91Ó°ÊÓ

Determine the number of each type of atom in each formula. $$ \text { a. }\mathrm{Ca}\left(\mathrm{NO}_{2}\right)_{2} \quad \text { b. } \mathrm{CuSO}_{4} \quad \text { c. }\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3} \quad \text { d. } \mathrm{Mg}\left(\mathrm{HCO}_{3}\right)_{2} $$

Write an electron configuration for \(N .\) Then write a Lewis symbol for \(N\) and show which electrons from the electron configuration are included in the Lewis symbol.

Write an electron configuration for \(\mathrm{N}\) . Then write a Lewis symbol fo \(\mathrm{Ne}\) and show which electrons from the electron configuration are included in the Lewis symbol.

Write a Lewis symbol for each atom or ion. $$ \text { a. }\mathrm{s}^{2-} \quad \text { b. } \mathrm{Mg} \quad \text { c. } \mathrm{Mg}^{2+} \quad \text { d. } \mathrm{P} $$

Write the Lewis symbols that represent the ions in each ionic compound. $$ { a. NaF }\quad \text { b. } \mathrm{CaO} \quad \text { c. SrBr }_{2} \quad \text { d. } \mathrm{K}_{2} \mathrm{O} $$

Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. $$ \text { a. }\mathrm{Sr} \text { and } \mathrm{Se} \quad \text { b. } \mathrm{Ba} \text { and } \mathrm{Cl} \quad \text { c.} \mathrm{Na} \text { and } \mathrm{S} \quad \text { d. } \mathrm{Al} \text { and } \mathrm{O} $$

Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. $$ \text { a. }\mathrm{Ca} \text { and } \mathrm{N} \quad \text { b. } \mathrm{Mg} \text { and } \mathrm{I} \quad \text { c. }\mathrm{Cand} \mathrm{S} \quad \text { d. } \mathrm{Cs} \text { and } \mathrm{F} $$

Rubidium iodide has a lattice energy of \(-617 \mathrm{k} / \mathrm{mol},\) while potassium bromide has a lattice energy of \(-671 \mathrm{kJ} / \mathrm{mol}\) . Why is the lattice energy of potassium bromide more exothermic than the lattice energy of rubidium iodide?

Write a formula for the ionic compound that forms between each pai of clements. \(\begin{array}{ll}{\text { a. calcium and oxygen }} & {\text { b. zinc and sulfur }} \\ {\text { c. rubidium and bromine }} & {\text { d. aluminum and oxygen }}\end{array}\)

Write a formula for the ionic compound that forms between each pair of elements. \(\begin{array}{ll}{\text { a. silver and chlorine }} & {\text { b. sodium and sulfur }} \\ {\text { c. aluminum and sulfur }} & {\text { d. potassium and chlorine }}\end{array}\)