Chapter 3 - Alkenes. Naming Alkenes Change the suffix from ane to ene.
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Transcript of Chapter 3 - Alkenes. Naming Alkenes Change the suffix from ane to ene.
Chapter 3 - Alkenes
Naming Alkenes
Change the suffix from ane to ene
CH3 CH3 CH2 CH2
ethane ethene
Naming Alkenes
The longest chain must include the double bond
Chain is numbered to give the double bond carbons the lowest numbers
Numbers indicating location of double bond are placed before chain length
12
345
76
3-propyl-2-heptene
Naming Alkenes
Cl
1234
56
789
8-chloro-4-nonene
Double bond gets precedence over substituents
Naming Alkenes
For more than one double bond
use diene, triene etc
Br
1234
56
78
6-bromo-2,4-octadiene
Naming Alkenes
Double bond in a cyclic always get
numbers 1 and 2
BrBr
3,4-dibromocyclohexene1
2
3
45
6
Naming Subtleties
ClBrCH3 Cl
Cl12345
67
8
2-chloro-4-bromo-7-methyl-4-octane
1,6-dichlorocyclohexene
Terms• Vinylic carbons – sp2 carbons
• Allylic carbons – ones next to the vinylic carbons
AlkenesDouble bond locks the molecule and there is
no rotation about the double bond
Energy for single bond 2.9 kcal/mol for double 62 kcal/mol
Lowest Energy
The Second Bond Must Break (Promote Electrons to the Antibonding Orbital). Then it Can Rotate
Different Molecules
The connections are the same, but that’s about all!!!
Cis/Trans – Just Not Good Enough
Configuration - E,Z
Z (zusammen) E (entgegen)
C
higherC
higher
lowerlower
C
lower higherC
lowerhigher
E/Z Rules
Assign priority based on the higher atomic number
(53)(35)(17)(16)(8)(7)(6)(1)
Increasing priority
-H -CH 3 -NH2 -OH -SH -Cl -Br -I .
Increasing priority
E/Z Rules
If priority cannot be assigned on the basis of the atoms bonded to the CARBON, look to the next set of atoms. Priority is
assigned at the first point of difference.
CH2CH2Br
CH2CH2F
Cl
H
E/Z Rules
When a double or tripple bond shows up, count it as though there are two
or three of the same atom
C CH2R R C CH2
C
R C H
O
R CH
OO
E/Z nomenclature
Thermodynamics and KineticsHow Far and How Fast
• Thermodynamics–Description of a reaction at
equilibrium (Keq)
• Kinetics–Description of rates of a chemical
reaction
rate = k [A] [B]2 / [C]0
For The Following Energy Discussion, Consider this Reaction
Energy considerations
• Mechanisms describe bond breaking-bond making
Energy considerations
• Exergonic vs. Endergonic Reactions
( Note: The more stable the species, the lower its energy. )
Ok, OK, OK, - What is exergonic and endergonic? Isn’t that supposed To be exothermic and endothermic???? Next slide!!!!!!!!
Energy Terms
• Endergonic and Exergonic describe the free energy used or expelled from a reaction.
• Endothermic and exothermic describe the heat ΔH used or expelled from a reaction
Go = Ho - TSo
G and H are often close to the same unless you have a large temperature value
For almost all normal processes the +/- value of G and H will be the same
Energy considerations
Go , Gibbs free energy change…
– Predicts whether a reaction will happen “spontaneously”
– Exergonic reactions = - Go (spontaneous)
– Endergonic reactions = + Go
Ho = energy bonds broken - energy bonds formed
Ho = energy bonds broken - energy bonds formed
Calculate ΔH
Notice the table doesn’t list the breaking of the pie bond without the breaking of the sigma bond. This value is 62 kcal/mol.
H
H
H
HH Cl
HH
H
H
HBr
Where are Calculations Valid
• Just in the Gas Phase
• The solvent makes a difference!– Solvents can have a large effect on H– Water can solvate cations +++ or anions - - -
Rate of Reaction
• Rate depends on:
1.The number of collisions/time
2.Fraction of collisions with sufficient energy
3.Fraction of collisions with proper orientation
Kinetics
• Energy of Activation, Ea (or G**)
• Fast vs. Slow reactions:
Organic Chemistry Lingo
• Kinetic Product : formed most rapidly
• Thermodynamic Product: most stable product
Many times the Kinetic Product is the Thermodynamic Product!
Thermodynamic vs. Kinetic Control
• If the kinetic product and thermodynamic product differ, the major product will depend on reaction conditions.
• If carried out at mild (low-temp) conditions, the reaction will be irreversible and the kinetic product will be favored.
Thermodynamic vs. Kinetic Control
• If carried out at sufficiently vigorous (hi-temp) conditions, the reaction will be reversible and the thermodynamic product will be favored.
Thermodynamic vs. Kinetic Control
• Kinetic product and thermodynamic product:
Formed fastest
Most stable
Reaction Coordinate Diagrams• Intermediate = product of one step, becomes
reactant of next step
• Transition state = intermediate that cannot be isolated (partially formed bonds, highest energy structures!)
• Rate determining step = step with highest energy Transition state Transition state
Reaction Coordinate Diagrams
• 1) How many intermediates are there?• 2) Is the first formed intermediate more apt to revert to reactants
or go on to form products?• 3) Which step in the reaction is the rate determining?• 4) Is the reaction endergonic or exergonic? What is the sign of
Go?• 5) Which step has the greatest free energy of activation?• 6) Where are the transition states?
Reaction Order
• First Order Reaction – reaction is proportional to the concentration of one reactant
• Second Order Reaction – reaction that is proportional to the concentration of two reactants
A B
A BB+A A B+