Oxidation number of nitrogen can be -

Options

A. From + 5 to -3
B. From -5 to -3
C. From -5 to +3
D. From + 10 to +6

Answer

To determine the oxidation number of nitrogen and its possible range, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Atomic Number and Electron Configuration**:
- The atomic number of nitrogen (N) is 7.
- Its electronic configuration is 1s² 2s² 2p³.

2. **Determine Valence Electrons**:
- Nitrogen has 5 valence electrons (2 in the 2s subshell and 3 in the 2p subshell).

3. **Assess Possible Oxidation States**:
- Nitrogen can either gain or lose electrons to achieve a stable electronic configuration.
- If nitrogen gains 3 electrons, it will have a total of 8 electrons in its outer shell (2s² 2p⁶), achieving a noble gas configuration. This results in an oxidation state of -3.
- If nitrogen loses all 5 valence electrons, it will have a positive charge of +5.

4. **Examples of Oxidation States**:
- In ammonia (NH₃), nitrogen has an oxidation state of -3. Here, hydrogen is +1, and since there are three hydrogens, the total contribution from hydrogen is +3, making nitrogen -3 to balance the overall charge to zero.
- In nitric acid (HNO₃), nitrogen has an oxidation state of +5. Here, hydrogen is +1, and each oxygen is -2 (total of -6 from three oxygens). To balance the overall charge to zero, nitrogen must be +5.

5. **Conclusion on the Range of Oxidation States**:
- Therefore, the oxidation number of nitrogen can vary from -3 to +5.

### Final Answer:
The oxidation number of nitrogen can be -3, 0, +1, +2, +3, +4, or +5, with common states being -3 in ammonia and +5 in nitric acid.

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