organic chemistry 171 section 201. 2 alkenes,chapter 3
TRANSCRIPT
3
Unsaturated hydrocarbons can be
1-open-chain (linear and branched alkenes)
2- cyclic (cycloalkenes)
Alkenes and Cycloalkenes
4
Unsaturated HydrocarbonsUnsaturated Hydrocarbons
Hydrocarbons that contain at least one C=C ( alkenes) are called unsaturated hydrocarbons
CH3
CH2C
CH2CH3
CH2
6
• Generic formula: Start with CnH2n+2 and minus two for each C=C
• one C=C e.g., C2H4, C3H6, etc.
C2H4
CnH2n
8
Common Names
• Usually used for small molecules.
• Examples:
CH2 CH2
ethylene
CH2 CH CH3
propylene
CH2 C CH3
CH3
isobutylene
=>
IUPAC Nomenclature of Alkenes
• 1. Find the longest continuous chain containing the double bond.
• 2. Name the corresponding alkane and change the “ane” ending to “ene” for alkenes.
• 3. Number the chain so as to give the double bond the lowest number. Place a numerical prefix in front of the parent name to indicate the position of the first carbon in the double bond.
• Number and name alkyl groups as with alkanes.
10
Nomenclature
• alkenes: parent chain contains C=CC=C gets lowest numbersposition of C=C indicated by lower of the two numbers
CH3 CH2 CH CH2
Br
1-butene
4-methyl-1-butene
3-bromocyclohexene
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Nomenclature
• C=C and OH: alkenol
higher priority group (OH) gets last suffixand lowest number
OH
OH
OH
2-propen-1-ol
5-methyl-4-hexen-2-ol
2-cyclohexenol
12
Nomenclature
• as side groups:
H2C CH
H2C CH CH2
H2C
C
H3C
CH2
ethenyl (vinyl)
2-propenyl (allyl)
1-methylethenyl (isopropenyl)
methylene
CH2
vinyl chloride
allyl alcohol
isopropenyl bromide
Cl
OH
Br
Examples
1-vinylcyclohexene methylenecyclopentane
Name the following compound:
C
H2C
CH
H2C CH3
CH3
H3C
The longest continuous chain containing the double bond is 5 carbons long and is indicated in blue, below:
C
H2C
CH
H2C CH3
CH3
H3C
The parent compound is derived from pentane. The parent alkene is pentene.
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NomenclatureE-Z notation
H
C
H3C
C
Cl
CH2CH3
H
C
H3C
C
CH2CH3
Cl
(E)-3-chloro-2-pentene (Z)-3-chloro-2-pentene
1. Determine the higher priority group on each end of the alkene.2. If the higher priority groups are:
on opposite sides: E (entgegen = opposite)on the same side: Z (zusammen = together)
CH3 > HCl > CH2CH3
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Name These Alkenes
CH2 CH CH2 CH3
CH3 C
CH3
CH CH3
CH3
CHCH2CH3H3C
1-butene
2-methyl-2-butene
3-methylcyclopentene
2-sec-butyl-1,3-cyclohexadiene
3-n-propyl-1-heptene =>
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ALKENE STRUCTURE AND BONDINGALKENE STRUCTURE AND BONDING
sp2
sp2
C C
R
R
R
R
SHAPE IS TRIGONAL PLANAR
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Orbital Description
• Sigma bonds around C are sp2 hybridized.• Angles are approximately 120 degrees.• No nonbonding electrons.• Molecule is planar around the double bond.• Pi bond is formed by the sideways overlap of
parallel p orbitals perpendicular to the plane of the molecule. =>
20
Bond Lengths and Angles
• Hybrid orbitals have more s character.
• Pi overlap brings carbon atoms closer.
• Bond angle with pi orbitals increases.– Angle C=C-H is 121.7 – Angle H-C-H is 116. 6 =>
21
C CH H
H H
2p
(sp2C + 1sH)
(sp2C + sp2
C)
overlapp orbitals C C
H H
H H
bond
no free rotation
HC
HC
H
H
trigonal planarsp2
Cis and Trans Isomers
• Some alkenes can have the same connection of atoms, but have a different arrangement in three dimensional space.
• This is due to the lack of free rotation about the double bond.
• The different arrangements are geometric isomers.
• One of the isomers is cis- the other is trans.
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CISCIS // TRANSTRANS ISOMERS ISOMERS
ciscis transtrans
substituents onthe same side ofmain chain
substituents onopposite sides ofmain chain
C C
H
C
C
H
C C
C
H
C
H
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C C
R
H
R
H
C C
H
R
R
H
RR
R
R
COMPARE COMPARE cis / transcis / trans ISOMERS IN RING COMPOUNDS ISOMERS IN RING COMPOUNDS
cis trans
In alkenes and rings cis / trans isomers are called stereoisomers or geometric isomers.
2-butene
C
CH3
C
H
cis-2-butene
H3C
H
C
CH3
C
H3C
trans-2-butene
H
H
mp = -139oC
CH3 groups same side CH3 groups opposite sides
mp = -106oC
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Physical Properties
• Low boiling points, increasing with mass.• Branched alkenes have lower boiling points.• Less dense than water.• Slightly polar
– Pi bond is polarizable, so instantaneous dipole-dipole interactions occur.
