What is the general relationship between electron affinity and increasing atomic number?

Answer 1

On a periodic table, affinity increases along a period from left to right between the alkali metals (which tend to give up electrons to gain a filled lower-energy valence shell) to the halogens (which tend to attract electrons to fill a valence shell). The noble gases do not tend to give up or attract electrons, as they already have a filled shell. Thus halogens have the largest electron affinities.

As period increases, more shells are filled. The outer shells have a higher potential energy and leave the atom more easily. Thus, the electron affinity decreases with increasing period along a given group.

Answer 2

Electron affinity increases as one goes across a row, but it does not always increase with atomic number in a group. There are some noted deviations to the general relationship, especially when you encounter atoms with completely filled or half-filled subshells (e.g. nitrogen has a lower electron affinity than carbon does, due to the half-filled 2p subshell).

Answer 3

E.A is similar to E.N... for example, a halogen has a great E.A because it wants the electron to complete its outer shell, whereas Alkali metals have low EA because it doesn't want electrons...
So from left to right, EA goes up (cept for the inert gasses)
from top to bottom EA goes down, but there are so many exceptions in this case

Answer 4

A ) order F, Cl, Br, I (order of length will develop with Z (atomic selection) B) order I, Br, Cl, F ( the order is inverse of A . The smaller the atom , the greater suitable the ionization power) C) I, Br, Cl, F as B

Answer 5

there electrons have to balance out the protons or else the charge isnt neutral.