Question

give formulas for the following ionic compounds: 22. cobalt(ii) nitrate (no2) 23. silver nitride 24. aluminum acetate 25. barium sulfate 26. cuprous chromate

Explanation:

Step1: Recall ion - charges

Cobalt(II) has a charge of $Co^{2 +}$, and nitrate has a charge of $NO_{3}^{-}$.

Step2: Balance charges

To balance the charges in an ionic compound, we need 2 nitrate ions for every cobalt(II) ion. So the formula is $Co(NO_{3})_{2}$.
Silver has a charge of $Ag^{+}$, and nitride has a charge of $N^{3 -}$. To balance the charges, we need 3 silver ions for every nitride ion. The formula is $Ag_{3}N$.
Aluminum has a charge of $Al^{3+}$, and acetate has a charge of $C_{2}H_{3}O_{2}^{-}$. To balance the charges, we need 3 acetate ions for every aluminum ion. The formula is $Al(C_{2}H_{3}O_{2})_{3}$.
Barium has a charge of $Ba^{2+}$, and sulfate has a charge of $SO_{4}^{2 -}$. The charges are already balanced in a 1:1 ratio, so the formula is $BaSO_{4}$.
Cuprous has a charge of $Cu^{+}$, and chromate has a charge of $CrO_{4}^{2 -}$. To balance the charges, we need 2 cuprous ions for every chromate ion. The formula is $Cu_{2}CrO_{4}$.

Answer:

1. $Co(NO_{3})_{2}$
2. $Ag_{3}N$
3. $Al(C_{2}H_{3}O_{2})_{3}$
4. $BaSO_{4}$
5. $Cu_{2}CrO_{4}$