Consider the addition of an electron to the following atoms from the fourth period. Rank the atoms in order from the most negative to the least negative electron affinity values based on their electron configurations. Atom or ion Electron configuration BrBr 1s22s22p63s23p64s23d104p51s22s22p63 s23p64s23d104p5 GeGe 1s22s22p63s23p64s23d104p21s22s22p63 s23p64s23d104p2 KrKr 1s22s22p63s23p64s23d104p61s22s22p63 s23p64s23d104p6 Rank the electron affinity from most negative to least negative. To rank items as equivalent, overlap them. View Available Hint(s)

Br>Ge>Kr

Explanation:

Electron affinity is the energy change that results from adding an electron to a gaseous atom(Khan Academy). It is also defined as "the amount of energy released when an electron is attached to a neutral atom or molecule in the gaseous state to form a negative ion" (Wikipedia).

Electron affinity increases from left to right in the periodic table. However, the noble gases possess a complete outermost electron shell.

Hence, electron affinity can be raked from the most negative to the least negative for the three atoms as follows; Br>Ge>Kr

i think it is true since you can test the answer and can use observations to complete it.