Chemical Reactions & Equations - Short Notes (Prashant Kirad)

Chemical Reaction

The transformation of chemical substances into another chemical substance.

Chemical Equation

Representation of a chemical reaction using symbols and formulae.

Balanced Chemical Equation

An equation with an equal number of atoms of each element in reactants and products.

Law of Conservation of Mass

Mass of reactants equals mass of products in a chemical reaction.

Decomposition Reaction

A reaction where a single reactant decomposes into two or more products.

Combination Reaction

A reaction in which two or more reactants combine to form a single product.

Exothermic Reaction

A reaction that releases heat during the formation of products.

Endothermic Reaction

A reaction that absorbs heat during the formation of products.

Single Displacement Reaction

A reaction where a more reactive element displaces a less reactive element from its compound.

Double Displacement Reaction

A reaction where two ionic compounds exchange ions to form new compounds.

Oxidation

The gain of oxygen or loss of hydrogen during a reaction.

Reduction

The loss of oxygen or gain of hydrogen during a reaction.

Corrosion

The gradual destruction of metals by chemical reactions with their environment.

Rancidity

The spoilage of fats and oils in food due to oxidation, leading to unpleasant taste and smell.

Reactivity Series of Metals

A series that ranks metals based on their reactivity.

Photolytic Decomposition

Decomposition induced by light.

Electrolytic Decomposition

Decomposition induced by electricity.

Thermal Decomposition

Decomposition induced by heat.

Reactant

A starting substance that undergoes change in a chemical reaction.

Product

A substance formed as a result of a chemical reaction.

Formation of Precipitate

The process of forming a solid from a solution during a chemical reaction.

Evolution of Gas

The release of gas during a chemical reaction.

Absorption of Heat

The process in which a substance takes in heat during a chemical reaction.

Irreversibility of Reactions

Many chemical reactions cannot be reversed or restored to their original state.

Change in State of Matter

Transformation of substances from one state (solid, liquid, gas) to another.

Magnesium Oxide

The white powder formed when magnesium burns in oxygen.

Hydrogen Gas Test

Bubbles of hydrogen burn with a popping sound when ignited.

Calcium Hydroxide

Another name for slaked lime, produced when calcium oxide reacts with water.

Lead Iodide

The yellow precipitate formed when lead nitrate and potassium iodide react.

Carbon Dioxide

A gas produced during respiration, represented in the equation C₆H₁₂O₆ + 6O₂ → 6CO₂ + 6H₂O.

Calcium Carbonate

Decomposes into calcium oxide and carbon dioxide when heated.

Ferrous Sulphate

Decomposed into ferric oxide, sulfur dioxide, and sulfur trioxide upon heating.