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LECTURE 4
Dr Ali El-Agamey
CHEM-103:
BASIC ORGANIC CHEMISTRY
DAMIETTA UNIVERSITY
Chapter 4 2
Reaction mechanism • Overall reaction: reactants → products • Mechanism: Step-by-step pathway.
Chapter 4 3
Chlorination of Methane
c
Chapter 4 4
Mechanism
c
Initiation Step
Chapter 4 5
Chlorination of Methane
• Reaction requires heat or light for initiation. • Many molecules of product are formed from
absorption of only one photon of light (chain reaction).
Chapter 4 6
Termination Steps
• A reaction is classified as a termination step when any two free radicals join together producing a nonradical compound.
• Combination of free radical with contaminant or collision with wall are also termination steps.
Chapter 4 7
More Termination Steps
Chapter 4 8
The Free-Radical Chain Reaction
• Initiation generates a radical intermediate. • Propagation: The intermediate reacts with a
stable molecule to produce another reactive intermediate (and a product molecule).
• Termination: Side reactions that destroy the reactive intermediate.
Chapter 4 9
Energy Diagram for the Chlorination of Methane
(3) Halogenation
Other Examples
Chapter 4 11
Examples
• Bromination of alkanes is much more selective than chlorination.1
• What is the relative reacitivity of primary and secondary hydrogens in each reaction?
Chapter 4
12
Chlorination: Reactivities of Primary, Secondary, and Tertiary Hydrogens
(3) Halogenation
• Secondary free radical is more stable than primary free radical.
14
Chlorination Energy Diagram Why is 2o H more reactive than 1o H?
• Lower Ea (more stable T.S.), faster rate, so more stable intermediate is formed faster.
Chapter 4 15
Bromination: Relative reactivity of hydrogens
Chapter 4 16
Energy Diagram for the Bromination of Propane
Chapter 4 17
Tertiary hydrogen atoms react with Cl• about 5.5 times as fast as primary ones. Predict the product ratios for chlorination of isobutane.
Problem
Chapter 8 18
Write the mechanism (initiation and propagation) of the following reaction:1
Homework
Calculate the relative reactivity of different hydrogens in isobutane toward chlorination using the following equation:2
Alkyl Halides
©2010, Prentice Hall
Chapter 6 20
Alkyl Halides Classification • Methyl halides: halide is attached to a methyl
group. • Primary alkyl halide: carbon to which halogen
is bonded is attached to only one other carbon. • Secondary alkyl halide : carbon to which
halogen is bonded is attached to two other carbons.
• Tertiary alkyl halide : carbon to which halogen is bonded is attached to three other carbon.
Chapter 6 21
primary alkyl halide secondary alkyl halide
tertiary alkyl halide
Primary, Secondary, Tertiary Alkyl Halides
*
* *
Chapter 6 22
Types of Dihalides
• Geminal dihalide: two halogen atoms are bonded to the same carbon.
• Vicinal dihalide: two halogen atoms are bonded to adjacent carbons.
geminal dihalide
vicinal dihalide
Write the IUPAC names of the following compounds
Fluoroethane 1-Chlorobutane 2-Bromopropane
Iodocyclohexane
Homework: Write the IUPAC name of the following compounds
Homework: Write the structures for the following compounds
(ii) 3-Bromo-2-methylpentane
(iv) 2-Bromo-3-ethyl-2-methylhexane
(v) 1,1-Dibromopropane
Preparation of Alkyl halides
Preparation of Alkyl halides
Chapter 6 27
Polarity and Reactivity
• Halogens are more electronegative than C. • Carbon—halogen bond is polar, so carbon has partial
positive charge. • Carbon can be attacked by a nucleophile. • Halogen can leave with the electron pair.
Chapter 6 28
• The halogen atom on the alkyl halide is replaced with a nucleophile (Nuc-).
• Since the halogen is more electronegative than carbon, the C—X bond breaks heterolytically and X- leaves.
Reactions of Alkyl halides (A) Substitution Reactions
Chapter 6 29
Reactions of Alkyl halides