Chemical Reactions and Equations Class 10 Notes Chapter 1

Introduction to Chemical Reactions and Equations 

Physical and chemical changes

Chemical change - One or more new substances with new physical and chemical properties are formed.

Example: Fe(s) + CuSO₄(aq) → FeSO₄(aq)                                                                 + Cu(s)                                          (Blue)               (Green)

Here, when copper sulphate reacts with iron, two new substances, i.e., ferrous sulphate and copper are formed.

Physical change - Change in colour or state occurs but no new substance is formed.

Example: Water changes to steam on boiling but no new substance is formed (even though steam and water look different when they are made to react with a piece of Na, they react the same way and give the exact same products). This involves only change in state (liquid to vapour).

Observations that help determine a chemical reaction

A chemical reaction can be determined with the help of any of the following observations:

(a) Evolution of a gas
(b) Change in temperature
(c) Formation of a precipitate
(d) Change in colour
(e) Change of state

Chemical reaction:

Chemical reactions are chemical changes in which reactants transform into products by making or breaking of bonds (or both) between different atoms.

Types of chemical reactions

Taking into consideration different factors, chemical reactions are grouped into multiple categories.

Few examples are:

• Combination Reaction
• Decomposition Reaction
• Single Displacement Reaction
• Double displacement Reaction
• Redox Reaction
• Endothermic Reaction
• Exothermic Reaction
• Precipitation Reaction
• Neutralisation Reaction

Chemical Reactions and Equations I :-

Word equation:

A word equation is a chemical reaction expressed in words rather than chemical formulas. It helps identify the reactants and products in a chemical reaction.

For example,

Sodium + Chlorine → Sodium chloride

The above equation means: "Sodium reacts with chlorine to form sodium chloride."

Symbols of elements and their valencies:

A symbol is the chemical code for an element. Each element has one or two letter atomic symbol, which is the abbreviated form of its name.

Valency is the combining capacity of an element. It can be considered as the number of electrons lost, gain or shared by an atom when it combines with another atom to form a molecule.

Writing chemical equations:

Representation of a chemical reaction in terms of symbols and chemical formulae of the reactants and products is known as a chemical equation.

Zn(s) + dil. H₂SO₄(aq) → ZnSO₄(aq) + H₂(↑)

   (Reactants)                            (Products)

• For solids, the symbol is "(s)".
• For liquids, it is "(l)".
• For gases, it is "(g)".
• For aqueous solutions, it is "(aq)".
• For gas produced in the reaction, it is represented by "(↑)".
• For precipitate formed in the reaction, it is represented by "(↓)".

Balancing of a Chemical Reaction:

Conservation of mass

According to the law of conservation of mass, no atoms can be created or destroyed in a chemical reaction, so the number of atoms for each element in the reactants side has to balance the number of atoms that are present in the products side.

In other words, the total mass of the products formed in a chemical reaction is equal to the total mass of the reactants participated in a chemical reaction.

Balanced chemical equation:

The chemical equation in which the number of atoms of each element in the reactants side is equal to that of the products side is called a balanced chemical equation.

Steps for balancing chemical equations:

Hit and trial method: While balancing the equation, change the coefficients (the numbers in front of the compound or molecule) so that the number of atoms of each element is same on each side of the chemical equation.

Short-cut technique for balancing a chemical equation:

Example:

aCaCO₃ + bH₃PO₄ → cCa₃(PO₄)₂ + dH₂CO₃

Set up a series of simultaneous equations, one for each element.

Ca: a=3c

C: a=d

O: 3a+4b=8c+3d

H: 3b=2d

P: b=2c

Let's set c=1

Then a=3 and

d=a=3

b=2c=2

So a=3; b=2; c=1; d=3

The balanced equation is

3CaCO₃ + 2H₃PO₄ → Ca₃(PO₄)₂ + 3H₂CO₃

Chemical Reactions and Equations II :-

Types of chemical reactions:

1. Combination reaction-

In a combination reaction, two elements or one element and one compound or two compounds combine to give one single product.

Example-

(i) H₂ + Cl₂ → 2HCl

[Element + Element → Compound]

(ii) 2CO + O₂ → 2CO₂

[Compound + Element → Compound]

NH₃ + HCl → NH₄Cl

[Compound + Compound → Compound]

2. Decomposition reaction-

A single reactant decomposes on the application of heat or light or electricity to give two or more products.

Types of decomposition reactions:

(a) Decomposition reactions which require heat - thermolytic decomposition or thermolysis.

(b) Decomposition reactions which require light - photolytic decomposition or photolysis.

(c) Decomposition reactions which require electricity - electrolytic decomposition or electrolysis.

3. Displacement reaction-

More reactive element displaces a less reactive element from its compound or solution.

(i) Zn(s) + CuSO₄(aq) → ZnSO₄(aq) + Cu(s)

(ii) Cu(s) + 2AgNO₃(aq) → Cu(NO₃)₂(aq) +                                                              2Ag(s)

4. Double displacement reaction-

An exchange of ions between the reactants takes place to give new products.

For example, 

Al₂(SO₄)₃(aq) + 3Ca(OH)₂(aq)  → 2Al(OH)₃(aq) + 3CaSO₄(s)

5. Precipitation reaction-

An insoluble compound called precipitate forms when two solutions containing soluble salts are combined.

For example, 

Pb(NO₃)₂(aq) + 2KI(aq) → 2KNO₃(aq) + PbI₂(↓)(s)(yellow)

6. Redox reaction-

Oxidation and reduction take place simultaneously.

Oxidation: Substance loses electrons or gains oxygen or loses hydrogen.

Reduction: Substance gains electrons or loses oxygen or gains hydrogen.

Oxidising agent: Substance that oxidises another substance and self-gets reduced.

Reducing agent - Substance that reduces another substance and self-gets oxidised.

Examples:

(i) Fe(s) + CuSO₄(aq) → FeSO₄(aq) + Cu(s)

                   (Blue)            (Green)

Fe → Fe⁺² + 2e⁻ (Oxidation) ; Fe - reducing agent.

Cu⁺² + 2e⁻ → Cu(s) (Reduction) ; Cu - oxidising agent.

(ii) ZnO + C → Zn + CO

ZnO reduces to Zn → reduction

C oxidises to CO → oxidation

ZnO - Oxidising agent

C - Reducing agent

7. Endothermic and exothermic reaction

Exothermic reaction: Heat is evolved during a reaction. Most of the combination reactions are exothermic.

Al + Fe₂O_{3 → Al2O3 + Fe + Heat}

CH₄ + 2O₂ → CO₂ + 2H₂O + Heat

Endothermic reaction: Heat is required to carry out the reaction.

6CO₂ + 6H₂O + Sunlight → C₆H₁₂O₆ + 6O₂

                                                  Glucose

Most of the decomposition reactions are endothermic.

Corrosion:

Gradual deterioration of a material, usually a metal, by the action of moisture, air or chemicals in the surrounding environment.

Rusting-

4Fe(s) + 3O₂(from air) + xH₂O(moisture) → 2Fe₂O₃. xH₂O(rust)

Corrosion of copper:

Cu(s) + H₂O(moisture) + CO₂(from air) → CuCO₃. Cu(OH)₂(green)

Corrosion of silver:

Ag(s) + H₂S(from air) → Ag₂S(black) + H₂(g)

Rancidity:

It refers to oxidation of fats and oils in food that is kept for a long time. It gives foul smell and bad taste to food. Rancid food causes stomach infection on consumption.

Prevention-

(i) Use of air-tight containers

(ii) Packaging with nitrogen

(iii) Refrigeration

(iv) Addition of antioxidants or preservatives

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