Question 1

The evaporation of seawater gives a mixture of ionic compounds containing sodium combined with chloride, sulfate, carbonate, and hydrogen carbonate.Write the chemical formulas of these compounds.

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Question 2

Carbonyl fluoride (COF₂) is similar in structure to phosgene (COCl₂), and both are highly toxic.Draw the Lewis structure of COF₂.

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Question 3

Draw the Lewis structure of boron trifluoride.

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Question 4

Two reasonable Lewis structures for sulfurous acid (H₂SO₃) are given below.Add the formal charges to each atom.

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Question 5

Ethanethiol and dimethyl sulfide share the same chemical formula (C₂H₆S) but different bonding arrangements.Ethanethiol has a central carbon, whereas dimethyl sulfide has a central sulfur.Draw their Lewis structures.

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Question 6

Identify which of the following molecules has a bond order of 3: Li₂, Be₂, N₂, F₂, C₂.

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Question 7

Draw the Lewis structure for the nitrate anion, NO₃-.Include resonance structures if necessary.

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Question 8

Using the positions of the atoms in the periodic table, identify which of the following bonds is expected to be the most polar: 
C - F, Cl - F, Si - F, S -F, O - F.

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Question 9

The complete combustion of carbon compounds produces carbon dioxide.The reaction of coal with water at high temperatures produces synthesis gas, which is a mixture of carbon monoxide and hydrogen.Use the bond energies in the table below to estimate how much more energy is released by reaction I than by reaction II. I) C(s) +O₂(g) $\rightarrow$ CO₂(g) II) C(s) + H₂O(g) $\rightarrow$ CO₂(g) +H₂(g) * C = O bond in CO₂

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Question 10

Draw the Lewis structure for the carbonate anion, CO₃^2-.Include resonance structures if necessary.

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Question 11

Which of the following bonds is considered to be ionic? Explain why.
C - O, Ca - Cl, S - N, Si - O.

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Question 12

Chlorofluorocarbons (CFCs or freons) are linked to the depletion of atmospheric ozone. Draw the Lewis structure of freon-1113, C₂ClF₃.

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Question 13

Based on electronegativities, which of the following bonds is the most polar, and which is the least polar? 
H - F, H - N, H - C, H - H, H- O

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Question 14

Describe the relationship between bond order, bond energy, and bond length.

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Question 15

Based on the positions of the atoms in the periodic table, arrange the following bonds in order of increasing bond length: 
C - O, S- O, C- C.

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Question 16

Describe how and why formal charges are used to choose between two possible Lewis structures for a molecule.

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Question 17

Hydrogen isocyanide (HNC) and hydrogen cyanide (HCN) have the same elemental composition.Is one structure more stable than the other? Support your answer with the Lewis structures and formal charges assigned to each atom for these molecules.

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Question 18

Three reasonable resonance structures are shown for the cyanate ion, OCN -.Assign formal charges to each atom.Which structure, if any, contributes most heavily to the resonance hybrid structure, and why?
A)  
B)  
C)

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Question 19

Which carbon-halogen bond is the most polar?

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Question 20

Draw the Lewis structures of PCl₃ and PCl₅.

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Quiz 4: Chemical Bonding Understanding Climate Change

The evaporation of seawater gives a mixture of ionic compounds containing sodium combined with chloride, sulfate, carbonate, and hydrogen carbonate.Write the chemical formulas of these compounds.

Carbonyl fluoride (COF2) is similar in structure to phosgene (COCl2), and both are highly toxic.Draw the Lewis structure of COF2.

Draw the Lewis structure of boron trifluoride.

Two reasonable Lewis structures for sulfurous acid (H2SO3) are given below.Add the formal charges to each atom.

Ethanethiol and dimethyl sulfide share the same chemical formula (C2H6S) but different bonding arrangements.Ethanethiol has a central carbon, whereas dimethyl sulfide has a central sulfur.Draw their Lewis structures.

Identify which of the following molecules has a bond order of 3: Li2, Be2, N2, F2, C2.

Draw the Lewis structure for the nitrate anion, NO3-.Include resonance structures if necessary.

Using the positions of the atoms in the periodic table, identify which of the following bonds is expected to be the most polar: C - F, Cl - F, Si - F, S -F, O - F.

Draw the Lewis structure for the carbonate anion, CO32-.Include resonance structures if necessary.

Which of the following bonds is considered to be ionic? Explain why. C - O, Ca - Cl, S - N, Si - O.

Chlorofluorocarbons (CFCs or freons) are linked to the depletion of atmospheric ozone. Draw the Lewis structure of freon-1113, C2ClF3.

Based on electronegativities, which of the following bonds is the most polar, and which is the least polar? H - F, H - N, H - C, H - H, H- O