CHEM1201 Lecture 5: Week 4 lecture 2
Why do we need sub-shell notation?
Maximum occupancy varies with principal quantum number
- n = 1 1s can hold 2 electrons
- n = 2 2s, 2p can hold 8 electrons
- n = 3 3s, 3p, 3d can hold 18 electrons
- n = 4 4s, 4p, 4d, 4f can hold 32 electrons
- but exceptions occur when we go past 18 electrons in total
- as 4s is lower in energy than 3d
- 1s22s22p63s23p3 = [Ne] 3s23p3
-
- [Ar] 4s23d104p3
Abbreviating configuration can make the number of valence electrons clearer
Core electrons are filled shells (the Ar part of the As configuration) i.e. 4s23d104p3 are the
valence electrons of As
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