Final answer:
The incorrect statement about bonding and hybridization is that sigma bonds represent a side-to-side overlap of orbitals, when in fact they represent an end-to-end overlap.
Step-by-step explanation:
The question is asking to identify the incorrect statement about bonding and hybridization. Upon reviewing the options:
- Hybridization explains the electron density around covalently bonded atoms and predicts the bond angles and shapes of molecules based on the types of hybrid orbitals formed. Therefore, the statement that hybridization does not account for observed bond angles in molecules is incorrect.
- Sigma bonds are indeed formed by the end-to-end overlap of orbitals directly between the nuclei of two atoms, so this statement is correct.
- Pi bonds form from the side-by-side overlap of unhybridized p or sometimes d orbitals, so this statement is also correct.
- It is accurate to say that multiple bonds consist of both sigma and pi bonds; for example, a double bond contains one sigma bond and one pi bond, and a triple bond contains one sigma bond and two pi bonds.
- Sigma bonds are formed by end-to-end, not side-to-side overlap of orbitals.
Hence, the incorrect statement is e. Sigma bonds represent a side-to-side overlap of orbitals because sigma bonds actually represent an end-to-end overlap of orbitals.