Li has the maximum value of ionisation potential among alkali metals i.e. lithium has the minimum tendency to ionise to give `Li^(+)` ion. Thus, in aq. Solution lithium is-

Options

A. Strongest reducing agent
B. Poorest reducing agent
C. Strongest oxidising agent
D. All

Answer

To solve the question regarding lithium's ionization potential and its behavior in aqueous solution, we can break down the solution into several steps:

### Step-by-Step Solution:

1. **Understanding Ionization Potential**:
- Ionization potential (or ionization energy) is the energy required to remove an electron from an isolated atom in its gaseous state.
- Among the alkali metals, lithium (Li) has the highest ionization potential, meaning it requires more energy to remove an electron compared to other alkali metals.

**Hint**: Remember that higher ionization potential indicates a stronger hold on the outer electron.

2. **Position of Lithium in the Alkali Metals**:
- Lithium is located at the top of the alkali metal group in the periodic table.
- Alkali metals have one electron in their outermost shell, which they tend to lose easily to form positive ions (cations).

**Hint**: Alkali metals are known for their reactivity due to their tendency to lose one electron.

3. **Effect of Atomic Size**:
- Lithium has a relatively small atomic size compared to other alkali metals.
- The smaller size results in a stronger attraction between the nucleus and the outer electron, making it harder to remove that electron.

**Hint**: Smaller atomic size generally leads to stronger nuclear attraction on the outermost electron.

4. **Oxidation and Reduction**:
- When lithium loses an electron, it undergoes oxidation (Li → Li⁺ + e⁻).
- Since lithium has a high ionization potential, it does not easily lose its electron, indicating that it is a poor reducing agent.

**Hint**: A poor reducing agent is one that does not readily oxidize itself.

5. **Conclusion on Lithium's Behavior in Aqueous Solution**:
- Because lithium is a poor reducing agent, it tends to act as a strong oxidizing agent in aqueous solutions.
- This means that while it does not easily lose electrons, it can facilitate oxidation reactions by accepting electrons from other substances.

**Hint**: The relationship between reducing and oxidizing agents is crucial; a substance that is a poor reducer can often act as a good oxidizer.

### Final Answer:
In aqueous solution, lithium is a poor reducing agent and a strong oxidizing agent.