Name each of the following compounds. Assume the acids are dissolved in water. a. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) b. \(\mathrm{NH}_{4} \mathrm{NO}_{2}\) c. \(\mathrm{Co}_{2} \mathrm{S}_{3}\) d. ICl e. \(\mathrm{Pb}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) f. \(\mathrm{KClO}_{3}\) g. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) h. \(\mathrm{Sr}_{3} \mathrm{N}_{2}\) i. \(\mathrm{Al}_{2}\left(\mathrm{SO}_{3}\right)_{3}\) j. \(\mathrm{SnO}_{2}\) k. \(\mathrm{Na}_{2} \mathrm{CrO}_{4}\) I. HClo

Determine if the compound is covalent (composed of nonmetals) or ionic (composed of metals and nonmetals or polyatomic ions).

For a covalent compound, use Greek numerical prefixes to indicate the number of atoms present for each element and add the suffix -ide to the second element: Example: ICl -> iodine monochloride

For ionic compounds, name the cation first and then the anion. If the cation is a metal with different possible charges, include the charge as a Roman numeral in parentheses. For polyatomic ions, use their common names: Example: \(\mathrm{KClO}_{3}\) -> potassium chlorate

For acids, use the prefix hydro- if the anion ends with -ide, and use the prefixes -ic and -ous for anions ending with -ate and -ite, respectively. For bases, simply name the ionic compound: Example: \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) -> acetic acid Solution: a. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\): acetic acid b. \(\mathrm{NH}_{4} \mathrm{NO}_{2}\): ammonium nitrite c. \(\mathrm{Co}_{2} \mathrm{S}_{3}\): cobalt(III) sulfide d. ICl: iodine monochloride e. \(\mathrm{Pb}_{3}\left(\mathrm{PO}_{4}\right)_{2}\): lead(II) phosphate f. \(\mathrm{KClO}_{3}\): potassium chlorate g. \(\mathrm{H}_{2} \mathrm{SO}_{4}\): sulfuric acid h. \(\mathrm{Sr}_{3} \mathrm{N}_{2}\): strontium nitride i. \(\mathrm{Al}_{2}\left(\mathrm{SO}_{3}\right)_{3}\): aluminum sulfite j. \(\mathrm{SnO}_{2}\): tin(IV) oxide k. \(\mathrm{Na}_{2} \mathrm{CrO}_{4}\): sodium chromate l. HClo: hypochlorous acid