Question 1

Classify the O - H bond in CH3OH as ionic, polar covalent, or nonpolar covalent.

Accepted Answer

A)  ionic 
B)  polar covalent 
C)  nonpolar covalent 
A)  ionic 
B)  polar covalent 
C)  nonpolar covalent

Question 2

The standard enthalpy of formation of ammonia at 25$\circ$C is -46.3 kJ/mol. Estimate the N-H bond enthalpy at this temperature.(Given: BE(N$\equiv$N) = 941.4 kJ/mol, BE(H-H) = 436.4 kJ/mol)

Accepted Answer

A)  360 kJ/mol 
B)  383 kJ/mol 
C)  391 kJ/mol 
D)  459 kJ/mol 
E)  475 kJ/mol 
A)  360 kJ/mol 
B)  383 kJ/mol 
C)  391 kJ/mol 
D)  459 kJ/mol 
E)  475 kJ/mol

Question 3

Shown here is a Lewis structure for the chlorite ion, ClO2-, that obeys the octet rule, showing all non-zero formal charges. How many resonance structures for ClO2- that obey the octet are possible ?

Accepted Answer

A)  four 
B)  three 
C)  two 
D)  one 
E)  none of the above 
A)  four 
B)  three 
C)  two 
D)  one 
E)  none of the above

Question 4

Shown here is a Lewis structure for SO3 that expands the octet to minimize formal charges. The formal charge on the sulfur atom is zero.

Accepted Answer

A) True 
 B)False

Question 5

Covalent bonding is the only type of bonding present in the ClO2- ion.

Accepted Answer

A) True 
 B)False

Question 6

Which one of the following is most likely to be a covalent compound

Accepted Answer

A)  KF 
B)  CaCl2 
C)  SF4 
D)  Al2O3 
E)  CaSO4 
A)  KF 
B)  CaCl2 
C)  SF4 
D)  Al2O3 
E)  CaSO4

Question 7

What is the formal charge on sulfur in the most favorable Lewis structure for the SCN- (thiocyanate) ion based on minimizing formal charge overall

Accepted Answer

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

Question 8

Of the species NO2, NO, and N2, only NO2 is an exception to the octet rule.

Accepted Answer

A) True 
 B)False

Question 9

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

Accepted Answer

A)  Mg 
B)  H 
C)  Al 
D)  O 
E)  Na 
A)  Mg 
B)  H 
C)  Al 
D)  O 
E)  Na

Question 10

Carbonic acid, H2CO3, is a weak acid that contributes to the taste and produces the carbon dioxide bubbles in all carbonated beverages. How many valence electrons are used to show the Lewis structure for H2CO3

Accepted Answer

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

Question 11

Which one of the following is most likely to be an ionic compound

Accepted Answer

A)  ClF3 
B)  FeCl3 
C)  NH3 
D)  PF3 
E)  SO3 
A)  ClF3 
B)  FeCl3 
C)  NH3 
D)  PF3 
E)  SO3

Question 12

Arrange the elements Ba, Br, and Ga in order of increasing electronegativity.

Accepted Answer

A)  Ba < Br < Ga 
B)  Br < Ga < Ba 
C)  Ba < Ga < Br 
D)  Ga < Ba < Br 
E)  Ga < Br < Ba 
A)  Ba < Br < Ga 
B)  Br < Ga < Ba 
C)  Ba < Ga < Br 
D)  Ga < Ba < Br 
E)  Ga < Br < Ba

Question 13

Classify the C - Cl bond in CCl4 as ionic, polar covalent, or nonpolar covalent.

Accepted Answer

A)  ionic 
B)  polar covalent 
C)  nonpolar covalent 
A)  ionic 
B)  polar covalent 
C)  nonpolar covalent

Question 14

Which of the following solids would have the highest melting point

Accepted Answer

A)  NaF 
B)  NaCl 
C)  NaBr 
D)  NaI 
A)  NaF 
B)  NaCl 
C)  NaBr 
D)  NaI

Question 15

Which one of the following compounds utilizes both ionic and covalent bonding

Accepted Answer

A)  C10H22O 
B)  NH3 
C)  Na2S 
D)  NH4NO3 
E)  K3N 
A)  C10H22O 
B)  NH3 
C)  Na2S 
D)  NH4NO3 
E)  K3N

Question 16

Use the Born-Haber cycle to calculate the lattice energy of MgO (s) given the following data: $\Delta$H(sublimation) Mg = 130 kJ/mol
I1 (Mg) = 738.1 kJ/mol
I2 (Mg) = 1450 kJ/mol
Bond energy (O=O) = 498.7 kJ/mol
EA (O) = 141 kJ/mol
EA (O-) = -780 kJ/mol
$\Delta{H}^{\circ}_f$(MgO(s)) = -601.8 kJ/mol

Accepted Answer

A)  2200 kJ/mol 
B)  2800 kJ/mol 
C)  3200 kJ/mol 
D)  3800 kJ/mol 
E)  4100 kJ/mol 
A)  2200 kJ/mol 
B)  2800 kJ/mol 
C)  3200 kJ/mol 
D)  3800 kJ/mol 
E)  4100 kJ/mol

Question 17

Assuming the octet rule is obeyed, how many covalent bonds will a neon atom form to give a formal charge of zero

Accepted Answer

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

Question 18

Shown here is the Lewis structure for the chlorite ion, ClO2-, that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s).

