Electronic configuration of four elements A, B, C and D are given below : (A) $1 s^2 2 s^2 2 p^3$ (B) $1 s^2 2 s^2 2 p^4$ (C) $1 s^2 2 s^2 2 p^5$ (D) $1 s^2 2 s^2 2 p^2$ Which of the following is the correct order of increasing electronegativity (Pauling's scale)?
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- $\mathrm{D}<\mathrm{A}<\mathrm{B}<\mathrm{C}$
- $\mathrm{A}<\mathrm{B}<\mathrm{C}<\mathrm{D}$
- $\mathrm{A}<\mathrm{C}<\mathrm{B}<\mathrm{D}$
- $\mathrm{A}<\mathrm{D}<\mathrm{B}<\mathrm{C}$
The Correct Option is A
Solution and Explanation
Electronegativity increases from left to right in a period: C < N < O < F, that is D < A < B < C.
The correct option is (1).
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