Question

Which of the following statements about bonds between two carbon atoms is/are correct?

(i) Bond strength increases as more electrons are shared between the atoms.
(ii) Bond strength increases as the overlap between atomic orbitals increases.
(iii) Hybrid orbitals are used to describe (account for) the geometry (bond angles) around each carbon atom.
A) All three are correct statements.
B) I only.
C) Two of these are correct statements.
D) II and III.

Answer 1

All three statements about bonds between two carbon atoms are correct: bond strength increases with more shared electrons, increased orbital overlap, and hybrid orbitals describe molecular geometry. Therefore, the correct option is A.

Step-by-step explanation:

The bond between two carbon atoms is influenced by various factors. Statement (i) states that bond strength increases as more electrons are shared between the atoms, which is correct. For example, a single bond involving one pair of shared electrons is weaker than a double bond, which involves two pairs of shared electrons, and a triple bond is stronger still, involving three pairs of shared electrons.

Statement (ii) mentions that bond strength increases as the overlap between atomic orbitals increases. This is also correct. The stability of the covalent bond is related to how much the atomic orbitals overlap, with greater overlap resulting in a stronger bond.

Lastly, statement (iii) correctly suggests that hybrid orbitals are used to describe the geometry and bond angles around each carbon atom, accounting for the three-dimensional structure of molecules. Hybridization helps explain the observed bond angles and the shapes of molecules.

Therefore, the correct answer is that all statements (i), (ii), and (iii) about bonds between two carbon atoms are correct, which corresponds to option A) All three are correct statements.