The outer orbitals of C in ethene molecule can be considered to be hybridized to given three equivalent `sp^(2)` orbitals. The total number of sigma `(sigma)` and pi `(pi)` bonds in ethene molecule is

Options

A. 3 sigma `(sigma)` and 2 pi `(pi)` bonds
B. 4 sigma `(sigma)` and 1 pi `(pi)` bonds
C. 5 sigma `(sigma)` and 1 pi `(pi)` bonds
D. 1 sigma `(sigma)` and 2 pi `(pi)` bonds

Answer

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

### Step 1: Understand the Structure of Ethene
Ethene (C₂H₄) consists of two carbon atoms double-bonded to each other and each carbon atom is also bonded to two hydrogen atoms.

### Step 2: Identify the Hybridization of Carbon in Ethene
In ethene, each carbon atom undergoes sp² hybridization. This means that one s orbital and two p orbitals mix to form three equivalent sp² hybrid orbitals.

### Step 3: Determine the Types of Bonds
1. **Sigma Bonds (σ)**:
- Each sp² hybrid orbital forms a sigma bond with another atom.
- Each carbon forms:
- One sigma bond with the other carbon atom (C=C).
- Two sigma bonds with two hydrogen atoms (C-H).
- Therefore, for each carbon atom, there are 3 sigma bonds (1 with another carbon and 2 with hydrogen).
- Since there are 2 carbon atoms, the total number of sigma bonds is 3 (from one carbon) + 3 (from the other carbon) = 6 sigma bonds.

2. **Pi Bonds (π)**:
- The remaining unhybridized p orbital on each carbon atom forms a pi bond with the other carbon atom.
- Since there is one double bond between the two carbon atoms, there is 1 pi bond.

### Step 4: Count the Total Number of Bonds
- Total Sigma Bonds (σ) = 6
- Total Pi Bonds (π) = 1

### Conclusion
In ethene, the total number of sigma bonds is 6 and the total number of pi bonds is 1. Therefore, the total number of sigma and pi bonds in ethene is:
- **Total Bonds = Sigma Bonds + Pi Bonds = 6 + 1 = 7**

### Final Answer
The total number of sigma and pi bonds in ethene is **6 sigma bonds and 1 pi bond**.