Back
Problem 55a
Determine if a bond between each pair of atoms would be pure covalent, polar covalent, or ionic. a. Br and Br
- 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.
Problem 56
Problem 57
Refer to Figure 9.10 to estimate the percent ionic character of the CO bond.
Problem 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.
Problem 58b
Refer to Figure 9.10 to estimate the percent ionic character of the BrF bond.
Problem 59
Write the Lewis structure for each molecule or ion. a. CI4 b. N2O c. SiH4 d. Cl2CO
Problem 60b
Write the Lewis structure for each molecule or ion. b. OH-
Problem 60c
Write the Lewis structure for each molecule or ion. c. BrO-
Problem 61a,b,c
Write the Lewis structure for each molecule or ion. a. N2H2 b. N2H4 c. C2H2
Problem 61d
Write the Lewis structure for each molecule or ion. d. C2H4
Problem 62a
Write the Lewis structure for each molecule or ion. a. H3COCH3
Problem 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
Problem 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. CO32– c. ClO– d. NO2–
Problem 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+
Problem 66
Use formal charges to identify the better Lewis structure.
Problem 67
How important is the resonance structure shown here to the overall structure of carbon dioxide? Explain.
Problem 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.
Problem 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.
Problem 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.
Problem 71
What are the formal charges of the atoms shown in red?
Problem 72
What are the formal charges of the atoms shown in red?
Problem 73b
Write the Lewis structure for each molecule (octet rule not followed). b. NO2
Problem 74
Write the Lewis structure for each molecule (octet rule not followed). a. BBr3 b. NO c. ClO2
- 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^-.
Problem 75
- 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^-
Problem 76
Problem 77a
Write Lewis structures for each molecule or ion. Use expanded octets as necessary. a. PF5
Problem 78b
Write Lewis structures for each molecule or ion. Use expanded octets as necessary. b. AsF6-
Problem 79a
Order these compounds in order of increasing carbon–carbon bond strength: HCCH, H2CCH2, H3CCH3.
Problem 79b
Order these compounds in order of decreasing carbon–carbon bond length: HCCH, H2CCH2, H3CCH3.
Problem 80
Which of the two compounds, H2NNH2 and HNNH, has the strongest nitrogen-nitrogen bond, and which has the shorter nitrogen-nitrogen bond.