In vinyl acetylene `CH=C-CH=CH_2` type of overlapping in `(C_2rarrC_3)`bond is

Options

A. `sp^2-sp`
B. `sp-sp^2`
C. `sp^3-sp^3`
D. `sp^3-sp^2`

Answer

To determine the type of overlapping in the bond between C2 and C3 in vinyl acetylene (CH=C-CH=CH2), we need to analyze the hybridization of the carbon atoms involved in this bond.

### Step 1: Identify the Structure
The structure of vinyl acetylene can be represented as:
```
H H
\ /
C
||
C
/ \
C C
| |
H H
```
In this structure, we have:
- C1: CH (attached to C2)
- C2: C (double bond with C3)
- C3: C (double bond with C2 and single bond with C4)
- C4: CH2 (attached to C3)

### Step 2: Determine the Hybridization of C2 and C3
- **C2**: This carbon is involved in a double bond with C3 and a single bond with C1. The double bond consists of one sigma bond and one pi bond. Therefore, C2 has:
- 1 sigma bond (with C3)
- 1 sigma bond (with C1)
- 1 pi bond (with C3)

The total number of bonds indicates that C2 is **sp² hybridized** (since it forms three sigma bonds).

- **C3**: This carbon is involved in a double bond with C2 and a single bond with C4. Similar to C2, C3 has:
- 1 sigma bond (with C2)
- 1 sigma bond (with C4)
- 1 pi bond (with C2)

Thus, C3 is also **sp² hybridized** (since it forms three sigma bonds).

### Step 3: Identify the Type of Overlapping
In the bond between C2 and C3:
- The sigma bond is formed by the head-on overlapping of **sp² hybrid orbitals** from both C2 and C3.
- The pi bond is formed by the side-to-side overlapping of the unhybridized p orbitals from both C2 and C3.

### Conclusion
The type of overlapping in the bond between C2 and C3 in vinyl acetylene is:
- **Sigma bond**: Head-on overlapping of sp² hybrid orbitals.
- **Pi bond**: Side-to-side overlapping of unhybridized p orbitals.

Thus, the answer is that the bond between C2 and C3 involves **sp² hybridization**.