Chapter –02 Chemistry of Alk ane s -...
Transcript of Chapter –02 Chemistry of Alk ane s -...
Basic Organic ChemistryCourse code : CHEM 12162
(Pre-requisites : CHEM 11122)
Chapter – 02Chapter – 02
Chemistry of Alkanes
Dr. Dinesh R. Pandithavidana
Office: B1 222/3
Phone: (+94)777-745-720 (Mobile)
Email: [email protected]
Introduction:
• Recall that alkanes are aliphatic hydrocarbons having C—C
and C—H σ bonds. They can be categorized as acyclic or
cyclic.
• Acyclic alkanes have the molecular formula CnH2n+2 (where n
= an integer) and contain only linear and branched chains of
carbon atoms. They are also called saturated hydrocarbons
Alkanes
carbon atoms. They are also called saturated hydrocarbons
because they have the maximum number of hydrogen atoms
per carbon.
• Cycloalkanes contain carbons joined in one or more rings.
Because their general formula is CnH2n, they have two fewer
H atoms than an acyclic alkane with the same number of
carbons.
Introduction:
• All C atoms in an alkane are surrounded by four groups,
making them sp3 hybridized and tetrahedral, and all bond
angles are 109.5°.
• The 3-D representations and ball-and-stick models for these
Alkanes
• The 3-D representations and ball-and-stick models for these
alkanes indicate the tetrahedral geometry around each C
atom. In contrast, the Lewis structures or structural formulas
are not meant to imply any 3-D arrangement.
• Additionally, in propane and higher molecular weight
alkanes, the carbon skeleton can be drawn in a variety of
ways and still represent the same molecule.
• The three-carbon alkane CH3CH2CH3, called propane, has a
Alkanes
• The three-carbon alkane CH3CH2CH3, called propane, has a
molecular formula C3H8. Note in the 3-D drawing that each
C atom has two bonds in the plane (solid lines), one bond in
front (on a wedge) and one bond behind the plane (on a
dashed line).
Introduction:
Alkanes
Alkanes
Number Molecular Name
of C atoms formula (n-alkane) .
11 C11H24 undecane
12 C12H26 dodecane
Names of straight chain alkanes:
12 26
13 C13H28 tridecane
14 C14H30 tetradecane
15 C15H32 pentadecane
16 C16H34 hexadecane
17 C17H36 heptadecane
18 C18H38 octadecane
19 C19H40 nonadecane
Cycloalkanes:
Cycloalkanes have molecular formula CnH2n and contain
carbon atoms arranged in a ring. Simple cycloalkanes are
named by adding the prefix cyclo- to the name of the acyclic
alkane having the same number of carbons.
Alkanes
Nomenclature:
The name of every organic molecule has 3 parts:
1. The parent name indicates the number of carbons in the
longest continuous chain.
2. The suffix indicates what functional group is present.
3. The prefix tells us the identity, location, and number of
Alkanes
3. The prefix tells us the identity, location, and number of
substituents attached to the carbon chain.
• The carbon substituents bonded to a long carbon chain are
called alkyl groups.
• An alkyl group is formed by removing one H atom from an
alkane.
• To name an alkyl group, change the –ane ending of the
Alkanes
Nomenclature:
• To name an alkyl group, change the –ane ending of the
parent alkane to –yl. Thus, methane (CH4) becomes
methyl (CH3-) and ethane (CH3CH3) becomes ethyl
(CH3CH2-).
Naming three- or four-carbon alkyl groups is more
complicated because the substituent can have isomeric
forms. For example, propane has both 1° and 2° H atoms,
and removal of each of these H atoms forms a different
alkyl group with a different name, propyl or isopropyl.
Alkanes
Nomenclature:
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1. Find the parent carbon chain and add the suffix.
Alkanes
Rule 1:
The parent is the longest continuous chain of carbon atoms.
Note that if there are two chains of equal length, pick the chain
with more substituents to simplify naming. In the following
example, two different chains in the same alkane have seven C
atoms. We circle the longest continuous chain as shown in the
diagram on the left, since this results in the greater number of
substituents.
Alkanes
2. Number the atoms in the carbon chain from the end
that gives the first substituent the lowest number.
Alkanes
Rule 2:
If the first substituent is the same distance from both ends,
number the chain to give the second substituent the lower
number.
Alkanes
When numbering a carbon chain results in the same numbers
from either end of the chain, assign the lower number
alphabetically to the first substituent.
Alkanes
3. Name and number the substituents.
• Name the substituents as alkyl groups.
• Every carbon is part of the longest chain or a part of a
substituent, not both.
• Each substituent needs its own number.
• If two or more identical substituents are bonded to the longest
AlkanesRule 3:
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• If two or more identical substituents are bonded to the longest
chain, use prefixes to indicate how many: di- for two groups,
tri- for three groups, tetra- for four groups, etc.
4. Finally, write the name.• Substituent names and numbers come before the parent.
• List substituents in alphabetical order, ignoring all prefixes except iso, as in
isopropyl and isobutyl.
