How do you account for the strong reducing power of lithium in aqueous solution?

Explanation

To account for the strong reducing power of lithium in aqueous solution, we can break down the explanation into three main steps: sublimation, ionization, and hydration. Here’s a step-by-step solution:

### Step 1: Sublimation
- **Explanation**: The first step involves the sublimation of lithium. This means converting lithium from its solid state to a gaseous state. The energy required for this process is known as sublimation energy.
- **Conclusion**: The sublimation energy is similar for all alkali metals, including lithium, and does not significantly contribute to its strong reducing power.

### Step 2: Ionization Energy
- **Explanation**: The second step is the ionization of gaseous lithium, where lithium loses one electron to form a Li⁺ ion. This process requires energy, known as ionization energy (IE). For lithium, the ionization energy is relatively high due to its small atomic size, which means the outermost electron is held tightly by the nucleus.
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