Consider the following neutral electron configurations in which n has a constant value. Which configuration would belong to the element with the most negative electron affinity, E-ea?

a. ns^2
b. ns^2 np^2
c. ns^2 np^5
d. ns^2 np^6

The answer cannot be ns^2 since any atom with this configuration must be a metal in group 2. Secondly, ns^2 np^2 is an element in group 14. Again, this specie cannot have the most negative electron affinity. The atom whose outermost electron configuration is ns^2 np^6 must be a noble gas since the outermost shell possesses eight electrons. This cannot be the answer we are seeking for.

However, an outermost electron configuration of ns^2 np^5 will apply to a halogen. Halogens have a very negative electron affinity. Hence a specie with this electron configuration must have the most negative electron affinity among the options.

Eduard22sly Eduard22sly · Answer 2 · 2021-09-27T16:48:43+02:00

The correct answer to the question is Option C. ns² np⁵

Let n represent the valence shell.

NOTE: Valence shell is the outermost shell of an atom.

Thus, we shall determine the valence electrons for each options given in the question.

For Option A

Valence shell = ns²

Valence electron = 2

For Option B

Valence shell = ns²np²

Valence electron = 2 + 2

Valence electron = 4

For Option C

Valence shell = ns²np⁵

Valence electron = 2 + 5

Valence electron = 7

For Option D

Valence shell = ns²np⁶

Valence electron = 2 + 6

Valence electron = 8

Electronegativity is the tendency of an atom to attract electron(s). Atoms with more valence electrons tends to attract electrons more.

From the illustraton above, we can see that Option C has 7 valence electrons while Option D has 8 valence

Option D shows that the atom has completely filled outermost shell and as such, it does not attract electron(s)

Option C has the highest valence electron (i.e 7) besides option D which do not attract electrons. Therefore, atom with 7 valence electrons will have a higher electronegativity.

Therefore, Option C. ns² np⁵ gives the correct answer to the question.

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Consider the following neutral electron configurations in which n has a constant value. Which configuration would belong to the element with the most negative electron affinity, E-ea? a. ns^2 b. ns^2 np^2 c. ns^2 np^5 d. ns^2 np^6

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