Question 1

In which of the following molecules would you expect the nitrogen-to-nitrogen bond to be the shortest?

Accepted Answer

A) N2H4  
B) N2  
C) N2O4  
D) N2O 
E) NH3  
A) N2H4  
B) N2  
C) N2O4  
D) N2O 
E) NH3

Question 2

Choose the INCORRECT statement.

Accepted Answer

A) Bonds between like atoms are nonpolar bonds. 
B) Polar bonds are caused by the bonding pair of electrons being attracted more to one atom than the other. 
C) Electronegativity is the ability of an atom to attract electrons when involved in a bond. 
D) A difference in electronegativity between two atoms causes a polar bond to be formed. 
E) If the difference in electronegativity between two atoms value is large the bond is polar covalent. 
A) Bonds between like atoms are nonpolar bonds. 
B) Polar bonds are caused by the bonding pair of electrons being attracted more to one atom than the other. 
C) Electronegativity is the ability of an atom to attract electrons when involved in a bond. 
D) A difference in electronegativity between two atoms causes a polar bond to be formed. 
E) If the difference in electronegativity between two atoms value is large the bond is polar covalent.

Question 3

In a Lewis structure,the central atom is typically the atom with the highest electronegativity.

Accepted Answer

A) True 
 B)False

Question 4

What is the formal charge on carbon in the bicarbonate ion HOCO2-?

Accepted Answer

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

Question 5

How many lone pairs are on the Br atom in BrCl2-?

Accepted Answer

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

Question 6

With the representations of "I" for ionic bond,"PC" for polar covalent bond,and "NP" for nonpolar covalent bond,which of the following descriptive combinations is correct?

Accepted Answer

A) CsF/PC 
B) F2/I 
C) NO/NP 
D) HCl/PC 
E) BrCl/NP 
A) CsF/PC 
B) F2/I 
C) NO/NP 
D) HCl/PC 
E) BrCl/NP

Question 7

Given the bond enthalpies C =O (707),O =O (498),H-O (464),and C-H (414)in kJ/mol,compute ΔH° in kJ/mol for: 
CH4(g)+ 2 O2(g)→ CO2(g)+ 2 H2O(g).

Accepted Answer

A) +618 kJ/mol 
B) +259 kJ/mol 
C) -519 kJ/mol 
D) -618 kJ/mol 
E) -259 kJ/mol 
A) +618 kJ/mol 
B) +259 kJ/mol 
C) -519 kJ/mol 
D) -618 kJ/mol 
E) -259 kJ/mol

Question 8

Choose the groups of molecules below in which all the molecules have a net dipole moment.

Accepted Answer

A) SiHCl3,O2,H2O 
B) HF,H2C=CH2,H2O 
C) HF,CH3Cl,H2O 
D) CCl4,HCl,NH3  
E) HF,H2O,N2  
A) SiHCl3,O2,H2O 
B) HF,H2C=CH2,H2O 
C) HF,CH3Cl,H2O 
D) CCl4,HCl,NH3  
E) HF,H2O,N2

Question 9

Which compound would be expected to have the shortest nitrogen-nitrogen bond?

Accepted Answer

A) H2NNH2  
B) HNNH 
C) N2  
D) O2NNO2  
E) (CH3)2NNH2  
A) H2NNH2  
B) HNNH 
C) N2  
D) O2NNO2  
E) (CH3)2NNH2

Question 10

Given the bond enthalpies N-H (389),Cl-Cl (243),N-Cl (201),and H-Cl (431)in kJ/mol,compute ΔH° in kJ/mol for: 
NH3(g)+ Cl2(g)→ NH2Cl + HCl(g).

Accepted Answer

A) -393 kJ/mol 
B) -1100 kJ/mol 
C) +71 kJ/mol 
D) +393 kJ/mol 
E) 0 kJ/mol 
A) -393 kJ/mol 
B) -1100 kJ/mol 
C) +71 kJ/mol 
D) +393 kJ/mol 
E) 0 kJ/mol

Question 11

The phosphorus atom in PCl3 would be expected to have a:

Accepted Answer

A) partial positive (δ+)charge 
B) partial negative (δ-)charge 
C) 3+ formal charge 
D) 3- formal charge 
A) partial positive (δ+)charge 
B) partial negative (δ-)charge 
C) 3+ formal charge 
D) 3- formal charge

Question 12

Which chloride should have the greatest covalent character?

Accepted Answer

A) NaCl 
B) BeCl2  
C) KCl 
D) BaCl2  
E) CaCl2  
A) NaCl 
B) BeCl2  
C) KCl 
D) BaCl2  
E) CaCl2

Question 13

What is the correct molecular geometry for each silicon atom in disilane Si2H6?

Accepted Answer

A) Tetrahedral 
B) Square planar 
C) Octahedral 
D) Linear 
E) Bent 
A) Tetrahedral 
B) Square planar 
C) Octahedral 
D) Linear 
E) Bent

Question 14

As indicated by Lewis structures,which of the following molecules would probably be unstable?

Accepted Answer

A) NH3  
B) N2H6  
C) SF4  
D) CH2F2  
E) SiH4 
A) NH3  
B) N2H6  
C) SF4  
D) CH2F2  
E) SiH4

Question 15

Choose the INCORRECT statement.

