This document provides an overview of chemical reactions and equations. It discusses chemical changes and how they can be represented by balanced chemical equations. The main types of chemical reactions covered are combination reactions, decomposition reactions, displacement reactions, and oxidation-reduction reactions. Examples of each type of reaction are given. The document also explains how to balance chemical equations by ensuring equal numbers of each type of atom on both sides of the reaction equation.

1. Chemical
reactions and
equations

2. Index
Chemical changes
Balanced chemical equations
Combination reactions
Decomposition reactions
Displacement reaction
Oxidation and reduction reactions

3. Chemical changes
The formation of new substances takes place
with different chemical properties is called
chemical changes. A chemical change can be
confirmed by any or all of the following
observations:
•change in state
•change in color
•change in temperature
•evolution of gas

5. • A chemical change is always accompanied by
a chemical reaction. Reaction is the term
used for depicting a change or
transformation in which a substance
decomposes, combines with other substances,
or interchanges constituents with other
substances.

6. Representing a reaction in a sentence form can be
quite complex and laborious at times. Thus, to write
a concise chemical reaction, equations of the
reactions are written. These equations can be
written in different ways such as word equations
and chemical equations. In a word equation,
reactants are written on the left hand side of a
forward arrow.

9. A chemical equation has reactants on the left
hand side. Reactants are substances that are
present at the initiation of a reaction. Hence,
magnesium (Mg) and oxygen (O2) are reactants.
On the other hand, new substances formed after
the completion of the reaction are termed as
products. Thus, magnesium oxide (MgO) which is
written on the right hand side of the equation is a
product. The arrow in the equation signifies the
direction of change.

10. Thus, a chemical equation is an easier and
more concise method for representing a
chemical reaction. It involves writing symbols
and formulae (instead of words) for all
substances involved in the reaction. A chemical
equation also indicates the number of atoms of
each element involved in a reaction.

11. Balanced Chemical
Equations
There are three ways of writing a chemical
equation:

12. Word equation
The above chemical reaction between zinc and
mineral acid can be represented as:
Zinc + Hydrogen chloride → Zinc chloride +
Hydrogen
In a word equation, the reactants are written on
the left hand side of a forward arrow. The products
are written on the right hand side of this arrow.
The arrow signifies that the reaction proceeds from
the reactants towards the products.

14. In a chemical reaction, the total mass of the
reactants should be equal to the total mass
of the products. This means that the total
number of atoms of each element should be
equal on both sides of a chemical equation. Such
an equation is called a balanced
chemical equation, and the method by which it
is obtained is called balancing of chemical
equations.

15. Balancing a chemical equation

16. Step-by-step process of
balancing a chemical equation

17. Step II: List the number of atoms of the various
elements present in the unbalanced equation in
the form of a table.
Element
Number of atoms on the Number of atoms on the
reactant side (L.H.S)
product side (R.H.S)
Ba
1
1
Cl
2
3
Al
2
1
S
3
1
O
12 (4×3)
4

18. Step III: In the next step, select a compound which
contains the maximum number of atoms. In this
case, the compound will be Aluminium sulphate (it
has 2 atoms of Al, 3 atoms of S, and 12 atoms of O).
From this compound, select the element which has
the maximum number of atoms, and which is
present in only one compound on both sides i.e.
oxygen in this case.

19. To balance the number of oxygen atoms, we
can multiply barium sulphate present on the
right hand side by 3 (as shown below). It should
be kept in mind that coefficient ‘3’ will be
written as 3BaSO4 and not as (BaSO4)3.
Oxygen atoms
Number of atoms Number of atoms
on L.H.S
on R.H.S
Before balancing
12 in Al2(SO4)3
4 in BaSO4
To balance
12
3×4

21. Ba
Number of
atoms on
L.H.S
1
Number of
atoms on
R.H.S
3
Cl
2
3
Al
2
1
S
3
3
O
12
12
Element

22. Step IV: As the atoms of both oxygen and
sulphur are balanced, balance the atoms of
Aluminium.
Aluminium atoms Number of atoms Number of atoms
on L.H.S
on R.H.S
2 in Al2(SO4)3
1 in AlCl3
Before balancing
To balance
2
2×1

24. Element
Number of atoms Number of atoms
on L.H.S
on R.H.S
Ba
3
3
Cl
6
6
Al
2
2
S
3
3
O
12
12

25. To make a chemical equation more informative,
the physical state of the reactants and the products
is mentioned along with their chemical formulae.
They are written in common brackets.
Solids are denoted by writing (s),
Liquids are denoted by writing (l),
Gases are denoted by writing (g), and
Solutions in water are denoted by writing (aq).

27. The energy changes involved in a reaction
are denoted by writing the changes
involved in the equation itself.
If energy is used in the reaction, then it will
be written on the left hand side. If it is
released in the process, then it is written on
the right hand side.

