On the basis of Lewis concept, which of the following are correct?

Options

A. `Ag^(+)+ 2NH_(3)to[ H_(3)N-Ag -NH_(3)]^(+)`
B. `Br_(2)+FeCl_(3)leftrightarrow Br-Br^(+) -FeCI_(3)`
C. `R-OH+ZnCl_(2)leftrightarrowR-underset( ZnCl_(2))underset(|)O^(+)H`
D. `NH_(4)^(+)+OH ^(-) hArr NH_(3) +H_(2)O`

Answer

To solve the question based on the Lewis concept of acids and bases, we need to analyze each option provided in the question. According to the Lewis concept:

1. **Lewis Acid**: A species that can accept a lone pair of electrons (it must have vacant orbitals).
2. **Lewis Base**: A species that can donate a lone pair of electrons (it must have lone pairs available).

Now, let's evaluate the options step by step:

### Step 1: Analyze AG⁺ and Nitrogen
- **AG⁺**: This ion has a vacant orbital and can accept a lone pair. Therefore, it acts as a Lewis acid.
- **Nitrogen**: Nitrogen typically has a lone pair of electrons that it can donate. Thus, it acts as a Lewis base.
- **Conclusion**: This interaction is valid according to the Lewis concept.

### Step 2: Analyze Br₂ and FeCl₃
- **Br₂**: Each bromine atom in Br₂ has three lone pairs. It can donate a lone pair, making it a Lewis base.
- **FeCl₃**: This compound is electron-deficient and can accept a lone pair, acting as a Lewis acid.
- **Conclusion**: This interaction is valid according to the Lewis concept.

### Step 3: Analyze Oxygen and Zinc
- **Oxygen**: In this case, oxygen donates a lone pair to zinc. If oxygen is forming bonds and has a positive charge, it indicates that it has donated a lone pair, making it a Lewis base.
- **Zinc**: Zinc can accept the lone pair, acting as a Lewis acid.
- **Conclusion**: This interaction is valid according to the Lewis concept.

### Step 4: Analyze Alcohols and CO₂
- **Alcohols**: Alcohols have lone pairs on the oxygen atom, allowing them to act as Lewis bases.
- **CO₂**: Carbon dioxide is electron-deficient and can accept a lone pair, acting as a Lewis acid.
- **Conclusion**: This interaction is valid according to the Lewis concept.

### Step 5: Analyze NH₄⁺ and S²⁻
- **NH₄⁺**: The ammonium ion has no lone pairs available for donation because all electrons of nitrogen are involved in bonding with hydrogen atoms. Therefore, it cannot act as a Lewis base.
- **S²⁻**: Sulfide ion can donate a lone pair, but since NH₄⁺ cannot donate a lone pair, this interaction is not valid.
- **Conclusion**: This interaction is NOT valid according to the Lewis concept.

### Final Conclusion
Based on the analysis:
- **Correct options**: A, B, C
- **Incorrect option**: D (NH₄⁺ cannot act as a Lewis base)

### Answer
The correct options according to the Lewis concept are A, B, and C.

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