Boric acid is weak monobasic acid and acts as Lewis acid

Explanation

### Step-by-Step Solution

1. **Identify the Chemical Nature of Boric Acid**:
- Boric acid has the chemical formula H₃BO₃. It consists of a boron atom bonded to three hydroxyl (OH) groups.

**Hint**: Remember the formula of boric acid and its structural components.

2. **Understand the Concept of Acidity**:
- An acid is typically defined as a substance that can donate protons (H⁺ ions) in solution. However, boric acid behaves differently.

**Hint**: Recall the general definition of acids and how they typically behave in water.

3. **Analyze the Electron Configuration of Boron**:
- The boron atom in boric acid has only six electrons in its valence shell, making it electron-deficient. This deficiency means that boron can accept electrons rather than donate protons.

**Hint**: Consider the electron configuration and how it relates to the acidity of the compound.

4. **Boric Acid as a Weak Monobasic Acid**:
- When boric acid is dissolved in water, it does not release H⁺ ions directly. Instead, it reacts with water to form the tetrahydroxyborate ion (BO₃(OH)₄⁻) by accepting a hydroxide ion (OH⁻) from water, which results in the release of one H⁺ ion. This is why it is classified as a weak monobasic acid.

**Hint**: Think about how the reaction with water changes the composition of boric acid.

5. **Boric Acid as a Lewis Acid**:
- A Lewis acid is defined as a substance that can accept an electron pair. Since boric acid is electron-deficient, it can accept electron pairs from Lewis bases, which further supports its classification as a Lewis acid.

**Hint**: Recall the definition of Lewis acids and bases and how they interact.

### Summary
Boric acid (H₃BO₃) is a weak monobasic acid because it does not release H⁺ ions directly but instead reacts with water to form BO₃(OH)₄⁻, releasing H⁺ in the process. Its electron-deficient nature allows it to act as a Lewis acid by accepting electron pairs from other species.