Hydrocarbon preeti bhatt

HYDROCARBONS are the compounds containing
carbon and hydrogen only.

Depending upon the types of carbon-carbon bonds present, they can
be classified into tree main categories:

1) Saturated Hydrocarbon
2) Unsaturated Hydrocarbon
3) Aromatic Hydrocarbon

The hydrocarbon that contain only carbon-carbon single bond is called
Saturated Hydrocarbon. These include open chain hydrocarbon as well as
closed chain hydrocarbons. These compounds are called saturated because they
have maximum number of bonded hydrogen
If different carbon atoms are joined together to form an open chain of
carbon atoms with single bonds, they are called Alkanes.
For example: 2-Methylpropane (Isobutane)

If carbon atoms form a closed chain or ring, they are called Cycloalkanes.
For example: Cyclopentane

The hydrocarbons which contain carbon-carbon multiple bond (Double
bonds or triple bond) are called unsturated hydrocarbon.
Depending upon multiple bond they are further classified as
alkenes and alkynes.

o Alkenes : These are hydrocarbon which contain at least one carbon-carbon bond.
For example: Ethene

o Alkynes: These are hydrocarbons which contain at least one carbon-carbon triple
bond. For example: Ethyle

The hydrocarbons which contain at least one special type of hexagonal ring of
carbon atoms with three double bond in the alternate positions are called
aromatic hydrocarbon. The ring is called aromatic ring.

For example: i) Toluene ii) o-Xylene

The aromatic compounds may also contain more than one benzene rings.
For example: i) Naphthalene ii) Anthracene

Hydrocarbon Type Characteristic Group Example

Saturated Hydrocarbon: No double or Triple Bond CH3CH2CH3
Propane
Alkanes

Unsaturated Hydrocarbon: Double Bond CH3–CH═CH2
Alkenes Propene

Alkynes Triple Bond CH3−C≡CH
Propyne

Aromatic Hydrocarbons: Benzene ring

Methyl Benzene

Alkanes are saturated hydrocarbon containing only carbon-carbon
single bond in their molecule. They are also called Paraffins. At high
temperatures and pressure do undergo some reaction. The alkanes may
be divided as:

1) Open chain or Acyclic alkanes .
2) Cycloalkanes or cyclic alkanes.

These are simple alkanes without any close chains and have
the general formula where CnH2n + 2 n is the number of
carbon atoms.

For example: i) Methane - CH4

These contain a closed chain or ring in their molecules. They have the general
formula CnH2n.

For example: i) Cyclopropane- or

ii)Cyclobutane- or

Methane is the first member of the family. It has Tetrahedral Structure
involving sp3 Hybridisation. The four sigma bond is formed by the
overlapping of sp3 hybrid orbitals of carbon and 1s orbital of hydrogen. In
this, carbon atom lies at the centre and the four hydrogen atoms lies at the
corners of a regular tetrahedron. Making H-C-H bond angle of 109.5˚.

a) b) c)

1.4 Nomenclature Of
Alkanes
Nomenclature implies assigning proper name to the basis of certain standard rules
so that the study of these compounds may become standard. The rules for naming
them are as follows:

i)
First of all, select the longest continues chain of carbon atoms in a molecule.
1 2 3 4 5 6 7 8 9
For eg. CH3– CH– CH2– CH2– CH2–CH– CH2– CH2–CH3

CH3 CH2−CH3

In the example ,the longest chain has nine carbons and it is considered as parent
root chain and carbon atoms which are not included in parent chain are called
substituents.

The carbon atoms of the parent chain are numbered to identify the
parent alkane and to locate the positions of the carbon atom at
which branching take place due to the substitution of alkyle group
in place of hydrogen atom. The numbering is done in such a way that
the branched carbon atoms get the lowest possible number.

For eg: 9 8 7 6 5 4 3 2 1
C−C−C−C−C−C−C−C−C

C C−C

When two or more substituents are present, then end of the parent chain
which gives the lowest set of the locants is preferred for numbering. This
rule is called lowest set of locants.
This means that when two or more different sets of locants are
possible, that set of locants which when compared term with other
sets, each in order of increasing magnitude, has the lowest term at the
first point of difference.

For eg: 6 5 4 3 2 1
H3C−CH−CH3−CH−CH−CH3

CH3 CH3 CH3

Set of locants: 2,3,5

If the same substituent or side chain occurs more than once, the prefix di(for
2), tri(for 3), tetra(for 4), penta(for 5),hexa(for 6)…etc., are attached to the
names of the substituents. The positions of the substituents are indicated
separately and the numerals representing their positions are separated by
commas.

