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Unformatted text preview: 1 C C h h e e m m 2 2 3 3 2 2 3 3 Study Sheet #1 Topic : Structure and Bonding Reference : McMurry chpt.1-2 I. Atomic Structure pages : 3-7 Modern organic chemistry involving structure, mechanism and classification was facilitated by quantum mechanics. Before this organic chemistry was essentially descriptive with little underlying form. (i) The theory of quantum mechanics provides us with the concept of quantum numbers. With quantum numbers we arrive at electronic orbitals, leading to the familiar concepts of S, P & D orbitals : principal n = 1,2,3.. angular l = 0,1,2,3.... n-1 magnetic m l = - l ,...0,...+ l l =0 m l = 0 l =1 m l = -1,0,+1 spin m s = 1/2 (ii) Pauli exclusion principle states that no two electrons can have the same four quantum numbers. This leads to the allocation of at most 2 electrons per atomic (and molecular) orbital. Filling orbitals follow the sequence of increasing n+l ., the aufbau principle , Hund's rule states that the most stable electronic configuration maximizes the number of unpaired electrons e.g C (6e- ) n=1 l=0 m l =0 m s = 1/2 1s 2 n=2 l=0 m l =0...
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