JEE Main 2025 Apr 2 Shift 2, Chemistry Q10: Periodicity In Atomic Properties

JEE Main2025Apr 2, Shift 2Chemistry

Electronic configuration of four elements A, B, C and D are given below :

(A) $1 s^{2} 2 s^{2} 2 p^{3}$

(B) $1 s^{2} 2 s^{2} 2 p^{4}$

(D) $1 s^{2} 2 s^{2} 2 p^{2}$

Which of the following is the correct order of increasing electronegativity (Pauling's scale) ?

Solution

Identifying the elements from the configurations: A is N, B is O, C is F and D is C, all in period 2.

Pauling electronegativities: C $= 2.55$ , N $= 3.04$ , O $= 3.44$ , F $= 3.98$ .

Across period 2, electronegativity increases from left to right, so:

$C < N < O < F$ , i.e. D $<$ A $<$ B $<$ C.

Concept behind this question

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