Back
Problem 0.95
Carbon ring structures are common in organic chemistry. Draw a Lewis structure for each carbon ring structure, including any necessary resonance structures. d. C6H6
Problem 35
Write the electron configuration for oxygen. Then write the Lewis symbol for oxygen and show which electrons from the electron configuration are included in the Lewis symbol.
Problem 37b
Write the Lewis symbol for each atom or ion. b. K+
Problem 37c
Write the Lewis symbol for each atom or ion. c. S
Problem 37d
Write the Lewis symbol for each atom or ion. d. S2-
Problem 39
Write the Lewis symbols for the ions in each ionic compound. d. K2O
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 40d
Write the Lewis symbols for the ions in each ionic compound. d. RbF
Problem 41
Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Mg and S b. Sr and Br c. K and Se d. Al and S
Problem 42
Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Sr and P b. Ba and S c. Sr and Se d. Rb and I
Problem 45
Rubidium iodide has a lattice energy of -617 kJ>mol, while potassium bromide has a lattice energy of -671 kJ>mol. Why is the lattice energy of potassium bromide more exothermic than the lattice energy of rubidium iodide?
Problem 47
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 48
Arrange these compounds in order of increasing magnitude of lattice energy: CaO, NaBr, CsI, BaS.
Problem 49
Use the Born–Haber cycle and data from Appendix IIB, Chapter 9 and this chapter to calculate the lattice energy of LiBr. (ΔHsub for lithium is 138 kJ>mol.)
Problem 50
Use the Born–Haber cycle and data from Appendix IIB and Table 10.3 to calculate the lattice energy of MgO. (ΔHsub for magnesium is 137 kJ/mol; IE1 and IE2 for magnesium are 738 kJ/mol and 1450 kJ/mol, respectively; EA1 and EA2 for O are −141 kJ/mol and 744 kJ/mol, respectively.)
Problem 55a
Write the Lewis structure for each molecule. a. PH3
Problem 55d
Write the Lewis structure for each molecule. d. CH4
Problem 57a
Write the Lewis structure for each molecule. a. SF2
Problem 57b
Write the Lewis structure for each molecule. b. SiH4
Problem 57d
Write the Lewis structure for each molecule. d. CH3SH (C and S central)
Problem 58
Write the Lewis structure for each molecule. a. CH2O b. C2Cl4 c. CH3NH2 d. CFCl3 (C central)
Problem 59a
Determine if a bond between each pair of atoms would be pure covalent, polar covalent, or ionic. a. Ba and O
Problem 61
Refer to Figure 10.10 to estimate the percent ionic character of the Hbr bond.
Problem 62a
Draw the Lewis structure for ClF with an arrow representing the dipole moment.
Problem 62b
Refer to Figure 10.10 to estimate the percent ionic character of the ClF bond.
Problem 64b
Write the Lewis structure for each molecule or ion. b. OH-
Problem 64c
Write the Lewis structure for each molecule or ion. c. BrO-
Problem 65d
Write the Lewis structure for each molecule or ion. d. C2H4
Problem 66a
Write the Lewis structure for each molecule or ion. a. H3COCH3
