Organic Chemistry

24.1

Classification of Hydrocarbons

• Hydrocarbons are organic compounds that contain only hydrogen and carbon

• Types of hydrocarbons include Alkanes Alkenes Alkynes Aromatic

Hydrocarbons

3

• Alkanes have only carbon to carbon single bonds

• Every carbon has four chemical bonds either to hydrogen or another carbon atom

Alkanes

4

• Alkanes have only carbon to carbon single bonds.• Each time a carbon atom is added to the chain there

are also two hydrogen atoms added.

Alkane Structures

5

• With carbon chains that are four carbon atoms or longer there are multiple ways to arrange the carbon

chains.

Alkane Structures

6

24.2

Alkanes

Alkanes have the general formula CnH2n+2 where n = 1,2,3,…

• only single covalent bonds

• saturated hydrocarbons because they contain the maximum number of hydrogen atoms that can bond with the number of carbon atoms in the molecule

• a homologous series (Compounds that have the same general

formula but differing lengths of carbon chains form a homologous series)

CH4 C2H6 C3H8

methane ethane propane

• Originally compounds were named based on their source or use

• Many organic compounds were given common names which are still in use

• However many ambiguities resulted • With the large number of organic compounds,

a method for systematically naming them is very important

Naming Organic Compounds

8

• The International Union of Pure and Applied Chemists (IUPAC) developed a system for naming organic compounds.

• This system eliminated many of the ambiguities that plagued earlier naming systems

• Common names for many substances are still widely used

IUPAC Names

9

A series of prefixes are used to designate the number of carbon atoms in a carbon chain

Naming Hydrocarbons using the IUPAC System

meth 1 C hex 6 C

eth 2 C hept 7 C

prop 3 C oct 8 C

but 4 C non 9 C

pent 5 C dec 10 C

10

• For straight chain hydrocarbons. The prefix indicates the number of carbon atoms.

• The suffix ane is added to designate that the compound is an alkane

Naming Alkanes

11

24.2

Alkane Nomenclature

• For branched chain hydrocarbons, identify the longest consecutive (straight) chain first. Then name the side chains or branches.

• The name of the branches end in “yl” and go before the name of the straight chain

Naming Alkanes with branched chains

-methylpropane

methylbutane

dimethylpropane

13

24.2

Alkane Nomenclature

1. The parent name of the hydrocarbon is that given to the longest continuous chain of carbon atoms in the molecule.

CH3 CH2 CH2 CH CH2 CH2 CH3

CH3

1 2 3 4 5 6 74-methylheptane

2. An alkane less one hydrogen atom is an alkyl group.

CH4

CH3

methane

methyl

24.2

Alkane Nomenclature

3. When one or more hydrogen atoms are replaced by other groups, the name of the compound must indicate the locations of carbon atoms where replacements are made. Number in the direction that gives the smaller numbers for the locations of the branches.

CH3 CH CH2 CH2 CH3

CH3

1 2 3 4 5

2-methylpentane

CH3 CH2 CH2 CH CH3

CH3

1 2 3 4 5

4-methylpentane

24.2

Alkane Nomenclature

4. Use prefixes di-, tri-, tetra-, when there is more than one alkyl branch of the same kind.

CH3 CH CH CH2 CH2 CH3

CH3

1 2 3 4 5 6

CH3

2,3-dimethylhexane

CH3 CH C CH2 CH2 CH3

CH3

1 2 3 4 5 6

CH3

3,3-dimethylhexane

24.2

Alkane Nomenclature

5. Use previous rules for other types of substituents. Branches are placed alphabetically in the compound name.

CH3 CH CH CH3

Br

1 2 3 4

NO2

2-bromo-3-nitrobutane

CH2 CH2 CH CH3

Br

1 2 3 4

NO2

1-bromo-3-nitrobutane

24.2

Structural isomers are molecules that have the same molecular formula but different structures

How many structural isomers does pentane, C5H12, have?

C C C C C

H H H H H

H

HHHHH

H

C C C C

H CH3 H H

H

HHHH

H

C C C

H CH3 H

H

HH

H

CH3

n-pentane

2-methylbutane

2,2-dimethylpropane

24.2

• Alkenes have one (or more) carbon to carbon double bonds

• Since there are fewer hydrogen atoms in alkenes as a result of the double bond, alkenes are referred to as unsaturated.

• Alkanes on the other hand have the maximum number of hydrogen atoms. They are referred to as saturated.

Alkenes

20

• Alkenes have one (or more) carbon to carbon double bonds

• When there are 4 or more carbon atoms in a chain, the location of the double bond is indicated by a number.

• Numbering the location of the double bond(s) takes precedence over the location of side chains

Alkenes

1 butene 2-butene methylpropene21

• Like alkanes, alkenes can have branched or consecutive chains. In the larger alkenes there are also multiple locations for the C=C. Hence multiple structural isomers are possible.

Alkene Structures

Branched chain

Straight chain. The double bond is between the first and second carbon

Straight chain. The double bond is between the second and third carbon 22

• Alkynes have one (or more) carbon to carbon triple bonds

• Since there are fewer hydrogen atoms in alkynes as a result of the triple bond, alkynes like alkenes are referred to as unsaturated.

Alkynes

23

• When there are 4 or more carbon atoms in a chain, the location of the triple bond is indicated by a number.

• Numbering the location of the triple bond(s) takes precedence over the location of side chains

Alkynes

24

• Like alkanes and alkenes, alkynes can have branched or consecutive chains. In the larger alkenes there are also multiple locations for the C=C. Multiple structural isomers are possible. The branch cannot originate on one of the carbons making up the triple bond

Alkyne Structures

Branched chain. The triple bond can occur in one of the branches but branches cannot be attached to any carbon in the triple bond

Straight chain. The triple bond is between the first and second carbon

Straight chain. The triple bond is between the second and third carbon 25

• Hydrocarbons that exist in chains are known as aliphatic hydrocarbons

• The ends of a chain may be joined to form a ring structure.

• These compounds are known as cyclic structures

Ring Structures

26

• A number of the smaller alkanes exist as cyclic structures including– Cyclopropane– Cyclobutane– Cyclopentane– Cyclohexane

Saturated Cyclic Hydrocarbons

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Cyclic alkanes have the general formula

CnH2n. The additional C-C bond results in the loss of two hydrogen atoms

Saturated Cyclic Hydrocarbons

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• A few cyclic hydrocarbons may contain C=C double bonds. Two of the most common are cyclopentene and cyclohexene shown in the diagram at the left

Unsaturated Cyclic Hydrocarbons –

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• Writing structural formulas for cyclic hydrocarbons can be tedious. These short form structures are commonly used.

• Each vertex represents a carbon atom and it is implied that there are enough H atoms on each vertex to make four bonds

Cyclic Hydrocarbons –Condensed structures

30

• The benzene ring is a common structure in organic molecules

• It consists of 6 carbon atoms and 6 hydrogen atoms.

• One would predict that there should also be 3 C=C bonds in a benzene ring

Aromatic Structures

31

• Further investigation reveals that the double bonds are not distinct in benzene. Rather it is a resonance hybrid.

• Either of these structures could be used to represent benzene.

Aromatic Structures

32

• Research shows that there are no differences in the C to C bonds in benzene.

• The current view of benzene holds that there are 6 C-C single bonds and 3 pairs or 6 delocalized electrons

Aromatic Structures

33

• The structure of benzene is shown as either of these two structures, or as a circle in a hexagon which depicts that the electrons are delocalized

Aromatic Structures

34

• Aromatic hydrocarbons are not limited to a single ring

• The fused ring structure shown is Naphthalene

Fused Aromatic Structures

35

Naming Compounds With Functional Groups

•Various functional groups have unique suffixes that designate the functional group. •The functional group takes precedence in numbering the carbon chain. •Branches to the carbon chain are named in the usual manner.

alcohols “ol” Amides “amide”

Aldehydes “al” Amines “amine” or amino as a prefix

Ketones “one” Ethers Ethoxy as prefix

Acids “oic” halohydrocarbons Fluoro, bromo, chloro or iodo

Esters “oate”36

24.4

Functional Group Chemistry

Alcohols contain the hydroxyl functional group and have the general formula R-OH.

Alcohols may be classified as - Primary - Secondary - TertiaryDepending on whether the carbon atom that is attached to the –OH group is surrounded by one, two or three other carbon atoms

Alcohol Classification

Primary Alcohols

A primary alcohol has only one carbon atom attached

A secondary alcohol has 2 carbon chains attached to the group on which the –OH resides

Secondary Alcohols

Tertiary Alcohols

24.4

Functional Group Chemistry

Aldehydes and ketones contain the carbonyl ( ) functional group.

O

C

R C H

O

• aldehydes have the general formula

R C R’

O

• ketones have the general formula

H C H

O

H C

O

CH3 C

O

CH3H3C

formaldehydeor methanal

acetaldehydeor ethanal

acetoneor propanone

24.4

Functional Group Chemistry

Carboxylic acids contain the carboxyl ( -COOH ) functional group.

methanoic acid ethanoic acid butanoic acid

benzoic acid

24.4

Functional Group Chemistry

Esters have the general formula R’COOR, where R is a hydrocarbon group.

CH3COOH + HOCH2CH3 CH3 C O CH2CH3 + H2O

O

ethyl acetate

24.2

Alkane Reactions

CH4 (g) + 2O2 (g) CO2 (g) + 2H2O (l) H0 = -890.4 kJ

Combustion

Halogenation - Also known as free radical substitution.

•Many organic molecules undergo substitution reactions.

•In a substitution reaction one atom or group of atoms is removed from a molecule and replaced with a different atom or group.

Example: Cl2 + CH4 CH3Cl + HCl

Three Basic Steps in a Free Radical Mechanism

• Chain initiationThe chain is initiated (started) by UV light breaking a chlorine molecule into free radicals.

Cl2 2Cl.

• Chain propagation reactionsThese are the reactions which keep the chain going.

CH4  +  Cl. CH3.  +  HCl

CH3.  +  Cl2 CH3Cl  +  Cl .

• Chain termination reactionsThese are reactions which remove free radicals from the system without replacing them by new ones.

2 Cl. Cl2 CH3. + Cl. CH3Cl

CH3. + CH3

. CH3CH3 46

Free Radical Mechanism-The Initiation Step

• The ultraviolet light is a source of energy that causes the chlorine molecule to break apart into 2 chlorine atoms, each of which has an unpaired electron

• The energies in UV are exactly right to break the bonds in chlorine molecules to produce chlorine atoms.

47

Homolytic Fission

• Free radicals are formed if a bond splits evenly - each atom getting one of the two electrons. The name given to this is homolytic fission.

48

Free Radical Propagation

• The productive collision happens if a chlorine radical hits a methane molecule.

• The chlorine radical removes a hydrogen atom from the methane. That hydrogen atom only needs to bring one electron with it to form a new bond to the chlorine, and so one electron is left behind on the carbon atom. A new free radical is formed - this time a methyl radical, CH3 .

49

Free Radical Propagation II

• If a methyl radical collides with a chlorine molecule the following occurs:

CH3.  +  Cl2 CH3Cl  +  Cl.

• The methyl radical takes one of the chlorine atoms to form chloromethane

• In the process generates another chlorine free radical.

• This new chlorine radical can now go through the whole sequence again, It will produce yet another chlorine radical - and so on and so on.

50

Termination Steps

• The free radical propagation does not go on for ever.

• If two free radicals collide the reaction is terminated.

2Cl. Cl2

CH3.  +  Cl . CH3Cl

CH3 .  +  CH3

. CH3CH3

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Exercise

• Write the steps in the free radical mechanism for the reaction of chlorine with methyl benzene. The overall reaction is shown below. The methyl group is the part of methyl benzene that undergoes attack.

52

Solution

• Initiation

Cl2 2Cl. • Propagation

Termination 2Cl. Cl2

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24.2

Alkene ReactionsCracking

Addition Reactions

CH2 CH2 (g) + HBr (g) CH3 CH2Br (g)

CH2 CH2 (g) + Br2 (g) CH2Br CH2Br (g)

C2H6 (g) CH2 CH2 (g) + H2 (g)Pt

catalyst