Accepted Answer

A) True 
 B)False

Question 19

The Lewis dot symbol for the calcium ion is

Accepted Answer

A)  $\text{: Ca :}^{2+}$ 
B)  -Ca- 
C)    
D)  Ca2+ 
E)  Ca 
A)  $\text{: Ca :}^{2+}$ 
B)  -Ca- 
C)    
D)  Ca2+ 
E)  Ca

Question 20

The total number of valence electrons in the compound NH4NO3 is

Accepted Answer

A)  28. 
B)  30. 
C)  32. 
D)  42. 
E)  80. 
A)  28. 
B)  30. 
C)  32. 
D)  42. 
E)  80.

Exam 9: Chemical Bonding I: Basic Concepts

Classify the O - H bond in CH3OH as ionic, polar covalent, or nonpolar covalent.

The standard enthalpy of formation of ammonia at 25 ∘\circ∘ C is -46.3 kJ/mol. Estimate the N-H bond enthalpy at this temperature.(Given: BE(N ≡\equiv≡ N) = 941.4 kJ/mol, BE(H-H) = 436.4 kJ/mol)

Shown here is a Lewis structure for the chlorite ion, ClO2-, that obeys the octet rule, showing all non-zero formal charges. How many resonance structures for ClO2- that obey the octet are possible ?

Shown here is a Lewis structure for SO3 that expands the octet to minimize formal charges. The formal charge on the sulfur atom is zero.

Covalent bonding is the only type of bonding present in the ClO2- ion.

Which one of the following is most likely to be a covalent compound

What is the formal charge on sulfur in the most favorable Lewis structure for the SCN- (thiocyanate) ion based on minimizing formal charge overall

Of the species NO2, NO, and N2, only NO2 is an exception to the octet rule.

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

Carbonic acid, H2CO3, is a weak acid that contributes to the taste and produces the carbon dioxide bubbles in all carbonated beverages. How many valence electrons are used to show the Lewis structure for H2CO3

Which one of the following is most likely to be an ionic compound

Arrange the elements Ba, Br, and Ga in order of increasing electronegativity.

Classify the C - Cl bond in CCl4 as ionic, polar covalent, or nonpolar covalent.

Which of the following solids would have the highest melting point

Which one of the following compounds utilizes both ionic and covalent bonding

Assuming the octet rule is obeyed, how many covalent bonds will a neon atom form to give a formal charge of zero

Shown here is the Lewis structure for the chlorite ion, ClO2-, that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s).

The Lewis dot symbol for the calcium ion is

The total number of valence electrons in the compound NH4NO3 is

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Filters

Classify the O - H bond in CH₃OH as ionic, polar covalent, or nonpolar covalent.

The standard enthalpy of formation of ammonia at 25^$\circ$C is -46.3 kJ/mol. Estimate the N-H bond enthalpy at this temperature.(Given: BE(N $\equiv$ N) = 941.4 kJ/mol, BE(H-H) = 436.4 kJ/mol)

Shown here is a Lewis structure for the chlorite ion, ClO₂^-, that obeys the octet rule, showing all non-zero formal charges. How many resonance structures for ClO₂^- that obey the octet are possible ?

Shown here is a Lewis structure for SO₃ that expands the octet to minimize formal charges. The formal charge on the sulfur atom is zero.

Covalent bonding is the only type of bonding present in the ClO₂^- ion.

What is the formal charge on sulfur in the most favorable Lewis structure for the SCN^- (thiocyanate) ion based on minimizing formal charge overall

Of the species NO₂, NO, and N₂, only NO₂ is an exception to the octet rule.

Carbonic acid, H₂CO₃, is a weak acid that contributes to the taste and produces the carbon dioxide bubbles in all carbonated beverages. How many valence electrons are used to show the Lewis structure for H₂CO₃

Classify the C - Cl bond in CCl₄ as ionic, polar covalent, or nonpolar covalent.

Shown here is the Lewis structure for the chlorite ion, ClO₂^-, that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s).

The total number of valence electrons in the compound NH₄NO₃ is