The total number of sigma (`sigma`) and pi (`pi`) bonds in an ethylene molecule are

Options

A. `4sigma, 2pi`
B. `4sigma, 1pi`
C. `5sigma, 2pi`
D. `5sigma, 1pi`

Answer

To determine the total number of sigma (σ) and pi (π) bonds in an ethylene molecule (C₂H₄), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Structure of Ethylene**:
Ethylene is a hydrocarbon with the formula C₂H₄. It consists of two carbon atoms connected by a double bond and each carbon atom is bonded to two hydrogen atoms. The structural representation can be written as:
\[ H_2C = CH_2 \]

2. **Count the Sigma Bonds**:
- Each single bond is a sigma bond.
- In ethylene, there are:
- 4 C-H bonds (2 from each carbon to hydrogen) which are all sigma bonds.
- 1 C=C double bond consists of 1 sigma bond.
- Therefore, the total number of sigma bonds is:
\[ \text{Total Sigma Bonds} = 4 \text{ (C-H)} + 1 \text{ (C=C)} = 5 \text{ sigma bonds} \]

3. **Count the Pi Bonds**:
- A double bond consists of one sigma bond and one pi bond.
- In ethylene, the C=C double bond contributes 1 pi bond.
- Therefore, the total number of pi bonds is:
\[ \text{Total Pi Bonds} = 1 \text{ (from C=C)} = 1 \text{ pi bond} \]

4. **Summarize the Total Bonds**:
- The total number of sigma bonds in ethylene is 5.
- The total number of pi bonds in ethylene is 1.

### Final Answer:
The total number of sigma and pi bonds in an ethylene molecule is:
- **Sigma bonds (σ)**: 5
- **Pi bonds (π)**: 1