QuestionPredicting the formula of binary ionic
Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions: $\mathrm{Fe}^{2+}, \mathrm{V}^{5+}, \mathrm{F}^{-}, \mathrm{S}^{2-}$ $\square$

Studdy Solution

STEP 1

Assumptions
1. We have four ions to work with: $\mathrm{Fe}^{2+}$ , $\mathrm{V}^{5+}$ , $\mathrm{F}^{-}$ , and $\mathrm{S}^{2-}$ .
2. Binary ionic compounds are formed by combining a cation (positively charged ion) with an anion (negatively charged ion).
3. The empirical formula of a compound is the simplest whole-number ratio of ions that results in a neutral compound.
4. We need to ensure that the total positive charge equals the total negative charge in each compound.

STEP 2

Form a compound using $\mathrm{Fe}^{2+}$ and $\mathrm{F}^{-}$ .
The charges are $\mathrm{Fe}^{2+}$ (2+) and $\mathrm{F}^{-}$ (1-). To balance the charges, we need two fluoride ions for each iron ion.
Empirical formula: $\mathrm{FeF}_2$

STEP 3

Form a compound using $\mathrm{Fe}^{2+}$ and $\mathrm{S}^{2-}$ .
The charges are $\mathrm{Fe}^{2+}$ (2+) and $\mathrm{S}^{2-}$ (2-). The charges are already balanced with one of each ion.
Empirical formula: $\mathrm{FeS}$

STEP 4

Form a compound using $\mathrm{V}^{5+}$ and $\mathrm{F}^{-}$ .
The charges are $\mathrm{V}^{5+}$ (5+) and $\mathrm{F}^{-}$ (1-). To balance the charges, we need five fluoride ions for each vanadium ion.
Empirical formula: $\mathrm{VF}_5$

STEP 5

Form a compound using $\mathrm{V}^{5+}$ and $\mathrm{S}^{2-}$ .
The charges are $\mathrm{V}^{5+}$ (5+) and $\mathrm{S}^{2-}$ (2-). To balance the charges, we need two vanadium ions and five sulfide ions, but the simplest ratio is achieved with two vanadium ions and three sulfide ions.
Empirical formula: $\mathrm{V}_2\mathrm{S}_5$
These are the empirical formulas for four binary ionic compounds that can be formed from the given ions:
1. $\mathrm{FeF}_2$
2. $\mathrm{FeS}$
3. $\mathrm{VF}_5$
4. $\mathrm{V}_2\mathrm{S}_5$

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