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

"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.

periodic trends is an atom that gets larger as the number of electronic shells increase, the radius of atoms increases as you go down a certain group in the periodic table of elements. in general, the size of an atom will decrease as you move from left to right of a certain period.

lol for the pointsss