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.

Write the Lewis symbol for each atom or ion. b. K⁺

Write the Lewis symbol for each atom or ion. c. S

Write the Lewis symbol for each atom or ion. d. S2-

Write the Lewis symbols for the ions in each ionic compound. d. K₂O

Write the Lewis symbols for the ions in each ionic compound. a. SrO d. RbF

Write the Lewis symbols for the ions in each ionic compound. b. Li₂S

Write the Lewis symbols for the ions in each ionic compound. c. CaI₂

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

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

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?

The lattice energy of CsF is -744 kJ/mol, whereas that of BaO is -3029 kJ/mol. Explain this large difference in lattice energy.

Arrange these compounds in order of increasing magnitude of lattice energy: CaO, NaBr, CsI, BaS.

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.)

Use the Born–Haber cycle and data from Appendix IIB and Table 10.3 to calculate the lattice energy of MgO. (ΔH_sub 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.)

Write the Lewis structure for each molecule. a. PH₃ b. SCl₂ c. HI

Write the Lewis structure for each molecule. d. CH₄

Write the Lewis structure for each molecule. a. SF₂

Write the Lewis structure for each molecule. b. SiH₄

Write the Lewis structure for each molecule. d. CH₃SH (C and S central)

Write the Lewis structure for each molecule. a. CH₂O b. C₂Cl₄ c. CH₃NH₂ d. CFCl₃ (C central)

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

Refer to Figure 10.10 to estimate the percent ionic character of the Hbr bond.

Draw the Lewis structure for ClF with an arrow representing the dipole moment.

Refer to Figure 10.10 to estimate the percent ionic character of the ClF bond.

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

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

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