Import Question JSON

$\text{HINT: Electronegativity difference directly proportional to ionic character.}$ $\text{Explanation:}$ $\text{The greater the electronegativity difference, the greater will be the ionic character of the molecule.}$ $\text{Also, the higher the dipole moment, the higher will be the ionic character e.g. in the case of ClF}_3\text{ the dipole moment is more as compared to SO}_2\text{. Thus, the ionic character of ClF}_3 > \text{SO}_2$. $\text{Electronegativity values of elements:}$ $\text{Li: 0.98}$ $\text{F: 3.98}$ $\text{Cl: 3.16}$ $\text{K: 0.82}$ $\text{O: 3.44}$ $\text{S: 2.58}$ $\text{N: 3.04}$ $\text{Let's calculate the electronegativity difference for each molecule:}$ $\text{LiF: } |3.98 - 0.98| = 3.00$ $\text{K}_2\text{O: For K-O bond, } |3.44 - 0.82| = 2.62$ $\text{N}_2: |3.04 - 3.04| = 0.00$ $\text{SO}_2: \text{For S-O bond, } |3.44 - 2.58| = 0.86$ $\text{ClF}_3: \text{For Cl-F bond, } |3.98 - 3.16| = 0.82$ $\text{Based on electronegativity difference:}$ $\text{N}_2 (0.00) < \text{ClF}_3 (0.82) < \text{SO}_2 (0.86) < \text{K}_2\text{O} (2.62) < \text{LiF} (3.00)$ $\text{Considering the given options and the slight discrepancy for ClF}_3\text{ and SO}_2\text{ in the hint:}$ $\text{The hint states that the ionic character of ClF}_3 > \text{SO}_2\text{ due to dipole moment, even though the electronegativity difference is slightly lower for ClF}_3\text{. This is an important consideration beyond just electronegativity difference, as molecular geometry and lone pairs also contribute to dipole moment.}$ $\text{So, the order based on this revised understanding would be:}$ $\text{N}_2 < \text{SO}_2 < \text{ClF}_3 < \text{K}_2\text{O} < \text{LiF}$ $\text{This matches option 1.}$