Question 1

Use the bond energies provided to estimate ΔH°rxn for the reaction below.
2 Br2(l) + C2H2(g) → C2H2Br4(l) ΔH°rxn = ?
Bond Bond Energy (kJ/mol) 
Br-Br 193
C≡C 837
C-C 347
C-Br 276
C-H 414

Accepted Answer

A)  +407 kJ
B)  -324 kJ
C)  -228 kJ
D)  +573 kJ
E)  -648 kJF) B) and E)
G) C) and E)

Question 2

Use the bond energies provided to estimate ΔH°rxn for the reaction below.
C2H4(g) + H2(g) → C2H6(g) ΔH°rxn = ?
Bond Bond Energy (kJ/mol) 
C-C 347
C-H 414
C=C 611
C≡C 837
H-H 436

Accepted Answer

A)  -128 kJ
B)  +98 kJ
C)  +700 kJ
D)  -102 kJ
E)  -166 kJF) A) and D)
G) A) and C)

Question 3

Place the following in order of increasing magnitude of lattice energy.
MgO LiI BaS

Accepted Answer

A)  BaS 
B)  LiI 
C)  MgO 
D)  LiI 
E)  MgO < LiI < BaSF) A) and E)
G) B) and E)

Question 4

Place the following in order of decreasing magnitude of lattice energy.
NaF RbBr KCl

Accepted Answer

A)  RbBr > NaF > KCl
B)  NaF > KCl > RbBr
C)  KCl > NaF > RbBr
D)  NaF > RbBr > KCl
E)  RbBr > KCl > NaFF) B) and C)
G) A) and E)

Question 5

Define electronegativity.

Accepted Answer

The ability of an at...

Question 6

Choose the best Lewis structure for OCl2.

Accepted Answer

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G) B) and C)

Question 7

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)  Mg2BrF) C) and E)
G) D) and E)

Question 8

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

Accepted Answer

A)  Mg3N2
B)  Mg2N3
C)  MgN2
D)  MgNE) None of the above
F) All of the above

Question 9

Give the number of valence electrons for SF4.

Accepted Answer

A)  28
B)  30
C)  32
D)  34E) A) and B)
F) A) and C)

Question 10

The electronegativity is 2.1 for H and 1.9 for Pb.Based on these electronegativities PbH4 would be expected to

Accepted Answer

A)  be ionic and contain H- ions.
B)  be ionic and contain H+ ions.
C)  have polar covalent bonds with a partial negative charges on the H atoms.
D)  have polar covalent bonds with a partial positive charges on the H atoms.E) B) and C)
F) A) and B)

Question 11

Of the following elements,which has the lowest electronegativity?

Accepted Answer

A)  Sr
B)  I
C)  Ba
D)  AtE) C) and D)
F) None of the above

Question 12

The iodine atom in I2 would be expected to have a

Accepted Answer

A)  charge of 1-.
B)  partial charge δ-.
C)  partial charge δ+.
D)  charge of 0.E) A) and C)
F) All of the above

Question 13

Which is most polar?

Accepted Answer

A)  HF
B)  HCl
C)  HBr
D)  HIE) A) and D)
F) C) and D)

Question 14

Which of the following elements can form compounds with an expanded octet?

Accepted Answer

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

Question 15

Place the following in order of increasing magnitude of lattice energy.
MgO LiI CaS

Accepted Answer

A)  CaS 
B)  LiI 
C)  MgO 
D)  LiI 
E)  MgO < LiI < CaSF) A) and B)
G) A) and E)

Question 16

Choose the bond below that is the weakest.

Accepted Answer

A)  Na-Cl
B)  I-I
C)  C=N
D)  Li-F
E)  C=OF) C) and D)
G) None of the above

Question 17

Lattice energy of NaF and CaO are -910 kJ/mol and -3414 kJ/mol respectively.Which accounts for almost four fold increase in the lattice energy of CaO?

Accepted Answer

A)  the higher ionic radius of CaO compared to that of NaF
B)  the higher magnitude of ionic charge of CaO compared to that of NaF
C)  factors other than ionic radius and ionic change
D)  Ca is a group II metal in the periodic table.E) B) and D)
F) All of the above

Question 18

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)  -2F) B) and E)
G) B) and C)

Question 19

Give the number of valence electrons for XeI2.

Accepted Answer

A)  22
B)  20
C)  18
D)  24E) All of the above
F) None of the above

Question 20

Choose the compound below that should have the highest melting point according to the ionic bonding model.

Accepted Answer

A)  AlN
B)  MgO
C)  NaF
D)  CaS
E)  RbIF) B) and D)
G) C) and E)

Exam 9: Chemical Bonding I: Lewis Theory

Choose the bond below that is the weakest.

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Place the following in order of increasing magnitude of lattice energy. MgO LiI CaS

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Lattice energy of NaF and CaO are -910 kJ/mol and -3414 kJ/mol respectively.Which accounts for almost four fold increase in the lattice energy of CaO?

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Give the number of valence electrons for SF4.

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Place the following in order of decreasing magnitude of lattice energy. NaF RbBr KCl

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Define electronegativity.

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Use the bond energies provided to estimate ΔH°rxn for the reaction below. 2 Br2(l) + C2H2(g) → C2H2Br4(l) ΔH°rxn = ? Bond Bond Energy (kJ/mol) Br-Br 193 C≡C 837 C-C 347 C-Br 276 C-H 414

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Choose the best Lewis structure for OCl2.

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Give the number of valence electrons for XeI2.

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

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Choose the compound below that should have the highest melting point according to the ionic bonding model.

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

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

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The iodine atom in I2 would be expected to have a

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Place the following in order of increasing magnitude of lattice energy. MgO LiI BaS

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Of the following elements,which has the lowest electronegativity?

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Use the bond energies provided to estimate ΔH°rxn for the reaction below. C2H4(g) + H2(g) → C2H6(g) ΔH°rxn = ? Bond Bond Energy (kJ/mol) C-C 347 C-H 414 C=C 611 C≡C 837 H-H 436

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Which is most polar?

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Which of the following elements can form compounds with an expanded octet?

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The electronegativity is 2.1 for H and 1.9 for Pb.Based on these electronegativities PbH4 would be expected to

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Give the number of valence electrons for SF₄.

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The ability of an at...
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Use the bond energies provided to estimate ΔH°_rxn for the reaction below. 2 Br₂(l) + C₂H₂(g) → C₂H₂Br₄(l) ΔH°_rxn= ? Bond Bond Energy (kJ/mol) Br-Br 193 C≡C 837 C-C 347 C-Br 276 C-H 414

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Choose the best Lewis structure for OCl₂.

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Give the number of valence electrons for XeI₂.

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

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The iodine atom in I₂ would be expected to have a

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Use the bond energies provided to estimate ΔH°_rxn for the reaction below. C₂H₄(g) + H₂(g) → C₂H₆(g) ΔH°_rxn= ? Bond Bond Energy (kJ/mol) C-C 347 C-H 414 C=C 611 C≡C 837 H-H 436

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The electronegativity is 2.1 for H and 1.9 for Pb.Based on these electronegativities PbH₄ would be expected to

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