Arrange the bonds in order of increasing ionic character in the molecules: LiF, K2O, N2, SO2 and ClF3

🧠 Ionic character increases with electronegativity difference between bonded atoms. Rank by increasing Δχ (electronegativity difference).

| Bond | Atoms | Δχ | Ionic character | |---|---|---|---| | $\ce{N2}$ | N–N | 0 | 0 (purely covalent) | | $\ce{SO2}$ | S–O | small | low | | $\ce{ClF3}$ | Cl–F | moderate | moderate | | $\ce{K2O}$ | K–O | large | high ionic | | LiF | Li–F | largest | highest ionic |

⚡ N–N bond is the anchor: identical atoms → Δχ = 0 → purely covalent → least ionic. Li–F has the greatest Δχ among common bonds.

$\boxed{\text{Answer: (c) } \ce{N2 < SO2 < ClF3 < K2O < LiF}}$