Total number of sigma bonds involved in ethylene molecule `C_(2)H_(4)` are

Options

A. 3
B. 5
C. 2
D. 1

Explanation

To determine the total number of sigma bonds in the ethylene molecule \( C_2H_4 \), we can follow these steps:

### Step 1: Understand the Structure of Ethylene
Ethylene (\( C_2H_4 \)) is an alkene, which means it contains a carbon-carbon double bond. The structural formula of ethylene is:

```
H H
\ /
C = C
/ \
H H
```

### Step 2: Identify the Bonds
In the structure of ethylene:
- Each carbon atom is bonded to two hydrogen atoms and one other carbon atom.
- The carbon-carbon bond is a double bond, which consists of one sigma bond and one pi bond.

### Step 3: Count the Sigma Bonds
1. **Carbon-Carbon Bond**:
- The double bond between the two carbon atoms contributes **1 sigma bond**.

2. **Carbon-Hydrogen Bonds**:
- Each carbon atom is bonded to two hydrogen atoms. Since there are two carbon atoms, the total number of carbon-hydrogen bonds is \( 2 \times 2 = 4 \) bonds. Each of these bonds is a sigma bond.

### Step 4: Total Sigma Bonds Calculation
Now, we can sum the sigma bonds:
- From the carbon-carbon bond: **1 sigma bond**
- From the carbon-hydrogen bonds: **4 sigma bonds**

Adding these together gives:
\[ 1 \text{ (C-C sigma bond)} + 4 \text{ (C-H sigma bonds)} = 5 \text{ sigma bonds} \]

### Conclusion
The total number of sigma bonds in the ethylene molecule \( C_2H_4 \) is **5**.

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