Number of and bonds present in ethylene molecule is respectively:

Step 1: Draw the structure of ethylene

Ethylene: $\ce{H2C=CH2}$

Both carbons are $sp^2$ hybridized, with a double bond ($\sigma + \pi$) between them.

Step 2: Count $\sigma$ bonds

• $\ce{C-H}$ bonds: Each carbon has 2 H atoms → $2 \times 2 = 4$ $\ce{C-H}$ $\sigma$ bonds
• $\ce{C=C}$ double bond contains 1 $\sigma$ bond

Total $\sigma$ bonds = $4 + 1 = \mathbf{5}$

Step 3: Count $\pi$ bonds

• The $\ce{C=C}$ double bond contains 1 $\pi$ bond (formed by lateral overlap of $p$ orbitals)

Total $\pi$ bonds = $\mathbf{1}$

Step 4: Answer

$\sigma$ bonds = 5, $\pi$ bonds = 1 → Option (d)

Key Points to Remember:

• Every bond contains at least 1 $\sigma$ bond
• Double bond = 1 $\sigma$ + 1 $\pi$; Triple bond = 1 $\sigma$ + 2 $\pi$
• $\ce{C-H}$ bonds are always $\sigma$ bonds
• For $\ce{CnH_{2n}}$ (alkene): $\sigma = 3n-1$... for ethylene ($n=2$): $\sigma = 5$