CARBON

& its compounds

Handwritten Notes

Gaurav Suthar
Carbon

➢ Carbon is Non-Metal. Its symbol is C.

➢ All the living things, Plants and animals are made up of Carbon.

➢ Carbon always forms covalent bonds

➢ The atomic number of carbon is 6.

Element configuration
K L
C(6) 2 4

Covalent Bond

➢ A covalent bond is formed when pairs of electrons are

shared between two atoms.

➢ It is mostly formed between two same nonmetallic atoms or

between nonmetallic atoms.
 Examples of Covalent Bonding

1) Single Bond in Hydrogen (H2)

Hydrogen needs 1 more e- in outermost shell to complete octet.

H + H H H Or H- H

2) Double Bond in Oxygen (O2)

Oxygen needs 2 more e- in outermost shell to complete octet.

O + O O O Or O=O

3) Triple Bond in Nitrogen (N2)

Nitrogen needs 3 more e- in outermost shell to complete octet.

N + N N N Or N=N
4) Water (H2O)

Oxygen needs 2 e to complete its octet while Hydrogen needs 1

e, So Oxygen shares one-one electron from 2 hydrogens to
complete its octet.

H + O + H H O H

Or H-O-H

Physical Properties of Covalent Compounds

a) Covalent compounds have low melting and boiling points as they

have weak intermolecular force.

b) They are generally poor conductor of electricity as electron are

shared between atoms therefore no charged particles are
formed.

How carbon attain Noble gas configuration?

Carbon is Tetravalent, it does not form ionic bond by either losing

four electrons (C4+) or by gaining four electrons (C4-). It is difficult
to hold four extra electron and would require large amount of
energy to remove four electrons. So, carbon can form bond by
sharing of its electrons with the electrons of other carbon atom or
with other element and attain noble gas configuration.

Versatile Nature of Carbon

The three characteristic properties of carbon element which lead

to the formation of large number of compounds.

1) Catenation -

The self-linking of atoms of an element to create chains

and rings by covalent bonds.
2) Tetravalency –

Carbon has 4 valence electrons. Carbon can bond with four

carbon atoms, monovalent atoms, oxygen, nitrogen and sulphur.

3) Tendency to form Multiple Bonds –

Due to its small size carbon has a strong tendency to form

multiple bonds (double and triple bonds) by sharing more than
one electron pair with its own atoms or with the atoms like
oxygen, nitrogen etc.

Allotropes of Carbon

Allotropy is the property by which an element exists in more than

one form and each form has different Physical Properties but
similar Chemical Properties.

Diamond

➢ It is formed by bonding of each carbon atom is Covalently

bonded to four other forming Rigid 3-D Structure.

➢ It is the hardest thing on Earth.

➢ It is a bad conductor of electricity. This is because all the

valence electrons of each Carbon are involved in the Covalent
Bonding, and no unpaired electrons are left in the crystal.
➢ It has very high melting point.

➢ It is used for making Jewellery and cutting Glasses

Kohinoor Structure of Diamond

Graphite

➢ It is formed by bonding of each carbon atom hexagonally (six-

member rings) in same plane.

➢ It is very soft and slippery because Layers can slide over one
another.

➢ It is a good conductor of electricity because in graphite every

carbon is bonded with three other carbon atoms. So last
electron in every carbon atom is free to move.

➢ It is used for making Pencil Leads, Engine Oils, Batteries and

Cells
 Fullerene

➢ Fullerenes form another class of carbon allotropes.

➢ First one to be identified was C – 60, which has carbon atom

arranged in the shape of football.

➢ It has 12 pentagons and 20 hexagons.

Hydrocarbon

Compounds made up of hydrogen and carbon are called hydrocarbon.

Hydrocarbon

Saturated Unsaturated

Saturated -

Compounds of carbon which are linked only by single bonds between

the carbon atoms.

Types of saturated hydrocarbons -

Alkanes - The hydrocarbons in which all the carbon atoms are

linked by only single covalent bonds are called alkanes.

General formula - CnH2n+2

Example -

H H

H C C H

H H

Ethane (C2H6)
Unsaturated -

Compounds of carbon having double or triple bonds between their

carbon atoms.

