Question 1

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 2

Draw the Lewis structure of ICl2+.

Accepted Answer

Question 3

The most electronegative atom of the ones listed below is ________.

Accepted Answer

A) B 
B) Al 
C) Ga 
D) In 
E) Tl 
A) B 
B) Al 
C) Ga 
D) In 
E) Tl

Question 4

The electron configuration of the P3- ion is ________.

Accepted Answer

A) [Ar]3s23p6 
B) [Ar]3s23p2 
C) [Ne]3s23p6 
D) [Ne]3s23p2 
E) [Kr]3s22p6 
A) [Ar]3s23p6 
B) [Ar]3s23p2 
C) [Ne]3s23p6 
D) [Ne]3s23p2 
E) [Kr]3s22p6

Question 5

A triple bond consists of ________ pairs of electrons shared between two atoms.

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 4 
E) 6 
A) 1 
B) 2 
C) 3 
D) 4 
E) 6

Question 6

Which of the following has the bonds correctly arranged in order of increasing polarity?

Accepted Answer

A) Be-F, Mg-F, N-F, O-F 
B) O-F, N-F, Be-F, Mg-F 
C) O-F, Be-F, Mg-F, N-F 
D) N-F, Be-F, Mg-F, O-F 
E) Mg-F, Be-F, N-F, O-F 
A) Be-F, Mg-F, N-F, O-F 
B) O-F, N-F, Be-F, Mg-F 
C) O-F, Be-F, Mg-F, N-F 
D) N-F, Be-F, Mg-F, O-F 
E) Mg-F, Be-F, N-F, O-F

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

Of the bonds below, ________ is the least polar.

Accepted Answer

A) C-O 
B) N-O 
C) C-F 
D) S-O 
E) K-Br 
A) C-O 
B) N-O 
C) C-F 
D) S-O 
E) K-Br

Question 9

The oxidation number of phosphorus in PF5 is ________.

Accepted Answer

A) +5 
B) +3 
C) +1 
D) -5 
E) 0 
A) +5 
B) +3 
C) +1 
D) -5 
E) 0

Question 10

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

Accepted Answer

A) P3+ 
B) P3- 
C) P5+ 
D) P5- 
E) P+ 
A) P3+ 
B) P3- 
C) P5+ 
D) P5- 
E) P+

Question 11

Of the atoms below, ________ is the most electronegative.

Accepted Answer

A) Ba 
B) Sr 
C) Ca 
D) Mg 
E) Be 
A) Ba 
B) Sr 
C) Ca 
D) Mg 
E) Be

Question 12

How many different types of resonance structures can be drawn for the ion SO32- where all atoms satisfy the octet rule?

Accepted Answer

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

Question 13

The electron configuration of the sulfide ion (S2-)is ________.

Accepted Answer

A) [Ne]3s2 
B) [Ne]3s23p1 
C) [Ne]3s23p4 
D) [Ne]3p2 
E) [Ne]3s23p6 
A) [Ne]3s2 
B) [Ne]3s23p1 
C) [Ne]3s23p4 
D) [Ne]3p2 
E) [Ne]3s23p6

Question 14

Using the Born-Haber cycle, the ΔH°f of KBr is equal to ________.

Accepted Answer

A) ΔH°f [K (g)] + ΔH°f [Br (g)] + I1(K) + E(Br) + ΔHlattice 
B) ΔH°f [K (g)] - ΔH°f [Br (g)] - I1(K) - E(Br) - ΔHlattice 
C) ΔH°f [K (g)] - ΔH°f [Br (g)] + I1(K) - E(Br) + ΔHlattice 
D) ΔH°f [K (g)] + ΔH°f [Br (g)] - I1 - E(Br) + ΔHlattice 
E) ΔH°f [K (g)] + ΔH°f [Br (g)] + I1(K) + E(Br) - ΔHlattice 
A) ΔH°f [K (g)] + ΔH°f [Br (g)] + I1(K) + E(Br) + ΔHlattice 
B) ΔH°f [K (g)] - ΔH°f [Br (g)] - I1(K) - E(Br) - ΔHlattice 
C) ΔH°f [K (g)] - ΔH°f [Br (g)] + I1(K) - E(Br) + ΔHlattice 
D) ΔH°f [K (g)] + ΔH°f [Br (g)] - I1 - E(Br) + ΔHlattice 
E) ΔH°f [K (g)] + ΔH°f [Br (g)] + I1(K) + E(Br) - ΔHlattice

Question 15

Electronegativity ________ from left to right within a period and ________ from top to bottom within a group.

