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8. Assign oxidation numbers to each element in the following compounds or polyatomic ions. Fe2O3 SO3 РО Cr,0,2- CuSO4

8. Assign oxidation numbers to each element in the following compounds or polyatomic ions. Fe2O3 SO3 РО Cr,0,2- CuSO4

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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### Assigning Oxidation Numbers Assignment: Assign oxidation numbers to each element in the following compounds or polyatomic ions. 1. **Magnesium Bromide (MgBr₂)** 2. **Iron(III) Oxide (Fe₂O₃)** 3. **Sulfur Trioxide (SO₃)** 4. **Phosphate Ion (PO₄³⁻)** 5. **Dichromate Ion (Cr₂O₇²⁻)** 6. **Copper(II) Sulfate (CuSO₄)** ### Detailed Explanation To solve these, use the rules for assigning oxidation numbers: 1. The oxidation number of an atom in a neutral substance that contains atoms of only one element is zero. 2. The oxidation number of a monatomic ion is equal to the charge of the ion. 3. Oxygen is usually assigned an oxidation number of -2 unless it is in a peroxide, where it is -1, or bonded to fluorine, where it can vary. 4. Hydrogen is +1 when bonded to non-metals and -1 when bonded to metals. 5. The sum of the oxidation numbers in a neutral compound is zero. The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion. #### Examples: 1. **MgBr₂**: - Mg: +2 - Br: -1 (each Br in Br₂, so it multiplies by 2 to match Mg). 2. **Fe₂O₃**: - Fe: +3 (each Fe) - O: -2 (each O). 3. **SO₃**: - S: +6. - O: -2 (each O). 4. **PO₄³⁻**: - P: +5. - O: -2 (each O). - Sum must equal the ion charge of -3. 5. **Cr₂O₇²⁻**: - Cr: +6 (each Cr). - O: -2 (each O). - Sum must equal the ion charge of -2. 6. **CuSO₄**: - Cu: +2. - S: +6. - O: -2 (each O). By following these steps, you can assign the oxidation numbers to each element in the compounds and
Transcribed Image Text:### Assigning Oxidation Numbers Assignment: Assign oxidation numbers to each element in the following compounds or polyatomic ions. 1. **Magnesium Bromide (MgBr₂)** 2. **Iron(III) Oxide (Fe₂O₃)** 3. **Sulfur Trioxide (SO₃)** 4. **Phosphate Ion (PO₄³⁻)** 5. **Dichromate Ion (Cr₂O₇²⁻)** 6. **Copper(II) Sulfate (CuSO₄)** ### Detailed Explanation To solve these, use the rules for assigning oxidation numbers: 1. The oxidation number of an atom in a neutral substance that contains atoms of only one element is zero. 2. The oxidation number of a monatomic ion is equal to the charge of the ion. 3. Oxygen is usually assigned an oxidation number of -2 unless it is in a peroxide, where it is -1, or bonded to fluorine, where it can vary. 4. Hydrogen is +1 when bonded to non-metals and -1 when bonded to metals. 5. The sum of the oxidation numbers in a neutral compound is zero. The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion. #### Examples: 1. **MgBr₂**: - Mg: +2 - Br: -1 (each Br in Br₂, so it multiplies by 2 to match Mg). 2. **Fe₂O₃**: - Fe: +3 (each Fe) - O: -2 (each O). 3. **SO₃**: - S: +6. - O: -2 (each O). 4. **PO₄³⁻**: - P: +5. - O: -2 (each O). - Sum must equal the ion charge of -3. 5. **Cr₂O₇²⁻**: - Cr: +6 (each Cr). - O: -2 (each O). - Sum must equal the ion charge of -2. 6. **CuSO₄**: - Cu: +2. - S: +6. - O: -2 (each O). By following these steps, you can assign the oxidation numbers to each element in the compounds and
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