Electron configuration

Electron configuration - Electron Configurations...

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1 Electron Configurations Polyelectronic Atoms What if you have an atom other than H? Need to consider the number of protons AND the other electrons! Ergo: Attraction is causing electrons to be ‘sucked down’ while repulsion is pushing them away! ( ) 1 2 2 2 2 1 2 12 attraction attraction repulsion to nucleus e to nucleus e between e's ( ) 4 4 4 o o o Ze Ze e V r for two electrons r r r !" = + + !"""# !"""# !"""#
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2 Shielding and Z eff Reduction in full attraction of e - ’s to the nucleus due to repulsion of other electron is called SHIELDING Effective nuclear charge = Z eff 2 2 ; eff n eff Z h E Z Z n ! = " Penetration: Ability of an electron in a particular orbital to get close (or closer) to the nucleus than another; more nodes, less ability to ‘burrow’ to nucleus; closer you can get to the nucleus, the lower your energy. Thus: s orbitals < p orbitals < d orbitals< f orbitals (precise order a function of number of e - ’s) Electron “Filling” Three rules are needed to be able to write electron configurations: 1. Aufbau Principle : electrons fill from the lowest energy orbital to the highest; 2. Pauli Exclusion Principle : no more than two electrons may occupy an orbital with the same n, l and ml values, and each must have a different ms value ( spin pairing ); 3. Hund s Rule : electrons only spin pair when they must since spin pairing costs energy.
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3 Orbital Filling Order For gas phase atoms, the filling order is as follows:
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Electron configuration - Electron Configurations...

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