In `I_(3)^(-)` , Lewis base is

Options

A. `I_(2)`
B. `I_(2)^(-)`
C. `I_(2)^(+)`
D. `I^(-)`

Explanation

To determine the Lewis base in the ion \( I_3^- \), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Components of \( I_3^- \)**:
- The ion \( I_3^- \) consists of three iodine atoms. It can also be represented as \( I_2I^- \), indicating that there are two neutral iodine atoms and one negatively charged iodine atom.

2. **Understand the Concept of Lewis Bases**:
- A Lewis base is defined as a species that can donate a pair of electrons to form a covalent bond. This typically involves atoms with lone pairs of electrons.

3. **Analyze the Structure of \( I_3^- \)**:
- In \( I_3^- \), the central atom is one of the iodine atoms. The other two iodine atoms are bonded to it. The negatively charged iodine \( I^- \) has an extra electron, which contributes to the overall charge of the ion.

4. **Determine the Lone Pairs**:
- The central iodine atom in \( I_3^- \) has three lone pairs of electrons. The two surrounding iodine atoms are bonded to the central atom through sigma bonds.

5. **Identify the Lewis Base**:
- The negatively charged iodine atom \( I^- \) acts as a Lewis base because it can donate its lone pair of electrons to form bonds with other atoms or ions. In this case, it participates in the formation of the \( I_3^- \) ion by donating its lone pair to the central iodine atom.

6. **Conclusion**:
- Therefore, in \( I_3^- \), the Lewis base is the iodine atom that carries the negative charge, \( I^- \).

### Final Answer:
The Lewis base in \( I_3^- \) is \( I^- \).