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

Chemistry

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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

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Question

### 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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