Bond energy is highest for :

Options

A. ` Sn-Sn`
B. ` C-C`
C. `Si -Si`
D. `Ge-Ge`

Explanation

To determine which member of the carbon family has the highest bond energy, we can follow these steps:

### Step 1: Identify the Members of the Carbon Family
The carbon family consists of the following elements:
- Carbon (C)
- Silicon (Si)
- Germanium (Ge)
- Tin (Sn)
- Lead (Pb)

### Step 2: Understand Bond Energy
Bond energy refers to the energy required to break a bond between two identical atoms. In this case, we are interested in the bond energy of the C-C bond (for carbon) and the corresponding bonds in silicon, germanium, tin, and lead.

### Step 3: Analyze the Trend in Bond Energy
As we move down the group from carbon to lead, the bond energy generally decreases. This is due to the increase in atomic size and the corresponding decrease in the overlap of atomic orbitals, which weakens the bond.

### Step 4: Consider the Property of Catenation
Catenation is the ability of an element to form chains or rings by bonding with itself. Carbon exhibits a high degree of catenation due to its strong C-C bond, allowing it to form a variety of complex structures.

### Step 5: Conclusion
Based on the analysis, carbon has the highest bond energy among the members of the carbon family. Therefore, the correct answer to the question is:
**Carbon (C)** has the highest bond energy.