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Very simple question I'm sure, but I'm not understanding why the answer is A instead of B. Wouldn't the excited electron skip the 3D subshell and jump to 4S?
Excited electron configuration
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Very simple question I'm sure, but I'm not understanding why the answer is A instead of B. Wouldn't the excited electron skip the 3D subshell and jump to 4S?
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4s electrons are lower in energy than 3d. That is why potassium and calcium are 4s1 and 4s2 then scandium is 4s2 3d1.
In answer A, the electrons skipped 3p6 and 4s2 to end up in 3d10. This is obviously the excited atom. Remember the pattern:
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 5d/4f (some switching in there to confuse the issue) 6p... And so on. Looking at the periodic table helps to see the pattern if you understand what the SHAPE of the periodic table means.
dsoz
In answer A, the electrons skipped 3p6 and 4s2 to end up in 3d10. This is obviously the excited atom. Remember the pattern:
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 5d/4f (some switching in there to confuse the issue) 6p... And so on. Looking at the periodic table helps to see the pattern if you understand what the SHAPE of the periodic table means.
dsoz
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