Question 1

The iodine atom in I2 would be expected to have a:

Accepted Answer

A) formal charge of 1- 
B) partial charge δ- 
C) partial charge δ+ 
D) formal charge of 0 
A) formal charge of 1- 
B) partial charge δ- 
C) partial charge δ+ 
D) formal charge of 0

Question 2

Which of the following molecules has both an electron group geometry and a molecular geometry described as trigonal planar?

Accepted Answer

A) SiH4  
B) PF3  
C) OF2  
D) CHF3  
E) BF3  
A) SiH4  
B) PF3  
C) OF2  
D) CHF3  
E) BF3

Question 3

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

Accepted Answer

A) True 
 B)False

Question 4

After drawing the Lewis dot structure of CH2CCl2,pick the INCORRECT statement of the following.

Accepted Answer

A) The C-C bond is a double bond. 
B) The H-C bonds are single bonds. 
C) The Cl-C bonds are single bonds. 
D) Each carbon has a lone pair. 
E) Each chlorine has three lone pairs. 
A) The C-C bond is a double bond. 
B) The H-C bonds are single bonds. 
C) The Cl-C bonds are single bonds. 
D) Each carbon has a lone pair. 
E) Each chlorine has three lone pairs.

Question 5

Write a Lewis structure for barium fluoride.

Accepted Answer

A)    
B)  F-Ba-F 
C)    
D)    
E)    
A)    
B)  F-Ba-F 
C)    
D)    
E)

Question 6

In the best Lewis structure for CN-,what is the formal charge on the N atom?

Accepted Answer

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

Question 7

Choose the INCORRECT statement.

Accepted Answer

A) In a Lewis structure,the number of valence electrons shown is one more for each negative charge. 
B) The central atom is typically the atom with the highest electronegativity. 
C) One atom supplies both electrons for a coordinate covalent bond. 
D) Formal charges are apparent charges associated with atoms in a Lewis structure. 
E) Resonance is when more than one plausible structure can be written but the "correct" structure cannot be written. 
A) In a Lewis structure,the number of valence electrons shown is one more for each negative charge. 
B) The central atom is typically the atom with the highest electronegativity. 
C) One atom supplies both electrons for a coordinate covalent bond. 
D) Formal charges are apparent charges associated with atoms in a Lewis structure. 
E) Resonance is when more than one plausible structure can be written but the "correct" structure cannot be written.

Question 8

In a Lewis structure,a terminal atom is bonded to two or more atoms.

Accepted Answer

A) True 
 B)False

Question 9

Which of the following species has a trigonal pyramidal structure?

Accepted Answer

A) ClO3-  
B) ClO4-  
C) ClO2-  
D) ClO2  
A) ClO3-  
B) ClO4-  
C) ClO2-  
D) ClO2

Question 10

Choose the correct statement about the compound SO2.

Accepted Answer

A) The S atom has an unshared electron pair. 
B) The S-O bonds are ionic in character. 
C) The two S-O bonds have different lengths since one is a single bond and the other a double bond. 
D) The molecule has a linear structure. 
E) The O atoms have no unshared electron pairs. 
A) The S atom has an unshared electron pair. 
B) The S-O bonds are ionic in character. 
C) The two S-O bonds have different lengths since one is a single bond and the other a double bond. 
D) The molecule has a linear structure. 
E) The O atoms have no unshared electron pairs.

Question 11

After drawing the Lewis dot structure for XeCl4,determine the number of single bond(s),double bond(s),and lone pair(s)on the central atom.

Accepted Answer

A) single bond(s)= 4,double bond(s)= 0,lone pair(s)= 0 
B) single bond(s)= 4,double bond(s)= 0,lone pair(s)= 2 
C) single bond(s)= 4,double bond(s)= 0,lone pair(s)= 1 
D) single bond(s)= 3,double bond(s)= 1,lone pair(s)= 0 
E) single bond(s)= 1,double bond(s)= 3,lone pair(s)= 0 
A) single bond(s)= 4,double bond(s)= 0,lone pair(s)= 0 
B) single bond(s)= 4,double bond(s)= 0,lone pair(s)= 2 
C) single bond(s)= 4,double bond(s)= 0,lone pair(s)= 1 
D) single bond(s)= 3,double bond(s)= 1,lone pair(s)= 0 
E) single bond(s)= 1,double bond(s)= 3,lone pair(s)= 0

Question 12

Write a Lewis structure for BaO.

Accepted Answer

A)    
B)    
C)    
D)  [Ba-O] 
E)    
A)    
B)    
C)    
D)  [Ba-O] 
E)

Question 13

Which of the following bonds is probably the most polar?

Accepted Answer

A) N-H in NH3  
B) O-H in H2O 
C) P-H in PH3  
D) Se-H in SeH2  
E) C-H in CH4  
A) N-H in NH3  
B) O-H in H2O 
C) P-H in PH3  
D) Se-H in SeH2  
E) C-H in CH4

Question 14

Which of the following species contains a triple bond?

