Oxidation number of iodine varies from -

Options

A. `-1` to `+1`
B. `-1` to `+7`
C. `+3` to `+5`
D. `-1` to `+5`

Answer

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

### Step-by-Step Solution:

1. **Identify the Atomic Number and Electronic Configuration**:
- The atomic number of iodine (I) is 53.
- Its electronic configuration is:
\[ [Kr] 4d^{10} 5s^2 5p^5 \]

2. **Determine the Valence Electrons**:
- The valence shell of iodine consists of the electrons in the 5s and 5p orbitals.
- Total valence electrons = 2 (from 5s) + 5 (from 5p) = 7 valence electrons.

3. **Identify Possible Oxidation States**:
- Iodine can gain 1 electron to achieve a noble gas configuration, resulting in an oxidation state of -1.
- Alternatively, it can lose all 7 valence electrons, resulting in a +7 oxidation state.

4. **List the Range of Oxidation States**:
- Based on the ability to gain or lose electrons, iodine can exhibit oxidation states ranging from -1 to +7.
- Common oxidation states include: -1, 0, +1, +3, +5, and +7.

5. **Examples of Oxidation States**:
- In molecular iodine (I2), the oxidation state is 0.
- In compounds like IF3, iodine can have an oxidation state of +3.
- In IF7, iodine has an oxidation state of +7.

6. **Conclusion**:
- The oxidation number of iodine varies from -1 to +7.

### Final Answer:
The oxidation number of iodine varies from -1 to +7.

---