Question

The correct order of electron affinities for nitrogen oxygen sulphur and chlorine is

Answer 1

Explanation:

increasing order : N, O, S, Cl

Answer 2

The correct order of electron affinities is  oxygen > nitrogen > chlorine > sulphur

Explanation:

Electron affinity is the amount of energy required when an electron is added to a gaseous neutral atom to form a negative ion. This is expressed in kJ/mol.

$X(g)+e^-\rightarrow X^-(g)$

Electron affinity would typically increase as you move across the periodic table. Electron affinity would typically decrease as you move down the periodic table.

a) Nitrogen : Electronic configuration of nitrogen = $1s^22s^22p^3$      

As the 2p sub-shell can acquire three electrons to form a negative ion. The energy released will be more because 2p sub-shell is close to the nucleus and the extra electron will be held strongly by the nucleus.

b) Oxygen :  Electronic configuration of Oxygen = $1s^22s^22p^4$      

As the 2p sub-shell can acquire two electrons to form a negative ion. The energy released will be more because 2p sub-shell is close to the nucleus and the extra electron will be held strongly by the nucleus.

c) Sulphur: Electronic configuration of sulphur = $1s^22s^22p^63s^23p^4$             

As the 3p sub-shell of this element can acquire two electrons to form a negative ion. But, the energy released will be less because 3p sub-shell is not close to the nucleus and the extra electron will not be held strongly by the nucleus.

d) Chlorine : Electronic configuration of chlorine = $1s^22s^22p^63s^23p^5$             

As the 3p sub-shell of this element can acquire one electron to form a negative ion. But, the energy released will be less because 3p sub-shell is not close to the nucleus and the extra electron will not be held strongly by the nucleus.

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