1) Alkenes are hydrocarbons containing a carbon-carbon double bond. They include many naturally occurring compounds like flavors and fragrances.
2) This chapter focuses on the general reaction of alkenes, which is electrophilic addition. It examines the consequences of alkene stereoisomerism and how double bonds are present in most organic molecules.
3) Electrophilic addition of alkenes involves the attack of an electrophile like HBr on the pi bond, forming a carbocation intermediate that then reacts with the bromide ion. This two-step process allows preparations using HCl or HI as well.
This presentation describes the concept of Hyperconjugation in simple words, gives definition of hyperconjugation, explains why it is called as 'No bond Resonance' and gives the effects of hyperconjugation on the chemical properties of compounds: alkyl cations and their relative stability, alkyl radicals and their relative stability, alkenes and their relative stability, bond length, anomeric effect and Baker - Nathan effect.
This presentation describes the concept of Hyperconjugation in simple words, gives definition of hyperconjugation, explains why it is called as 'No bond Resonance' and gives the effects of hyperconjugation on the chemical properties of compounds: alkyl cations and their relative stability, alkyl radicals and their relative stability, alkenes and their relative stability, bond length, anomeric effect and Baker - Nathan effect.
THE PERICYCLIC REACTION THE MOST COMMON TOPIC INCLUDE THE SYLLABUS OF MANY SCIENCE STUDY INCLUDING BSC, MSC , PHARMA STUDY, AND MORE HENCE WE ARE COVERED ALL THE DATA OF IT HOPE THIS WILL MAKE READER EASY.
Introduction to benzene, orbital picture, resonance in benzene, Huckel‟s rule
Reactions of benzene - nitration, sulphonation, halogenation- reactivity, Friedel- Craft‟s alkylation- reactivity, limitations, Friedel-Craft‟s acylation.
Substituents, effect of substituents on reactivity and orientation of mono substituted benzene compounds towards electrophilic substitution reaction.
Alkenes Final chemicals can lead to the opposite product result, but the reactive-intermediate structures and mechanisms are different.Hydrobromic acid in particular is prone to forming radicals in the presence of various impurities or even atmospheric oxygen, leading to the reversal of the Markovnikov result.
THE PERICYCLIC REACTION THE MOST COMMON TOPIC INCLUDE THE SYLLABUS OF MANY SCIENCE STUDY INCLUDING BSC, MSC , PHARMA STUDY, AND MORE HENCE WE ARE COVERED ALL THE DATA OF IT HOPE THIS WILL MAKE READER EASY.
Introduction to benzene, orbital picture, resonance in benzene, Huckel‟s rule
Reactions of benzene - nitration, sulphonation, halogenation- reactivity, Friedel- Craft‟s alkylation- reactivity, limitations, Friedel-Craft‟s acylation.
Substituents, effect of substituents on reactivity and orientation of mono substituted benzene compounds towards electrophilic substitution reaction.
Alkenes Final chemicals can lead to the opposite product result, but the reactive-intermediate structures and mechanisms are different.Hydrobromic acid in particular is prone to forming radicals in the presence of various impurities or even atmospheric oxygen, leading to the reversal of the Markovnikov result.
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2. 2
Alkene - Hydrocarbon With
Carbon-Carbon Double Bond
Also called an olefin but alkene is better
Includes many naturally occurring materials
Flavors, fragrances, vitamins
3. 3
Why this Chapter?
C-C double bonds are present in most
organic and biological molecules
To examine consequences of alkene
stereoisomerism
To focus on general alkene reaction:
electrophilic addition
4. 4
6.1 Industrial Preparation and Use of Alkenes
Ethylene and propylene are the most important
organic chemicals produced
Made by thermal cracking of light alkanes
(petroleum)
5. 5
6.2 Calculating Degree of
Unsaturation
Relates molecular formula to possible structures
Degree of unsaturation: number of multiple bonds or rings
Formula for a saturated acyclic compound is CnH2n+2
Each ring or multiple bond replaces 2 H's
6. 6
Example: C6H10
Saturated is C6H14
Therefore 4 H's are not present
This has two degrees of unsaturation
Two double bonds?
or triple bond?
or two rings
or ring and double bond
7. 7
Degree of Unsaturation With
Other Elements
Organohalogens (X: F, Cl, Br, I)
Halogen replaces hydrogen
C4H6Br2 and C4H8 have one degree of unsaturation
Organoxygen compounds (C,H,O) - if connected by single bonds
These don't affect the total count of H's
8. 8
Organonitrogen compounds
Nitrogen has three bonds
So if it connects where H was, it adds a connection
point
Subtract one H for equivalent degree of unsaturation in
hydrocarbon
9. 9
Method 1
Count pairs of H's below CnH2n+2
Add number of halogens to number of H's (X equivalent to H)
Ignore oxygens (oxygen links H)
Subtract N's - they have three connections
Method 2
Summary - Degree of
Unsaturation
2
H
-
H
ion
Unsaturat
of
Degree
S)
O,
(ignore
N
X
2
2C
H
act
sat
sat
10. 10
6.3 Naming of Alkenes
Name the parent hydrocarbon—change ending to “–ene”
Number carbons in chain so that double bond carbons have
lowest possible numbers
Rings have “cyclo” prefix—double bond always C#1, C#2
Multiple “C=C“ are named as “diene” “triene” “tetraene” etc…
Alkenes higher priority than alkanes: even shorter chain
12. 12
6.4 Cis-Trans Isomerism in Alkenes
Carbon atoms in a double bond are sp2-hybridized
Three equivalent orbitals at 120º separation in plane
Fourth orbital is atomic p orbital
Combination of electrons in two sp2 orbitals of two
atoms forms bond between them
Additive interaction of p orbitals creates a bonding
orbital
Occupied orbital prevents rotation about -bond
Rotation prevented by bond - high barrier, about
268 kJ/mole in ethylene
13. 13
Rotation of Bond Is Prohibitive
This prevents rotation about a carbon-carbon
double bond (unlike a carbon-carbon single
bond).
