Question 1

Based on the octet rule, boron will most likely form a ________ ion.

Accepted Answer

A) B3- 
B) B+ 
C) B3+ 
D) B2+ 
E) B2- 
A) B3- 
B) B+ 
C) B3+ 
D) B2+ 
E) B2-

Question 2

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 3

There are ________ valence electrons in the Lewis structure of CH3OCH3.

Accepted Answer

A) 20 
B) 16 
C) 18 
D) 24 
E) 22 
A) 20 
B) 16 
C) 18 
D) 24 
E) 22

Question 4

What is the electron configuration for the Fe2+ ion?

Accepted Answer

A) [Ar]4s03d6 
B) [Ar]4s23d4 
C) [Ar]4s03d8 
D) [Ar]4s23d8 
E) [Ar]4s63d2 
A) [Ar]4s03d6 
B) [Ar]4s23d4 
C) [Ar]4s03d8 
D) [Ar]4s23d8 
E) [Ar]4s63d2

Question 5

How many equivalent resonance structures can be drawn for the molecule of SO3 without having to violate the octet rule on the sulfur atom?

Accepted Answer

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

Question 6

The formal charge on sulfur in SO42- is ________, where the Lewis structure of the ion is:

Accepted Answer

A) -2 
B) 0 
C) +2 
D) +4 
E) -4 
A) -2 
B) 0 
C) +2 
D) +4 
E) -4

Question 7

From the information given below, calculate the heat of combustion of methane. Start by writing the balanced equation.

Accepted Answer

CH₄ + 2O₂ → CO₂ + 2H₂O ΔH_combustion = (4 mol

Question 8

The electron configuration of the phosphide ion (P3-)is ________.

Accepted Answer

A) [Ne]3s2 
B) [Ne]3s23p1 
C) [Ne]3s23p3 
D) [Ne]3p2 
E) [Ne]3s23p6 
A) [Ne]3s2 
B) [Ne]3s23p1 
C) [Ne]3s23p3 
D) [Ne]3p2 
E) [Ne]3s23p6

Question 9

Using the noble gas shorthand notation, write the electron configuration for Fe3+.

Accepted Answer

Question 10

As electronegativity difference increases, bond length will decrease.

Accepted Answer

A) True 
 B)False

Question 11

The ion ICl4- has ________ valence electrons.

Accepted Answer

A) 34 
B) 35 
C) 36 
D) 28 
E) 8 
A) 34 
B) 35 
C) 36 
D) 28 
E) 8

Question 12

The ________ ion is represented by the electron configuration [Ar]3d2.

Accepted Answer

A) Cr4+ 
B) V4+ 
C) Ti4+ 
D) Mn4+ 
E) Sc4+ 
A) Cr4+ 
B) V4+ 
C) Ti4+ 
D) Mn4+ 
E) Sc4+

Question 13

Electron affinity is a measure of how strongly an atom can attract additional electrons.

Accepted Answer

A) True 
 B)False

Question 14

The ________ ion has eight valence electrons.

Accepted Answer

A) Sc3+ 
B) Ti3+ 
C) V3+ 
D) Cr3+ 
E) Mn3+ 
A) Sc3+ 
B) Ti3+ 
C) V3+ 
D) Cr3+ 
E) Mn3+

Question 15

What species has the electron configuration [Ar]3d2?

Accepted Answer

A) Mn2+ 
B) Cr2+ 
C) V3+ 
D) Fe3+ 
E) K+ 
A) Mn2+ 
B) Cr2+ 
C) V3+ 
D) Fe3+ 
E) K+

Question 16

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

Accepted Answer

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

Question 17

For the questions that follow, consider the BEST Lewis structures of the following oxyanions:
(i)NOS1U1B12S1U1B0S1U1P1-S1S1P0 
(ii)NOS1U1B13S1U1B0S1U1P1-S1S1P0 
(iii)SOS1U1B13S1U1B0S1U1P12-S1S1P0 
(iv)SOS1U1B14S1U1B0S1U1P12-S1S1P0 
(v)BrOS1U1B13S1U1B0S1U1P1-S1S1P0
-In which of the ions do all X-O bonds (X indicates the central atom)have the same length?

Accepted Answer

A) none 
B) all 
C) (i)and (ii) 
D) (iii)and (v) 
E) (iii), (iv), and (v) 
A) none 
B) all 
C) (i)and (ii) 
D) (iii)and (v) 
E) (iii), (iv), and (v)

Question 18

There are ________ paired and ________ unpaired electrons in the Lewis symbol for a fluorine atom.

Accepted Answer

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

Question 19

Of the molecules below, the bond in ________ is the most polar.

Accepted Answer

A) HBr 
B) HI 
C) HCl 
D) HF 
E) H2 
A) HBr 
B) HI 
C) HCl 
D) HF 
E) H2

Question 20

How many equivalent resonance forms can be drawn for SO2 without expanding octet on the sulfur atom? (Sulfur is the central atom.)

Accepted Answer

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

Exam 8: Basic Concepts of Chemical Bonding

Based on the octet rule, boron will most likely form a ________ ion.

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

There are ________ valence electrons in the Lewis structure of CH3OCH3.

What is the electron configuration for the Fe2+ ion?

How many equivalent resonance structures can be drawn for the molecule of SO3 without having to violate the octet rule on the sulfur atom?

The formal charge on sulfur in SO42- is ________, where the Lewis structure of the ion is:

From the information given below, calculate the heat of combustion of methane. Start by writing the balanced equation.

The electron configuration of the phosphide ion (P3-)is ________.

Using the noble gas shorthand notation, write the electron configuration for Fe3+.

As electronegativity difference increases, bond length will decrease.

The ion ICl4- has ________ valence electrons.

The ________ ion is represented by the electron configuration [Ar]3d2.

Electron affinity is a measure of how strongly an atom can attract additional electrons.

The ________ ion has eight valence electrons.

What species has the electron configuration [Ar]3d2?

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

For the questions that follow, consider the BEST Lewis structures of the following oxyanions: (i)NO2- (ii)NO3- (iii)SO32- (iv)SO42- (v)BrO3- -In which of the ions do all X-O bonds (X indicates the central atom)have the same length?

There are ________ paired and ________ unpaired electrons in the Lewis symbol for a fluorine atom.

Of the molecules below, the bond in ________ is the most polar.

How many equivalent resonance forms can be drawn for SO2 without expanding octet on the sulfur atom? (Sulfur is the central atom.)

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

There are ________ valence electrons in the Lewis structure of CH₃OCH₃.

What is the electron configuration for the Fe²⁺ ion?

How many equivalent resonance structures can be drawn for the molecule of SO₃ without having to violate the octet rule on the sulfur atom?

The formal charge on sulfur in SO₄^2- is ________, where the Lewis structure of the ion is:

The electron configuration of the phosphide ion (P^3-)is ________.

Using the noble gas shorthand notation, write the electron configuration for Fe³⁺.

The ion ICl₄^- has ________ valence electrons.

The ________ ion is represented by the electron configuration [Ar]3d².

What species has the electron configuration [Ar]3d²?

For the questions that follow, consider the BEST Lewis structures of the following oxyanions: (i)NO₂^- (ii)NO₃^- (iii)SO₃^2- (iv)SO₄^2- (v)BrO₃^- -In which of the ions do all X-O bonds (X indicates the central atom)have the same length?

There are paired and unpaired electrons in the Lewis symbol for a fluorine atom.

How many equivalent resonance forms can be drawn for SO₂ without expanding octet on the sulfur atom? (Sulfur is the central atom.)