Answer
$(a) KClO$
$(b) Ag_2CrO_4$
$(c) Fe_2(CO_3)_3$
Work Step by Step
1. Use the table 2.5 (Page 63) to find the formulas for each second name.
(a) Hypochlorite: $ClO^-$
(b) Chromate: $CrO_4^{2-}$
(c) Carbonate: $CO_3^{2-}$
2. Now, write the formula for the metal ion in the first name, and then the ion identified on the first step:
(a) $K^+$ and $ClO^-$
(b) $Ag^+$ and $CrO_4^{2-}$
(c) $Fe^{3+}$ and $CO_3^{2-}$
3. Now, put them together, not forgeting to adjust the charge by adding more ions.
(a) Charges are already equal: $KClO$
(b) We have to put one extra positive charge: +1 $Ag^+$: $Ag_2CrO_4$.
(c) To fix the charge, we will have to put 2 irons (III) and 3 carbonates: $Fe_2(CO_3)_3$ so that the overall charge is neutral.