For eg: 1 2 3 4 5
CH3–CH–CH2–CH–CH3

CH3 CH3

2,4-Dimethylpentane

If two or more different substituents or side chains are present in the
molecule, they are named in the alphabetical order along with their
appropriate positions. Prefix are ignored while comparing the substituents.

For eg: CH3CH3
5 4 3 2 1
CH3−CH3−C−CH3−CH3

CH3CH3

3 -Ethyl-2,3-dimethylpentane

If two different substituents are in equivalent positions from the two ends
of the chain, then the numbering of the chain is done in such a way that
the group which comes first in the alphabetical order gets lower down.
For eg: 1 2 3 4 5 6 7 7 6 5 4 3 2 1
CH3−CH2−CH−CH2−CH−CH2−CH3 CH3−CH2−CH−CH2−CH−CH2−CH3

CH3 CH2CH3 CH3 CH3CH3

( Methyl at C-3) (Ethyl at C-3)
The carbon bearing ethyl group gets lower position because it is cited first in the
name according to alphabetical order of substituents. So correct name of
compound is :3-Ethyl-5-methylheptane
CH3−CH2−CH−CH2−CH2−CH− CH2 −CH3
(3-Ethyl-6-methyloctane)
CH2CH3 CH3

If the substituent on the parent chain is complex it is named as substituted alkyl
group by numbering the carbon atom of this group attached to the parent chain
as 1.the name of such substituents is given in brackets in order to avoid
confusion with the numbering of the parent chain.
For eg: 1 2 3 4 5 6 7 8 9
CH3−CH3−CH3−CH3−CH3−CH3−CH3−CH3−CH3
1
CH3
2
CH3 Complex Substituent
3
CH3

5-(1,2- Dimenthylpropyl) nonane

Petroleum and natural gas are the main source of alkanes.
However, alkanes can be prepared by three methods.

The unsaturated hydrocarbons (alkenes and alkynes) are converted into alkanes by
catalytic hydrogenation. In this process dihydrogen is passed through alkenes or
alkynes in the presence of finely divided catalysts such as Raney Ni, Pt or Pd.
These metals absorb dihydrogen gas on their surfaces and activate the hydrogen-
hydrogen bond. Platinum and palladium catalyse the reaction at room
tempreture. However,higher tempreture (523-573k) and pressure are required
with nickle catalysts.
The hydrogenation reaction of unsaturated hydrocarbon using nickle at
a tempreture of 523-573K is commonly known as Sabatier and Sender’s reaction
or reduction.
Methane cannot be prepared by this method because starting
alkene or alkyne must contain at least two carbon atom.

For eg:

i) Alkyl halides (except fluorides) on reduction with zinc and dilute hydrochloric
acid give alkanes.
For eg:

ii) Alkyl halides on treatment with sodium metal in dry ethereal (free from
moisture)solution give higher alkanes. This reaction is known as Wurtz
reaction and is used for the preparation of higher alkanes containing even
number of carbon atom.
For eg:

Decarboxylation Kolbe’s electrolytic
reaction method

i) Decarboxylation reaction :
Sodium salts of carboxylic acids on heating with soda lime (mixture of sodium
hydroxide and calcium oxide)gives alkanes containing one carbon atom less
than the carboxylic acid. This process of elimination of carbon dioxide from a
carboxylic acid is known as decarboxylation.
For eg:

ii) Kolbe’s electrolytic method:
An aqueous solution of sodium or potassium salt of a carboxylic acid on
electrolysis gives alkane containing even number of carbon atoms at the anode.

The reaction is supposed to follow the following path:
 .

i)

ii)At anode:

iii)

iv)At cathode:

Alkanes

Alkanes are almost non-polar molecules and therefore the molecules are hold
only by weak Van der Waals forces. The weak intermolecular forces depend only
upon the size and the structure of the molecule. Due to weak forces, the C1 to C4
are gases, the next thirteen alkanes from C5 to C17 are liquid and the higher
member with more than 18 carbon atoms are solid at 298 K.

Alkanes have generally low boiling points because these are non-polar and the
molecules are held together only by weak Van der Waals’ forces. With the
increase in the number of carbon atoms, the molecular size increases and
therefore, the magnitude of Van der Waals forces also increases.
Consequently, the boiling points increase with increase in number of carbon
atoms.
It has been observed that each carbon added to the chain increases
the boiling point by 20-30 k. the boiling point of n-alkanes with increase in
number of carbon per molecule of the homologous series.

