Summary
Aromaticity summary notes
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Includes everything you need to know about aromatic hydrocarbons , as well as most of questions about aromaticity such as evidence of the delocalised bonding model of benzene.
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Model of Benzene mustrememberring
each carbonatom isbonded with twoothercarbonatoms and a hydrogen atom
bySigma bond
a hexagon of 6 Sigma bonds are formed
theforth outer shell electronof a carbon atom in
is a Ip orbital
These Porbitalsoverlap
togive a donutshaped cloud ofelectrons aboveand below
thering andform one Tv bond The electrons inthis Tvbend aredelocalised
it burns with a very
luminous smoky flame
Evidence fordelocalisation
Modern X ray diffraction studies showthat thestructure of Benzene
2 The energy containedin realbenzene is lessthan thatcalculated the
benzene
ismorestable thanthekeKale structure suggests
the difference
ofenergy is thebend de
localisation
energy
energy thatisneeded todisrupt thedelocalised
sp orbitals in
benzene
note Benzenedoes not decolourise
Br
Benzenegenerallyreacts
bysubstitutionreactions
foradditionreaction the process disrupts the stable de
localised electron system
The activation energyneeded tobreak theTusystem istoobig
, One possible structure forColt6 that is not a ring
why not fit withKekule's for benzene
structure
CHECH CE C CH CHz
not fit as
Carbon carbonlength
not allthesame
therewillbe several isomers
thedoubleandtriplebondswillbevery reactive
Existence ofweak attractive forces between benzene molecules unchargedand
nonpolar
When benzene
molecules
approach each other movement
ofelectrons delocalised t electrons
sets
uptemporary dipoles
attractions between these
temporary dipole give vie te weak intermolecular forces
Van derWaals forces
us dipole dipole forces
1
interaction between molecule
attractionwhen two Polar molecules interact
44between moleculeExit
Tta ft f molecule
dipole dipoleforceare a type of Vander waals forces
d d more strongerthan vanderwaalsforces
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