In thiosulphuric acid: — p Block Elements Chemistry Question

💡 Solution & Explanation

Step 1: Analyze the statements: (a) Cl2 has a higher bond dissociation energy than F2 because of the high inter-electronic repulsion between lone pairs in the small F2 molecule; (b) Chlorine has a higher electron affinity than fluorine; (c) HCl is a stronger acid than HF. Step 2: Down the halogen group (from F2 to I2), the molecular size and mass increase, which systematically increases the strength of London dispersion (van der Waals) forces. Step 3: This stronger intermolecular attraction leads to a regular increase in boiling points down the group (F2 < Cl2 < Br2 < I2). Thus, statement (d) is correct.