The melting points of alkanes do not shows regular variation with increase in
molecular size. It has been observed that, in general, the alkanes with even
number of carbon atoms have higher melting points as compared to the
immediately next lower alkanes with odd number of carbon atoms.

Alkane C3H8 C4H10 C5H12 C6H14 C7H16 C8H18

m.p.(K) 85.9 138 143.3 178.5 182.5 216.2

This is because the alkanes with even number of carbon atoms have more
symmetrical structures and result in closer packing in the crystal structure as
compared to alkanes with odd number of carbon atoms. Therefore, the attractive
forces in the former are more and the melting points are higher as compared to the
alkanes with odd number of carbon atoms.

Alkanes being non-polar in nature, are expected to be insoluble in water(polar
solvent). They dissolve in non-polar solvents such as ether, benzene, carbon
tetrachloride etc. The solubility generally decreases with increase in molecular
mass. As we know, petrol is a mixture of hydrocarbon and is used as a fuel for
automobiles.

Alkanes are lighter than water. The density increase with the increase in the number
of the carbon atoms.

The reaction in which an atom or a group of atoms in a
molecule is replaced by some other atom or group of atom.
Alkanes undergo substitution reaction in which one or more
hydrogen atoms are replaced or substituted by different
atoms or groups such as halogen atom (Cl, Br or I), nitro
group(-NO2) or sulphonic acid (-SO3H) group.

This involves the replacement of one or more atoms of alkanes by the
corresponding number of halogens atoms. It is found that the rate of
reaction of alkanes with halogen is F2>Cl2>Br2>I2. Rate of
replacement of hydrogen of alkanes is:3˚>2˚>1˚.

For eg:

The reaction is initiated by homolysis of chlorine molecule in the presence of light
or heat, the Cl-Cl bond is weaker than the C-C and C-H bond and hence, is
easiest to break.

Chlorine free radicals attacks the methane molecule and takes the reaction in the
forward direction by breaking the C-H bond to generate methyl free radical
with the formation of H-Cl.

The methyl radical thus obtained attacks the second molecule of chlorine to form
CH3-Cl with the liberation of another chlorine free radical by homolysis of
chlorine molecule.

The reaction stops after some time due to consumption of reactants and/or due to
following side reaction:
The possible chain terminating steps are:
a)
b)
c)

Though in (c) CH3-Cl, the one of the product is formed bur free radicals are
consumed and the chain is terminated.

Alkanes on heating in the presence of air or dioxygen are completely oxidized to
carbon dioxide and water with the evolution of large amount of heat.

The general combustion equation for any alkane is:

Due to the evolution of large amount of heat during combustion, alkanes are used
as fuels

Alkanes on heating with a regulated supply of dioxygen or air at high pressure and
in the presence of suitable catalyst give a variety of oxidation product:

i)When a mixture of methane and oxygen in the molar ratio of 9:1 is compressed to
about1100 atmospheres and passed through copper tubes at 575 K, methane is
oxidised to methanol.

2CH4 + O2 Cu/575K/1100 atm. 2CH3OH

ii) When methane is mixed with oxygen and passed through heated molybdenum
oxide (Mo2O3), under pressure it is oxidised to methanal.

(CH3)3CH + O alk.KMnO4 HCHO + H2O

Alkane isomerise to branched chain alkanes when heated with anhydrous
aluminium chloride (AlCl3) and hydrogen chloride at 573 K under a pressure of
about 30-35 atmosphere. CH3

CH3CH2CH2CH3 anhy.AlCl3,HCl CH3−CH−CH3
n-butane isopropane

The alkanes containing six or more carbon atoms when heated at about 773K
under high pressure of 10-20 atm in the presence of catalyst on alumina gel get
converted to aromatic compounds. This process is called aromatization.

