Which of the following statements is not correct for `BF_3` ?

Options

A. It can form adduct
B. It acts as a Lewis base
C. It forms an ionic bond
D. It also forms dative bonds with compounds like `NH_3`, etc.

Explanation

To determine which statement is not correct for \( BF_3 \), we will analyze each statement based on the properties and behavior of boron trifluoride.

### Step 1: Analyze the structure of \( BF_3 \)
- **Boron trifluoride (\( BF_3 \))** consists of a boron atom bonded to three fluorine atoms.
- Boron is **sp² hybridized**, which means it has one empty p-orbital and is electron-deficient.

### Step 2: Evaluate the statements
1. **It can form an adduct.**
- This statement is correct. \( BF_3 \) can accept an electron pair from a Lewis base (like \( NH_3 \)) to form an adduct.

2. **It acts as a Lewis base.**
- This statement is incorrect. \( BF_3 \) is a Lewis acid because it is electron-deficient and can accept electrons, not donate them.

3. **It forms an ionic bond.**
- This statement is also incorrect. \( BF_3 \) does not form ionic bonds; it typically forms covalent bonds and coordinate (or dative) bonds with Lewis bases.

4. **It also forms dative bonds with compounds like \( NH_3 \).**
- This statement is correct. \( BF_3 \) can form dative bonds with \( NH_3 \) when \( NH_3 \) donates its lone pair to \( BF_3 \).

### Conclusion
The statements that are not correct for \( BF_3 \) are:
- **It acts as a Lewis base.**
- **It forms an ionic bond.**

### Final Answer
The statements that are not correct for \( BF_3 \) are:
- It acts as a Lewis base.
- It forms an ionic bond.

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