Chemistry · Covalent Bonding: Concept of electronegativity, Fajan's rule, dipole moment, Valence Shell Electron Pair Repulsion (VSEPR) theory and shapes of simple molecules
Bond angle in \) is higher than the bond angle of . \) The difference is due to:
Bond angle in \( H_{2} O\left(104.5^{\circ}\right) \) is higher than the bond angle of \( H_{2} S\left(92.1^{\circ}\right) . \) The difference is due to:
- A. 0 is diatomic and \( S \) is tetra-atomic
- B. difference in electronegativity of S and 0
- C. difference in oxidation states of S and 0
- D. difference in shapes of hybrid orbitals of S and
Step-by-step solution
The bond angle in H2O (104.5°) is larger than in H2S (92.1°) due to the higher electronegativity of oxygen compared to sulfur. Oxygen attracts the bonding electrons more strongly, causing greater repulsion between lone pairs and bond pairs, which expands the bond angle. In contrast, sulfur's lower electronegativity and larger size result in less electron density on the central atom, reducing repulsion and decreasing the bond angle.