CH3−(CH2)4−CH3 773K, 10-20 atm

Hexane Benzene

On passing a mixture of steam and methane over heated nickle (supported over
alumina, Al2O3) catalyst at 1273 K, methane is oxidised to carbon monoxide and
hydrogen is evolved.
CH4 +H2O CO + 3H2

When higher alkanes are heated to high tempreture in the presence of alumina or
silica catalysts, the alkanes break down to lower alkanes and alkenes. For eg:
C3H8 C2H4 + CH4 or C3H6 + H2
This reaction is called Fragmentation or Cracking or Pyrolysis. Pyrolysis of hexane
gives following product:

Chemist represent conformations in two simple ways:
a)Sawhorse representation b)Newman projection

In this projection, the molecule is viewed along the axis of the model from an
oblique angle. The central carbon-carbon bond (C-C) s drawn as a straight
line slightly tilted to right for the sake of clarity. The front carbon is shown
as the lower left hand carbon and there are carbon is shown as the upper
right hand carbon.

In this method, the molecule is viewed from the front along the carbon-carbon
bond axis. The two carbon atoms forming the σ bond are represented by two
circle; one behind the other so that only the front carbon is seen. The front
carbon atom is shown by a point whereas the carbon further from the eye is
represented by the circle. Therefore, the C-H bonds of the front carbon are
depicted from the centre of the circle while C-H bonds of the back carbon are
drawn from the circumference of the circle at an angle of 120˚ at each other.

Alkenes are unsaturated hydrocarbons containing carbon-carbon double bond
(C═C)in their molecules. They have the general formula CnH2n. The simplest
member of alkene family is ethene, C2H4. The alkenes are also called olefins
(Greek olefiant meaning oil forming) because the larger member of the series
(such as ethylene, propylene, etc react with chlorine to form oily products.

Propylene

Carbon-Carbon double bond in alkenes consists of one strong sigma(σ) bond (bond
enthalpy about 397kJ mol-1 due to head on overlapping of sp2 hybridised orbitals
and one weak pi() bond(bond enthalpy about 284 kJ mol-1)obtained by lateral or
sideways overlapping of the two 2p orbitals of the two carbon atom. The double
bond is shorter in bond length (134pm) than the single bond (154pm). Alkenes are
easily attacked by reagents or compounds which are in search of
electron(electrophilic reagents)because they behave as source of loosely held mobile
electron. The presence of weaker  bond makes alkenes unstable molecules in
comparison to alkanes and thus, alkenes can be changed into single bond
compounds by combining with the electrophilic reagents.

According to IUPAC system alkenes are named similar to alkanes with the
following modification:
i)The longest continues chain should include both the carbon atoms of the double
bond.
ii)The suffix used for alkene is –ene
iii)The chain is numbered from the end that gives the lower number to the first
carbon atom of the double bond.
iv)If there are two or more double bonds the ending ane of the alkane is replaced by
adiene or atiene.
1 2 3 4 5 1 2 3 4
For eg: CH3CH=CHCHCH3 CH2=CH−CH=CH2
Buta-1,3-diene

CH3
4-Methylpent-2-ene

Isomerism in
Alkanes

Structural Geometrical
Isomerism Isomerism

Chain Position
Isomerism Isomerism

Alkenes show following types of structural isomerisms:

The isomers differ with respect to the chain of carbon atoms. as in alkanes, ethene
(C2H4) and propene(C3H6) can have only one structure but alkenes higher
than propene have different structures.
For eg: 4 3 2 1 But-1-ene
CH3−CH2−CH=CH2

The isomers differ in the position of the double bonds. For eg:
CH2−CH=CH2−CH3 (But-1-ene) CH3−CH=CH−CH3 (But-2-ene)

The compounds which have the same structural formula but differ in the spatial
arrangement of atoms or groups of atoms about the double bond are called
geometrical isomers and the phenomena is known as geometrical isomerism. The
isomers in which similar atoms or groups lie on the same side of the double
bond is called cis-isomers while the other in which they are displaced on
opposite sides, is called trans-isomerism.

Cis-isomer is more polar than trans-isomers. These are distinguish on the basis of
their physical properties such as melting point, boiling point etc.

Alkynes can be reduced to alkenes using palladium charcoal (palladised charcoal)
catalyst partially deactivated with poison like sulphur compounds or quioline.
Partially deactivated palladised charcoal is known as Lindlar’s catalyst.
Alkynes can also be reduced to alkenes with sodium in liquid ammonia (called
Birch reduction).

For eg: CH3−C≡C−CH3 Pd- C, H2 CH3CH═CHCH3
But-2-yne But-2-ene
CH3–C≡CH+H2 CH3–CH=CH2
Propyne Propene
CH≡CH+H2 Pd/C CH2=CH2
Ethyne Ethene

Alkene can be prepared from alkyl halides(usually bromides or iodides) by treating
with alcoholic potash(potassium hydroxide dissolved in ethanol). This reaction
removes a molecule of HX and therefore, the reaction is called
dehydrohalogenation. In this reaction, the hydrogen atom is eliminated from β
carbon atom (carbon atom next to the carbon to which halogen is attached).
Therefore, the reaction is also called β–elimination reaction.

