QQuestionChemistry
QuestionChemistry
"Which formula/name pair is incorrect?
A. FeSO₄ - iron(II) sulfate
B. Fe₂(SO₃)₃ - iron(III) sulfite
C. FeS - iron(II) sulfide
D. FeSO₃ - iron(II) sulfite
E. Fe₂(SO ₄)₃ - iron(III) sulfide"
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Answer
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Step 1: Identify the correct formula-name pairs.
Iron can have oxidation states of + 2 or + 3. When it has an oxidation state of + 2, it is called iron(II), and when it has an oxidation state of + 3, it is called iron(III). Sulfate has a charge of - 2, sulfite has a charge of - 2, and sulfide has a charge of - 2. To balance the charges, we need to ensure that the sum of the oxidation states of iron equals the total charge on the sulfate, sulfite, or sulfide ion.
Step 2: Analyze each option.
A. FeSO₄ - iron(II) sulfate: Correct. The sulfate ion has a charge of - 2, so iron must have an oxidation state of + 2 to balance the charge, which is iron(II). B. Fe₂(SO₃)₃ - iron(III) sulfite: Correct. The sulfite ion has a charge of - 2, so three sulfite ions will have a total charge of - 6. Two iron atoms with an oxidation state of + 3 will have a total charge of + 6, balancing the charge. C. FeS - iron(II) sulfide: Correct. The sulfide ion has a charge of - 2, so iron must have an oxidation state of + 2 to balance the charge, which is iron(II).
Final Answer
The incorrect formula-name pair is FeSO₃ - iron(II) sulfite.
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