Types of Unsaturated hydrocarbons -

Alkenes – Those unsaturated hydrocarbons which have at least one

double bond along with single bonds are called alkenes.

General formula - CnH2n

Example -

H H

H C C H

Ethene (C2H4)

Alkynes - Those unsaturated hydrocarbons which have one or more

triple bonds along with the single bonds are called
alkynes.

General formula - CnH2n-2

Example -

H C C H

Ethyne (C2H2)
IUPAC Nomenclature of Hydrocarbons

Name of Hydrocarbon = Prefix + Suffix

Prefix – Based on Number of carbon atoms in the chain.

No. of Carbons Present Prefix

1 Meth

2 Eth

3 Prop

4 But

5 Pent

6 Hex

7 Hept

8 Oct

9 Non

10 Dec
Suffix – Based on type of Bond

For Single Bond - (Alkane → ane)

For Double Bond - (Alkene → ene)

For Triple Bond - (Alkyne → yne)

For Example -

CH3 CH2 CH3 Propane

CH3 CH2 CH2 Propene

CH3 C CH Propyne

Carbon Compounds on the Basis of structure

1) Straight (unbranched) chain

H H H

H C C C H

H H H
2) Branched chain

H H H

H C C C H

H H

H C H

3) Cyclic Chain

H H

H C C H

H C C H

H H
Functional Groups

- An atom or group of atom that makes a carbon compound reactive

and decides its chemical property is called a functional group.

Functional Group Family Suffix

OH Alcohol ol

O
Aldehyde al
C H

O
Ketones one
C

O
Carboxylic Acid oic acid
C OH

Halogen chloro, bromo

ClClor Br
(Chlorine, Bromine) (Prefix)
 Steps of Nomenclature

Prefix + Root Word + Suffix

Step 1) - Identify the number of carbon atoms in compounds. It

will give us Root Word (like Meth, Eth, Prop, etc).

Step 2) - Identify the type of bond (single, double, triple) between

carbon atoms. It will give us Suffix (like -ane, -ene, -yne).

Step 3) - Identify the Functional group. It will give us Suffix (like

-one, -ol, -al) or Prefix (like Chloro, Bromo).

Homologous Series

- A series of carbon Compound in which same functional Group and

differ by CH2 are known as Homologous Series.

Example –
Alcohols – CH3OH, C2H5OH, C3H7OH, C4H9OH

Some Properties -

➢ All members are represented by same General Formula

➢ 2 adjacent members differ by -CH2 group.

➢ 2 adjacent members differ by molecular mass of 14u.

➢ All shows similar chemical properties. (but not physical)

 Chemical Properties of Carbon Compounds

1) Combustion -

- A chemical reaction in which heat and light are given out is

called combustion.

i) Combustion of Carbon -

C + O2 CO2 + Heat + Light

ii) Combustion of Hydrocarbon -

CH4 + O2 CO2 + H2O + Heat + Light

iii) Combustion of Alcohol -

CH3CH2OH + O2 CO2 + H2O + Heat + Light

2) Oxidation –

- Alcohols can be converted to carboxylic acid in the presence

of oxidizing agent Alkaline KMnO4 (potassium permanganate)
or K2Cr2O7 Acidified potassium dichromate.

Alkaline KMnO4
CH3–CH2–OH CH3COOH
Acidified K2Cr2O7
(ethanol)
 Catalyst

A substance that makes a chemical reaction happen faster,

without being used up in the reaction.

Examples - Nickel(Ni), Palladium(Pd), Potassium permanganate

(KMnO4), Potassium dichromate (K2Cr2O7)

3) Addition Reaction -

- Unsaturated hydrocarbons add hydrogen in the presence of

catalyst such as palladium or Nickel to give saturated
hydrocarbons

Ni or Pd
CH2 CH2 CH3 CH3
H2
(ethene) (ethane)

Above reaction is also known as Hydrogenation reaction.

Uses of Hydrogenation Reaction -

➢ Vegetable oils are converted into vegetable ghee using this

process.

