Indicate whether the following conversions represent an oxidation, a reduction or none (neither oxidation nor reduction).
(i) `HClO_(3) ` to `HClO_(4) " " ` (ii) `NH_(4)^(+)` to `NH_(3)`
(iii) `NO_(2)` to `N_(2)O_(4) " " ` (iv) `HSO_(3)^(-)` to `SO_(4)^(2-)`
(v) `H_(2)O_(2)` to `H_(2)O`

Options

A. `{:(," (i)"," (ii)","(iii)","(iv)"," (v)",),(,"Oxidation","Reduction","None","None","Oxidation",):}`
B. `{:(," (i)"," (ii)","(iii)"," (iv)"," (v)",),(,"Oxidation","None","None","Oxidation","Reduction",):}`
C. `{:(," (i)"," (ii)","(iii)"," (iv)"," (v)",),(,"Reduction","Oxidation","Reduction","None","Reduction",):}`
D. `{:(," (i)"," (ii)","(iii)"," (iv)"," (v)",),(,"Oxidation","Reduction","None","Reduction","Reduction",):}`

Explanation

To determine whether the conversions represent oxidation, reduction, or neither, we need to analyze the changes in oxidation states of the elements involved in each conversion. Let's go through each conversion step by step.

### Step 1: Analyze the conversion of `HClO3` to `HClO4`
1. **Identify the oxidation states:**
- In `HClO3`:
- H = +1
- O = -2 (3 O atoms contribute -6)
- Let the oxidation state of Cl = X
- Equation: +1 + X - 6 = 0 → X = +5
- In `HClO4`:
- H = +1
- O = -2 (4 O atoms contribute -8)
- Let the oxidation state of Cl = Y
- Equation: +1 + Y - 8 = 0 → Y = +7

2. **Determine the change:**
- Cl changes from +5 to +7, indicating an increase in oxidation state.
- This represents **oxidation**.

### Step 2: Analyze the conversion of `NH4+` to `NH3`
1. **Identify the oxidation states:**
- In `NH4+`:
- H = +1 (4 H atoms contribute +4)
- Let the oxidation state of N = X
- Equation: X + 4 = +1 → X = -3
- In `NH3`:
- H = +1 (3 H atoms contribute +3)
- Let the oxidation state of N = Y
- Equation: Y + 3 = 0 → Y = -3

2. **Determine the change:**
- N remains at -3 in both cases.
- There is **no change** in oxidation state, indicating **neither oxidation nor reduction**.

### Step 3: Analyze the conversion of `NO2` to `N2O4`
1. **Identify the oxidation states:**
- In `NO2`:
- O = -2 (2 O atoms contribute -4)
- Let the oxidation state of N = X
- Equation: X - 4 = 0 → X = +4
- In `N2O4`:
- O = -2 (4 O atoms contribute -8)
- Let the oxidation state of N = Y
- Equation: 2Y - 8 = 0 → 2Y = +8 → Y = +4

2. **Determine the change:**
- N remains at +4 in both cases.
- There is **no change** in oxidation state, indicating **neither oxidation nor reduction**.

### Step 4: Analyze the conversion of `HSO3-` to `SO4^2-`
1. **Identify the oxidation states:**
- In `HSO3-`:
- H = +1
- O = -2 (3 O atoms contribute -6)
- Let the oxidation state of S = X
- Equation: +1 + X - 6 = -1 → X = +4
- In `SO4^2-`:
- O = -2 (4 O atoms contribute -8)
- Let the oxidation state of S = Y
- Equation: Y - 8 = -2 → Y = +6

2. **Determine the change:**
- S changes from +4 to +6, indicating an increase in oxidation state.
- This represents **oxidation**.

### Step 5: Analyze the conversion of `H2O2` to `H2O`
1. **Identify the oxidation states:**
- In `H2O2`:
- H = +1 (2 H atoms contribute +2)
- O = -1 (2 O atoms contribute -2)
- Let the oxidation state of O = X (in peroxide, O is -1).
- In `H2O`:
- H = +1 (2 H atoms contribute +2)
- O = -2 (1 O atom contributes -2)

2. **Determine the change:**
- O changes from -1 in H2O2 to -2 in H2O, indicating a decrease in oxidation state.
- This represents **reduction**.

### Summary of Results:
- (i) `HClO3` to `HClO4`: **Oxidation**
- (ii) `NH4+` to `NH3`: **Neither**
- (iii) `NO2` to `N2O4`: **Neither**
- (iv) `HSO3-` to `SO4^2-`: **Oxidation**
- (v) `H2O2` to `H2O`: **Reduction**

### Final Answers:
1. Oxidation
2. Neither
3. Neither
4. Oxidation
5. Reduction