s23P6 
B) [Ar]3s23P2 
C) [Ne]3s23P2 
D) [Ne]3s23P6 
E) [Kr]3s23P-6 
A) [Ar]3s23P6 
B) [Ar]3s23P2 
C) [Ne]3s23P2 
D) [Ne]3s23P6 
E) [Kr]3s23P-6

Question 10

The reaction below is used to produce methanol:
CO (g)+ 2H2 (g)→ CH3OH (l)ΔHrxn = -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) ΔH_rxn = D(C≡O)+ 2 D(H-H)- [3 D(C-H)+ D(

Question 11

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

Accepted Answer

A) NF3 
B) IF3 
C) PF3 
D) SbF3 
E) SO42- 
A) NF3 
B) IF3 
C) PF3 
D) SbF3 
E) SO42-

Question 12

Which of the following has eight valence electrons?

Accepted Answer

A) Ti4+ 
B) Kr 
C) Cl- 
D) Na+ 
E) all of the above 
A) Ti4+ 
B) Kr 
C) Cl- 
D) Na+ 
E) all of the above

Question 13

The Lewis structure of the COH32- ion is __________.

Accepted Answer

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

Question 14

Determining lattice energy from Born-Haber cycle data requires the use of __________.

Accepted Answer

A) the octet rule 
B) Coulomb's law 
C) Periodic law 
D) Hess's law 
E) Avogadro's number 
A) the octet rule 
B) Coulomb's law 
C) Periodic law 
D) Hess's law 
E) Avogadro's number

Question 15

The principal quantum number of the electrons that are lost when tungsten forms a cation is __________.

Accepted Answer

A) 6 
B) 5 
C) 4 
D) 3 
E) 2 
A) 6 
B) 5 
C) 4 
D) 3 
E) 2

Question 16

Based on the octet rule, iodine most likely forms an __________ ion.

Accepted Answer

A) I2+ 
B) I4+ 
C) I4- 
D) I+ 
E) I- 
A) I2+ 
B) I4+ 
C) I4- 
D) I+ 
E) I-

Question 17

When a metal gains an electron, the process is endothermic.

Accepted Answer

A) True 
 B)False

Question 18

Fe+2 ions are represented by __________.

Accepted Answer

A) [Ar]3d1 
B) [Ar]3d4 
C) [Ar]3d6 
D) [Ar]3d104s1 
E) [Ar]3d3 
A) [Ar]3d1 
B) [Ar]3d4 
C) [Ar]3d6 
D) [Ar]3d104s1 
E) [Ar]3d3

Question 19

There are __________ valence electrons in the Lewis structure of CH3CH2Cl.

Accepted Answer

A) 14 
B) 12 
C) 18 
D) 20 
E) 10 
A) 14 
B) 12 
C) 18 
D) 20 
E) 10

Question 20

In the Lewis symbol for a sulfur atom, there are __________ paired and __________ unpaired electrons.

Accepted Answer

A) 2, 2 
B) 4, 2 
C) 2, 4 
D) 0, 6 
E) 5, 1 
A) 2, 2 
B) 4, 2 
C) 2, 4 
D) 0, 6 
E) 5, 1

Exam 8: Basic Concepts of Chemical Bonding

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

Alternative but equivalent Lewis structures are called __________.

Using the table of average bond energies below, the ΔH for the reaction is __________ kJ. H-C≡C-H (g)+ H-I (g)→ H2C-CHI (g) Bond: C≡C C=C H-I C-I C-H D (kJ/mol): 839 614 299 240 413

As electronegativity difference increases, bond length will decrease.

The ion NO- has __________ valence electrons.

What is the electron configuration for the Fe3+ ion?

Dynamite consists of nitroglycerine mixed with __________.

Which of the following does not have eight valence electrons?

The electron configuration of the S2- ion is __________.

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

Which of the following has eight valence electrons?

The Lewis structure of the COH32- ion is __________.

Determining lattice energy from Born-Haber cycle data requires the use of __________.

The principal quantum number of the electrons that are lost when tungsten forms a cation is __________.

Based on the octet rule, iodine most likely forms an __________ ion.

When a metal gains an electron, the process is endothermic.

Fe+2 ions are represented by __________.

There are __________ valence electrons in the Lewis structure of CH3CH2Cl.

In the Lewis symbol for a sulfur atom, there are __________ paired and __________ unpaired electrons.

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

Using the table of average bond energies below, the ΔH for the reaction is __________ kJ. H-C≡C-H (g)+ H-I (g)→ H₂C-CHI (g) Bond: C≡C C=C H-I C-I C-H D (kJ/mol): 839 614 299 240 413

The ion NO^- has __________ valence electrons.

What is the electron configuration for the Fe³⁺ ion?

The electron configuration of the S^2- ion is __________.

The Lewis structure of the COH₃2^- ion is __________.

Fe⁺² ions are represented by __________.

There are __________ valence electrons in the Lewis structure of CH₃CH₂Cl.

In the Lewis symbol for a sulfur atom, there are paired and unpaired electrons.