CHEM103 Lecture Notes - Lecture 5: Electron Configuration, Effective Nuclear Charge, Problem Set
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Chem 103 lecture 5 shape of orbitals and their energies//electrostatic effects and splitting of energy levels. The case if hydrogen atom considered thus far is representative of one electron atoms, (solution obtained directly from the schr dinger equation). However, for marry-electron species, the presence of electron-electron repulsions causes the energy of the orbitals to vary in a complicated way. To account for these additional interactions, we need to consider 3 additional features: electron-spin quantum number, ms, maximum number of electrons an orbital can take, splitting of energy levels into sub-levels. An e- has magnetic properties ms = - (cid:2869)(cid:2870) (or spin down (counter clockwise)), (cid:2869)(cid:2870) (or spin up (clockwise)) Electrons with the same spin parallel spin. Electrons with different spin opposite spin http://boomeria. org/chemtextbook/cch9. html. No two electrons in an atom can have the same four quantum numbers. H = 1p 1e- n=1 l=0 ml = 0 ms = +1/2 or -1/2 n=1, l = 0, ml = 0, ms = +1/2.