Problem: Which of the following is the correct noble gas electron configuration for an ion of barium?a) [Kr]5s24d105p66s2b) [Kr]5s25p6 c) [Kr] 5s24d105p66s1d) [Kr] 5s24d105p6 e) [Kr] 5s24d105p66s26p2

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We’re being asked to determine the correct noble gas electron configuration of a Barium (Ba) ion

Before we can do that, we have to first write the electron configuration of a neutral ground state barium (Ba).


You can determine the ground-state electron configuration of Barium (Ba) by locating the position Ba in the periodic table.

Ground-state means that the element is in its lowest energy form (not in excited state). Neutral barium means it has no charge, meaning no electrons are removed or added in the atom.

You see in the above illustration of the periodic table that Ba is in Period 6, Group 2A, and s-block

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Problem Details

Which of the following is the correct noble gas electron configuration for an ion of barium?

a) [Kr]5s24d105p66s2

b) [Kr]5s25p6 

c) [Kr] 5s24d105p66s1

d) [Kr] 5s24d105p

e) [Kr] 5s24d105p66s26p2



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