Chapter 3

.

Alcohol and Alkyl Halides

Alkyl Halides

• An organic compound containing at least one carbonhalogen bond (C-X)

– X (F, Cl, Br, I) replaces H

• Can contain many C-X bonds

• Properties and some uses

– Fire-resistant solvents

– Refrigerants

– Pharmaceuticals and precursors

2

3

Naming Alkyl Halides

• Name is based on longest carbon chain

– (Contains double or triple bond if present)

– Number from end nearest any substituent (alkyl or halogen)

4

5

6

Many Alkyl Halides That Are Widely

Used Have Common Names

• Chloroform

• Carbon tetrachloride

• Methylene chloride

• Methyl iodide

• Trichloroethylene

7

Alcohols

• Alcohols contain an OH group connected to a a saturated C (sp 3 )

• They are important solvents and synthesis intermediates

• Phenols contain an OH group connected to a carbon in a benzene ring

• Methanol, CH

3

OH, called methyl alcohol, is a common solvent, a fuel additive, produced in large quantities

• Ethanol, CH

3

CH

2

OH, called ethyl alcohol, is a solvent, fuel, beverage

• Phenol, C

6

H

5

OH (“phenyl alcohol”) has diverse uses - it gives its name to the general class of compounds

8

Naming Alcohols

• General classifications of alcohols based on substitution on C to which OH is attached

• Methyl (C has 3 H’s), Primary (1°) (C has two H’s, one

R), secondary (2 °) (C has one H, two R’s), tertiary (3°)

(C has no H, 3 R’s),

9

IUPAC Rules for Naming Alcohols

• Select the longest carbon chain containing the hydroxyl group, and derive the parent name by replacing the e ending of the corresponding alkane with ol

• Number the chain from the end nearer the hydroxyl group

• Number substituents according to position on chain, listing the substituents in alphabetical order

10

Many Alcohols Have Common

Names

• These are accepted by IUPAC

11

Hybridization of Methanol

12

Properties of Alcohols: Hydrogen Bonding

• The structure around O of the alcohol or phenol is similar to that in water, sp 3 hybridized

• Alcohols and phenolshave much higher boiling points than similar alkanes and alkyl halides

Hydrogen bonding in ethanol

Figure 4.4

Francis A. Carey, Organic Chemistry, Fourth Edition. Copyright © 2000 The McGraw-Hill Companies, Inc. All rights reserved.

13

H-Bonding between Ethanol and

Figure 4.5

Francis A. Carey, Organic Chemistry, Fourth Edition. Copyright © 2000 The McGraw-Hill Companies, Inc. All rights reserved.

14

Acids and Bases

The Br ønsted-Lowry Definition

• Acid – A proton (H + ) donor

• Base – A proton acceptor

Acid Base Conjugate Conjugate

Acid Base

15

Energy diagram for concerted proton transfer

Figure 4.6

Francis A. Carey, Organic Chemistry, Fourth Edition. Copyright © 2000 The McGraw-Hill Companies, Inc. All rights reserved.

16

Acid and Base Strength

HA H

+

+ A

-

K a

[ H

][ A

-

]

[ HA] pK a

  log K a

17

Relative Strengths of Some Common Acids and

Their Conjugate Bases

Acid

CH

3

CH

2

OH

H

2

O

HCN

CH

3

CO

2

H

HF

HNO

3

HCl

Name

Ethanol

Water

Hydrocyanic Acid

Acetic Acid

Hydrofluoric Acid

Nitric Acid

Hydrochloric Acid pK a

16.00

15.74

9.31

4.76

3.45

-1.3

-7.0

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Predicting Acid – Base Reactions from p

K a

Values

The proton will always go from the stronger acid to the stronger base

H

H

C

H

O

C

Acetic Acid p K a

= 4.76

O

H

+ O H

Hydroxide Ion

H

H

C

O

C

H

Acetate Ion

O + H O

H

Water p K a

= 15.74

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Organic Acids

20

Lewis Acids and Bases

• Lewis Acid – electron-pair acceptor

• Lewis Base – electron-pair donor

• Lewis Acids usually have at least one empty orbital

• Lewis Bases usually have at least one set of paired electrons

21

22

H

2

O

Examples of Lewis Acids

HCl HNO

3 H

2

SO

4

H

H

C

H

C

O

O H

OH

H

H

C

H

H

C

H

O

H

Li

+ Mg

2+

AlCl

3

BF

3

FeCl

3

23

H

H

C

H

Examples of Lewis Bases

H

C

H

O

H

H

H O H

C C C

H H

H

H

H O

C C H

H

H

H

C

H

C

O

O H

H

H

C

H

C

O

H

O C

H

H

H

H H

C O C

H H

H

H

H H

C N C

H H H

H

24

Kinds of Organic Reactions

• In general, we look at what occurs and try to learn how it happens

• Common patterns describe the changes

– Addition reactions – two molecules combine

– Elimination reactions – one molecule splits into two

– Substitution – parts from two molecules exchange

– Rearrangement reactions – a molecule undergoes changes in the way its atoms are connected

