Question

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, Eea? View Available Hint(s) 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, a. 5s2 b. 5s25p2 c. 5s25p5 d. 5s25p6

Answer 1

Answer:

"c" is the element with the most negative electron affinity.

Explanation:

We can obtain the following information from the electron configuration:

Period: Is the level in which the differential electron is in.

Group: Is the sum of all electrons in the last level.

Knowing their ubication in the periodic table, we can classify them as metals, nonmetals or noble gases.

a. 5s²            P: 5    G: IIA (2) Metal

b. 5s²5p²      P: 5    G: 2 + 2 = IVA (14) Nonmetal

c. 5s²5p⁵      P: 5    G: 2 + 5 = VIIA (17) Nonmetal

d. 5s²5p⁶      P: 5    G: 2 + 6 = VIIIA (18) Noble gas

Noble metals have a low tendency to gain electrons so their electron affinity is neglectable. For elements in the same period, the electron affinity gets more negative from left to right. Therefore, "c" is the element with the most negative electron affinity.

Answer 2

The configuration 5s25p5  must correspond to a halogen and must have the greatest electrons affinity.

Electron affinity is the ability of an atom to accept electrons and form a negative ion. It is a periodic property that decreases down the group but increases across the period.

The halogens usually have the greatest electron affinity as you move across the period. The halogens have outermost electron configuration ns2np5. Therefore, the configuration 5s25p5  must correspond to a halogen and must have the greatest electrons affinity.

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