Electronic configuration of four elements A, | vedclass

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(D) Identify the elements based on their electronic configurations: $A: 1s^2 2s^2 2p^3$ is Nitrogen $(N)$,Electronegativity $\approx 3.04$. $B: 1s^2 2

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$D < A < B < C$

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(D) Identify the elements based on their electronic configurations: $A: 1s^2 2s^2 2p^3$ is Nitrogen $(N)$,Electronegativity $\approx 3.04$. $B: 1s^2 2s^2 2p^4$ is Oxygen $(O)$,Electronegativity $\approx 3.44$. $C: 1s^2 2s^2 2p^5$ is Fluorine $(F)$,Electronegativity $\approx 3.98$. $D: 1s^2 2s^2 2p^2$ is Carbon $(C)$,Electronegativity $\approx 2.55$. Electronegativity increases across a period from left to right in the periodic table. The order of increasing electronegativity is $C < N < O < F$,which corresponds to $D < A < B < C$.

Electronic configuration of four elements $A, B, C$ and $D$ are given below $:$
$(A) 1s^2 2s^2 2p^3$
$(B) 1s^2 2s^2 2p^4$
$(C) 1s^2 2s^2 2p^5$
$(D) 1s^2 2s^2 2p^2$
Which of the following is the correct order of increasing electronegativity $(Pauling's scale)$?

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Electronic configuration of four elements $A, B, C$ and $D$ are given below $:$$(A) 1s^2 2s^2 2p^3$$(B) 1s^2 2s^2 2p^4$$(C) 1s^2 2s^2 2p^5$$(D) 1s^2 2s^2 2p^2$Which of the following is the correct order of increasing electronegativity $(Pauling's scale)$?