Final answer:
All three statements about carbon-carbon bonds are correct, reflecting that bond strength increases with more electron sharing and greater orbital overlap, and hybrid orbitals explain the geometry around each carbon atom.
option d is the correct
Step-by-step explanation:
When considering the statements about bonds between two carbon atoms, all three provided statements are correct:
- Bond strength increases as more electrons are shared between the atoms.
- Bond strength increases as the overlap between atomic orbitals increases.
- Hybrid orbitals are used to describe (account for) the geometry (bond angles) around each carbon atom.
Bonds between atoms, including carbon atoms, are formed through the sharing of electron pairs. The overlap of atomic orbitals is a key factor influencing bond strength. The greater the overlap, the stronger the bond.
For example, a carbon-carbon single bond involves one sigma (σ) bond, a double bond includes one σ bond and one pi (π) bond, and a triple bond consists of one σ bond and two π bonds. Each additional shared electron pair results in a stronger and shorter bond. Additionally, the concept of hybrid orbitals helps explain the spatial arrangement around each carbon atom, contributing to the molecular geometry and bond angles seen in molecules.