Name each of the following chlorides. Assuming that the compounds are ionic, what charge is associated with the metallic element in each case? (a) $\mathrm{AgCl},(\mathbf{b}) \mathrm{TiCl}_{4},(\mathbf{c}) \operatorname{Ir} \mathrm{C} 1_{3},\( (d) \)\mathrm{LiCl}$.

Naming the compounds involves identifying the metallic element and the non-metallic element (in this case, chlorine) and adding the suffix "-ide" to the non-metallic element. For some compounds, it is important to mention the oxidation state of the metallic element. (a) \(\mathrm{AgCl}\): Silver Chloride (b) \(\mathrm{TiCl}_{4}\): Titanium(IV) Chloride (c) \(\mathrm{IrCl}_{3}\): Iridium(III) Chloride (d) \(\mathrm{LiCl}\): Lithium Chloride

The charge associated with the metallic element can be determined by understanding the charges present on the non-metallic element (in this case, chlorine) and using the oxidation state of the metallic element. (a) Silver Chloride (AgCl): Chlorine has a charge of -1, so silver (Ag) must have a charge of +1 to balance the charges. The charge associated with Ag is +1. (b) Titanium(IV) Chloride (TiCl\(_{4}\)): Chlorine has a charge of -1, and there are four chlorine atoms, resulting in a total charge of -4. The oxidation state of titanium is IV (4), resulting in a charge of +4. The charge associated with Ti is +4. (c) Iridium(III) Chloride (IrCl\(_{3}\)): Chlorine has a charge of -1, and there are three chlorine atoms, resulting in a total charge of -3. The oxidation state of iridium is III (3), resulting in a charge of +3. The charge associated with Ir is +3. (d) Lithium Chloride (LiCl): Chlorine has a charge of -1, so lithium (Li) must have a charge of +1 to balance the charges. The charge associated with Li is +1.