Question 1

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

Accepted Answer

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

Question 2

Polyatomic ions with an even number of electrons will follow the ________ rule.

Accepted Answer

The answer of Polyatomic ions with an even number of...

Question 3

A nonpolar bond will form between two ________ atoms of ________ electronegativity.

Accepted Answer

A) different, opposite 
B) identical, different 
C) different, different 
D) similar, different 
E) identical, equal 
A) different, opposite 
B) identical, different 
C) different, different 
D) similar, different 
E) identical, equal

Question 4

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 5

There are ________ unpaired electrons in the Lewis symbol for an oxygen atom .

Accepted Answer

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

Question 6

Lattice energy is ________.

Accepted Answer

A) the energy required to convert a mole of ionic solid into its constituent ions in the gas phase 
B) the energy given off when gaseous ions combine to form one mole of an ionic solid 
C) the energy required to produce one mole of an ionic compound from its constituent elements in their standard states 
D) the sum of ionization energies of the components in an ionic solid 
E) the sum of electron affinities of the components in an ionic solid 
A) the energy required to convert a mole of ionic solid into its constituent ions in the gas phase 
B) the energy given off when gaseous ions combine to form one mole of an ionic solid 
C) the energy required to produce one mole of an ionic compound from its constituent elements in their standard states 
D) the sum of ionization energies of the components in an ionic solid 
E) the sum of electron affinities of the components in an ionic solid

Question 7

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 8

How many different types of resonance structures can be drawn for the ion SO32-?

Accepted Answer

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

Question 9

Which two bonds are most similar in polarity?

Accepted Answer

A) O-F and Cl-F 
B) B-F and Cl-F 
C) Al-Cl and I-Br 
D) I-Br and Si-Cl 
E) C-Cl and Be-Cl 
A) O-F and Cl-F 
B) B-F and Cl-F 
C) Al-Cl and I-Br 
D) I-Br and Si-Cl 
E) C-Cl and Be-Cl

Question 10

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 11

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 12

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 13

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 14

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

Accepted Answer

A) two, three 
B) one, three 
C) three, two 
D) zero, five 
E) two, two 
A) two, three 
B) one, three 
C) three, two 
D) zero, five 
E) two, two

Question 15

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 16

The Lewis structure of the CO32- ion is ________.

Accepted Answer

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

Question 17

What is the electron configuration for the Cu2+ ion?

Accepted Answer

A) [Ar]4sS1U1P10S1S1P03dS1U1P110S1S1P0 
B) [Ar]4sS1U1P10S1S1P03dS1U1P110S1S1P0. 
C) [Ar]4sS1U1P10S1S1P03dS1U1P19S1S1P0 
D) [Ar]4sS1U1P12S1S1P03dS1U1P19S1S1P0. 
E) [Ar]4sS1U1P10S1S1P03dS1U1P111S1S1P0 
A) [Ar]4sS1U1P10S1S1P03dS1U1P110S1S1P0 
B) [Ar]4sS1U1P10S1S1P03dS1U1P110S1S1P0. 
C) [Ar]4sS1U1P10S1S1P03dS1U1P19S1S1P0 
D) [Ar]4sS1U1P12S1S1P03dS1U1P19S1S1P0. 
E) [Ar]4sS1U1P10S1S1P03dS1U1P111S1S1P0

Question 18

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

Accepted Answer

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

Question 19

Which of the following noble gas electron configurations represents the Ru+ cation?

Accepted Answer

A) [Kr]5s24d5 
B) [Kr]5s24d7 
C) [Kr]4d5 
D) [Ar]4s13d6 
E) [Kr]5s14d6 
A) [Kr]5s24d5 
B) [Kr]5s24d7 
C) [Kr]4d5 
D) [Ar]4s13d6 
E) [Kr]5s14d6

Question 20

A positive change in bond enthalpy is required to break a bond.

Accepted Answer

A) True 
 B)False

Exam 8: Basic Concepts of Chemical Bonding

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

Polyatomic ions with an even number of electrons will follow the ________ rule.

A nonpolar bond will form between two ________ atoms of ________ electronegativity.

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

There are ________ unpaired electrons in the Lewis symbol for an oxygen atom .

Lattice energy is ________.

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

How many different types of resonance structures can be drawn for the ion SO32-?

Which two bonds are most similar in polarity?

Of the atoms below,________ is the most electronegative.

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

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

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

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

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

The Lewis structure of the CO32- ion is ________.

What is the electron configuration for the Cu2+ ion?

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

Which of the following noble gas electron configurations represents the Ru+ cation?

A positive change in bond enthalpy is required to break a bond.

Introduction: Matter, energy, and Measurement

Atoms, molecules, and Ions

Chemical Reactions and Reaction Stoichiometry

Reactions in Aqueous Solution

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

A nonpolar bond will form between two atoms of electronegativity.

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

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

How many different types of resonance structures can be drawn for the ion SO₃^2-?

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

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

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

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

The Lewis structure of the CO₃^2- ion is ________.

What is the electron configuration for the Cu²⁺ ion?

Which of the following noble gas electron configurations represents the Ru⁺ cation?