orbital-shape-orientation-handout - Periodic table and...

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Shapes and Orientations of Orbitals Periodic table and quantum theory • The 2, 6, 10, 14 columns of the periodic table correspond to s (l=0, m l =0), p (l=1, m l = -1,0,1), d (l=2, m l = -2,-1,0,1,2) and f (-3,-2,-1,0,1,2,3) • See fig. 6.21 (pg. 208) and fig. 6.22 (pg. 209) • Note that electron configurations are true whether we are speaking of an atom or ion: 1s 2 2s 2 2p 6 describes both Ne and Na + Q – based on figure 6.22 what are the shorthand electron configurations for Br , Sn, Sn 2+ , Pb? Unusual electron configurations • Reference: 6.8 (pg. 207 - 8) • Look at your value for Cu ([Ar]4s 2 3d 9 ). • The actual value for Cu is [Ar]4s 1 3d 10 … why? • The explanation is that there is some sort of added stability provided by a filled (or half- filled subshell). • The only exceptions that you need to remember are Cr, Cu, Ag, and Au. • The inner transition elements also do not follow expected patterns. However, we do not address this in OAC chemistry. Heisenberg’s uncertainty principle
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