Question 1

Which of the following species has a Lewis structure similar to iodine tetrafluoride, IF4-?

Accepted Answer

A)  XeF4 
B)  SO42- 
C)  PF4+ 
D)  SF4 
E)  IO4- 
A)  XeF4 
B)  SO42- 
C)  PF4+ 
D)  SF4 
E)  IO4-

Question 2

How many hydrogen atoms are needed to complete the following hydrocarbon structure?

Accepted Answer

A)  10 
B)  12 
C)  8 
D)  14 
E)  6 
A)  10 
B)  12 
C)  8 
D)  14 
E)  6

Question 3

Which combination of atoms is most likely to produce a compound with covalent bonds?

Accepted Answer

A)  K and Br 
B)  Al and S 
C)  S and Cl 
D)  Sn and F 
E)  Li and I 
A)  K and Br 
B)  Al and S 
C)  S and Cl 
D)  Sn and F 
E)  Li and I

Question 4

Which of the following is the correct Lewis structure of IF3?

Accepted Answer

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

Question 5

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of nitrogen trichloride, NCl3.

Accepted Answer

A)  The electron-pair geometry is linear, the molecular geometry is linear. 
B)  The electron-pair geometry is trigonal-planar, the molecular geometry is trigonal-planar. 
C)  The electron-pair geometry is trigonal-planar, the molecular geometry is bent. 
D)  The electron-pair geometry is tetrahedral, the molecular geometry is tetrahedral. 
E)  The electron-pair geometry is tetrahedral, the molecular geometry is trigonal-pyramidal. 
A)  The electron-pair geometry is linear, the molecular geometry is linear. 
B)  The electron-pair geometry is trigonal-planar, the molecular geometry is trigonal-planar. 
C)  The electron-pair geometry is trigonal-planar, the molecular geometry is bent. 
D)  The electron-pair geometry is tetrahedral, the molecular geometry is tetrahedral. 
E)  The electron-pair geometry is tetrahedral, the molecular geometry is trigonal-pyramidal.

Question 6

Based on the following data, what is the F-F bond energy? 
${ }^{\frac{1}{2}} \mathrm{H}_{2}(\mathrm{~g})+{ }^{\frac{1}{2}} \mathrm{~F}_{2}(\mathrm{~g}) \rightarrow \mathrm{HF}(\mathrm{g}) ; \Delta_{r} H=-272.5 \mathrm{~kJ} / \mathrm{mol}-\mathrm{rxn}$

$\begin{array}{ll}
Bond &Bond~Energy(kJ/mol)\
\text { H-H } & 435 \
\text { H-F } & 565
\end{array}$

Accepted Answer

A)  500 kJ/mol 
B)  150 kJ/mol 
C)  -150 kJ/mol 
D)  -695 kJ/mol 
E)  695 kJ/mol 
A)  500 kJ/mol 
B)  150 kJ/mol 
C)  -150 kJ/mol 
D)  -695 kJ/mol 
E)  695 kJ/mol

Question 7

Use VSEPR theory to predict the molecular geometry around either carbon atom in acetylene, C2H2.

Accepted Answer

A)  linear 
B)  bent 
C)  trigonal-planar 
D)  tetrahedral 
E)  octahedral 
A)  linear 
B)  bent 
C)  trigonal-planar 
D)  tetrahedral 
E)  octahedral

Question 8

Which of the following is a correct Lewis structure for H2SO4?

Accepted Answer

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

Question 9

Atoms having equal or nearly equal electronegativities are expected to form

Accepted Answer

A)  no bonds 
B)  polar covalent bonds 
C)  nonpolar covalent bonds 
D)  ionic bonds 
E)  covalent bonds 
A)  no bonds 
B)  polar covalent bonds 
C)  nonpolar covalent bonds 
D)  ionic bonds 
E)  covalent bonds

Question 10

What is the bond angle in a trigonal planar molecule or ion?

Accepted Answer

A)  109° 
B)  180° 
C)  90° 
D)  72° 
E)  120° 
A)  109° 
B)  180° 
C)  90° 
D)  72° 
E)  120°

Question 11

How many lone pairs of electrons are assigned to the carbon atom in CO?

Accepted Answer

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

Question 12

Which of the following compounds has polar covalent bonds: CCl4, Cl2, HCl, and KCl?

Accepted Answer

A)  CCl4 only 
B)  Cl2 only 
C)  HCl and KCl 
D)  Cl2 and KCl 
E)  CCl4 and HCl 
A)  CCl4 only 
B)  Cl2 only 
C)  HCl and KCl 
D)  Cl2 and KCl 
E)  CCl4 and HCl

Question 13

The molecular geometry of a molecule whose central atom has four single bonds and one lone pair of electrons is ________.

Accepted Answer

trigonal-b

Question 14

Which of the following pairs of compounds contains ionic bonds?

Accepted Answer

A)  KI and O3 
B)  NaF and H2O 
C)  PCl5 and HF 
D)  Na2SO3 and BH3 
E)  RbBr and MgS 
A)  KI and O3 
B)  NaF and H2O 
C)  PCl5 and HF 
D)  Na2SO3 and BH3 
E)  RbBr and MgS

Question 15

What is the total number of electrons (both lone and bond pairs) in the Lewis structure of SO42-?

Accepted Answer

A)  18 
B)  20 
C)  32 
D)  24 
E)  22 
A)  18 
B)  20 
C)  32 
D)  24 
E)  22

Question 16

The Lewis structure of which of the following molecules violates the octet rule?

