Acidity of `BF_(3)` can be explained on ths basis of which of the follwoing concepts? (A)Arrhenius concept (B)Bronsted - Lowry concept (C)Lewis concept (D)Bronsted - Lowry as well as Lewis concept

Options

A. Arrhenius concept
B. Bronsted - Lowry concept
C. Lewis concept
D. Bronsted - Lowry as well as Lewis concept

Explanation

To determine the acidity of BF₃ (Boron Trifluoride) and which concept explains it best, we can analyze the options provided:

1. **Understanding BF₃**:
- Boron (B) has an electronic configuration of 1s² 2s² 2p¹. In its ground state, boron has three valence electrons and can form three bonds with fluorine (F) atoms.
- When BF₃ is formed, boron shares its electrons with fluorine, but it does not have a complete octet; it has an empty p-orbital.

2. **Analyzing the Concepts**:
- **Arrhenius Concept**: This concept defines acids as substances that produce H⁺ ions in aqueous solution. BF₃ does not produce H⁺ ions, so it does not fit this definition.
- **Bronsted-Lowry Concept**: This theory defines acids as proton donors. BF₃ does not donate protons; rather, it accepts electron pairs, so it does not fit this definition either.
- **Lewis Concept**: According to Lewis theory, acids are defined as electron pair acceptors. BF₃ has an empty p-orbital and can accept a lone pair of electrons from a Lewis base, which makes it a Lewis acid.

3. **Conclusion**:
- The acidity of BF₃ can be best explained by the **Lewis concept** because it acts as an electron pair acceptor.

Thus, the correct answer is:
**(C) Lewis concept**