Question

Statement-I : The electronegativity order in F, O, N is \(F > O > N\).
Statement-II : Oxidation state of O in \(OF_2\) is \(+2\) and in \(Na_2O\) is \(-2\). Choose the correct option.

• A. Both statement-I \& statement-II are correct.
• B. Both statement-I \& statement-II are incorrect.
• C. Statement-I is correct \& statement-II is incorrect.
• D. Statement-I is incorrect \& statement-II is correct.

Answer 1

The Correct Option is A

Concept:
Electronegativity measures the tendency of an atom to attract bonding electrons. It generally increases across a period from left to right. Step 1: Check electronegativity order. Approximate Pauling electronegativity values: \[ F = 4.0 \] \[ O = 3.5 \] \[ N = 3.0 \] Thus, \[ F > O > N \] Statement-I is correct. Step 2: Determine oxidation states of oxygen. In \(OF_2\): Fluorine is the most electronegative element and always has oxidation state \(-1\). Let oxidation state of oxygen be \(x\): \[ x + 2(-1) = 0 \] \[ x = +2 \] In \(Na_2O\): Sodium has oxidation state \(+1\). \[ 2(+1) + x = 0 \] \[ x = -2 \] Thus, Statement-II is correct. Step 3: Conclusion. \[ \boxed{\text{Both statements are correct}} \]