At room temperature and pressure, $\text{H}_2\text{O}$ exists as a liquid, whereas $\text{H}_2\text{S}$ exists as a gas. What accounts for this difference?
- AO has higher first and second ionisation energies than S.
- BThe covalent bond between O and H is stronger than the covalent bond between S and H.
- CThere is significant hydrogen bonding between $\text{H}_2\text{O}$ molecules but not between $\text{H}_2\text{S}$ molecules.
- DThe instantaneous dipole-induced dipole forces between $\text{H}_2\text{O}$ molecules are stronger than the instantaneous dipole-induced dipole forces between $\text{H}_2\text{S}$ molecules.