Question 1

Rank the following molecules in decreasing bond energy. Cl2 Br2 F2 I2

Accepted Answer

A)  I2 > Br2 > Cl2 > F2 
B)  Cl2 > Br2 > F2 > I2 
C)  I2 > Cl2 > Br2 > F2 
D)  Cl2 > I2 > F2 > Br2 
A)  I2 > Br2 > Cl2 > F2 
B)  Cl2 > Br2 > F2 > I2 
C)  I2 > Cl2 > Br2 > F2 
D)  Cl2 > I2 > F2 > Br2

Question 2

Describe a covalent bond.

Accepted Answer

A bond for

Question 3

Place the following elements in order of decreasing electronegativity. S Cl Se

Accepted Answer

A)  Se > S > Cl 
B)  Cl > Se > S 
C)  Se > Cl > S 
D)  S > Cl > Se 
E)  Cl > S > Se 
A)  Se > S > Cl 
B)  Cl > Se > S 
C)  Se > Cl > S 
D)  S > Cl > Se 
E)  Cl > S > Se

Question 4

Draw the best Lewis structure for CH3+. What is the formal charge on the C?

Accepted Answer

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

Question 5

Using periodic trends, place the following bonds in order of increasing ionic character. Si-P Si-Cl Si-S

Accepted Answer

A)  Si-P < Si-Cl < Si-S 
B)  Si-P < Si-S < Si-Cl 
C)  Si-S < Si-Cl < Si-P 
D)  Si-Cl < Si-P < Si-S 
E)  Si-Cl < Si-S < Si-P 
A)  Si-P < Si-Cl < Si-S 
B)  Si-P < Si-S < Si-Cl 
C)  Si-S < Si-Cl < Si-P 
D)  Si-Cl < Si-P < Si-S 
E)  Si-Cl < Si-S < Si-P

Question 6

Identify the compound with ionic bonding.

Accepted Answer

A)  HS1U1B12S1U1B0O 
B)  CHS1U1B14S1U1B0 
C)  HS1U1B12S1U1B0 
D)  COS1U1B12S1U1B0 
E)  RbFS1U1B0 
A)  HS1U1B12S1U1B0O 
B)  CHS1U1B14S1U1B0 
C)  HS1U1B12S1U1B0 
D)  COS1U1B12S1U1B0 
E)  RbFS1U1B0

Question 7

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 8

Draw the Lewis structure for NO2⁻, including any valid resonance structures. Which of the following statements is TRUE?

Accepted Answer

A)  The nitrite ion contains one N-O single bond and one N=O double bond. 
B)  The nitrite ion contains two N-O bonds that are equivalent to 1   bonds. 
C)  The nitrite ion contains two N=O double bonds. 
D)  The nitrite ion contains two N-O single bonds. 
E)  None of the above is true. 
A)  The nitrite ion contains one N-O single bond and one N=O double bond. 
B)  The nitrite ion contains two N-O bonds that are equivalent to 1   bonds. 
C)  The nitrite ion contains two N=O double bonds. 
D)  The nitrite ion contains two N-O single bonds. 
E)  None of the above is true.

Question 9

Identify the shortest bond.

Accepted Answer

A)  single covalent bond 
B)  double covalent bond 
C)  triple covalent bond 
D)  All of the above bonds are the same length. 
A)  single covalent bond 
B)  double covalent bond 
C)  triple covalent bond 
D)  All of the above bonds are the same length.

Question 10

How are electron affinity and electronegativity different?

Accepted Answer

Electron affinity is the process of a si

Question 11

The most electronegative atom is ________.

Accepted Answer

The answer of The most electronegative atom is ________....

Question 12

Place the following elements in order of increasing electronegativity. Sr N Na

Accepted Answer

A)  Sr < Na < N 
B)  Na < N < Sr 
C)  Sr < N < Na 
D)  N < Sr < Na 
E)  N < Na < Sr 
A)  Sr < Na < N 
B)  Na < N < Sr 
C)  Sr < N < Na 
D)  N < Sr < Na 
E)  N < Na < Sr

Question 13

Describe the difference between a pure covalent bond and a polar covalent bond.

