QQuestionChemistry
QuestionChemistry
"Predicting the formula of binary ionic compounds
Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions:
Fe^2 +,Cr^4 +,I-,O^2 -"
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Answer
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Step 1:
First, let's write the empirical formula for an ionic compound formed between Fe²⁺ and I⁻ ions. We need to ensure that the compound is neutral, meaning the total positive charge equals the total negative charge. Since Fe²+(aq) has a + 2 charge and I⁻(aq) has a - 1 charge, we need two I⁻ ions to balance the charge of one Fe²⁺ ion, resulting in FeI₂. \text{Fe}^{2 +} + 2\text{I}^{-} \rightarrow \text{FeI}_2
Step 2:
Now, let's consider the compound formed between Cr⁴⁺ and I⁻ ions. Similar to the previous example, we need to balance the charges. With Cr⁴⁺(aq) having a + 4 charge and I⁻(aq) having a - 1 charge, we need four I⁻ ions to balance the charge of one Cr⁴⁺ ion, resulting in CrI₄. \text{Cr}^{4 +} + 4\text{I}^{-} \rightarrow \text{CrI}_4
Step 3:
For the compound formed between Fe²⁺ and O²⁻ ions, we need two O²⁻ ions to balance the charge of one Fe²⁺ ion, resulting in FeO. \text{Fe}^{2 +} + 2\text{O}^{2 -} \rightarrow \text{FeO}
Step 4:
Lastly, let's consider the compound formed between Cr⁴⁺ and O²⁻ ions. We need four O²⁻ ions to balance the charge of one Cr⁴⁺ ion, resulting in CrO₂. \text{Cr}^{4 +} + 4\text{O}^{2 -} \rightarrow \text{CrO}_2
Final Answer
The empirical formulas for the binary ionic compounds are FeI₂, CrI₄, FeO, and CrO₂.
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