Nature of halogen atom and the alkyl group determine rate of the reaction. It is
observed that for halogens, the rate is: Iodine>Bromine>Chlorine while for alkyl
group it is Tertiary> Secondary>Primary.

Dihalogen derivatives of alkanes in which two halogens atoms are attached to
adjacent carbon atoms (called vicinal dihalogen derivatives) are converted to
alkenes by heating with zinc dust in ethyl alcohol. For eg:
CH3CHBr−CH2Br+Zn CH3CH=CH2+ZnBr

Alkenes are prepared from alcohols by heating with protonic acids such as sulphuric
acid at about 443K. This reaction is called dehydration of alcohols
CH3CH2OH H2SO4 or H3PO4 CH2=CH2+H2O
This reaction is also an example of β-elimination reaction because –OH group takes
out one hydrogen atom from the β- carbon atom.

In general, alkenes have higher melting point than the corresponding alkanes. This is due
to the reason that p-electrons of a double bond are more polarizable than s-electron of
single bonds. As a result, the intermolecular force of attraction are stronger in alkenes
than alkanes. The melting and boiling point of alkenes in general, increase with
increase in molecular mass.

The boiling points of alkene show a regular gradation with the increase in number of
carbon atoms like alkanes. In general, for each added –CH2 group the boiling point
rises by 20˚-30˚.

Alkenes are weakly polar. The p-electron of the double bond can be easily polarized.
Therefore, their dipole moments are higher than those of alkanes. The dipole
moment of alkene depends upon the position of the groups bonded to the two
double bonded carbon atoms. The symmetrical trans alkenes are non-polar and
hence have zero dipole moment. However, unsymmetrical trans-alkenes have
small dipole moment because the two dipoles opposes each other but they do not
cancel out each other exactly since they are unequal. On the other hand, both
symmetrical and asymmetrical cis-alkenes are polar and hence have finite dipole
moments. This is because the two dipoles of individual bonds are on the same side
and hence have a resultant dipole moment.

Alkenes are lighter than water. These are insoluble in water because they are non-
polar. However, they readily dissolve in organic solvents like alcohol, benzene,
ether, carbon tetrachloride, etc.

Alkenes add up on molecule of dihydrogen gas in the presence of finally divided
nickle, palladium or platinum to form alkanes.

Halogens like bromine or chlorine add up to alkene to form vicinal dihalides. The reddish
orange colour of bromine solution in carbon tetrachloride is discharged when bromine
adds up to an unsaturation site. This reaction is used as a test for unsaturation.
Addition of halogen to alkene is an example of electrophilic addition reaction.

Hydrogen halides (HCl, HBr, HI) add up to alkenes to form alkyl halides. The order of
reactivity of the hydrogen halides is HI>HBr>HCl. Like addition of halogens to
alkenes, addition of hydrogen halides is also an example of electrophilic addition
reaction

Markovnikov, a Russian chemist made a generalisation in 1869. these
generalisation led Markovnikov to frame a rule call Markovnikov
rule. The rule stated that:

“During the addition across unsymmetrical multiple
bond, the negative part of the addendum (attacking
molecule)joins with the carbon atom which carries
smaller number of hydrogen atoms while the positive
part goes to the carbon atom with more hydrogen atom.”

Cold concentrated sulphuric acid adds to alkenes in accordance with
Markovnikov rule to form alkyl hydrogen sulphate by the electrophilic addition
reaction.

In the presence of a few drops of concentrated sulphuric acid alkenes react with
water to form alcohols, in accordance with the Markovnikov rule.

Alkenes react with cold dilute aqueous or alkaline potassium permanganate
solution to form 1,2-diols called glycols. The glycols contain two –OH groups
on adjacent carbon atoms. This reaction of addition of two hydroxyl groups
to each end of double bond is called hydroxylation of the double bond.
2KMnO4+H2O 2KOH+2MnO2+3[O]

When alkene is treated with hot acidic potassium permanganate or potassium
dichromate solution the alkene gets split up at the double bond forming
carboxylic acids or ketones. This is also called oxidative cleavage of alkanes.
For eg: CH3−CH=CH−CH3 KMnO4/H+ 2CH3COOH
But-2-ene Ethanoic acid

Alkenes are oxidised with ozone to form ozonides which are unstable compounds.
These are reduced with zinc and water forming aldehydes and ketones. The
reaction is called ozonolysis.

