Name each of the following compounds: a. CsF b. \(\mathrm{Li}_{3} \mathrm{N}\) c. \(A g_{2} S\) d. \(\mathrm{MnO}_{2}\) e. \(\mathrm{TiO}_{2}\) f. \(\mathrm{Sr}_{3} \mathrm{P}_{2}\)

First, we will need to know the symbols of the chemical elements making up each compound. a. CsF : Cs is Cesium, F is Fluorine b. Li3N : Li is Lithium, N is Nitrogen c. Ag2S : Ag is Silver, S is Sulfur d. MnO2 : Mn is Manganese, O is Oxygen e. TiO2 : Ti is Titanium, O is Oxygen f. Sr3P2 : Sr is Strontium, P is Phosphorus

Compounds consisting of metals and non-metals typically form ionic bonds. Metals are elements from groups 1, 2 and 13-15 of the periodic table, while non-metals are elements from groups 14-18. In each case given, the compounds are made up of a metal and a non-metal, so they are ionic compounds.

Naming ionic compounds involves writing the name of the metal followed by the name of the non-metal with the ending changed to -ide. If the metal has more than one oxidation state (charge), we use a Roman numeral to indicate the oxidation state. a. CsF -> Cesium Fluoride b. Li3N -> Lithium Nitride c. Ag2S -> Silver Sulfide (Since Silver has only one common oxidation state, +1, no Roman numeral is needed) d. MnO2 -> Manganese (IV) Oxide (Manganese has a +4 oxidation state, as it binds to 2 Oxygens with -2 charge each) e. TiO2 -> Titanium (IV) Oxide (Titanium has a +4 oxidation state, as it binds to 2 Oxygens with -2 charge each) f. Sr3P2 -> Strontium Phosphide The names of the compounds are: a. Cesium Fluoride b. Lithium Nitride c. Silver Sulfide d. Manganese (IV) Oxide e. Titanium (IV) Oxide f. Strontium Phosphide