The catenation tendency of C, Si and Ge is in the order Ge < Si < C. The bond energies (in kJ mol$$^{-1}$$) of C-C, Si-Si and Ge-Ge bonds are respectively ;

The catenation tendency refers to the ability of an element to form bonds with atoms of the same element. The order given is Ge < Si < C, meaning germanium has the least tendency, silicon has a medium tendency, and carbon has the highest tendency for catenation.

Bond energy is a measure of the strength of a bond between two atoms. A higher bond energy indicates a stronger bond, which typically corresponds to a higher catenation tendency. Therefore, the bond energies should follow the same order as the catenation tendency: Ge-Ge bond energy < Si-Si bond energy < C-C bond energy.

Now, examining the options, the bond energies are given respectively for C-C, Si-Si, and Ge-Ge:

• Option A: C-C = 348 kJ/mol, Si-Si = 297 kJ/mol, Ge-Ge = 260 kJ/mol
• Option B: C-C = 297 kJ/mol, Si-Si = 348 kJ/mol, Ge-Ge = 260 kJ/mol
• Option C: C-C = 348 kJ/mol, Si-Si = 260 kJ/mol, Ge-Ge = 297 kJ/mol
• Option D: C-C = 260 kJ/mol, Si-Si = 297 kJ/mol, Ge-Ge = 348 kJ/mol

We need to find which option satisfies Ge-Ge < Si-Si < C-C.

Checking Option A: Ge-Ge = 260 kJ/mol, Si-Si = 297 kJ/mol, C-C = 348 kJ/mol. Comparing the values: 260 < 297 is true, and 297 < 348 is true. So, 260 < 297 < 348 holds.

Checking Option B: Ge-Ge = 260 kJ/mol, Si-Si = 348 kJ/mol, C-C = 297 kJ/mol. Here, 260 < 348 is true, but 348 < 297 is false because 348 is greater than 297. This violates the required order.

Checking Option C: Ge-Ge = 297 kJ/mol, Si-Si = 260 kJ/mol, C-C = 348 kJ/mol. Here, 297 < 260 is false because 297 is greater than 260. This violates the required order.

Checking Option D: Ge-Ge = 348 kJ/mol, Si-Si = 297 kJ/mol, C-C = 260 kJ/mol. Here, 348 < 297 is false because 348 is greater than 297. This violates the required order.

Only Option A satisfies the condition that Ge-Ge bond energy < Si-Si bond energy < C-C bond energy, which aligns with the catenation tendency order Ge < Si < C.

Hence, the correct answer is Option A.