Question 1

In compounds of __________ and __________, the octet rule is violated due to the presence of fewer than eight valence electrons.

Accepted Answer

The answer of In compounds of __________ and __________, the...

Question 2

A double 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 3

In a reaction, if the bonds in the reactants are stronger than the bonds in the product, the reaction is __________.

Accepted Answer

The answer of In a reaction, if the bonds in...

Question 4

Which of the following does not have eight valence electrons?

Accepted Answer

A) Ca+ 
B) Rb+ 
C) Xe 
D) Br- 
E) All of the above have eight valence electrons. 
A) Ca+ 
B) Rb+ 
C) Xe 
D) Br- 
E) All of the above have eight valence electrons.

Question 5

How many single covalent bonds must a chlorine atom form to have a complete octet in its valence shell?

Accepted Answer

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

Question 6

Bond enthalpy is __________.

Accepted Answer

A) always positive 
B) always negative 
C) sometimes positive, sometimes negative 
D) always zero 
E) unpredictable 
A) always positive 
B) always negative 
C) sometimes positive, sometimes negative 
D) always zero 
E) unpredictable

Question 7

The electron configuration [Kr]4d10 represents __________.

Accepted Answer

A) Sr+2 
B) Sn+2 
C) Te+2 
D) Ag+1 
E) Rb+1 
A) Sr+2 
B) Sn+2 
C) Te+2 
D) Ag+1 
E) Rb+1

Question 8

Using the Born-Haber cycle, the ΔHf° of KBr is equal to __________.

Accepted Answer

A) ΔHf°[K (g)] + ΔHf°[Br (g)] + Il(K)+ E(Br)+ ΔHlattice 
B) ΔHf°[K (g)] - ΔHf°[Br (g)] - Il(K)- E(Br)- ΔHlattice 
C) ΔHf°[K (g)] - ΔHf°[Br (g)] + Il(K)- E(Br)+ ΔHlattice 
D) ΔHf°[K (g)] + ΔHf°[Br (g)] - Il - E(Br)+ ΔHlattice 
E) ΔHf°[K (g)] + ΔHf°[Br (g)] + Il(K)+ E(Br)- ΔHlattice 
A) ΔHf°[K (g)] + ΔHf°[Br (g)] + Il(K)+ E(Br)+ ΔHlattice 
B) ΔHf°[K (g)] - ΔHf°[Br (g)] - Il(K)- E(Br)- ΔHlattice 
C) ΔHf°[K (g)] - ΔHf°[Br (g)] + Il(K)- E(Br)+ ΔHlattice 
D) ΔHf°[K (g)] + ΔHf°[Br (g)] - Il - E(Br)+ ΔHlattice 
E) ΔHf°[K (g)] + ΔHf°[Br (g)] + Il(K)+ E(Br)- ΔHlattice

Question 9

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 10

The chloride of which of the following metals should have the greatest lattice energy?

Accepted Answer

A) potassium 
B) rubidium 
C) sodium 
D) lithium 
E) cesium 
A) potassium 
B) rubidium 
C) sodium 
D) lithium 
E) cesium

Question 11

Draw the Lewis structure of ICl2+.

Accepted Answer

Question 12

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

Accepted Answer

A) [Ne]3s2 
B) [Ne]3s23Pl 
C) [Ne]3s23P4 
D) [Ne]3P2 
E) [Ne]3s23P6 
A) [Ne]3s2 
B) [Ne]3s23Pl 
C) [Ne]3s23P4 
D) [Ne]3P2 
E) [Ne]3s23P6

Question 13

Of the possible bonds between carbon atoms (single, double, and triple), __________.

Accepted Answer

A) a triple bond is longer than a single bond 
B) a double bond is stronger than a triple bond 
C) a single bond is stronger than a triple bond 
D) a double bond is longer than a triple bond 
E) a single bond is stronger than a double bond 
A) a triple bond is longer than a single bond 
B) a double bond is stronger than a triple bond 
C) a single bond is stronger than a triple bond 
D) a double bond is longer than a triple bond 
E) a single bond is stronger than a double bond

Question 14

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-C H3 
A) H2C-CH2 
B) H-C≡C-H 
C) H3C-CH3 
D) H2C-C-CH2 
E) H3C-CH2-C H3

Question 15

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 16

Atoms surrounded by eight valence electrons tend to lose electrons.

Accepted Answer

A) True 
 B)False

Question 17

The halogens, alkali metals, and alkaline earth metals have __________ valence electrons, respectively.

Accepted Answer

A) 7, 4, and 6 
B) 1, 5, and 7 
C) 8, 2, and 3 
D) 7, 1, and 2 
E) 2, 7, and 4 
A) 7, 4, and 6 
B) 1, 5, and 7 
C) 8, 2, and 3 
D) 7, 1, and 2 
E) 2, 7, and 4

Question 18

Of the atoms below, __________ is the most electropositive.

Accepted Answer

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

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

A __________ covalent bond between the same two atoms is the longest.

Accepted Answer

A) single 
B) double 
C) triple 
D) They are all the same length. 
E) strong 
A) single 
B) double 
C) triple 
D) They are all the same length. 
E) strong

Exam 8: Basic Concepts of Chemical Bonding

In compounds of __________ and __________, the octet rule is violated due to the presence of fewer than eight valence electrons.

A double bond consists of __________ pairs of electrons shared between two atoms.

In a reaction, if the bonds in the reactants are stronger than the bonds in the product, the reaction is __________.

Which of the following does not have eight valence electrons?

How many single covalent bonds must a chlorine atom form to have a complete octet in its valence shell?

Bond enthalpy is __________.

The electron configuration [Kr]4d10 represents __________.

Using the Born-Haber cycle, the ΔHf° of KBr is equal to __________.

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

The chloride of which of the following metals should have the greatest lattice energy?

Draw the Lewis structure of ICl2+.

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

Of the possible bonds between carbon atoms (single, double, and triple), __________.

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

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

Atoms surrounded by eight valence electrons tend to lose electrons.

The halogens, alkali metals, and alkaline earth metals have __________ valence electrons, respectively.

Of the atoms below, __________ is the most electropositive.

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

A __________ covalent bond between the same two atoms is the longest.

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

In compounds of and , the octet rule is violated due to the presence of fewer than eight valence electrons.

The electron configuration [Kr]4d¹⁰ represents __________.

Using the Born-Haber cycle, the ΔH_f° of KBr is equal to __________.

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

Draw the Lewis structure of ICl₂⁺.

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

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