Assertion (A) : A covlent single bonds in biological molecules have energies similar to the energy of the C-C bond in ethane.
Reason (R) : It is because less electrons are shared between atoms in double bonds they require more energy to break than single bonds.
In the light of the above statements, choose the most appropriate answer from the options given below :
Covalent Bond Energy Analysis in Biological Molecules
Assertion (A) Analysis
Assertion (A) states that covalent single bonds in biological molecules have energies similar to the C-C bond in ethane. This is generally considered correct. Single covalent bonds (like C-C, C-H, C-O, C-N) form the structural framework of biological molecules, and their bond energies fall within a comparable range. For example, the C-C single bond energy in ethane is approximately 347 kJ/mol, and other single bonds in biological contexts are often in a similar order of magnitude.
Reason (R) Analysis
Reason (R) claims that less electrons are shared in double bonds, making them require more energy to break than single bonds. This statement contains a factual error in its premise:
- Electron Sharing: Double bonds share *more* electrons (typically 4) between atoms compared to single bonds (typically 2).
- Bond Strength: While it is true that double bonds require more energy to break than single bonds between the same pair of atoms due to this increased sharing, the reason's incorrect statement about electron count makes it fundamentally flawed.
Because the premise about electron sharing in double bonds is incorrect, Reason (R) is not a correct explanation for Assertion (A).
Conclusion
Based on the analysis:
- Assertion (A) is correct: Single covalent bonds in biological molecules exhibit energies comparable to the C-C bond in ethane.
- Reason (R) is incorrect: The statement misrepresents the number of electrons shared in double bonds.
Therefore, the most appropriate choice is that (A) is correct, but (R) is not correct.
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