Which of the following cannot act as a Lewis or Bronsted acid

Options

A. `BF_(3)`
B. `AlCl_(3)`
C. `SnCl_(4)`
D. `"CCl"_(4)`

Explanation

To determine which of the given options cannot act as a Lewis or Bronsted acid, we need to understand the definitions of both types of acids:

1. **Lewis Acid**: A Lewis acid is defined as an electron pair acceptor. This means it must have the ability to accept a pair of electrons, which typically requires the presence of an empty orbital (such as a vacant p-orbital).

2. **Bronsted Acid**: A Bronsted acid is defined as a proton (H⁺) donor. This means it must be able to release a proton in a chemical reaction.

Now, let's analyze the options provided in the question:

1. **BF3 (Boron Trifluoride)**:
- BF3 has a vacant p-orbital and can accept an electron pair, making it a Lewis acid.
- It does not have any protons to donate, so it cannot act as a Bronsted acid.

2. **HCl (Hydrochloric Acid)**:
- HCl can donate a proton (H⁺), making it a Bronsted acid.
- It can also act as a Lewis acid by accepting an electron pair from a base.

3. **H2SO4 (Sulfuric Acid)**:
- H2SO4 can donate protons (H⁺), making it a Bronsted acid.
- It can also act as a Lewis acid by accepting electron pairs due to the presence of sulfur's vacant d-orbitals.

4. **C (Carbon)**:
- Carbon does not have a vacant p-orbital and cannot accept an electron pair, so it cannot act as a Lewis acid.
- Carbon also does not have any protons to donate, so it cannot act as a Bronsted acid.

Based on this analysis, the option that cannot act as either a Lewis or Bronsted acid is **C (Carbon)**.

### Final Answer:
**C (Carbon)** cannot act as a Lewis or Bronsted acid.