Ch.9 - Chemical Bonding I: The Lewis Model

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Ch.9 - Chemical Bonding I: The Lewis Model

Problema 55a

Determine if a bond between each pair of atoms would be pure covalent, polar covalent, or ionic. a. Br and Br

Problema 56

Determine whether the bond between each of the following pairs of atoms would be pure covalent, polar covalent, or ionic: a. C and N b. N and S c. K and F d. N and N.

Problema 57

Refer to Figure 9.10 to estimate the percent ionic character of the CO bond.

Problema 58a

Draw the Lewis structure for BrF with an arrow representing the dipole moment. Refer to Figure 9.10 to estimate the percent ionic character of the BrF bond.

Problema 58b

Refer to Figure 9.10 to estimate the percent ionic character of the BrF bond.

Problema 59

Write the Lewis structure for each molecule or ion. a. CI₄ b. N₂O c. SiH₄ d. Cl₂CO

Problema 60b

Write the Lewis structure for each molecule or ion. b. OH^-

Problema 60c

Write the Lewis structure for each molecule or ion. c. BrO^-

Problema 61a,b,c

Write the Lewis structure for each molecule or ion. a. N₂H₂ b. N₂H₄ c. C₂H₂

Problema 61d

Write the Lewis structure for each molecule or ion. d. C₂H₄

Problema 62a

Write the Lewis structure for each molecule or ion. a. H₃COCH₃

Problema 63a

Write a Lewis structure that obeys the octet rule for each molecule or ion. Include resonance structures if necessary and assign formal charges to each atom. a. SeO₂

Problema 63b,c,d

Write a Lewis structure that obeys the octet rule for each molecule or ion. Include resonance structures if necessary and assign formal charges to each atom. b. CO₃^2– c. ClO^– d. NO₂^–

Problema 64

Write a Lewis structure that obeys the octet rule for each ion. Include resonance structures if necessary and assign formal charges to each atom. a. ClO₃^- b. ClO₄^- c. NO₃^- d. NH₄⁺

Problema 66

Use formal charges to identify the better Lewis structure.

Problema 67

How important is the resonance structure shown here to the overall structure of carbon dioxide? Explain.

Problema 68

In N₂O, nitrogen is the central atom and the oxygen atom is terminal. In OF₂, however, oxygen is the central atom. Use formal charges to explain why.

Problema 69

Draw the Lewis structure (including resonance structures) for the acetate ion (CH₃COO^-). For each resonance structure, assign formal charges to all atoms that have formal charge.

Problema 70

Draw the Lewis structure (including resonance structures) for methyl azide (CH₃N₃). For each resonance structure, assign formal charges to all atoms that have formal charge.

Problema 71

What are the formal charges of the atoms shown in red?

Problema 72

What are the formal charges of the atoms shown in red?

Problema 73b

Write the Lewis structure for each molecule (octet rule not followed). b. NO₂

Problema 74

Write the Lewis structure for each molecule (octet rule not followed). a. BBr₃ b. NO c. ClO₂

Problema 75

Write the Lewis structure for each ion. Include resonance structures if necessary and assign formal charges to all atoms. If necessary, expand the octet on the central atom to lower formal charge for the following ions: a. PO4^3- b. CN^- c. SO3^2- d. ClO2^-.

Problema 76

Write Lewis structures for each molecule or ion. Include resonance structures if necessary and assign formal charges to all atoms. If you need to, expand the octet on the central atom to lower formal charge. a. SO4^2- b. HSO4^- c. SO3 d. BrO2^-

Problema 77a

Write Lewis structures for each molecule or ion. Use expanded octets as necessary. a. PF₅

Problema 78b

Write Lewis structures for each molecule or ion. Use expanded octets as necessary. b. AsF₆^-

Problema 79a

Order these compounds in order of increasing carbon–carbon bond strength: HCCH, H₂CCH₂, H₃CCH₃.

Problema 79b

Order these compounds in order of decreasing carbon–carbon bond length: HCCH, H₂CCH₂, H₃CCH₃.

Problema 80

Which of the two compounds, H₂NNH₂ and HNNH, has the strongest nitrogen-nitrogen bond, and which has the shorter nitrogen-nitrogen bond.