Polymerisation is a process in which a large number of simple (same or different)
molecules combine to form a bigger molecule of higher molecular mass. The
small molecule are called monomers while the bigger molecule are called
macromolecules or polymers.

Alkynes are unsaturated hydrocarbon having carbon-carbon triple bonds in their
molecules. There general formula is CnH2n-2. The simplest member of this class is
ethyne (C2H2) which is properly known on acetylene.

 C2H2 H:C:::C:H H—C C—H
Acetylene
(ethyne)

 C3H4 CH3C CH Methylacetylene
Propyne

Ethyne is the simplest molecule of alkyne series. In the triple bond formation, one
sp hybridised orbital of one carbon atom overlaps axially (head on) with the
similar sp hybrid orbital of the other carbon atom to form σ bond. Each of the
two unhybridised orbitals of one carbon overlaps sidewise with the similar
orbital of the other carbon atom to form two weak  bonds. The remaining sp
hybrid of each carbon atom overlaps with 1s orbital of hydrogen to form C-H
bond. Thus, carbon to carbon triple bond is made up of one σ bond and two 
bonds.

In IUPAC system they are named as derivatives of corresponding alkanes replacing
‘ane’ by the suffix ‘yne’. The following rules should be followed:
i)The longest continues chain should include both the carbon atoms of the triple
bond.
ii) The suffix used for alkyne is – yne.
iii) The chain is numbered from the end which gives the lower number to the first
carbon atom of the triple bond.
iv) The positions of the substituents are indicated.

For eg: 4 3 2 1 1 2 3 4 5 6
CH3CH2C≡CH CH3CH2C≡C−CH2CH3
But-1-yne Hex-3-yne

Alkynes exhibit the following structural isomerisms:

The isomers differ in the chain of carbon atoms. For example, the molecule having
molecular formula C5H8 shows chain isomers as:
5 4 3 2 1
CH3−CH2−CH2−C≡CH
Pent-1-yen

Alkynes having more than four carbon atoms show position isomerism. For
example: 4 3 2 1
CH3−CH2−C≡CH CH3−C≡C−CH3
But-1-yne But-2-yne

Preparation Of
Alkynes

From calcium carbide From Vicinal Dihalides

Acetylene is prepared in the laboratory as well as an industrial scale by the action
of water on calcium carbide.
CaC2 + 2H2O HC≡CH + Ca(OH)2
Calcium carbide required for this purpose is obtained by heating calcium oxide
(from limestone) and coke in an electric furnace at 2275 K.
CaCO3 Heat CaO + CO2

Vicinal dihalides on treatment with alcoholic potassium hydroxide
undergo dehydrohalogenation. One molecule of hydrogen halides is
eliminated to form alkenyl halide which on treatment with sodamide
gives alkyne.

The first three members (ethyne, propyne, butyne) of the family are gases at room
tempreture, the next eight are liquid while the higher ones are . All alkynes
are colourless. However, ethyne has characteristic odour of garlic smell.

Alkynes are weakly polar in nature. They are lighter than water and immiscible
with water but are soluble in organic solvents such as petroleum ether, carbon
tetrachloride, benzene, etc.

The melting and boiling point of the members of the family are slightly
higher as compared to those of the corresponding members of alkane
and alkene families. This is due to the fact that the alkynes have
linear structure and therefore, their molecules are more closely packed
in space as compared to alkanes and alkenes. The magnitude of
attractive forces among them are higher and therefore, the melting
and boiling point are also higher. The melting and boiling point
increase with increase in molecular mass of the alkynes.
Hydrocarbon Ethane Ethene Ethyne
m.p. (K) 101 104 191

b.p. (K) 184.5 171 198

Alkynes react readily with hydrogen in the presence of finely divided Ni, Pt or Pd
as a catalyst. The reaction is called hydrogenation.
HC≡CH+H2 Pt/Pd/Ni [H2C=CH2] H
2 CH3−CH3

Reddish orange colour of the solution of bromine in carbon tetrachloride is
decolourised. This is used as a test for unsaturation.

