Electronic configuration of elements:
Electronic configuration of elements Electrons are distributed around the nucleus in an orbital The distribution of electron density is described using quantum numbers: n Principle quantum number Position l Angular quantum number Shape m l Magnetic quantum number Orientation m s Spin quantum number Spin
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n Principle QN (n = 1, 2, …) l Angular QN (l = n – 1) ml Magnetic QN — l to + l ms Spin QN +1/2, -1/2 no. e -1 s 1 2 3 4 0 (s) 0 (s) 1(p) 0 (s) 1(p) 2 (d) 0 (s) 1(p) 2 (d) 3 (f) 0 0 -1, 0,+1 0 -1,0,+1 -2,-1,0,+1,+2 0 -1,0,+1 -2,-1,0,+1,+2 -3, -2,-1,0,+1,+2,+3 +1/2, -1/2 +1/2, -1/2 +1/2, -1/2 +1/2, -1/2 +1/2, -1/2 +1/2, -1/2 +1/2, -1/2 +1/2, -1/2 +1/2, -1/2 +1/2, -1/2 1*2=2 2 1*2=2 3*2=6 8 1*2=2 3*2=6 5*2=10 18 1*2=2 3*2=6 5*2=10 7*2=14 32 1s 2 , 2s 2 , 2p 6 , 3s 2 , 3p 6 ,3d 10 , 4s 2 , 4p 6 ,4d 10 ,4f 14 …
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Rules Auf Bau principle - Lower E first Pauli’s exclusion principle ( No same n, l, m l and m s ) n, l, m l can be same, m s has to be different Hundt’s rule (Empty orbitals first, pairing later)
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1s 2 , 2s 2 ,2p 6 , 3s 2 ,3p 5 1s 2 ,2s 2 ,2p 6 , 3s 1 1s 2 , 2s 2 ,2p 6 , 3s 2 ,3p 1 1s 2 ,2s 2 ,2p 6 1s 2 , 2s 2 ,2p 6 ,3s 2 ,3p 6 1s 2 , 2s 2 ,2p 6 ,3s 2 ,3p 6 , 4S 2 [Ne]3S 1 [Ne]3S 2 ,3p 1 [Ne]3S 2 ,3p 5 [Ar]4S 2 1s 2 2s 2 2p 4