– Alkyl groups are electron-donating toward the pi bond, so may have a small dipole moment. =>
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Polarity Examples
= 0.33 D = 0
=>
cis-2-butene, bp 4°C
C CH
H3C
H
CH3
trans-2-butene, bp 1°C
C CH
H
H3C
CH3
I. Preparation
• 1. Dehydration
C C
OH
C C + H2O
excess conc. H2SO4 at 170oC
or Al2O3/SiO2 at 350oC
This is intermolecular dehydration.
What kinds of dehydration?
H
H
H
H
H
OH
O H
H
H
H
H
H
H
H
H
H + OH2
conc.H2SO4
140 Co
Another reaction occur!
I. Preparation - Dehydration
Saytzeff Rule:Hydrogen is preferably removed from the carbon with least no. of hydrogen since the alkene formed is more highly branched and is energetically more stable.
C C C C
H HOH
C C C C C C C C+
(major) (minor)
How do you which one is major product?
I. Preparation
• 2. Dehydrohalogenation
Example:
alcoholic KOH
EtO- (ethoxide ion) in EtOH (ethanol)
H H
H
X
H
H
strong base
alcoholic reflux+ HX
KX + OH2
H
H
H
H
EtOH EtO + H+
weakconjugate acid
strongconjugate base
Press
35
Hofmann Product
• Bulky bases abstract the least hindered H+
• Least substituted alkene is major product.
CH3 C
H
H
C
CH3
Br
CH2
H
CH3CH2O
CH3CH2OH
_
C CCH3
CH3H
H3CC C
H
HH3C
CH3CH2
71% 29%
72%28%
C CH
HH3C
CH3CH2
C CCH3
CH3H
H3C_
CH3CH2OHCH3 C
H
H
C
CH3
Br
CH2
H
(CH3)3CO =>
I. Preparation
3.Dehalogenation
C C
X X
+ Zn dust C C + ZnX2
alcoholic reflux
(vicinal dihalide)
(c.f. gem-dihalide )
X
X
I. Preparation - dehalogenation (application)
H OH
H
H
H
H
HH
H OH
O
H
HHH[O]
X2
H OH
H
H
H
H
HH
X X
KMnO4 / H+
H OH
O
H
HHH
X X
Zn dustalcoholic reflux
I. Preparation
• 4. Hydrogenation
– This makes use of a catalyst which activity has been decreased by sulphur containing compound. E.g. Pd (palladium) in BaSO4
C C + H2 C C
H HPd/BaSO4
Chapter 8 40
Reactivity of C=C
• Electrons in pi bond are loosely held.
• Electrophiles are attracted to the pi electrons.
• Carbocation intermediate forms.
• Nucleophile adds to the carbocation.
• Net result is addition to the double bond. =>
Markownikoff’s rule– The more electronegative atom (or group of
atoms) attached to carbon having least no. of H.In general, the greater the no. of alkyl grops present, or the larger is the alkyl group, the more stable is the carbonium ion.
– Stability of carbonium ion:– 3ry C+ > 2ry C+ > 1ry C+ > CH3
+
(Mechanism of Addition Reactions)
CH2CH3CH + H X
CH3CH2CH2X CH3CHCH3
X
CH3CH2CH2
+X
(I)
CH3CHCH3
+X
(II)
• Electrophilic Addition Reactions (cont’d)
2-With conc. sulphuric acidH OSO3H+ -
C C + H .H SO 4 C C
H O SO 3 H
C C
H O H
H 2Obo il
alkyl hydrogen sulphate
Hence, this is used in preparation of alcohol.
Proof for the formation of brominium ion
+ Br2
CCl4 / C2H5OH Br
Br
Trans-addition(anti-addition)
The bromide ions attack carbon of the ring from the side opposite to that of the “positive” brominium ion.
• Addition Reactions (NOT electrophilic)
4-Hydrogenation
C C + H2 C C
H H
a. It is used analytically to find the number of mole of double bond or triple bond by the number of mole of hydrogen absorbed per mole of molecule.
b. It is used in converting vegetable oil.
5-Ozonolysis
C C
R
R' R''
R'''
+ O3
ice-cold
chloroformC
O
C
O O
R
R' R''
R'''ozonide
H2O /H
Zn dustC O
R'
R
CO
R''
R'''
6-Oxidationa.at room temperature (Hydroxylation)
(addition)
C C + [O] + H2O C C
OH OHfrom MnO4
-/OH-
b.at vigorous condition (bond breaking)
C C
H H
R R' + [O] C O CO
H H
R R'+
C O
OH
R
MnO4- / H+
Further oxidation
In acidic condition, the products will be oxidised to acid or ketone.
7-Addition Polymerization– This is a process by which simple molecules are joined
up to form large molecule with same empirical formula.
– condition : high temperature and pressure– with Ziegler’s catalyst
C Cn C C( )n
C C
R'
Rn C C
R
R'
( )n
• Free radical addition mechanismInitiation:
Propagation:
RO OR 2RO
RO C C
R'C C
R'
RO
C C
R'
C C
R'
RO C C C C
R'R'
RO
Termination:
C C C C
R'R'
RO CCCC
R' R'
RO
RO OR RO OR
C C C C
R'R'
RO OR C C C C
R'R'
RO OR
C C OR
R'
RO
n n
n m
n+m+2
e.g. polythenemoleclar mass: 50000g
melting point: 126oC – 135oC (having diff. Isomer)
Properties:Light, inert (strong sigma bonds) and water-resistance (do
not form H-bonding), tough and capable of moulding. It is a thermo-plastic since chains of hydrocarbons causes the chain to move apart and to come closer again on cooling.