• Separate numbers by commas and separate numbers from letters by
hyphens. The name of an alkane is a single word, with no spaces after
hyphens and commas.
Alkanes
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Cycloalkanes are named by using similar rules, but the prefix
cyclo- immediately precedes the name of the parent.
CycloalkanesCycloalkane Nomenclature:
1. Find the parent cycloalkane.
2. Name and number the substituents. No number is
needed to indicate the location of a single substituent.
For rings with more than one substituent, begin numbering at
one substituent and proceed around the ring to give the second
Cycloalkanes
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one substituent and proceed around the ring to give the second
substituent the lowest number.
With two different substituents, assign numbers to the
substituents alphabetical order.
Cycloalkanes
In the case of an alkane having a long chain substituent, if the number of
carbons in the ring is greater than or equal to the number of carbons in the
longest chain, the compound is named as a cycloalkane.
Naming compounds containing both a ring and a long
chain of carbon atoms
Examples of cycloalkane nomenclature
Cis-Trans Isomerism
• Cis: like groups on same side of ring
• Trans: like groups on opposite sides of ring
Major Uses of Alkanes
• C1-C2: gases (natural gas)
• C3-C4: liquified petroleum (LPG)
• C5-C8: gasoline
• C9-C16: diesel, kerosene, jet fuel
• C17-up: lubricating oils, heating oil
• Origin: petroleum refining
Synthesis of Alkanes
1. Reduction of an alkyl halide
a) hydrolysis of a Grignard reagent
b) with an active metal and an acid
2. Corey-House synthesis
(coupling of an alkyl halide with lithium
dialkylcopper)
1.Reduction of an alkyl halide
a) hydrolysis of a Grignard reagent (two steps)
i) R—X + Mg � RMgX (Grignard reagent)
ii) RMgX + H2O � RH + Mg(OH)X
CH3CH2CH2-Br + Mg � CH3CH2CH2-MgBr
n-propyl bromide n-propyl magnesium bromide
CH3CH2CH2-MgBr + H2O � CH3CH2CH3 + Mg(OH)Br
propane
CH3 CH3
CH3CH-Br + Mg � CH3CH-MgBrisopropyl bromide isopropyl magnesium bromide
CH3
CH3CH-MgBr + H2O � CH3CH2CH3
propane
CH3CH2CH2-MgBr + D2O � CH3CH2CH2D
heavy water
CH3 CH3
CH3CH-MgBr + D2O � CH3CHD
b) with an active metal and an acid
R—X + metal/acid � RH
active metals = Sn, Zn, Fe, etc.
acid = HCl, etc. (H+)
CH CH CHCH + Sn/HCl � CH CH CH CH + ClCH3CH2CHCH3 + Sn/HCl � CH3CH2CH2CH3 + Cl2Cl
sec-butyl chloride n-butane
CH3 CH3
CH3CCH3 + Zn/H+ � CH3CHCH3 + ZnBr2
Brtert-butyl bromide isobutane
2. Corey-House synthesis
R-X + Li � R-Li + CuI � R2CuLi
R2CuLi + R´-X � R—R´ (alkane)
(R´-X should be 1o or methyl)
This synthesis is important because it affords a synthesis
of a larger alkane from two smaller alkyl halides.
note: the previous equations are not balanced:
R-X + 2 Li � R-Li + LiX
2 R-Li + CuI � R2CuLi + LiX
R
R2CuLi = R-Cu-, Li+
R2CuLi + R´X � R-R´ + RCu + LiX
CH3 CH3 CH3
CH3CH-Br + Li � CH3CH-Li + CuI � (CH3CH)2-CuLiisopropyl bromide
CH3 CH3
(CH3CH)2-CuLi + CH3CH2CH2-Br � CH3CH-CH2CH2CH3(CH3CH)2-CuLi + CH3CH2CH2-Br � CH3CH-CH2CH2CH3
2-methylpentane
(isohexane)
Note: the R´X should be a 1o or methyl halide for the best yields
of the final product.
Reactions of Alkanes
1. Combustion (oxidation)
2. Pyrolysis (cracking)
3. Halogenation
1. Combustion
CnH2n+2 + O2, flame � n CO2 + (n+1) H2O + heat
gasoline, diesel, heating oilG
2. Pyrolyis (cracking)2. Pyrolyis (cracking)
alkane, 400-600oC � smaller alkanes + alkenes + H2
Used to increase the yield of gasoline from petroleum. Higher
boiling fractions are “cracked” into lower boiling fractions that
are added to the raw gasoline. The alkenes can be
separated and used in to make plastics.
