Statement I : Water (H2O) is more polar than Hydrogen Sulphide . Statement II: Oxygen is more electro-negative than Sulphur.

Statement I is true as water (H2O) is significantly more polar than hydrogen sulphide (H2S). Polarity is determined by the net dipole moment, which depends on bond polarity and molecular geometry. Statement II is also true and provides the correct explanation: oxygen has a higher electronegativity (approximately 3.5) compared to sulphur (approximately 2.4-2.5). This greater electronegativity difference between oxygen and hydrogen (compared to sulphur and hydrogen) results in more polar O-H bonds. Since both molecules have a similar bent molecular geometry, the stronger bond dipoles in H2O lead to a much larger net molecular dipole moment than in H2S. Consequently, the higher electronegativity of oxygen directly causes the increased polarity of water molecules.