`{:("List-I" ,"List-II"),((A) "CC"I_(4),P. "Lewis acid"),((B)AICI_(3),"Q.Lewis base"),((C )NH_(3),R."Bronsted acid"),((D) HCIO_(4) ,S."Bronsted base"),(,T."Neither lewis acid nor Lewis base"):}`

Answer

To solve the problem, we need to match the compounds in List-I with their corresponding classifications in List-II. The classifications include Lewis acid, Lewis base, Bronsted acid, Bronsted base, and neither Lewis acid nor Lewis base.

### Step-by-Step Solution:

1. **Identify the nature of CCl₄ (Carbon Tetrachloride)**:
- CCl₄ is a neutral compound and does not have the ability to accept or donate electron pairs. Therefore, it does not act as either a Lewis acid or a Lewis base.
- **Match**: CCl₄ → T (Neither Lewis acid nor Lewis base)

2. **Identify the nature of AlCl₃ (Aluminum Chloride)**:
- AlCl₃ can accept a pair of electrons due to the presence of an empty p-orbital in aluminum. This makes it a Lewis acid.
- **Match**: AlCl₃ → P (Lewis acid)

3. **Identify the nature of NH₃ (Ammonia)**:
- NH₃ has a lone pair of electrons on the nitrogen atom, which can be donated to form a bond. Thus, NH₃ acts as a Lewis base.
- **Match**: NH₃ → Q (Lewis base)

4. **Identify the nature of HClO₄ (Perchloric Acid)**:
- HClO₄ can donate a proton (H⁺) due to the presence of the hydroxyl group (–OH). Therefore, it acts as a Bronsted acid.
- **Match**: HClO₄ → R (Bronsted acid)

### Final Matches:
- A (CCl₄) → T (Neither Lewis acid nor Lewis base)
- B (AlCl₃) → P (Lewis acid)
- C (NH₃) → Q (Lewis base)
- D (HClO₄) → R (Bronsted acid)

### Summary of Matches:
- A → T
- B → P
- C → Q
- D → R