Accepted Answer

A) decreases, increases 
B) increases, increases 
C) increases, decreases 
D) stays the same, increases 
E) increases, stays the same 
A) decreases, increases 
B) increases, increases 
C) increases, decreases 
D) stays the same, increases 
E) increases, stays the same

Question 16

The electron configuration of the S2- ion is ________.

Accepted Answer

A) [Ar]3s23p6 
B) [Ar]3s23p2 
C) [Ne]3s23p2 
D) [Ne]3s23p6 
E) [Kr]3s22p6 
A) [Ar]3s23p6 
B) [Ar]3s23p2 
C) [Ne]3s23p2 
D) [Ne]3s23p6 
E) [Kr]3s22p6

Question 17

In the resonance form of ozone shown below, the formal charge on the central oxygen atom is ________.

Accepted Answer

A) 0 
B) +1 
C) -1 
D) +2 
E) -2 
A) 0 
B) +1 
C) -1 
D) +2 
E) -2

Question 18

Given that the average bond energies for C-H and C-Br bonds are 413 and 276 kJ/mol, respectively, the heat of atomization of bromoform (CHBr3)is ________ kJ/mol.

Accepted Answer

A) 1241 
B) 689 
C) -689 
D) 1378 
E) -1378 
A) 1241 
B) 689 
C) -689 
D) 1378 
E) -1378

Question 19

In the Lewis structure of ClF, the formal charge on Cl is ________, and the formal charge on F is ________.

Accepted Answer

A) -1, -1 
B) 0, 0 
C) 0, -1 
D) +1, -1 
E) -1, +1 
A) -1, -1 
B) 0, 0 
C) 0, -1 
D) +1, -1 
E) -1, +1

Question 20

In which of the molecules below is the carbon-carbon distance the shortest?

Accepted Answer

A) H2C   CH2 
B) H-C≡C-H 
C) H3C-CH3 
D) H2C   C   CH2 
E) H3C-CH2-CH3 
A) H2C   CH2 
B) H-C≡C-H 
C) H3C-CH3 
D) H2C   C   CH2 
E) H3C-CH2-CH3

Exam 8: Basic Concepts of Chemical Bonding

Which of the following has eight valence electrons?

Draw the Lewis structure of ICl2+.

The most electronegative atom of the ones listed below is ________.

The electron configuration of the P3- ion is ________.

A triple bond consists of ________ pairs of electrons shared between two atoms.

Which of the following has the bonds correctly arranged in order of increasing polarity?

Dynamite consists of nitroglycerine mixed with ________.

Of the bonds below, ________ is the least polar.

The oxidation number of phosphorus in PF5 is ________.

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

Of the atoms below, ________ is the most electronegative.

How many different types of resonance structures can be drawn for the ion SO32- where all atoms satisfy the octet rule?

The electron configuration of the sulfide ion (S2-)is ________.

Using the Born-Haber cycle, the ΔH°f of KBr is equal to ________.

Electronegativity ________ from left to right within a period and ________ from top to bottom within a group.

The electron configuration of the S2- ion is ________.

In the resonance form of ozone shown below, the formal charge on the central oxygen atom is ________.

Given that the average bond energies for C-H and C-Br bonds are 413 and 276 kJ/mol, respectively, the heat of atomization of bromoform (CHBr3)is ________ kJ/mol.

In the Lewis structure of ClF, the formal charge on Cl is ________, and the formal charge on F is ________.

In which of the molecules below is the carbon-carbon distance the shortest?

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

Draw the Lewis structure of ICl₂⁺.

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

The oxidation number of phosphorus in PF₅ is ________.

How many different types of resonance structures can be drawn for the ion SO₃^2- where all atoms satisfy the octet rule?

The electron configuration of the sulfide ion (S^2-)is ________.

Using the Born-Haber cycle, the ΔH°_f of KBr is equal to ________.

Electronegativity from left to right within a period and from top to bottom within a group.

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

Given that the average bond energies for C-H and C-Br bonds are 413 and 276 kJ/mol, respectively, the heat of atomization of bromoform (CHBr₃)is ________ kJ/mol.

In the Lewis structure of ClF, the formal charge on Cl is , and the formal charge on F is .