Two molecule of hydrogen halides(HCl, HBr and HI) add to alkynes to form gem
dihalides (in which two halogens are attached to the same carbon atom). For
example:

Alkenes react with water in the presence of mercuric sulphate (HgSO4) and
sulphuric acid at 337K. The product are carbonyl compounds (aldehydes and
ketones). For eg:

Linear polymerisation of ethyne takes place to produce polyacetylene of polythyne
which is a high molecular weight polyene containing repeating units of
(CH=CH−CH=CH).

Alkynes have larger tendency to polymerize then alkenes and, therefore these give
low molecular mass polymers alkynes when passed through a red hot iron tube
at 873k polymerize to give aromatic hydrocarbons. For eg:

This is the best route for entering from aliphatic to aromatic compounds.

These hydrocarbons are also known as ‘arenes’. Since most of them possess
pleasant odour (Greek; aroma means pleasant smelling), the class of compounds
was named as ‘aromatic compounds’. The parent member of the family is
benzene having the molecular formula C6H6. it has hexagonal ring of six
carbon atoms with three double bond in alternate position.

Aromatic compounds containing benzene ring are known as benzenoids and those
not containing a benzene ring are known as non-benzenoids. For eg:

The stability of benzene can be explained on the basis of concept of resonance.
Kekule in1865 gave a ring structure for benzene in which the positions of the
three double bonds are not fixed. He suggested that the double bond keep on
changing their positions an this is called Resonance. The resonance structure of
benzene is supported by the following facts:
i)The carbon-carbon bond length in benzene is 139 pm which is intermediate
between bond lengths for C-C bond (154 pm)and C=C bond (134 pm) and the
value is the same for all the bonds.
ii)Due to resonance the -electron charge in benzene gets distributed over greater area
i.e., it gets delocalised. As a result of delocalisation the energy of the resonance
hybrid decreases as compared to contributing structure by about 50kJ mol-1. the
decrease in energy is called resonance energy. Therefore, it is stabilised and
behaves as a saturated hydrocarbon.
iii)If the positions of double bonds are fixed. We expect two isomers of 1,2-
dichlorobenzene as shown below (one having Cl atoms attached to C-C bond and
the other having Cl atoms attached to C=C bond).

According to the orbital concept, each carbon atom in benzene is sp2- hybridised
and one orbital remains unhybridised. Out of the three hybrid orbitals, two
overlap axially with the orbitals of the neighbouring carbon atoms on both side
to form σ-bond. The third hybridised orbital of the carbon atom overlaps with the
half-filled orbital of the hydrogen atom resulting in C-H bonds. Thus, benzene
has a planar structure –with bond angle of120˚ each.

There is still one unhybridised 2p-orbital left on each carbon atom. Each one of
these orbitals can overlap sidewise with similar orbital of the carbon atoms on
either sides to form two sets of -bonds. (Shown in fig a. and b. respectively)
a) b)

The resultant -orbital cloud is spread over all the six carbon atoms
(shown in fig c.). As a result, there are two continuous rings of -
electron clouds, one above and the other below the plane of the
carbon atoms(shown in fig d.).

c)

d) electron cloud

Aromatic compounds are those which resembles benzene in chemical
behaviour. These compounds contain alternate double and single
bonds in a cyclic structure. They undergo substitution reaction rather
than addition reaction. This characteristic be behaviour is called
aromaticity. The aromaticity depends upon the electronic structure of
the molecule.

Cyclopentadienyl anion

The main essential for aromaticity are:
 Delocalisation: the molecule should contain a cyclic cloud of delocalized 
electron above and below the plane of the molecule
 Planarity: for the delocalisation of -electron the ring must be planar to allow
cyclic overlap of p-orbitals. Therefore, for a molecule to be aromatic, the ring
must be planar.
 (4n+2) electron: for aromaticity, the -electron could must contain a total of
(4n+2) electrons where n is an integer equal to 0,1,2,3……..n . This is known
as Huckel Rule.

Benzene, 6  e- Naphthalene, 10  e- Anthracene, 14  e-
(n=1) (n=2) (n=3)

 Decarboxylation of aromatic acid
benzene is prepared in the laboratory by heating sodium benzoate with soda lime.

 Reduction of phenol
Benzene can be prepared from phenol by distillation with zinc.

