Question 1

A double covalent bond contains ________ of electrons.

Accepted Answer

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

Question 2

Choose the bond below that is most polar.

Accepted Answer

A) H-I 
B) H-Br 
C) H-F 
D) H-Cl 
E) C-H 
A) H-I 
B) H-Br 
C) H-F 
D) H-Cl 
E) C-H

Question 3

Place the following in order of increasing bond length. 
C-F $\quad$C-S $\quad$C-Cl

Accepted Answer

A) C-S < C-Cl < C-F 
B) C-Cl < C-F < C-S 
C) C-F < C-S < C-Cl 
D) C-F < C-Cl < C-S 
E) C-S < C-F < C-Cl 
A) C-S < C-Cl < C-F 
B) C-Cl < C-F < C-S 
C) C-F < C-S < C-Cl 
D) C-F < C-Cl < C-S 
E) C-S < C-F < C-Cl

Question 4

Use the bond energies provided to estimate ΔrH° for the reaction below. PCl3(g)+ Cl2(g)→ PCl5(l)ΔrH° = ?
Bond $\quad$$\quad$Bond Energy (kJ mol-1)
Cl-Cl $\quad$$\quad$$\quad$$\quad$243
P-Cl $\quad$$\quad$$\quad$$\quad$ 331

Accepted Answer

A) -243 kJ mol-1 
B) -419 kJ mol-1 
C) -662 kJ mol-1 
D) -67 kJ mol-1 
E) -905 kJ mol-1 
A) -243 kJ mol-1 
B) -419 kJ mol-1 
C) -662 kJ mol-1 
D) -67 kJ mol-1 
E) -905 kJ mol-1

Question 5

Draw the best Lewis structure for BrO4-.What is the formal charge on bromine?

Accepted Answer

A) -1 
B) +1 
C) 0 
D) +2 
E) +3 
A) -1 
B) +1 
C) 0 
D) +2 
E) +3

Question 6

Place the following in order of increasing bond length. 
NO2- $\quad$NO3- $\quad$NO

Accepted Answer

A) NO 2- 3- 
B) NO2- 3- 3- 2- 
D) NO 3- 2- 
E) NO3- 2- < NO 
A) NO 2- 3- 
B) NO2- 3- 3- 2- 
D) NO 3- 2- 
E) NO3- 2- < NO

Question 7

Choose the best Lewis structure for XeI2.

Accepted Answer

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

Question 8

Draw the best Lewis structure for Cl3-.What is the formal charge on the central Cl atom?

Accepted Answer

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

Question 9

Of the following elements,which has the lowest electronegativity?

Accepted Answer

A) Sr 
B) I 
C) Ba 
D) At 
A) Sr 
B) I 
C) Ba 
D) At

Question 10

Place the following in order of decreasing magnitude of lattice energy. 
K2O$\quad$ Rb2S $\quad$Li2O

Accepted Answer

A) Li2O > K2O > Rb2S 
B) Li2O > Rb2S > K2O 
C) Rb2S > K2O > Li2O 
D) Rb2S > Li2O > K2O 
E) K2O > Li2O > Rb2S 
A) Li2O > K2O > Rb2S 
B) Li2O > Rb2S > K2O 
C) Rb2S > K2O > Li2O 
D) Rb2S > Li2O > K2O 
E) K2O > Li2O > Rb2S

Question 11

Which molecule or compound below contains an ionic bond?

Accepted Answer

A) CO2 
B) C2Br4 
C) SCl2 
D) OCl2 
E) NH4NO3 
A) CO2 
B) C2Br4 
C) SCl2 
D) OCl2 
E) NH4NO3

Question 12

Which of the following statements is TRUE?

Accepted Answer

A) A covalent bond is formed through the transfer of electrons from one atom to another. 
B) A pair of electrons involved in a covalent bond are sometimes referred to as "lone pairs." 
C) It is not possible for two atoms to share more than two electrons. 
D) Single bonds are shorter than double bonds. 
E) A covalent bond has a lower potential energy than the two separate atoms. 
A) A covalent bond is formed through the transfer of electrons from one atom to another. 
B) A pair of electrons involved in a covalent bond are sometimes referred to as "lone pairs." 
C) It is not possible for two atoms to share more than two electrons. 
D) Single bonds are shorter than double bonds. 
E) A covalent bond has a lower potential energy than the two separate atoms.

Question 13

Draw the Lewis structure for CO32-,including any valid resonance structures.Which of the following statements is TRUE?

Accepted Answer

A) The CO32- ion contains one C-O single bond and two C=O double bonds. 
B) The CO32- ion contains three C-O bonds that are equivalent to 4/3 bonds. 
C) The CO32- ion contains three C-O double bonds. 
D) The CO32- ion contains two C-O single bonds and one C≡O triple bond. 
E) None of the above is true. 
A) The CO32- ion contains one C-O single bond and two C=O double bonds. 
B) The CO32- ion contains three C-O bonds that are equivalent to 4/3 bonds. 
C) The CO32- ion contains three C-O double bonds. 
D) The CO32- ion contains two C-O single bonds and one C≡O triple bond. 
E) None of the above is true.

Question 14

Use Lewis theory to determine the chemical formula for the compound formed between Mg and Br.

Accepted Answer

A) MgBr 
B) Mg2Br3 
C) Mg3Br2 
D) MgBr2 
E) Mg2Br 
A) MgBr 
B) Mg2Br3 
C) Mg3Br2 
D) MgBr2 
E) Mg2Br

Question 15

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

Question 16

Which of the following represent the Lewis structure for S2-?

Accepted Answer

A)    
B)  $\mathrm { S } ^ { 2 - }$ 
C)    
D)    
E)  $S : ^ { 2 - }$ 
A)    
B)  $\mathrm { S } ^ { 2 - }$ 
C)    
D)    
E)  $S : ^ { 2 - }$

Question 17

Choose the best Lewis structure for PO43-.

Accepted Answer

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

Question 18

Identify the number of bonding pairs and lone pairs of electrons in water.

Accepted Answer

A) 1 bonding pair and 1 lone pair 
B) 1 bonding pair and 2 lone pairs 
C) 2 bonding pairs and 2 lone pairs 
D) 2 bonding pairs and 1 lone pair 
E) 3 bonding pairs and 2 lone pairs 
A) 1 bonding pair and 1 lone pair 
B) 1 bonding pair and 2 lone pairs 
C) 2 bonding pairs and 2 lone pairs 
D) 2 bonding pairs and 1 lone pair 
E) 3 bonding pairs and 2 lone pairs

Question 19

Use the data given below to construct a Born-Haber cycle to determine the bond energy of O2.
$$\begin{array} { l r } 
& \Delta H ^ { \circ } \left( \mathrm { kJ } \mathrm { mol } ^ { - 1 } \right) \
\mathrm { Na } ( s ) \rightarrow \mathrm { Na } ( g ) & 107 \
\mathrm { Na } ( g ) \rightarrow \mathrm { Na } ^ { + } ( g ) + \mathrm { e } ^ { - } & 496 \
\mathrm { O } ( g ) + \mathrm { e } ^ { - } \rightarrow \mathrm { O } ^ { - } ( g ) & - 141 \
\mathrm { O } ^ { - } ( g ) + \mathrm { e } ^ { - } \rightarrow \mathrm { O } ^ { 2 - } ( g ) & 878 \
2 \mathrm { Na } ( s ) + \frac { 1 } { 2 } \mathrm { O } 2 ( g ) \rightarrow \mathrm { Na } 2 \mathrm { O } ( s ) & - 416 \
2 \mathrm { Na } ^ { + } ( g ) + \mathrm { O } ^ { 2 - } ( g ) \rightarrow \mathrm { Na } 2 \mathrm { O } ( s ) & - 2608
\end{array}$$

Accepted Answer

A) 426 kJ mol-1 
B) 249 kJ mol-1 
C) 852 kJ mol-1 
D) 498 kJ mol-1 
E) 356 kJ mol-1 
A) 426 kJ mol-1 
B) 249 kJ mol-1 
C) 852 kJ mol-1 
D) 498 kJ mol-1 
E) 356 kJ mol-1

Question 20

Draw the best Lewis structure for the free radical NO2.What is the formal charge on the N?

Accepted Answer

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

Exam 9: Chemical Bonding I: Lewis Theory

A double covalent bond contains ________ of electrons.

Choose the bond below that is most polar.

Place the following in order of increasing bond length. C-F \quad C-S \quad C-Cl

Use the bond energies provided to estimate ΔrH° for the reaction below. PCl3(g)+ Cl2(g)→ PCl5(l)ΔrH° = ? Bond \quad\quad Bond Energy (kJ mol-1) Cl-Cl \quad\quad\quad\quad 243 P-Cl \quad\quad\quad\quad 331

Draw the best Lewis structure for BrO4-.What is the formal charge on bromine?

Place the following in order of increasing bond length. NO2- \quad NO3- \quad NO

Choose the best Lewis structure for XeI2.

Draw the best Lewis structure for Cl3-.What is the formal charge on the central Cl atom?

Of the following elements,which has the lowest electronegativity?

Place the following in order of decreasing magnitude of lattice energy. K2O \quad Rb2S \quad Li2O

Which molecule or compound below contains an ionic bond?

Which of the following statements is TRUE?

Draw the Lewis structure for CO32-,including any valid resonance structures.Which of the following statements is TRUE?

Use Lewis theory to determine the chemical formula for the compound formed between Mg and Br.

The phosphorus atom in PCl3 would be expected to have a

Which of the following represent the Lewis structure for S2-?

Choose the best Lewis structure for PO43-.

Identify the number of bonding pairs and lone pairs of electrons in water.

Use the data given below to construct a Born-Haber cycle to determine the bond energy of O2. \Delta (s)\rightarrow(g) 107 (g)\rightarrow(g)+ 496 (g)+\rightarrow(g) -141 (g)+\rightarrow(g) 878 2(s)+2(g)\rightarrow2(s) -416 2(g)+(g)\rightarrow2(s) -2608

Draw the best Lewis structure for the free radical NO2.What is the formal charge on the N?

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules,compounds,and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding II: Molecular Shapes, valence Bond Theory, and Molecular Orbital Theory

Liquids, solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Place the following in order of increasing bond length. C-F $\quad$ C-S $\quad$ C-Cl

Use the bond energies provided to estimate Δ_rH° for the reaction below. PCl₃(g)+ Cl₂(g)→ PCl₅(l)Δ_rH°= ? Bond $\quad$ $\quad$ Bond Energy (kJ mol^-1) Cl-Cl $\quad$ $\quad$ $\quad$ $\quad$ 243 P-Cl $\quad$ $\quad$ $\quad$ $\quad$ 331

Draw the best Lewis structure for BrO₄^-.What is the formal charge on bromine?

Place the following in order of increasing bond length. NO₂^- $\quad$ NO₃^- $\quad$ NO

Choose the best Lewis structure for XeI₂.

Draw the best Lewis structure for Cl₃^-.What is the formal charge on the central Cl atom?

Place the following in order of decreasing magnitude of lattice energy. K₂O $\quad$ Rb₂S $\quad$ Li₂O

Draw the Lewis structure for CO₃²^-,including any valid resonance structures.Which of the following statements is TRUE?

The phosphorus atom in PCl₃ would be expected to have a

Which of the following represent the Lewis structure for S²^-?

Choose the best Lewis structure for PO₄³^-.

Use the data given below to construct a Born-Haber cycle to determine the bond energy of O₂. \Delta (s)\rightarrow(g) 107 (g)\rightarrow(g)+ 496 (g)+\rightarrow(g) -141 (g)+\rightarrow(g) 878 2(s)+2(g)\rightarrow2(s) -416 2(g)+(g)\rightarrow2(s) -2608

Draw the best Lewis structure for the free radical NO₂.What is the formal charge on the N?