Multi-Electronic Atoms

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Presentation transcript:

Multi-Electronic Atoms The “electron correlation problem” Total energy of the electron Since electron pathways are unknown…electron-electron repulsions can not be calculated exactly Electrostatic interactions will influence the potential energy nucleus-electron (attractions) electron-electron (repulsions)

Zeff = Zact – repulsive effects Potential energy electron possesses as a result of what it appears to feel from the nucleus can be simulated in the Wave Equation to calculate possible positions were electron can be found: The amount of energy the electron must receive to be taken to the infinite energy level produces 2p+ 2p+ e- e- e- Hydrogen-like orbitals He the atom He the ion Ionization energy = 3.94 x 10-21 kJ Ionization energy = 8.718 x 10-21 kJ Charge felt by the electron from the nucleus is apparently lessened!

Rules for configuring electrons in orbitals The AUFBAU Principle: Fill up the lowest energy orbitals available first. The PAULI EXCLUSION Principle: No electron in the same atom can have the same set of quantum numbers (i.e. only two electrons per orbital). HUNDS Rule: Fill up degenerate orbitals individually with the same spin before you pair them up.

x 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f

Outermost Configuration & Number of Unpaired Electrons Outside Desks ….Hafnium 5d2, 2 unpaired electrons Inside Desks ….Holmium 4f11, 3 unpaired electrons