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OBJECTIVES:OBJECTIVES:
CHAPTER 13 : HYDROCARBONSCHAPTER 13 : HYDROCARBONS
13.1 ALKANES13.1 ALKANES
1. State the natural sources of alkanes
2. Describe the combustion of alkanes in
-excess oxygen
-limited oxygen
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-limited oxygen
3. Explain the unreactivity of alkanes
4. Explain the halogenation reaction of alkanes
5. Explain the free radical subsitution mechanism
for methane, ethane and propane.
6. Explain the monosubstitution of alkane containing
equivalent type of hydrogen atoms as in neopentane
• Natural gas
• crude oil (petroleum)
Nature sources of Alkanes
CHAPTER 13 : HYDROCARBONSCHAPTER 13 : HYDROCARBONS
13.1 ALKANES13.1 ALKANES
Natural gas contains primarily methane (70%) and ethane (10%), with some propane (15%).
Crude oil is a mixture of liquid alkanes and other hydrocarbons
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Reaction of alkanes with oxygen
• Complete combustion (in excess of oxygen) of
alkanes to give carbon dioxide gas, water and heat.
CH4 + 2O2 → CO2 + 2H2O + heat
CHAPTER 13 : HYDROCARBONSCHAPTER 13 : HYDROCARBONS
13.1 ALKANES13.1 ALKANES
4 2 2 2
C2H6 + 7/2 O2 → 2CO2 + 3H2O + heat
• In limited supply of oxygen, combustion of alkanes
produces carbon monoxide and water.
CH4 + O2 → CO + 2H2O + heat
C2H6 + 5/2O2 → 2CO + 3H2O + heat
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Alkanes are nonreactive (inert) towards most reagents such
as acids, alkalis, oxidising agents or reducing agents because:
• are saturated hydrocarbons with no functional group; do
not undergo addition reactions.
Chemical Properties of Alkanes
CHAPTER 13 : HYDROCARBONSCHAPTER 13 : HYDROCARBONS
13.1 ALKANES13.1 ALKANES
not undergo addition reactions.
• are non-polar, electronegativity values of C & H almost
similar.
•have strong C — C and C — H covalent bonds
• have no unpaired electrons.
However under right conditions, alkanes may undergo
substitution rxn e.g.halogenation.
Halogenation of Alkanes
Alkanes react with halogens to produce haloalkanes in the presence of light or when heated.
R–H + X2
R–X + HX hv
or ∆
CHAPTER 13 : HYDROCARBONSCHAPTER 13 : HYDROCARBONS
13.1 ALKANES13.1 ALKANES
or ∆
The halogenation is a free-radical substitution reaction.
The mechanism involves initiation, propagation and
termination steps.
In the example; If CH3Cl is allowed to react with more
chlorine, further chlorination produces mixture of
CH2Cl2,CHCl3 & CCl4.
Example:
CH4+ Cl
2CH
3Cl + HCl
hv
Mechanism : Chlorination of methane
CH4 + Cl2 CH3Cl + HClhv
The equation of reaction is;
Mechanism
CHAPTER 13 : HYDROCARBONSCHAPTER 13 : HYDROCARBONS
13.1 ALKANES13.1 ALKANES
Step 1 : Chain initiation step:
In the presence of ultra-violet light / heat, the covalent
bond in the chlorine molecule undergoes homolyticfission to produce chlorine free radicals, Cl•.
Cl Cl
heatCl Cl+
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Step 2 : Chain propagation step:
Cl+H3C H CH3 + HCl
Mechanism : Chlorination of methane
CHAPTER 13 : HYDROCARBONSCHAPTER 13 : HYDROCARBONS
13.1 ALKANES13.1 ALKANES
These involve reaction between a free radical species
(Cl•) and a molecule (CH4) to produce a new free radical
species (CH3•).
CH3• propagates a chain reaction when it reacts with
another chlorine molecule to form CH3Cl and Cl•
Cl Cl ClCH3 + CH3Cl +
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Step 3 : Chain termination step:
Cl2Cl + Cl
Mechanism : Chlorination of methane
CHAPTER 13 : HYDROCARBONSCHAPTER 13 : HYDROCARBONS
13.1 ALKANES13.1 ALKANES
The chain is terminated when two free radicals
combine to form molecules.
CH3 + Cl CH3Cl
CH3 + CH3CH3CH3
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Note: in excess of chlorine, the propagation steps proceed with the reaction between chlorine free radical with
chloromethane to produce dichloromethane.
The reaction may continue to produce trichloromethane
and finally tetrachloromethane.
CH3Cl + Cl• → CH2Cl• + HCl
CHAPTER 13 : HYDROCARBONSCHAPTER 13 : HYDROCARBONS
13.1 ALKANES13.1 ALKANES
CH3Cl + Cl• → CH2Cl• + HCl
CH2Cl• + Cl2 → CH2Cl2 + Cl•
CH2Cl2 + Cl• → CHCl2• + HCl
CHCl2• + Cl2 → CHCl3 + •Cl
CHCl3 + Cl• → CCl3• + HCl
CCl3• + Cl2 → CCl4 + •Cl
2nd propagation
3rd propagation
4th propagation
CH3Cl + HClCH
4+ Cl2 →
hv
methane
Product of monochlorination of alkanes
CHAPTER 13 : HYDROCARBONSCHAPTER 13 : HYDROCARBONS
13.1 ALKANES13.1 ALKANES
CH3CH
2Cl + HCl
methane
CH3CH
3+ Cl2 →
hv
ethane
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CH3CH
2CH2Cl +
CH3CHClCH3 + HClCH
3CH
3CH3 + Cl2 →
hv
propane
Product of monochlorination of alkanes
CHAPTER 13 : HYDROCARBONSCHAPTER 13 : HYDROCARBONS
13.1 ALKANES13.1 ALKANES
C
CH3
H3C
CH3
CH2Cl + HClC
CH3
H3C
CH3
CH3+ Cl2 →
hv
neopentane
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• Bromine is less reactive toward alkanes than chlorine.
• Therefore bromine is more selective.• The % product yield is based on the stability of the free radical, 3o > 2o > 1o.
CH CHCH
Bromination of alkanes
CHAPTER 13 : HYDROCARBONSCHAPTER 13 : HYDROCARBONS
13.1 ALKANES13.1 ALKANES
+C
CH3
H3C CH3
Br
C
CH3
H3C CH2Br
H
>99 %
(major)trace
(minor)
C
CH3
H3C CH3
H
+ Br2
hν
127oC
C
CH3
H3C CH3
H
+ Cl2
hν
25oC
C
CH3
H3C CH2Cl
H
C
CH3
H3C CH3
Cl
+
37 % 63 %
The difference in selectivity between chlorination and bromination of alkanes need to be kept in mind when one wishes to prepare an alkyl halide from an alkane:
Halogenation of alkanes
CHAPTER 13 : HYDROCARBONSCHAPTER 13 : HYDROCARBONS
13.1 ALKANES13.1 ALKANES
1. Because chlorination of an alkane yields every possible monochloride, it is used only when all the hydrogen in an alkane are equivalent.
2. Bromination is normally used only to prepare tertiary alkyl bromides from alkanes.
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Exercises:
When a few drops of liquid bromine are added to
neopentane and the mixture is exposed to sunlight,
a reaction occurs.
CHAPTER 13 : HYDROCARBONSCHAPTER 13 : HYDROCARBONS
13.1 ALKANES13.1 ALKANES
a) State two observations that prove that a reaction
has indeed occurred.
b) Write the chemical equation for the reaction
between bromine and neopentane.
c) Write the mechanism for the reaction.
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