C2323SS1 - 1 C C h h e e m m 2 2 3 3 2 2 3 3 Study Sheet #1...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

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...
View Full Document

This note was uploaded on 04/29/2008 for the course CHEM 2323 taught by Professor Healy during the Spring '07 term at St. Edwards.

Page1 / 2

C2323SS1 - 1 C C h h e e m m 2 2 3 3 2 2 3 3 Study Sheet #1...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online