 Benzene and its containing up to eight carbon atoms are colourless
liquids with characteristic smell.
 Aromatic hydrocarbons are immiscible with water but are soluble in organic
solvents.
 They are inflammable and burn with sooty flame.
 They are toxic and carcinogenic in nature.
 The melting and boiling point of aromatic hydrocarbon increase with increasing
molecular mass. This is due to increase in magnitude of van der Waals’ forces
of attraction with increase in molecular size. Amongst isomeric arenes, (i.e., o-
,m- and p- xylenes), the p- isomer has the highest melting point because it is
most symmetrical.

Chemical
Properties

Mechanism of
Electrophilic
electrophilic Addition reaction
substitution reaction
substitution reaction

The replacement of a hydrogen atom in the ring by a nitro (-NO2) group is called
nitration. It is carried out by heating benzene with the nitrating mixture
consisting of concentrated nitric acid and sulphuric acid to about 330K.

The replacement of a hydrogen atom in the ring by a halogen atom (F, Cl, Br or I)
is called halogenation. Arenes react with halogen in the presence of a Lewis
acid like anhydrous FeCl3, FeBr3 or AlCl3 to yield haloarenes.

The replacement of a hydrogen atom in the ring by a sulphonic acid (-SO3H) group
is called sulphonation. It is carried out by heating benzene with fuming
sulphuric acid and oleum.

When benzene is treated with an alkyl halide in the presence of anhydrous
aluminium chloride, alkylbenene is formed.

The reaction of benzene with acyl halide or acid anhydride in the presence of lewis
acid (AlCl3) Yields acyl benzene

According to experimental evidences, SE (S= substitution; E= electrophilic)
reaction are supposed to proceed via the following three steps:
a)Generation of the electrophile.
b)Formation of carbocation intermediate.
c)Removal of proton from the carbonation intermediate.

The attacking reagent may not be strong electrophile. Therefore, first of all an
electrophile is generated by some preliminary reaction. For example , during
chlorination of benzene, an electrophile (Cl +) is generated by reacting with
anhydrous AlCl3 used as catalyst.
Cl2 + AlCl3 Cl+ + AlClˉ4

The electrophile E+ approaches the -electron cloud of the aromatic ring and forms
a bond with carbon, creating a positive charge on the ring. This results in the
formation of a sigma complex (called arenium ion).

The arenium ion gets stabilized by resonance

The resulting carbocation has three important contributing structures which
spread the positive charge over the remaining carbon atom.

The carbocation formed loses a proton to the nucleophile (Nuˉ) present in the
reaction mixture to form a substitution product. During this step, the aromatic
character of the benzene ring is restored and this step is fast.
The loss of proton allows the two electrons from the carbon-
hydrogen bond to move to regenerate the aromatic ring and thus restoring the
aromatic character.

Benzene reacts with hydrogen in the presence of a catalyst such as nickel, or
platinum at 473 to 573 K under pressure to form cyclohexane.

Benzene reacts with chlorine or bromine in the presence of sunlight and absence of
halogen carrier to form benzene hexachloride.

On completely burning with oxygen, benzene gives carbon dioxide and water with
the evolution of a large amount of energy.

When monosubstituted benzene is subjected to further
substitution, three possible disubstituted products are not formed in
equal amounts. Two types of behaviour are observed. Either ortho
and para products or meta product is predominantly formed. This
behaviour depends on the nature of the substituent already present
in the benzene ring and not on the nature of the entering group.
This is known as directive influence of substituents.
a)Ortho and para directing groups
b)Meta directing group

The groups which direct the incoming group to ortho and para position are called
ortho and para directing groups. As an example, let us discuss the directive
influence of –OH (phenolic) group.

The resonance structures of phenol show that the overall electron density on the
benzene ring increases in comparison to benzene. Therefore, it is an activating
group.

The groups which direct the incoming group to meta position are called meta
directing groups. Some examples of meta directing groups are –NO2, -CN, -
CHO, -COR, -COOH, -COOR, -SO3H, etc. Let us take an example of Nitro
group.

Nitro group reduces the electron density in the benzene ring due to its strong-I
effect. Nitrobenzene is the resonance hybrid of the following structures.

Benzene and polynuclear hydrocarbon containing more than two benzene rings
fused together are toxic and said to possess cancer producing (Carcinogenic)
property. Such polynuclear hydrocarbons are formed on incomplete combustion
of organic materials like tobacco, coal and petroleum. They enter into human
body and undergo various biochemical reaction and finally damage DNA and
cause cancer.

Presented By: G. L. Kapde
PGT (Chem) KV-1, Colaba.

Hydrocarbon preeti bhatt

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