➢ Animal fats generally contain saturated fatly acid which are

harmful for health.
4) Substitution Reaction -

- It is a single replacement chemical reaction during which one

functional group in chemical compounds is replaced by another
functional groups.

Example -

CH3OH + HBr CH3Br + H2O

Sunlight
CH4 + Cl2 CH3Cl + HCl

Important Carbon Compounds

Ethanol (CH3CH2OH)

Physical Properties of Ethanol -

➢ Colourless, Good smell and Burning taste.

➢ Ethanol is Liquid, soluble in water

➢ Ethanol is commonly called alcohol and is the active ingredient

of Alcoholic drinks.

➢ Ethanol is a good solvent, so it is used in medicines such as

tincture iodine, cough syrups and many tonics.
Chemical Properties of Ethanol -

1) Reaction with Sodium -

2CH3–CH2–OH + 2Na 2CH3CH2ONa + H2

(sodium
ethoxide)

This reaction is used as a test for ethanol by evolution of H2

gas (Burn with pop sound).

2) Dehydration –

Hot concentrated
CH3–CH2–OH CH2 CH2 + H2O
H2SO4
(ethanol)

Hot concentrated H2SO4 act as Dehydrating Agent

Ethanoic Acid (CH3COOH)

Physical Properties of Ethanoic acid -

➢ Ethanoic acid is also known as Acetic Acid.

➢ Melting point of pure ethanoic Acid is 290 K.

➢ Solution of Acetic Acid in water is called Vinegar and is used as
preservative in pickles

➢ Ethanoic Acid is weak acid.

Chemical Properties of Ethanoic Acids -

1) Esterification Reaction –

Reaction of Acid and Alcohol gives Ester.

Acid
CH3-COOH + CH3–CH2–OH CH3-COOCH2CH3 + H2O
(Ethanoic Acid) (Ethanol) (ethyl acetate ester)

- Esters are sweet smelling substances

- Used in Making Perfumes and as Flavouring Agents.

Saponification Reaction

This reaction is used in for making Soap.

Ester + Base → Alcohol + Soap

Example –

NaOH
CH3–COOCH2CH3 CH3CH2OH + CH3COONa
(Ester) (Ethanol) (Soap)
2) Reaction with base (Neutralisation Reaction) –

CH3COOH + NaOH CH3COONa + H2O

3) Reaction with Carbonates -

2CH3COOH + Na2CO3 2CH3COONa + H2O + CO2

4) Reaction with Hydrogen carbonates -

CH3COOH + NaHCO3 CH3COONa + H2O + CO2

Distinguish between Ethanol & Ethanoic acid

We can distinguish experimentally between alcohol and
Carboxylic acid by reacting them with sodium Carbonate, turning
lime water milky. Alcohols do not react to give lime water milky
 Soaps and Detergents

Soap -

- Soap is sodium or potassium salt of long chain carboxylic acid.

Example –
C17H35COONa+

- Soaps are effective only in soft water.

Soap molecule has –

a) Ionic (hydrophilic part)

b) Long hydrocarbon chain (hydrophobic part)

Example of Soaps -

Cleansing Action of Soap

1) When soap is added to water, the soap molecules uniquely

orient themselves to form spherical shape micelles.
2) The non-polar hydrophobic part or tail of the soap molecules
attracts the dirt or oil part of the fabric, while the polar
hydrophilic part or head,(−COO−Na+, remains attracted to
water molecules.

3) The agitation or scrubbing of the fabric helps the micelles to

carry the oil or dirt particles and detach them from the
fibres of the fabric.
Detergents -

- Detergents are ammonium or sulphonate salt of long chain of

carboxylic acid.

- Detergents are effective in both hard and soft water.

Example of Detergents -

Hard Water

- Hard water means, water having a very high amount of

minerals like Calcium and Magnesium

- When soap is added to hard water, calcium and magnesium ions

of hard water react with soap forming insoluble product called
Scum. This scum create difficulty in cleansing action.

- By use of detergent, insoluble scum is not formed with hard

water and cloths get cleaned effectively. So, Detergents can
only be used in Hard Water but not Soap.
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