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Home :FAQ :Electrons in atomsPrint | Comment
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Why does the 4s subshell fill before the 3d subshell?

When filling subshells in an electron configuration, why do you get to level 4s, then jump back to level 3d and so forth?
sboone@llion.org

Quantum theory shows that each atom's electronic structure is a unique compromise between several different effects. Electronic configurations of the fourth period elements can be appreciated by considering these effects:

  • Raising n raises orbital energy. Electrons are attracted to the nucleus. To pull an electron farther away from the nucleus, you have to work against that attraction. That means an electron farther from the nucleus has more energy than electron closer in; energy is required to move the electron out, and energy can be released when the electron moves in. So we expect outer shells to have higher energies than inner shells, because increasing n increases the average distance between the nucleus and the electron.

    For atoms heavier than copper this effect dominates, and 4s electrons have higher energy than 3d electrons.

  • Raising l raises orbital energy. Higher l values result in orbitals with more nuclear nodes (a node being a place where the probability of finding the electron is zero). We say high-l orbitals are "less penetrating" because their electrons have a lower probability of being found at or near the nucleus. That gives high-l orbitals (like d orbitals) more energy than low-l orbitals (like s orbitals) within the same shell.

    This effect causes 4s orbitals to have lower energy than 3d orbitals for elements lighter than copper. (Although for hydrogen, the unoccupied 4s and 3d orbitals have nearly identical energies).

  • Within a subshell, more unpaired spins means a lower overall energy. Quantum mechanics predicts that the motions of electrons with paired spins are "correlated". Paired electrons move together, while electrons with unpaired spins can stay farther away from each other on average. Since electrons repel each other, paired electrons have more energy than unpaired electrons, all other things being equal. This spin correlation effect explains why Cr has a [Ar] 4s13d5 configuration rather than a [Ar]4s23d4 configuration- the former has more unpaired electron interactions than the latter.

Author: Fred Senese senese@antoine.frostburg.edu



General Chemistry Online! Why does the 4s subshell fill before the 3d subshell?

Copyright © 1997-2010 by Fred Senese
Comments & questions to fsenese@frostburg.edu
Last Revised 02/15/10.URL: http://antoine.frostburg.edu/chem/senese/101/electrons/faq/4s-3d.shtml