The oxidation number of N and Cl in `NOClO_(4)` respectively are

Options

A. `+2 " and " +7`
B. `+3 " and " +7`
C. `-3 " and " +5`
D. `+2 " and " -7`

Explanation

To determine the oxidation numbers of nitrogen (N) and chlorine (Cl) in the compound NOClO₄, we can follow these steps:

### Step 1: Identify the oxidation states of known elements
In the compound NOClO₄, we know the oxidation states of oxygen (O) and the overall charge of the molecule. Oxygen typically has an oxidation state of -2.

### Step 2: Write the formula for the oxidation state of nitrogen (N)
The compound can be viewed as consisting of NO⁺ and ClO₄⁻.
For NO⁺:
Let the oxidation state of nitrogen be \( x \).
The oxidation state equation for NO is:
\[ x + (-2) = +1 \]
This simplifies to:
\[ x - 2 = 1 \]
\[ x = 1 + 2 \]
\[ x = +3 \]
Thus, the oxidation state of nitrogen (N) in NOClO₄ is +3.

### Step 3: Write the formula for the oxidation state of chlorine (Cl)
Now, let's analyze ClO₄⁻:
Let the oxidation state of chlorine be \( y \).
The oxidation state equation for ClO₄ is:
\[ y + 4(-2) = -1 \]
This simplifies to:
\[ y - 8 = -1 \]
\[ y = -1 + 8 \]
\[ y = +7 \]
Thus, the oxidation state of chlorine (Cl) in NOClO₄ is +7.

### Step 4: Summarize the oxidation states
From our calculations:
- The oxidation state of nitrogen (N) in NOClO₄ is +3.
- The oxidation state of chlorine (Cl) in NOClO₄ is +7.

### Final Answer
The oxidation numbers of N and Cl in NOClO₄ are +3 and +7, respectively.

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