Accepted Answer

A) NH3  
B) HCCl3  
C) NO3-  
D) CO32-  
E) CN-  
A) NH3  
B) HCCl3  
C) NO3-  
D) CO32-  
E) CN-

Question 15

Polar bonds are caused by the bonding pair of electrons being attracted more to one atom than the other.

Accepted Answer

A) True 
 B)False

Question 16

Given the bond enthalpies Cl-Cl (243),C-Cl (339),H-Cl (431),C-H (414)all in kJ/mol,estimate ΔH° for the following reaction: 
CH4(g)+ Cl2(g)→ CH3Cl(g)+ HCl(g).

Accepted Answer

A) -113 kJ/mol 
B) -356 kJ/mol 
C) 301 kJ/mol 
D) -1427 kJ/mol 
E) -30 kJ/mol 
A) -113 kJ/mol 
B) -356 kJ/mol 
C) 301 kJ/mol 
D) -1427 kJ/mol 
E) -30 kJ/mol

Question 17

Which of the following molecules is polar?

Accepted Answer

A) NBr3  
B) CH4  
C) CS2  
D) NH4+  
E) PCl5  
A) NBr3  
B) CH4  
C) CS2  
D) NH4+  
E) PCl5

Question 18

Based on the Lewis structures,which of the following molecules would you expect to exhibit resonance?

Accepted Answer

A) LiH 
B) CH4  
C) HNO2  
D) OF2  
E) none of these 
A) LiH 
B) CH4  
C) HNO2  
D) OF2  
E) none of these

Question 19

Covalent bonds are formed by atoms sharing electrons.

Accepted Answer

A) True 
 B)False

Question 20

After drawing the Lewis dot structure for PCl3,determine the number of single bond(s),double bond(s),and lone pair(s)on the central atom.

Accepted Answer

A) single bond(s)= 2,double bond(s)= 1,lone pair(s)= 1 
B) single bond(s)= 3,double bond(s)= 0,lone pair(s)= 1 
C) single bond(s)= 2,double bond(s)= 0,lone pair(s)= 2 
D) single bond(s)= 3,double bond(s)= 1,lone pair(s)= 0 
E) single bond(s)= 3,double bond(s)= 1,lone pair(s)= 1 
A) single bond(s)= 2,double bond(s)= 1,lone pair(s)= 1 
B) single bond(s)= 3,double bond(s)= 0,lone pair(s)= 1 
C) single bond(s)= 2,double bond(s)= 0,lone pair(s)= 2 
D) single bond(s)= 3,double bond(s)= 1,lone pair(s)= 0 
E) single bond(s)= 3,double bond(s)= 1,lone pair(s)= 1

Exam 10: Chemical Bonding I: Basic Concepts

The iodine atom in I2 would be expected to have a:

Which of the following molecules has both an electron group geometry and a molecular geometry described as trigonal planar?

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

After drawing the Lewis dot structure of CH2CCl2,pick the INCORRECT statement of the following.

Write a Lewis structure for barium fluoride.

In the best Lewis structure for CN-,what is the formal charge on the N atom?

Choose the INCORRECT statement.

In a Lewis structure,a terminal atom is bonded to two or more atoms.

Which of the following species has a trigonal pyramidal structure?

Choose the correct statement about the compound SO2.

After drawing the Lewis dot structure for XeCl4,determine the number of single bond(s),double bond(s),and lone pair(s)on the central atom.

Write a Lewis structure for BaO.

Which of the following bonds is probably the most polar?

Which of the following species contains a triple bond?

Polar bonds are caused by the bonding pair of electrons being attracted more to one atom than the other.

Given the bond enthalpies Cl-Cl (243),C-Cl (339),H-Cl (431),C-H (414)all in kJ/mol,estimate ΔH° for the following reaction: CH4(g)+ Cl2(g)→ CH3Cl(g)+ HCl(g).

Which of the following molecules is polar?

Based on the Lewis structures,which of the following molecules would you expect to exhibit resonance?

Covalent bonds are formed by atoms sharing electrons.

After drawing the Lewis dot structure for PCl3,determine the number of single bond(s),double bond(s),and lone pair(s)on the central atom.

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

The iodine atom in I₂ would be expected to have a:

After drawing the Lewis dot structure of CH₂CCl₂,pick the INCORRECT statement of the following.

In the best Lewis structure for CN^-,what is the formal charge on the N atom?

Choose the correct statement about the compound SO₂.

After drawing the Lewis dot structure for XeCl_4,determine the number of single bond(s),double bond(s),and lone pair(s)on the central atom.

Given the bond enthalpies Cl-Cl (243),C-Cl (339),H-Cl (431),C-H (414)all in kJ/mol,estimate ΔH° for the following reaction: CH₄(g)+ Cl₂(g)→ CH₃Cl(g)+ HCl(g).

After drawing the Lewis dot structure for PCl_3,determine the number of single bond(s),double bond(s),and lone pair(s)on the central atom.