Accepted Answer

A) In a Lewis structure,a covalent bond can be represented by a pair of electrons or a dash. 
B) Pairs of electrons not involved in bonding are called lone pairs. 
C) A molecule comprised of two atoms is called a diatomic molecule. 
D) Two electrons involved in a bond produce a double bond. 
E) Three electron pairs involved in a bond produce a triple bond. 
A) In a Lewis structure,a covalent bond can be represented by a pair of electrons or a dash. 
B) Pairs of electrons not involved in bonding are called lone pairs. 
C) A molecule comprised of two atoms is called a diatomic molecule. 
D) Two electrons involved in a bond produce a double bond. 
E) Three electron pairs involved in a bond produce a triple bond.

Question 16

A chemical bond for which one of the bonded atoms provides both electrons for the bond is referred to as a:

Accepted Answer

A) double covalent bond 
B) coordinate covalent bond 
C) formal covalent bond 
D) free radical bond 
E) VSEPR bond 
A) double covalent bond 
B) coordinate covalent bond 
C) formal covalent bond 
D) free radical bond 
E) VSEPR bond

Question 17

Given the listed bond lengths,what would be the most reasonable estimate for the carbon-oxygen bond length in carbon dioxide?
C-C/154 pm C =C/120 pm C-O/143 pm O-O/145 pm O =O/121 pm

Accepted Answer

A) ca.120 pm 
B) ca.130 pm 
C) ca.140 pm 
D) ca.150 pm 
E) > 150 pm 
A) ca.120 pm 
B) ca.130 pm 
C) ca.140 pm 
D) ca.150 pm 
E) > 150 pm

Question 18

Write a Lewis structure for potassium oxide.

Accepted Answer

A)    
B)  K-O 
C)  K-O-K 
D)    
E)    
A)    
B)  K-O 
C)  K-O-K 
D)    
E)

Question 19

The electronegativity is 2.1 for H and 1.9 for Pb.Based on these electronegativities,PbH4 would be expected to:

Accepted Answer

A) be ionic and contain H- ions 
B) be ionic and contain H+ ions 
C) have polar covalent bonds with a partial negative charge on the H atoms 
D) have polar covalent bonds with a partial positive charge on the H atoms 
A) be ionic and contain H- ions 
B) be ionic and contain H+ ions 
C) have polar covalent bonds with a partial negative charge on the H atoms 
D) have polar covalent bonds with a partial positive charge on the H atoms

Question 20

Which of the following exhibits covalent bonding?

Accepted Answer

A) NaF 
B) SrO 
C) LiH 
D) OF2  
E) K2S 
A) NaF 
B) SrO 
C) LiH 
D) OF2  
E) K2S

Exam 10: Chemical Bonding I: Basic Concepts

In which of the following molecules would you expect the nitrogen-to-nitrogen bond to be the shortest?

Choose the INCORRECT statement.

In a Lewis structure,the central atom is typically the atom with the highest electronegativity.

What is the formal charge on carbon in the bicarbonate ion HOCO2-?

How many lone pairs are on the Br atom in BrCl2-?

With the representations of "I" for ionic bond,"PC" for polar covalent bond,and "NP" for nonpolar covalent bond,which of the following descriptive combinations is correct?

Given the bond enthalpies C =O (707),O =O (498),H-O (464),and C-H (414)in kJ/mol,compute ΔH° in kJ/mol for: CH4(g)+ 2 O2(g)→ CO2(g)+ 2 H2O(g).

Choose the groups of molecules below in which all the molecules have a net dipole moment.

Which compound would be expected to have the shortest nitrogen-nitrogen bond?

Given the bond enthalpies N-H (389),Cl-Cl (243),N-Cl (201),and H-Cl (431)in kJ/mol,compute ΔH° in kJ/mol for: NH3(g)+ Cl2(g)→ NH2Cl + HCl(g).

The phosphorus atom in PCl3 would be expected to have a:

Which chloride should have the greatest covalent character?

What is the correct molecular geometry for each silicon atom in disilane Si2H6?

As indicated by Lewis structures,which of the following molecules would probably be unstable?

Choose the INCORRECT statement.

A chemical bond for which one of the bonded atoms provides both electrons for the bond is referred to as a:

Given the listed bond lengths,what would be the most reasonable estimate for the carbon-oxygen bond length in carbon dioxide? C-C/154 pm C =C/120 pm C-O/143 pm O-O/145 pm O =O/121 pm

Write a Lewis structure for potassium oxide.

The electronegativity is 2.1 for H and 1.9 for Pb.Based on these electronegativities,PbH4 would be expected to:

Which of the following exhibits covalent bonding?

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Intermolecular Forces: Liquids and Solids

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acidbase Equilibria

Solubility and Complex-Ion Equilibria

Electrochemistry

Chemical Kinetics

Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

What is the formal charge on carbon in the bicarbonate ion HOCO₂^-?

How many lone pairs are on the Br atom in BrCl₂^-?

Given the bond enthalpies C =O (707),O =O (498),H-O (464),and C-H (414)in kJ/mol,compute ΔH° in kJ/mol for: CH₄(g)+ 2 O₂(g)→ CO₂(g)+ 2 H₂O(g).

Given the bond enthalpies N-H (389),Cl-Cl (243),N-Cl (201),and H-Cl (431)in kJ/mol,compute ΔH° in kJ/mol for: NH₃(g)+ Cl₂(g)→ NH₂Cl + HCl(g).

The phosphorus atom in PCl₃ would be expected to have a:

What is the correct molecular geometry for each silicon atom in disilane Si₂H₆?

The electronegativity is 2.1 for H and 1.9 for Pb.Based on these electronegativities,PbH₄ would be expected to: