Question 1

The covalent bond with the greatest polarity would form in which of the atom pairs below

Accepted Answer

A)  Br - Br 
B)  S - O 
C)  C - P 
D)  C - O 
E)  B - O 
A)  Br - Br 
B)  S - O 
C)  C - P 
D)  C - O 
E)  B - O

Question 2

The azide ion, N3-, is very reactive although it is isoelectronic with the very stable CO2 molecule. This reactivity is reasonable considering that

Accepted Answer

A)  a Lewis structure cannot be written for the azide ion that has nitrogen formal charges of zero. 
B)  there is no valid Lewis structure possible for the azide ion. 
C)  there are resonance structures for azide ion but not for carbon dioxide. 
D)  nitrogen cannot form multiple bonds. 
E)  charged species always decompose in solution. 
A)  a Lewis structure cannot be written for the azide ion that has nitrogen formal charges of zero. 
B)  there is no valid Lewis structure possible for the azide ion. 
C)  there are resonance structures for azide ion but not for carbon dioxide. 
D)  nitrogen cannot form multiple bonds. 
E)  charged species always decompose in solution.

Question 3

Arrange the following bonds in order of increasing ionic character: 
H - Cl
C - H
H - H
O - H

Accepted Answer

A)  H - Cl < C - H < H - H < O - H 
B)  H - H < C - H < O - H < H - Cl 
C)  H - H < C - H < H - Cl < O - H 
D)  C - H < O - H < H - Cl < H - H 
E)  C - H < H - Cl < O - H < H - H 
A)  H - Cl < C - H < H - H < O - H 
B)  H - H < C - H < O - H < H - Cl 
C)  H - H < C - H < H - Cl < O - H 
D)  C - H < O - H < H - Cl < H - H 
E)  C - H < H - Cl < O - H < H - H

Question 4

Which one of the following compounds does not follow the octet rule

Accepted Answer

A)  NF3 
B)  CF4 
C)  PF5 
D)  AsH3 
E)  HCl 
A)  NF3 
B)  CF4 
C)  PF5 
D)  AsH3 
E)  HCl

Question 5

Which of the elements listed below would most likely form a nonpolar covalent bond when bonded to bromine

Accepted Answer

A)  Rb 
B)  Br 
C)  C 
D)  O 
E)  H 
A)  Rb 
B)  Br 
C)  C 
D)  O 
E)  H

Question 6

List all types of bonding present in the compound NH4NO3.
I. ionic bond 
II. polar covalent bond
III. nonpolar covalent bond

Accepted Answer

A)  I only 
B)  II only 
C)  III only 
D)  I and II 
E)  II and III 
A)  I only 
B)  II only 
C)  III only 
D)  I and II 
E)  II and III

Question 7

List all types of bonding present in the ion SO42-.
I. ionic bond 
II. polar covalent bond
III. nonpolar covalent bond

Accepted Answer

A)  I only 
B)  II only 
C)  III only 
D)  I and II 
E)  II and III 
A)  I only 
B)  II only 
C)  III only 
D)  I and II 
E)  II and III

Question 8

Use the bond enthalpy data given to estimate the heat released when 6.50 g of nitrogen gas reacts with excess hydrogen gas to form ammonia at 25$\circ$C.
BE(N$\equiv$N) = 941.4 kJ/mol 
BE(H-H) = 436.4 kJ/mol
BE(N-H) = 393 kJ/mol

Accepted Answer

A)  340 kJ 
B)  228 kJ 
C)  107 kJ 
D)  46.1 kJ 
E)  24.9 kJ 
A)  340 kJ 
B)  228 kJ 
C)  107 kJ 
D)  46.1 kJ 
E)  24.9 kJ

Question 9

Estimate the enthalpy change for the combustion of one mole of acetylene, C2H2, to form carbon dioxide and water vapor.
BE(C-H) = 456 kJ/mol 
BE(C$\equiv$C) = 962 kJ/mol
BE(O=O) = 499 kJ/mol
BE(C=O) = 802 kJ/mol
BE(O-H) = 462 kJ/mol

Accepted Answer

A)  +1010 kJ/mol 
B)  +653 kJ/mol 
C)  -155 kJ/mol 
D)  -1010 kJ/mol 
E)  -1759 kJ/mol 
A)  +1010 kJ/mol 
B)  +653 kJ/mol 
C)  -155 kJ/mol 
D)  -1010 kJ/mol 
E)  -1759 kJ/mol

Question 10

The ion O22- shows both ionic and covalent bonding.

Accepted Answer

A) True 
 B)False

Question 11

The number of lone electron pairs in the NH4+ ion is ___.

Accepted Answer

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

Question 12

The total number of valence electrons in the molecule CO2 is

Accepted Answer

A)  4. 
B)  10. 
C)  14. 
D)  16. 
E)  20. 
A)  4. 
B)  10. 
C)  14. 
D)  16. 
E)  20.

Question 13

The formal charge on the sulfur atom in the resonance structure of sulfur dioxide which has one single bond and one double bond is

Accepted Answer

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

Question 14

Which of the following substances will display an incomplete octet in its Lewis structure

Accepted Answer

A)  CO2 
B)  Cl2 
C)  ICl 
D)  NO 
E)  SO2 
A)  CO2 
B)  Cl2 
C)  ICl 
D)  NO 
E)  SO2

Question 15

Calculate the energy required for the gas phase process represented by Na(g) + Br(g) $\rarr$ Na+(g) + Br- (g). 
Given: Ionization energy (Na) = 496 kJ/mol
Electron affinity (Br) = 324 kJ/mol
Electron affinity (Na) = 53 kJ/mol

Accepted Answer

A)  152 kJ/mol 
B)  162 kJ/mol 
C)  172 kJ/mol 
D)  182 kJ/mol 
E)  None of the above 
A)  152 kJ/mol 
B)  162 kJ/mol 
C)  172 kJ/mol 
D)  182 kJ/mol 
E)  None of the above

Question 16

Examine this Lewis structure for the phosphate ion, PO43-. How many valence electrons are around the P atom in this structure

Accepted Answer

A)  Eight 
B)  Four 
C)  Twelve 
D)  Nine 
E)  None of the above 
A)  Eight 
B)  Four 
C)  Twelve 
D)  Nine 
E)  None of the above

Question 17

Which of the elements listed below would most likely form an ionic bond when bonded to chlorine

Accepted Answer

A)  H 
B)  Br 
C)  O 
D)  Sr 
E)  N 
A)  H 
B)  Br 
C)  O 
D)  Sr 
E)  N

Question 18

The Lewis structure for CS2 is:

Accepted Answer

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

Question 19

What type of chemical bond holds the atoms together within a water molecule

Accepted Answer

A)  Ionic bond 
B)  Nonpolar covalent bond 
C)  Polar covalent bond 
D)  Coordinate covalent bond 
A)  Ionic bond 
B)  Nonpolar covalent bond 
C)  Polar covalent bond 
D)  Coordinate covalent bond

Question 20

Of the following substances, KCl, KBr, and KF, KF will have the highest melting point.

Accepted Answer

A) True 
 B)False

Exam 9: Chemical Bonding I: Basic Concepts

The covalent bond with the greatest polarity would form in which of the atom pairs below

The azide ion, N3-, is very reactive although it is isoelectronic with the very stable CO2 molecule. This reactivity is reasonable considering that

Arrange the following bonds in order of increasing ionic character: H - Cl C - H H - H O - H

Which one of the following compounds does not follow the octet rule

Which of the elements listed below would most likely form a nonpolar covalent bond when bonded to bromine

List all types of bonding present in the compound NH4NO3. I. ionic bond II. polar covalent bond III. nonpolar covalent bond

List all types of bonding present in the ion SO42-. I. ionic bond II. polar covalent bond III. nonpolar covalent bond

Use the bond enthalpy data given to estimate the heat released when 6.50 g of nitrogen gas reacts with excess hydrogen gas to form ammonia at 25 ∘\circ∘ C. BE(N ≡\equiv≡ N) = 941.4 kJ/mol BE(H-H) = 436.4 kJ/mol BE(N-H) = 393 kJ/mol

Estimate the enthalpy change for the combustion of one mole of acetylene, C2H2, to form carbon dioxide and water vapor. BE(C-H) = 456 kJ/mol BE(C ≡\equiv≡ C) = 962 kJ/mol BE(O=O) = 499 kJ/mol BE(C=O) = 802 kJ/mol BE(O-H) = 462 kJ/mol

The ion O22- shows both ionic and covalent bonding.

The number of lone electron pairs in the NH4+ ion is ___.

The total number of valence electrons in the molecule CO2 is

The formal charge on the sulfur atom in the resonance structure of sulfur dioxide which has one single bond and one double bond is

Which of the following substances will display an incomplete octet in its Lewis structure

Calculate the energy required for the gas phase process represented by Na(g) + Br(g) →\rarr→ Na+(g) + Br- (g). Given: Ionization energy (Na) = 496 kJ/mol Electron affinity (Br) = 324 kJ/mol Electron affinity (Na) = 53 kJ/mol

Examine this Lewis structure for the phosphate ion, PO43-. How many valence electrons are around the P atom in this structure

Which of the elements listed below would most likely form an ionic bond when bonded to chlorine

The Lewis structure for CS2 is:

What type of chemical bond holds the atoms together within a water molecule

Of the following substances, KCl, KBr, and KF, KF will have the highest melting point.

Chemistry: The Study of Change

Atoms Molecules and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

Organic Chemistry

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Filters

The azide ion, N₃^-, is very reactive although it is isoelectronic with the very stable CO₂ molecule. This reactivity is reasonable considering that

List all types of bonding present in the compound NH₄NO₃. I. ionic bond II. polar covalent bond III. nonpolar covalent bond

List all types of bonding present in the ion SO₄^2-. I. ionic bond II. polar covalent bond III. nonpolar covalent bond

Use the bond enthalpy data given to estimate the heat released when 6.50 g of nitrogen gas reacts with excess hydrogen gas to form ammonia at 25^$\circ$C. BE(N $\equiv$ N) = 941.4 kJ/mol BE(H-H) = 436.4 kJ/mol BE(N-H) = 393 kJ/mol

Estimate the enthalpy change for the combustion of one mole of acetylene, C₂H₂, to form carbon dioxide and water vapor. BE(C-H) = 456 kJ/mol BE(C $\equiv$ C) = 962 kJ/mol BE(O=O) = 499 kJ/mol BE(C=O) = 802 kJ/mol BE(O-H) = 462 kJ/mol

The ion O₂^2- shows both ionic and covalent bonding.

The number of lone electron pairs in the NH₄⁺ ion is ___.

The total number of valence electrons in the molecule CO₂ is

Calculate the energy required for the gas phase process represented by Na(g) + Br(g) $\rarr$ Na⁺(g) + Br^- (g). Given: Ionization energy (Na) = 496 kJ/mol Electron affinity (Br) = 324 kJ/mol Electron affinity (Na) = 53 kJ/mol

Examine this Lewis structure for the phosphate ion, PO₄^3-. How many valence electrons are around the P atom in this structure

The Lewis structure for CS₂ is: