What are the hybridization and shapes of the following molecules?
(i) `CH_(3)F`
(ii) `HC-=N`

Options

A. (i) `sp^(2)`, trigonal planar, (ii) `sp^(3)`, tetrahedral
B. (i) `sp^(3)`, tetrahedral, (ii) sp, linear
C. (i) sp, linear, (ii) `sp^(2)`, trigonal planar
D. (i) `sp^(2)`, trigonal planar, (ii) `sp^(2)`, trigonal planar

Answer

To determine the hybridization and shapes of the molecules `CH₃F` and `HC≡N`, we can follow these steps:

### Step 1: Analyze the first molecule `CH₃F`
1. **Identify the central atom**: In `CH₃F`, carbon (C) is the central atom.
2. **Count the number of atoms attached to the central atom**:
- Carbon is bonded to three hydrogen atoms (H) and one fluorine atom (F).
- Therefore, the total number of atoms attached to carbon is 4.
3. **Determine hybridization**:
- The hybridization can be determined based on the number of atoms attached:
- 4 atoms → sp³ hybridization.
4. **Determine the shape**:
- With sp³ hybridization, the shape of the molecule is tetrahedral.

### Step 2: Analyze the second molecule `HC≡N`
1. **Identify the central atom**: In `HC≡N`, carbon (C) is again the central atom.
2. **Count the number of atoms attached to the central atom**:
- Carbon is bonded to one hydrogen atom (H) and one nitrogen atom (N) through a triple bond.
- Therefore, the total number of atoms attached to carbon is 2.
3. **Determine hybridization**:
- The hybridization can be determined based on the number of atoms attached:
- 2 atoms → sp hybridization.
4. **Determine the shape**:
- With sp hybridization, the shape of the molecule is linear.

### Summary of Results
- For `CH₃F`:
- Hybridization: sp³
- Shape: Tetrahedral
- For `HC≡N`:
- Hybridization: sp
- Shape: Linear