Match the compounds listed in column I with characteristic listed in column II.
`{:("Column-I","Column-II"),((A)SF_2,(p)sp^3"and bent"),((B)KrF_4,(q)"Lone pair"),((C )NOCl,(r)"Bond angle less than"109^@28'),((D )N(Me)_3,(s)sp^2"and bent"),(,(t)sp^3d^2"and square planar"):}`

Explanation

To solve the problem of matching the compounds in Column I with their characteristics in Column II, we will analyze each compound step by step, determining its hybridization, geometry, and any lone pairs present.

### Step 1: Analyze SF₂
1. **Identify the central atom**: Sulfur (S) is the central atom.
2. **Count valence electrons**: Sulfur has 6 valence electrons.
3. **Count surrounding atoms**: There are 2 fluorine (F) atoms, which are monovalent.
4. **Calculate hybridization**:
\[ \text{Hybridization} = \frac{(6 + 2)}{2} = \frac{8}{2} = 4 \quad \Rightarrow \quad \text{sp}^3 \]
5. **Determine geometry**: With 2 bond pairs and 2 lone pairs, the shape is bent.
6. **Bond angle**: The bond angle is less than 109.28° due to lone pair repulsion.

**Matching for SF₂**:
- Hybridization: sp³ (p)
- Lone pairs: Yes (q)
- Bond angle less than 109.28° (r)

### Step 2: Analyze KrF₄
1. **Identify the central atom**: Krypton (Kr) is the central atom.
2. **Count valence electrons**: Krypton has 8 valence electrons.
3. **Count surrounding atoms**: There are 4 fluorine atoms.
4. **Calculate hybridization**:
\[ \text{Hybridization} = \frac{(8 + 4)}{2} = \frac{12}{2} = 6 \quad \Rightarrow \quad \text{sp}^3d^2 \]
5. **Determine geometry**: With 4 bond pairs and 2 lone pairs, the shape is square planar.
6. **Bond angle**: The bond angle is 90°, which is less than 109.28°.

**Matching for KrF₄**:
- Hybridization: sp³d² (t)
- Lone pairs: Yes (q)
- Bond angle less than 109.28° (r)

### Step 3: Analyze NOCl
1. **Identify the central atom**: Nitrogen (N) is the central atom.
2. **Count valence electrons**: Nitrogen has 5 valence electrons.
3. **Count surrounding atoms**: There are 1 chlorine (Cl) and 1 oxygen (O) atom. Only count Cl as it is monovalent.
4. **Calculate hybridization**:
\[ \text{Hybridization} = \frac{(5 + 1)}{2} = \frac{6}{2} = 3 \quad \Rightarrow \quad \text{sp}^2 \]
5. **Determine geometry**: With 2 bond pairs and 1 lone pair, the shape is bent.
6. **Bond angle**: The bond angle is slightly less than 120°, which is more than 109.28°.

**Matching for NOCl**:
- Hybridization: sp² (s)
- Lone pairs: Yes (q)

### Step 4: Analyze N(Me)₃
1. **Identify the central atom**: Nitrogen (N) is the central atom.
2. **Count valence electrons**: Nitrogen has 5 valence electrons.
3. **Count surrounding atoms**: There are 3 methyl (Me) groups.
4. **Calculate hybridization**:
\[ \text{Hybridization} = \frac{(5 + 3)}{2} = \frac{8}{2} = 4 \quad \Rightarrow \quad \text{sp}^3 \]
5. **Determine geometry**: With 3 bond pairs and 1 lone pair, the shape is pyramidal.
6. **Bond angle**: The bond angle is less than 109.28°.

**Matching for N(Me)₃**:
- Hybridization: sp³ (p)
- Lone pairs: Yes (q)
- Bond angle less than 109.28° (r)

### Summary of Matches:
- **A (SF₂)**: p, q, r
- **B (KrF₄)**: q, r, t
- **C (NOCl)**: q, s
- **D (N(Me)₃)**: q, r

### Final Answer:
- A: p, q, r
- B: q, r, t
- C: q, s
- D: q, r