Structure and Properties of Organic Molecules
I.  Wave Properties of Electrons - Review s and p orbitals
II.  Bonding involving atomic orbitals 
	LCAO (linear combination of AO) on different atoms gives rise to Molecular 
Orbitals (MO) whereas LCAO on same atom gives rise to hybrid orbitals
	in general, linear combination of X atomic orbitals results in generation of either X
 molecular orbitals or X hybrid orbitals
III.  Types of bonding
	A.  sigma bonding
		a.  involving combination of two s-orbitals: H-H molecule
		MO = 1s1 +- 1 s1 gives rise to two MO
		the lower energy one is bonding and the higher energy is anti-bonding
		two electrons go into bonding MO where electron density is between the 
hydrogen atoms, that is in the sigma bonding MO
		b.  involving combination of two p-orbitals - F-F - same story.
	B. Pi bonding - sidewise overlapping of p orbitals - 
		consider ethylene and acetylene
IV. Hybridization - linear combination of s and p orbitals on same atom.
	A.  sp3 - combination of an s orbital with 3 pi orbitals gives rise to four sp3 orbitals
	bonds are separated from each other as far as possible- tetrahedral molecule 109 o
 bond angles
	NOTE that the number of hybrid orbitals is equal to number of sigma bonds plus 
lone pair electrons.
		Case I - four sigma bonds - methane CH4 
		Case II - three sigma bonds and one lone pair - ammonia - 
		NOTE: Shapes of molecular as deduce by x-ray crystallography are 
determined by nuclear positions - can't see lone pair electrons- thus ammonia is pyramidal
		Case III- two sigma bonds and two lone pair - methanol 
	can't see two lone pair so shape of methanol is bent
	B.  sp2 - combination of an s orbital with 2 pi orbitals - three sp2 hybrid orbitals
 - trigonal planar 120 o bond angles. 	
		Case I - three sigma bonds + one pi bond
		ethylene and formaldehyde
	C. sp - combination of an s and p orbital - linear bond angle of 180o.
	acetylene, HCN
	D.  resonance structures - consider CH2NH2 +
		need to have p-orbitals for resonance delocalization - thus hybridization with 
largest number of p-orbitals is required.  in cation depicted above nitrogen is sp2 
hybridized which allows it to donate a pair of electrons to give a second resonance 
structure.
V.  Miscellaneous items
	A.  rotation about single bonds	
	B.  rigidity of pi bonds - cis-trans isomerism
	C.  polarity of bonds and molecules	
VI.  Intermolecular attraction between molecules
	A.  London forces
	B.  Dipole-dipole forces
	C.  H-bonding
VII.  Polar effects on solubility
VIII.  Functional Groups concept
	Hydrocarbons: alkanes, alkenes, alkynes, aromatics
	Oxygen-containing aldehydes, ketones, alcohols, carboxylic acids and their 
derivatives - esters and anhydrides
	Nitrogen-containing amines, amides and nitriles