25

How Organic Reactions Occur:

Mechanisms

• In a clock the hands move but the mechanism behind the face is what causes the movement

• In an organic reaction, we see the transformation that has occurred. The mechanism describes the steps behind the changes that we can observe

• Reactions occur in defined steps that lead from reactant to product

26

Steps in Mechanisms

• We classify the types of steps in a sequence

• A step involves either the formation or breaking of a covalent bond

• Steps can occur in individually or in combination with other steps

• When several steps occur at the same time they are said to be concerted

27

Types of Steps in Reaction

Mechanisms

• Formation of a covalent bond

– Homogenic or heterogenic

• Breaking of a covalent bond

– Homogenic or heterogenic

• Oxidation of a functional group

• Reduction of a functional group

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Breaking of Covalent Bonds

Homolytic Cleavage

• Each product gets one electron from the bond

• Not common in organic chemistry

Heterolytic Cleavage

• Both electrons from the bond that is broken become associated with one resulting fragment

• A common pattern in reaction mechanisms

29

Formation of a Bond

Homogenic

• One electron comes from each fragment

• No electronic charges are involved

• Not common in organic chemistry

Heterogenic

• One fragment supplies two electrons

• One fragment supplies no electrons

• Combination can involve electronic charges

• Common in organic chemistry

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Indicating Steps in Mechanisms

• Curved arrows indicate breaking and forming of bonds

• Arrowheads with a “half” head (“fishhook”) indicate homolytic and homogenic steps (called ‘radical processes’)

• Arrowheads with a complete head indicate heterolytic and heterogenic steps (called ‘polar processes’)

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5.6 Using Curved Arrows in Polar

Reaction Mechanisms

• Curved arrows are a way to keep track of changes in bonding in polar reaction

• The arrows track “electron movement”

• Electrons always move in pairs

• Charges change during the reaction

• One curved arrow corresponds to one step in a reaction mechanism

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5.4 Polar Reactions and How They

Occur

• Molecules can contain local unsymmetrical electron distributions due to differences in electronegativities

• This causes a partial negative charge on an atom and a compensating partial positive charge on an adjacent atom

• The more electronegative atom has the greater electron density

33

Electronegativity of Some Common

Elements

• The relative electronegativity is indicated

• Higher numbers indicate greater electronegativity

• Carbon bonded to a more electronegative element has a partial positive charge (

+)

34

Polarizability

• Polarization is a change in electron distribution as a response to change in electronic nature of the surroundings

• Polarizability is the tendency to undergo polarization

• Polar reactions occur between regions of high electron density and regions of low electron density

35

Generalized Polar Reactions

• An electrophile , an electron-poor species, combines with a nucleophile , an electron-rich species

• An electrophile is a Lewis acid

• A nucleophile is a Lewis base

• The combination is indicate with a curved arrow from nucleophile to electrophile

36

10.7 Preparing Alkyl Halides from

Alcohols

• Reaction of tertiary C-OH with HX is fast and effective

– Add HCl or HBr gas into ether solution of tertiary alcohol

• Primary and secondary alcohols react very slowly and often rearrange, so alternative methods are used

37

Energy diagram for formation of tert -butyl chloride from tert -butyl alcohol and hydrogen chloride

Figure 4.7

Francis A. Carey, Organic Chemistry, Fourth Edition. Copyright © 2000 The McGraw-Hill Companies, Inc. All rights reserved.

38

5.10 Describing a Reaction:

Intermediates

• If a reaction occurs in more than one step, it must involve species that are neither the reactant nor the final product

• These are called reaction intermediates or simply

“intermediates”

• Each step has its own free energy of activation

• The complete diagram for the reaction shows the free energy changes associated with an intermediate

39

Structure of methyl cation

Figure 4.8

Francis A. Carey, Organic Chemistry, Fourth Edition. Copyright © 2000 The McGraw-Hill Companies, Inc. All rights reserved.

40

Combination of a carbocation and a halide anion

Figure 4.11

Francis A. Carey, Organic Chemistry, Fourth Edition. Copyright © 2000 The McGraw-Hill Companies, Inc. All rights reserved.

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