29. Combination
Reactions
Chemical reactions are primarily of five types.
They are listed as follows:
1.Combination reactions
2.Decomposition reactions
3.Displacement reactions
4.Double displacement reactions
5.Oxidation and reduction reactions

30. Combination reactions

32. 1. Combination of two
elements

33. 2. Combination of two
compounds

34. Decomposition
Reactions

35. Decomposition reactions require a source of energy
in the form of heat, light, or electricity to decompose
the compound involved. Hence, these reactions can
be classified into three types, depending on the
source of energy for the reaction.
a) Decomposition by heat or thermal decomposition
b) Decomposition by electricity or electrolysis
c) Decomposition by light or photolysis

36. a) Decomposition by heat or
thermal energy

37. In this reaction, one compound i.e. calcium
carbonate breaks down to form two
compounds, namely calcium oxide and carbon
dioxide. Hence, it is an example of
decomposition reactions. Commercially, this
reaction is very important as calcium oxide
(obtained as a product in this reaction) is used
in cement and glass industries.

38. b) Decomposition by electricity
When electricity is passed through water
containing a few drops of sulphuric acid, it
breaks down to give its constituent elements as
products i.e. hydrogen and oxygen. This is
known as electrolysis of water.

39. c) Decomposition by light
When silver chloride is kept in the sun, it
decomposes to form chlorine gas and silver. As
the reaction proceeds, the white coloured silver
chloride turns grey because of the formation of
silver. Chlorine produced in the reaction escapes
into the environment as it is produced in the
gaseous state.

42. Displacemen
t Reactions
In displacement reactions, a more reactive
metal replaces a less reactive metal from the
latter’s salt.
Displacement reactions are of two types:
1.Single Displacement Reactions
2.Double Displacement Reactions

43. Single Displacement Reactions can be
better understood with the help of the
following figure.
In the above figure, you have three blocks. It
will be observed that while red and blue blocks
are fixed in, green block is aloof. Now, if a blue
block is detached from the red and fixed into
the green, it will mean that the green block
displaces the red block.

44. Thus, in a single displacement reaction, an
uncombined single element replaces the other
in a compound.

45. These blocks are detached. Then, the blue block is
exchanged with the yellow block. This represents
a double displacement reaction.
A Double Displacement Reaction is a bimolecular
process in which parts of two compounds are
exchanged to give two new compounds. The
general equation used to represent double
displacement reactions can be written as:
AB + CD → AD + BC

46. Double Displacement Reactions have two common
features: 1.Firstly, two compounds exchange their ions
resulting in the formation of new compounds.
2. Secondly, one of the new products formed would
be separated from the mixture in some way
(commonly as a solid or gas).
Double Displacement Reactions can be further
classified as precipitation, gas formation, and acidbase neutralization reactions.

47. Oxidation and
Reduction
Reactions
Oxidation is defined as a process that involves
a gain of oxygen or a loss of hydrogen. When a
substance gains oxygen or loses hydrogen
during a reaction, it is oxidized.
Reduction is defined as a process that involves
a gain of hydrogen or a loss of oxygen. When a
substance loses oxygen or gains hydrogen
during a reaction, it is reduced.

48. Oxidation and reduction always take place
simultaneously. Therefore, reactions
involving oxidation and reduction are
known as Redox (‘Red’ for reduction and
‘ox’ for oxidation) reactions. In a redox
reaction, one substance is oxidized, while the
other is reduced.

49. The substances that are reduced (provide
oxygen or remove hydrogen) in course of the
reaction are called oxidizing agents. These
substances oxidize other chemicals in the
reaction and are reduced in the process. On the
other hand, the substances that are oxidized
(remove oxygen or provide hydrogen) are
called reducing agents.

50. For example:
In the above reaction, CO2 gets reduced to CO
and here, CO2 is the oxidizing agent. On the
other hand, hydrogen gets oxidized to form
water and here, H2 is the reducing agent.

51. Corrosion
It may be defined as a process where materials,
usually metals, are deteriorated because of a
chemical reaction with air, moisture, chemicals,
etc. For example, corrosion causes damage to
car bodies, bridges, iron railings, ships, and all
objects made of metals (especially those made
from iron).

53. Rancidity
When fats and oils are oxidized, they become
rancid and their smell and taste also changes.
Thus, the oxidation of fats and oils can be easily
observed by a change in their taste and smell.

54. Oxidation of food can be prevented in many ways. Two
common methods are discussed below.
1. Storing food in air tight containers. By doing so, the
oxygen available for oxidation becomes limited. Hence,
oxidation can be prevented.
2. Sometimes, antioxidants are added to food to
prevent their oxidation. These antioxidants are oxidized
first, which slows down the process of rancidity. These
are reducing agents. Normally, vitamin C and vitamin E
are added as antioxidants.

55. Made by-Anushka
Ninama
Class- 10th
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