Accepted Answer

A)  SF4 
B)  NF3 
C)  OF2 
D)  HF 
E)  SiF4 
A)  SF4 
B)  NF3 
C)  OF2 
D)  HF 
E)  SiF4

Question 17

In benzene, C6H6, the six carbon atoms are arranged in a ring. Two equivalent Lewis structures can be drawn for benzene. In both structures, the carbon atoms have a trigonal planar geometry. These two equivalent structures are referred to as ________ structures.

Accepted Answer

Question 18

Using the following data reactions:$$\begin{array} { l l } 
& \Delta H ^ { \circ } ( \mathrm { kJ } / \text { mol-rxn) } \
\mathrm { H } _ { 2 } ( g ) + \mathrm { Cl } _ { 2 } ( g ) \rightarrow 2 \mathrm { HCl } ( g ) & - 184 \
\mathrm { H } _ { 2 } ( g ) \rightarrow 2 \mathrm { H } ( g ) & 432 \
\mathrm { Cl } _ { 2 } ( g ) \rightarrow 2 \mathrm { Cl } ( g ) & 239
\end{array}$$
Calculate the energy of an H-Cl bond.

Accepted Answer

A)  92 kJ/mol 
B)  855 kJ/mol 
C)  487 kJ/mol 
D)  428 kJ/mol 
E)  244 kJ/mol 
A)  92 kJ/mol 
B)  855 kJ/mol 
C)  487 kJ/mol 
D)  428 kJ/mol 
E)  244 kJ/mol

Question 19

When you draw the Lewis structure for PF2Cl3, how many single bonds, double bonds, and lone pair electrons reside on the central phosphorus atom?

Accepted Answer

A)  5 single bonds, 0 double bonds, 0 lone pairs 
B)  4 single bonds, 1 double bond, 0 lone pairs 
C)  5 single bonds, 0 double bonds, 1 lone pair 
D)  4 single bonds, 1 double bond, 1 lone pair 
E)  3 single bonds, 2 double bonds, 0 lone pairs 
A)  5 single bonds, 0 double bonds, 0 lone pairs 
B)  4 single bonds, 1 double bond, 0 lone pairs 
C)  5 single bonds, 0 double bonds, 1 lone pair 
D)  4 single bonds, 1 double bond, 1 lone pair 
E)  3 single bonds, 2 double bonds, 0 lone pairs

Question 20

Which of the following bonds would be the most polar?

Accepted Answer

A)  N--C 
B)  N--Si 
C)  N--P 
D)  N--Al 
E)  N--Ga 
A)  N--C 
B)  N--Si 
C)  N--P 
D)  N--Al 
E)  N--Ga

Exam 9: Bonding and Molecular Structure

Which of the following species has a Lewis structure similar to iodine tetrafluoride, IF4-?

How many hydrogen atoms are needed to complete the following hydrocarbon structure?

Which combination of atoms is most likely to produce a compound with covalent bonds?

Which of the following is the correct Lewis structure of IF3?

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of nitrogen trichloride, NCl3.

Use VSEPR theory to predict the molecular geometry around either carbon atom in acetylene, C2H2.

Which of the following is a correct Lewis structure for H2SO4?

Atoms having equal or nearly equal electronegativities are expected to form

What is the bond angle in a trigonal planar molecule or ion?

How many lone pairs of electrons are assigned to the carbon atom in CO?

Which of the following compounds has polar covalent bonds: CCl4, Cl2, HCl, and KCl?

The molecular geometry of a molecule whose central atom has four single bonds and one lone pair of electrons is ________.

Which of the following pairs of compounds contains ionic bonds?

What is the total number of electrons (both lone and bond pairs) in the Lewis structure of SO42-?

The Lewis structure of which of the following molecules violates the octet rule?

In benzene, C6H6, the six carbon atoms are arranged in a ring. Two equivalent Lewis structures can be drawn for benzene. In both structures, the carbon atoms have a trigonal planar geometry. These two equivalent structures are referred to as ________ structures.

Using the following data reactions: \Delta(/ mol-rxn) (g)+(g)\rightarrow2(g) -184 (g)\rightarrow2(g) 432 (g)\rightarrow2(g) 239 Calculate the energy of an H-Cl bond.

When you draw the Lewis structure for PF2Cl3, how many single bonds, double bonds, and lone pair electrons reside on the central phosphorus atom?

Which of the following bonds would be the most polar?

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

Which of the following species has a Lewis structure similar to iodine tetrafluoride, IF₄^-?

Which of the following is the correct Lewis structure of IF₃?

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of nitrogen trichloride, NCl₃.

Use VSEPR theory to predict the molecular geometry around either carbon atom in acetylene, C₂H₂.

Which of the following is a correct Lewis structure for H₂SO₄?

Which of the following compounds has polar covalent bonds: CCl₄, Cl₂, HCl, and KCl?

What is the total number of electrons (both lone and bond pairs) in the Lewis structure of SO₄2-?

In benzene, C₆H₆, the six carbon atoms are arranged in a ring. Two equivalent Lewis structures can be drawn for benzene. In both structures, the carbon atoms have a trigonal planar geometry. These two equivalent structures are referred to as ________ structures.

When you draw the Lewis structure for PF₂Cl₃, how many single bonds, double bonds, and lone pair electrons reside on the central phosphorus atom?