Accepted Answer

A pure covalent bond occurs when bonding

Question 14

Use the data given below to construct a Born-Haber cycle to determine the heat of formation of KCl. ΔH°(kJ mol-1)
K(s) → K(g) 89
K(g) → K⁺(g) + e⁻ 418
Cl2(g) → 2Cl(g) 244
Cl(g) + e⁻ → Cl⁻(g) -349
KCl(s) → K⁺(g) + Cl⁻(g) 717

Accepted Answer

A)  -1119 kJ mol-1 
B)  -997 kJ mol-1 
C)  -437 kJ mol-1 
D)  +631 kJ mol-1 
E)  +158 kJ mol-1 
A)  -1119 kJ mol-1 
B)  -997 kJ mol-1 
C)  -437 kJ mol-1 
D)  +631 kJ mol-1 
E)  +158 kJ mol-1

Question 15

Identify the compound with the highest magnitude of lattice energy.

Accepted Answer

A)  NaCl 
B)  KCl 
C)  LiCl 
D)  CsCl 
A)  NaCl 
B)  KCl 
C)  LiCl 
D)  CsCl

Question 16

Match the following.
-Se-I

Accepted Answer

A) strongest covalent bond 
B) longest covalent bond 
C) weakest ionic bond 
D) metallic bond 
E) highest melting point 
A) strongest covalent bond 
B) longest covalent bond 
C) weakest ionic bond 
D) metallic bond 
E) highest melting point

Question 17

Identify the compound with covalent bonding.

Accepted Answer

A)  NaCl 
B)  KCl 
C)  H2O 
D)  CaO 
E)  SrBr2 
A)  NaCl 
B)  KCl 
C)  H2O 
D)  CaO 
E)  SrBr2

Question 18

Which of the following elements can form hypercoordinate compounds?

Accepted Answer

A)  N 
B)  Br 
C)  F 
D)  Be 
E)  None of the above can form compounds with an expanded octet. 
A)  N 
B)  Br 
C)  F 
D)  Be 
E)  None of the above can form compounds with an expanded octet.

Question 19

Use the data given below to construct a Born-Haber cycle to determine the lattice energy of CaO.

Accepted Answer

A)  -3414 kJ mol-1 
B)  +1397 kJ mol-1 
C)  -2667 kJ mol-1 
D)  +3028 kJ mol-1 
E)  -2144 kJ mol-1 
A)  -3414 kJ mol-1 
B)  +1397 kJ mol-1 
C)  -2667 kJ mol-1 
D)  +3028 kJ mol-1 
E)  -2144 kJ mol-1

Question 20

Use Lewis theory to determine the chemical formula for the compound formed between K and I.

Accepted Answer

A)  KI2 
B)  K2I 
C)  KI 
D)  K2I2 
A)  KI2 
B)  K2I 
C)  KI 
D)  K2I2

Exam 9: Chemical Bonding I: Lewis Theory

Rank the following molecules in decreasing bond energy. Cl2 Br2 F2 I2

Describe a covalent bond.

Place the following elements in order of decreasing electronegativity. S Cl Se

Draw the best Lewis structure for CH3+. What is the formal charge on the C?

Using periodic trends, place the following bonds in order of increasing ionic character. Si-P Si-Cl Si-S

Identify the compound with ionic bonding.

Which molecule or compound below contains an ionic bond?

Draw the Lewis structure for NO2⁻, including any valid resonance structures. Which of the following statements is TRUE?

Identify the shortest bond.

How are electron affinity and electronegativity different?

The most electronegative atom is ________.

Place the following elements in order of increasing electronegativity. Sr N Na

Describe the difference between a pure covalent bond and a polar covalent bond.

Use the data given below to construct a Born-Haber cycle to determine the heat of formation of KCl. ΔH°(kJ mol-1) K(s) → K(g) 89 K(g) → K⁺(g) + e⁻ 418 Cl2(g) → 2Cl(g) 244 Cl(g) + e⁻ → Cl⁻(g) -349 KCl(s) → K⁺(g) + Cl⁻(g) 717

Identify the compound with the highest magnitude of lattice energy.

Match the following. -Se-I

Identify the compound with covalent bonding.

Which of the following elements can form hypercoordinate compounds?

Use the data given below to construct a Born-Haber cycle to determine the lattice energy of CaO.

Use Lewis theory to determine the chemical formula for the compound formed between K and I.

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

Rank the following molecules in decreasing bond energy. Cl₂ Br₂ F₂ I₂

Draw the best Lewis structure for CH₃⁺. What is the formal charge on the C?

Draw the Lewis structure for NO₂⁻, including any valid resonance structures. Which of the following statements is TRUE?

Use the data given below to construct a Born-Haber cycle to determine the heat of formation of KCl. ΔH°(kJ mol^-1) K(s) → K(g) 89 K(g) → K⁺(g) + e⁻ 418 Cl₂(g) → 2Cl(g) 244 Cl(g) + e⁻ → Cl⁻(g) -349 KCl(s) → K⁺(g) + Cl⁻(g) 717