Name each of the following compounds: a. \(\mathrm{CsF}\) b. \(\mathrm{Li}_{7} \mathrm{~N}\) c. \(\mathrm{Ag}_{2} \mathrm{~S}\) d. \(\mathrm{MnO}_{2}\) e. \(\mathrm{TiO}_{2}\) f. \(\mathrm{Sr}_{3} \mathrm{P}_{2}\)

We will identify the elements in each compound and their charges based on their location in the periodic table. Remember that elements in Group 1 have a charge of +1, Group 2 have a charge of +2, and so on. Non-metal elements typically have negative charges based on the number of electrons they need to fill their outer energy level. a. \(\mathrm{CsF}\): Cesium (Cs, Group 1, charge of +1) and Fluorine (F, Group 17, charge of -1) b. \(\mathrm{Li}_{7} \mathrm{~N}\): Lithium (Li, Group 1, charge of +1) and Nitrogen (N, Group 15, charge of -3) c. \(\mathrm{Ag}_{2} \mathrm{~S}\): Silver (Ag, transition metal, charge of +1) and Sulfur (S, Group 16, charge of -2) d. \(\mathrm{MnO}_{2}\): Manganese (Mn, transition metal, charge of +4) and Oxygen (O, Group 16, charge of -2) e. \(\mathrm{TiO}_{2}\): Titanium (Ti, transition metal, charge of +4) and Oxygen (O, Group 16, charge of -2) f. \(\mathrm{Sr}_{3} \mathrm{P}_{2}\): Strontium (Sr, Group 2, charge of +2) and Phosphorus (P, Group 15, charge of -3)

Now, we will name each compound accordingly. We will name the metal first, followed by the non-metal with an "-ide" ending. a. \(\mathrm{CsF}\): Cesium fluoride b. \(\mathrm{Li}_{7} \mathrm{~N}\): Lithium nitride c. \(\mathrm{Ag}_{2} \mathrm{~S}\): Silver sulfide d. \(\mathrm{MnO}_{2}\): Manganese(IV) oxide (Note: The roman numeral "IV" indicates the charge of the transition metal, Mn) e. \(\mathrm{TiO}_{2}\): Titanium(IV) oxide (Note: The roman numeral "IV" indicates the charge of the transition metal, Ti) f. \(\mathrm{Sr}_{3} \mathrm{P}_{2}\): Strontium phosphide