Creates possible alternative structures
14. 14
The presence of a carbon-carbon double bond can
create two possible structures
cis isomer - two similar groups on same side of the
double bond
trans isomer - similar groups on opposite sides
Each carbon must have two different groups for these
isomers to occur
15. 15
Cis, Trans Isomers Require That End
Groups Must Differ in Pairs
180°rotation superposes
Bottom pair cannot be superposed without breaking C=C
16. 16
6.5 Sequence Rules: The E,Z
Designation
Neither compound is clearly “cis” or “trans”
Substituents on C1 are different than those on C2
We need to define “similarity” in a precise way to
distinguish the two stereoisomers
Cis, trans nomenclature only works for disubstituted
double bonds
E/Z Nomenclature for 3 or 4 substituents
17. 17
E,Z Stereochemical Nomenclature
Priority rules of Cahn,
Ingold, and Prelog
Compare where higher
priority groups are with
respect to bond and
designate as prefix
E -entgegen, opposite
sides
Z - zusammen,
together on the same
side
Hi(C1)-Low(C1)-Hi(C2)-Lo(C2)
18. 18
Ranking Priorities: Cahn-Ingold-
Prelog Rules
RULE 1
Must rank atoms that are connected at comparison point
Higher atomic number gets higher priority
Br > Cl > S > P > O > N > C > H
19. 19
RULE 2
If atomic numbers are the same, compare at next
connection point at same distance
Compare until something has higher atomic number
Do not combine – always compare
Extended Comparison
20. 20
RULE 3
Substituent is drawn with connections shown and no
double or triple bonds
Added atoms are valued with 0 ligands themselves
Dealing With Multiple Bonds:
21. 21
6.6 Stability of Alkenes
Cis alkenes are less stable than trans alkenes
Compare heat given off on hydrogenation: Ho
Less stable isomer is higher in energy
And gives off more heat
tetrasubstituted > trisubstituted > disubstituted > monosusbtituted
hyperconjugation stabilizes
22. 22
Comparing Stabilities of Alkenes
Evaluate heat given off when C=C is converted to C-C
More stable alkene gives off less heat
trans-Butene generates 5 kJ less heat than cis-butene
23. 23
Hyperconjugation
Electrons in neighboring filled orbital stabilize vacant
antibonding orbital – net positive interaction
Alkyl groups are better than H
Alternative Explanation:
sp3—sp2 bond > sp3—sp3 bond
24. 24
6.7 Electrophilic Addition of
Alkenes
General reaction
mechanism:
electrophilic addition
Attack of electrophile
(such as HBr) on bond
of alkene
Produces carbocation
and bromide ion
Carbocation is an
electrophile, reacting
with nucleophilic bromide
ion
25. 25
Two step process
First transition state is high energy point
Electrophilic Addition Energy Path
27. 27
6.8 Orientation of Electrophilic
Addition: Markovnikov’s Rule
In an unsymmetrical alkene, HX reagents can add in two different
ways, but one way may be preferred over the other
If one orientation predominates, the reaction is regiospecific
Markovnikov observed in the 19th century that in the addition of HX
to alkene, the H attaches to the carbon with the most H’s and X
attaches to the other end (to the one with the most alkyl
substituents) This is Markovnikov’s rule.
28. 28
Addition of HCl to 2-methylpropene
Regiospecific – one product forms where two are possible
If both ends have similar substitution, then not regiospecific
Example of Markovnikov’s Rule
29. 29
Markovnikov’s Rule (restated)
More highly substituted carbocation forms as intermediate
rather than less highly substituted one
Tertiary cations and associated transition states are more
stable than primary cations
30. 30
6.9 Carbocation Structure and
Stability
Carbocations are planar and the tricoordinate carbon is
surrounded by only 6 electrons in sp2 orbitals
The fourth orbital on carbon is a vacant p-orbital
The stability of the carbocation (measured by energy
needed to form it from R-X) is increased by the presence
of alkyl substituents (Hyperconjugation stabilizes C+)
33. 33
6.10 The Hammond Postulate
If carbocation intermediate is more stable than another,
why is the reaction through the more stable one faster?
The relative stability of the intermediate is related to an
equilibrium constant (Gº)
The relative stability of the transition state (which
describes the size of the rate constant) is the activation
energy (G‡)
The transition state is transient and cannot be
examined
34. 34
Transition State Structures
A transition state is the highest energy species in a
reaction step
By definition, its structure is not stable enough to exist for
one vibration
But the structure controls the rate of reaction
So we need to be able to guess about its properties in an
informed way
We classify them in general ways and look for trends in
reactivity – the conclusions are in the Hammond Postulate
“The structure of the transition state resembles the
structure of the nearest stable species. T.S. for
Endergonic steps resemble products. T.S. for Exergonic
steps resemble reactants.”
35. 35
Examination of the Hammond
Postulate
A transition state
should be similar
to an intermediate
that is close in
energy
Sequential states
on a reaction path
that are close in
energy are likely
to be close in
structure - G. S.
Hammond
36. 36
Competing Reactions and the
Hammond Postulate
Normal Expectation: Faster reaction gives stable intermediate
Intermediate resembles transition state
37. 37
6.11 Mechanism of Electrophilic Addition:
Rearrangements of Carbocations
Carbocations undergo structural rearrangements following set patterns
1,2-H and 1,2-alkyl shifts occur
Goes to give more stable carbocation
Can go through less stable ions as intermediates