Chemistry · Covalent Bonding: Concept of electronegativity, Fajan's rule, dipole moment, Valence Shell Electron Pair Repulsion (VSEPR) theory and shapes of simple molecules
Statement 1: The molecule has a net dipole. Statement 2: Oxygen has the higher e
Statement 1: The molecule \( S O_{2} \) has a net dipole. Statement 2: Oxygen has the higher electronegativity than sulfur.
- A. Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of statement 1
- B. Both Statement 1 and Statement 2 are correct, but Statement 2 is NOT the correct explanation of Statement 1.
- C. Statement 1 is correct, but Statement 2 is not correct
- D. Statement 1 is not correct, but Statement 2 is correct
Step-by-step solution
Statement 1 is correct because SO2 has a bent shape (due to a lone pair on sulfur) and polar S-O bonds, resulting in a net dipole moment. Statement 2 is correct because oxygen is more electronegative than sulfur. However, statement 2 alone is not the correct explanation for statement 1, as the net dipole also depends on the molecular geometry (VSEPR theory). Thus, both statements are true, but statement 2 is not the direct explanation.