3. Halogenation
R-H + X2, heat or hv � R-X + HX
a) heat or light required for reaction.a) heat or light required for reaction.
b) yields mixtures �
c) H: 3o > 2o > 1o > CH4
d) bromine is more selective
CH3CH3 + Cl2, hv � CH3CH2-Cl + HClethane ethyl chloride
CH3CH2CH3 + Cl2, hv � CH3CH2CH2-Cl + CH3CHCH33 2 3 2 3 2 2 3 3
propane n-propyl chloride Cl
isopropyl chloride45%
55%
gives a mixture of both the possible
alkyl halides! �
CH3CH2CH2CH3 + Cl2, hv � CH3CH2CH2CH2-Cl
28%n-butane n-butyl chloride
+
CH3CH2CHCH3 72%
Cl
sec-butyl chloride
CH3 CH3
CH3CHCH3 + Cl2, hv � CH3CHCH2-Cl 64%
isobutane isobutyl chloride
+
CH3
CH3CCH3 36%
Cltert-butyl chloride
CH3CH3 + Br2, hv � CH3CH2-Br + HBrethane ethyl bromide
CH3CH2CH3 + Br2, hv � CH3CH2CH2-Br + CH3CHCH33 2 3 2 3 2 2 3 3
propane n-propyl bromide Br
isopropyl bromide3%
97%
In the reaction of alkanes with halogens, bromine is less
reactive but more selective. Why? How?
CH3CH2CH2CH3 + Br2, hv � CH3CH2CH2CH2-Br
2%n-butane n-butyl bromide
+
CH3CH2CHCH3 98%
Br
sec-butyl bromide
CH3 CH3
CH3CHCH3 + Br2, hv � CH3CHCH2-Br <1%
isobutane isobutyl bromide
+
CH3
CH3CCH3 99%
Brtert-butyl bromide
Mechanism of Halogenation
1) Initiating step:
X—X � 2 X•
2) Propagating steps:
X• + R—H � H—X + R•
R• + X—X � R—X + X•R• + X—X � R—X + X•
3) Terminating steps:
2 X• � X—X
R• + X• � R—X
2 R• � R—R
Mechanism of Chlorination of Propane
1) Cl—Cl � 2 Cl•
2) abstraction of 1o hydrogen:
Cl• + CH3CH2CH3 � CH3CH2CH2• + HCl
or abstraction of 2o hydrogen:
Cl• + CH3CH2CH3 � CH3CHCH3 + HCl Cl• + CH3CH2CH3 � CH3CHCH3 + HCl •
3) CH3CH2CH2• + Cl2 � CH3CH2CH2Cl + Cl•
or CH3CHCH3 + Cl2 � CH3CHCH3 + Cl•• Cl
plus terminating steps
Relative Reactivity in Halogenation
Stability of free radicals:
Ease of formation of free radicals:
Ease of abstraction of H’s:Ease of abstraction of H’s:
3o > 2o > 1o > CH4
Factors Affected on Hydrogen Abstraction
Cl• + CH3CH2CH3 � CH3CH2CH2• + HCl
or abstraction of 2o hydrogen:
Cl• + CH3CH2CH3 � CH3CHCH3 + HCl •
The chloride that is produced depends on which hydrogen
is abstracted by the chlorine free radical in step 2. The n-
propyl free radical gives the n-propyl chloride while the
isopropyl free radical yields the isopropyl chloride.
The relative reactivity in chlorination:
H: 3o : 2o : 1o = 5.0 : 3.8 : 1.0
The number of hydrogens (probability factor) may also be
important.
CH3CH2CH2CH3 + Cl2, hv � CH3CH2CH2CH2-Cl
n-butane
+ CH3CH2CHCH3
Cl
n-butyl chloride = (# of 1o hydrogens) x (reactivity of 1o)n-butyl chloride = (# of 1o hydrogens) x (reactivity of 1o)
= 6 x 1.0 = 6.0
sec-butyl chloride = (# of 2o hydrogens) x (reactivity of 2o)
= 4 x 3.8 = 15.2
% n-butyl chloride = 6.0/(6.0 + 15.2) x 100% = 28%
% sec-butyl chloride = 15.2/(6.0 + 15.2) x 100% = 72%
CH3 CH3 CH3
CH3CHCH3 + Cl2, hv � CH3CHCH2-Cl + CH3CCH3
isobutane Cl
isobutyl chloride = (# of 1o H’s) x (reactivity of 1o)
= 9 x 1.0 = 9.0
tert-butyl chloride = (# of 3o H’s) x (reactivity of 3o)
= 1 x 5.0 = 5.0= 1 x 5.0 = 5.0
% isobutyl = (9.0/(9.0 + 5.0)) x 100% = 64%
In this case the probability factor outweighs the difference in
relative reactivity of 1o and 3o hydrogens.
Relative Reactivity in Bromination
3o : 2o : 1o = 1600 : 82 : 1
In bromination the relative reactivity differences are much
greater than any probability differences.
isobutane + Br2, hv � isobutyl bromide + tert-butyl isobutane + Br2, hv � isobutyl bromide + tert-butyl
bromide
isobutyl bromide = 9 H x 1 = 9
tert-butyl bromide = 1 H x 1600 = 1600
% tert-butyl bromide = (1600/1601) x 100% = >99%