handout - halogenoalkanes1
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Transcript of handout - halogenoalkanes1
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8/7/2019 handout - halogenoalkanes1
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alcohol
Primary amine
Halogenoalkanes
nitrileHeat under reflux NaOH(aq) in ethanol or water in ethanol
BOX 7a-A: REACTIONS OF HALOGENOALKANES
BOX 7a-B: HETEROLYTIC NUCLEOPHILIC SUBSTITUTION
HANDOUT 7a REACTIONS OF HALOGENOALKANES
Objectives:
recall the chemistry of halogenoalkanes as exemplified by the following nucleophilic substitution reactions of
bromoethane: hydrolysis, formation of nitriles, formation of primary amines by reaction with ammonia and by the elimination of hydrogen bromide from 2-bromopropane
describe the mechanism of nucleophilic substitution (by both SN1 and SN2 mechanisms) in halogenoalkanes
NH3(aq) in ethanol
Heat
KCN(aq) in ethanolHeat under reflux
Nucleophilic
substitutionNucleophilic
substitution
Nucleophilic
substitution
Heat under reflux
Pure NaOH in ethanol
alkene
This mechanism is associated with polar covalent bonds (e.g. carbon-halogen).
C B r
The positive charge on the carbon
allows attack by nucleophiles suchas :OH or :CN which have lone pairs to
donate.
SN2 MechanismThe mechanism involves the substitution of a nucleophile which is second order (two molecules in rate determining step).
C Br
H3C
HH
HO C Br
H3C
HH
HO C Br
CH3
HH
HO
transition state
The nucleophile attacks the C+ and
starts to form a covalent bond with it. At
the same time the C+-Hal bond starts
to break heterolytically.This is one continuous process with the
carbon-nucleophile bond gettingstronger and the carbon-halogen getting
weaker.
There are two mechanisms for
nucleophilic substitution, (1) SN1
and (2) SN2.
SN1 Mechanism
This mechanism involves the substitution of a
nucleophile which is first order (one molecule in rate
determining step). This mechanism occurs in two stages:
C
CH3
H3C Br
CH3
C
CH3
H3C Br
CH3
BOX 7a-B contd.
C
CH3
H3C
CH3
C
CH3
H3C
CH3
OH OH
Stage 1:
Stage 2:
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8/7/2019 handout - halogenoalkanes1
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HANDOUT 7b RELATIVE STRENGTH OF C-HAL BONDS
Objectives:
Interpret the different reactivities of halogenoalkanes e.g. CFCs, anaesthetics, flame retardants, and plastics with particular reference to hydrolysis and to the relative strengths of the
C-Hal bonds)
explain the uses of fluoroalkanes and fluorohalogenoalkanes in terms of their relative chemical inertness
recognise the concern about the effect of chlorofluoroalkanes on the ozone layernes
BOX 7b-A: REACTIVITIES OF HALOGENOALKANES
The relative strength of C-Hal bond is C-Cl > C-F > C-Br > C-I.
In general the greater the bond strength the lower the reactivity so that
fluorocarbons are less reactive than alkanes and the other haloalkanesincreasingly more reactive and less stable from Cl to I.
BOX 7b-B: THE USES OF HALOGEN COMPOUNDS
Due to their inertness and stability, many halogenoalkanes are used in
several purposes.
Plastics
Poly(chloroethene) or PVC and poly(tetrafluoroethene)/PTFE, also
known as Teflon are polymers which are synthesised from
halogenoalkanes.
Anaesthetics
Trichloromethane (chloroform), CHCl3, was once used as anaesthetics.
It was a better anaesthetics than ethoxyethane (ether) which was also
used an Anaesthetics Since ether is highly flammable. However,
although chloroform is not flammable, it causes liver damage. Therefore,
it is seldom in use now.
Flame retardants
Bromochlorodifluoromethane (BCF) is very effective at extinguishing fire.
However, it is not in beneral use because the breakdown products arepoisonous.
BOX 7b-B contd.
CFCs
Chlorofluorocarbons, for example dichlorodifluoromethane or
trichlorofluoromethane, have been used as refrigerant, aerosolpropellants or blowing agents.
The inertness and the high stability of CFCs are the reasons for
choosing these.
However, due to the stability, these agents accumulate in the
atmosphere and when they reach stratosphere, they undergo
photodissociation by ultraviolet radiation which produces chlorine free
radicals.The radicals decompose ozone into oxygen, thus depleting ozone layer
in the atmosphere.
Therefore, some governments have decided to restrict the uses of CFCs
and change to alternatives such as 1,1,1,2-tetrafluoroethane (CF3CH2F).
The presence of hydrogen atom increases its reactivity so it is brokendown more easily in atmosphere. Even if it reaches stratosphere, it does
not produce the damaging chlorine free radicals.