ch8 - Chem 31D F07 Lecture Notes Ch. 8 Electron...

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Chem 31D F07 Ch. 8 – Electron Configuration and Chemical Periodicity Page 1 of 13 Chem 31D F07 – Lecture Notes Ch. 8 – Electron Configuration and Chemical Periodicity I. Many Electron Atoms ± For atoms with more than one electron, we use the same orbitals (phew!) BUT their energies are not the same. ± Electron energies can be related to the effective nuclear charge (Z eff ) they experience in an orbital: eff Z ZS = Electrons in inner shells can shield the outer shell electrons from the full positive charge ( Z ) of the nucleus. S is the shielding factor. However, shielding is incomplete, so the negative charge of each inner electron does not completely neutralize a single positive charge in the nucleus. In general , the ability to shield nuclear charge decreases with increasing l quantum number (i.e., S s > S p > S d > S f ). Note that the subscript represents the inner electrons, not the outer electron we are considering. Now: 2 2 eff nH Z ER n ⎛⎞ =− ⎜⎟ ⎝⎠
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Chem 31D F07 Ch. 8 – Electron Configuration and Chemical Periodicity Page 2 of 13 Many electron energy levels ± Energy increases with increasing n ± In general : for a fixed value of n , energies increase with increasing values of l . (i.e., E d > E p > E s ) Electron spin – the 4 th quantum number The Electron Spin Quantum Number: m s = +½ or -½ Specifies a specific electron in an orbital (Note: electrons don’t really spin)
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Chem 31D F07 Ch. 8 – Electron Configuration and Chemical Periodicity Page 3 of 13
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This note was uploaded on 02/17/2012 for the course CHEM 212 taught by Professor Staff during the Fall '10 term at Rutgers.

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ch8 - Chem 31D F07 Lecture Notes Ch. 8 Electron...

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