The oxidation state of nitrogen is highest in

Options

A. `N_(3)H`
B. `NH_(3)`
C. `NH_(2)OH`
D. `N_(2)H_(4)`

Explanation

To determine the highest oxidation state of nitrogen in the given compounds, we will analyze each compound step by step.

### Step 1: Analyze the Compound N3H
1. Let the oxidation state of nitrogen be \( x \).
2. There are 3 nitrogen atoms, so their contribution is \( 3x \).
3. There is 1 hydrogen atom with a charge of +1.
4. The total charge of the molecule is neutral (0).
5. Therefore, we can set up the equation:
\[ 3x + 1 = 0 \]
6. Solving for \( x \):
\[ 3x = -1 \quad \Rightarrow \quad x = -\frac{1}{3} \]

### Step 2: Analyze the Compound NH3
1. Let the oxidation state of nitrogen be \( x \).
2. There is 1 nitrogen atom, contributing \( x \).
3. There are 3 hydrogen atoms, contributing \( 3 \times (+1) = +3 \).
4. The total charge is neutral (0).
5. The equation is:
\[ x + 3 = 0 \]
6. Solving for \( x \):
\[ x = -3 \]

### Step 3: Analyze the Compound NH2OH
1. Let the oxidation state of nitrogen be \( x \).
2. There is 1 nitrogen atom, contributing \( x \).
3. There are 2 hydrogen atoms contributing \( 2 \times (+1) = +2 \).
4. There is 1 oxygen atom with a charge of -2.
5. The total charge is neutral (0).
6. The equation is:
\[ x + 2 - 2 + 1 = 0 \]
7. Simplifying gives:
\[ x + 1 = 0 \quad \Rightarrow \quad x = -1 \]

### Step 4: Analyze the Compound N2H4
1. Let the oxidation state of nitrogen be \( x \).
2. There are 2 nitrogen atoms, contributing \( 2x \).
3. There are 4 hydrogen atoms contributing \( 4 \times (+1) = +4 \).
4. The total charge is neutral (0).
5. The equation is:
\[ 2x + 4 = 0 \]
6. Solving for \( x \):
\[ 2x = -4 \quad \Rightarrow \quad x = -2 \]

### Summary of Oxidation States
- For N3H: \( -\frac{1}{3} \)
- For NH3: \( -3 \)
- For NH2OH: \( -1 \)
- For N2H4: \( -2 \)

### Conclusion
The highest oxidation state of nitrogen among the compounds is \( -\frac{1}{3} \) in N3H.

### Final Answer
The oxidation state of nitrogen is highest in **N3H**.

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