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Problem 3.46
Arrange these compounds in order of increasing magnitude of lattice energy: KCl, SrO, RbBr, CaO.
Problem 35
Write the electron configuration for N. Then write the Lewis symbol for N and show which electrons from the electron configuration are included in the Lewis symbol.
Problem 37a,c
Write the Lewis symbol for each atom or ion. a. Al c. Cl
Problem 37b
Write the Lewis symbol for each atom or ion. b. Na+
Problem 37d
Write the Lewis symbol for each atom or ion. d. Cl-
Problem 40a,d
Write the Lewis symbols for the ions in each ionic compound. a. SrO d. RbF
Problem 40b
Write the Lewis symbols for the ions in each ionic compound. b. Li2S
Problem 40c
Write the Lewis symbols for the ions in each ionic compound. c. CaI2
Problem 41
Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Sr and Se b. Ba and Cl c. Na and S d. Al and O
Problem 42
Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Ca and N b. Mg and I c. Ca and S d. Cs and F
Problem 45
The lattice energy of CsF is -744 kJ/mol, whereas that of BaO is -3029 kJ/mol. Explain this large difference in lattice energy.
Problem 47
Use the Born–Haber cycle and data from Appendix IIB, Chapter 9 and this chapter to calculate the lattice energy of KCl. (ΔHsub for potassium is 89.0 kJ>mol.)
Problem 48
Use the Born–Haber cycle and data from Appendix IIB and Table 10.3 to calculate the lattice energy of CaO. (ΔHsub for calcium is 178 kJ>mol; IE1 and IE2 for calcium are 590 kJ>mol and 1145 kJ>mol, respectively; EA1 and EA2 for O are -141 kJ>mol and 744 kJ>mol, respectively.)
- Use covalent Lewis structures to explain why each element or family of elements occurs as diatomic molecules: a. hydrogen b. the halogens c. oxygen d. nitrogen.
Problem 49
Problem 51a,b,c
Write the Lewis structure for each molecule. a. PH3 b. SCl2 c. HI
Problem 51d
Write the Lewis structure for each molecule. d. CH4
Problem 53a
Write the Lewis structure for each molecule. a. SF2
Problem 53b
Write the Lewis structure for each molecule. b. SiH4
Problem 53d
Write the Lewis structure for each molecule. d. CH3SH (C and S central)
Problem 54
Write the Lewis structure for each molecule. a. CH2O b. C2Cl4 c. CH3NH2 d. CFCl3 (C central)
Problem 57
Refer to Figure 10.10 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 10.10 to estimate the percent ionic character of the BrF bond.
Problem 58b
Refer to Figure 10.10 to estimate the percent ionic character of the BrF bond.
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 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 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.