QuestionWrite the correct formula for the following compounds. (a) strontium iodide $\mathrm{Sr}^{-} \mathrm{I}_{2}$ (b) iron(II) sulfide $\square$ (c) ammonium sulfite $\square$ (d) sodium chromate $\square$

Studdy Solution

STEP 1

1. The problem involves writing chemical formulas for given compounds.
2. Each compound name corresponds to a specific chemical formula based on the ions involved.
3. The charges of common ions are known and used to balance the formulas.

STEP 2

1. Identify the ions and their charges for each compound.
2. Balance the charges to write the correct chemical formula.

STEP 3

Identify the ions and their charges for each compound.
(a) Strontium iodide: - Strontium ion: $\text{Sr}^{2+}$ - Iodide ion: $\text{I}^-$
(b) Iron(II) sulfide: - Iron(II) ion: $\text{Fe}^{2+}$ - Sulfide ion: $\text{S}^{2-}$
(c) Ammonium sulfite: - Ammonium ion: $\text{NH}_4^+$ - Sulfite ion: $\text{SO}_3^{2-}$
(d) Sodium chromate: - Sodium ion: $\text{Na}^+$ - Chromate ion: $\text{CrO}_4^{2-}$

STEP 4

Balance the charges to write the correct chemical formula.
(a) Strontium iodide: - The formula is $\text{SrI}_2$ because two iodide ions ( $\text{I}^-$ ) are needed to balance one strontium ion ( $\text{Sr}^{2+}$ ).
(b) Iron(II) sulfide: - The formula is $\text{FeS}$ because one iron(II) ion ( $\text{Fe}^{2+}$ ) balances one sulfide ion ( $\text{S}^{2-}$ ).
(c) Ammonium sulfite: - The formula is $(\text{NH}_4)_2\text{SO}_3$ because two ammonium ions ( $\text{NH}_4^+$ ) are needed to balance one sulfite ion ( $\text{SO}_3^{2-}$ ).
(d) Sodium chromate: - The formula is $\text{Na}_2\text{CrO}_4$ because two sodium ions ( $\text{Na}^+$ ) are needed to balance one chromate ion ( $\text{CrO}_4^{2-}$ ).
The correct formulas for the compounds are: (a) Strontium iodide: $\text{SrI}_2$ (b) Iron(II) sulfide: $\text{FeS}$ (c) Ammonium sulfite: $(\text{NH}_4)_2\text{SO}_3$ (d) Sodium chromate: $\text{Na}_2\text{CrO}_4$

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