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Question

Arrange the elements with the following electronic configurations in the increasing order of electron affinity

(i) 1s2 2s2 2p3 (ii) 1s2 2s2 2p4 (iii) 1s2 2s2 2p5 (iv) 1s2 2s2 2p63s2 3p4


A

i < iv < ii< iii

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B

iv < iii < ii < i

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C

i < ii < iv < iii

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D

ii < iii < i < iv

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Solution

The correct option is C

i < ii < iv < iii


The elements are

(i) N (ii) O (iii) F (iv) S

Now, we can arrange them in the order of electron affinity. Nitrogen has a negative electron affinity - meaning, it would "take" energy to put in one more electron into the already exactly half-filled 2p3 orbital. We can consider the electron affinity to be 0 as per the recent convention. Flourine is the most electronegative element and from the given elements, it will have the highest EA value. Sulphur has a higher electron affinity than oxygen. This is an anomaly.

N < O < S < F


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