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Complete Matter and Chemistry Revision Notes

This lecture covers the fundamental concepts of matter, atomic structure, the modern periodic table, chemical bonding, and everyday chemistry for competitive teaching exams. It details the properties and states of matter, isotopes and isobars, metals and non-metals, alloys and ores, acids, bases, salts, hydrocarbons, and types of chemical reactions.

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Science
English · 10 topics
Checked against the video on 25 Oct 2026

Made by AI from the YouTube video Super TET Science 2026 | पदार्थ एवं पदार्थ की अवस्थाएँ | Matter & States of Matter | Part-1 CLASS-25 (opens YouTube in a new tab) by Balaji Study Adda, then checked against it. All credit for the teaching goes to the creator. Tap a topic’s time to confirm a fact in the video.

Complete Matter and Chemistry Revision Notes

English10 topics · 8 MCQs · 15 flashcardsWatch the video (opens YouTube in a new tab)

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In short

This lecture covers the fundamental concepts of matter, atomic structure, the modern periodic table, chemical bonding, and everyday chemistry for competitive teaching exams. It details the properties and states of matter, isotopes and isobars, metals and non-metals, alloys and ores, acids, bases, salts, hydrocarbons, and types of chemical reactions.

Matter, its Properties, and States

Matter is defined as anything that has mass, occupies space (volume), and of which objects are made.
Physical properties can be observed or measured without altering the chemical composition, including color, odor, taste, density, melting point, boiling point, hardness, luster, elasticity, and solubility.
Chemical properties describe how a substance undergoes a chemical change, such as rusting, burning, acidity, and basicity.
Must knowThe three common states of matter are solid, liquid, and gas; solids have fixed shape and volume, liquids have fixed volume but no fixed shape, and gases have neither fixed shape nor fixed volume.
In solids, particles are tightly packed and incompressible; in liquids, particles are slightly separated and flow; in gases, particles are far apart, highly compressible, and diffuse in all directions.
Must knowThe fourth state of matter is plasma, formed when gases get ionized at extremely high temperatures (found in lightning, the Sun, stars, and neon lights).
At temperatures near absolute zero (approx. -273°C), certain gases form the Bose-Einstein Condensate (BEC), regarded as the fifth state of matter.

Physical vs Chemical Changes and Measurement of Matter

Physical changes alter only the physical form without creating new substances, such as the melting of ice or dissolving sugar in water.
Chemical changes lead to the formation of entirely new substances, such as the rusting of iron and the burning of a candle.
Mass measures the inertia of an object; its SI unit is the kilogram (kg) and it is measured using a beam balance.
Must knowMass remains constant everywhere, whereas weight depends on the force of gravity and varies by location (measured in Newtons).
Volume refers to the space occupied by matter; its SI unit is the cubic meter (m³), commonly measured in liters (L) using measuring cylinders, beakers, or flasks.
Length measures the distance between two points; its SI unit is the meter (m), measured using meter scales, tapes, or vernier calipers.

Metric Unit	Equivalent Value
1 gram (g)	10⁻³ kg
1 milligram (mg)	10⁻⁶ kg
1 microgram (µg)	10⁻⁹ kg
1 Liter (L)	10⁻³ m³
1 milliliter (mL)	1 cm³ = 10⁻⁶ m³
1 centimeter (cm)	10⁻² m
1 millimeter (mm)	10⁻³ m
1 micrometer (µm)	10⁻⁶ m
1 nanometer (nm)	10⁻⁹ m

Elements, Compounds, Mixtures, and State Transitions

An element consists of only one type of atom and cannot be broken down by chemical methods (examples: gold Au, silver Ag, oxygen O₂, iron Fe, copper Cu).
A compound is formed by two or more elements chemically combined in a fixed ratio and can be separated into constituents by chemical methods (examples: water H₂O, common salt NaCl, carbon dioxide CO₂).
A mixture consists of two or more substances physically mixed in any ratio without a chemical reaction, which can be separated by physical methods.
Mixtures are classified as homogeneous (uniform composition throughout, e.g., salt solution, air) or heterogeneous (non-uniform composition, e.g., sand in water, oil in water).
Sublimation is the process where a solid converts directly into gas without passing through the liquid state (examples: camphor, ammonium chloride/nausadar, naphthalene balls, dry ice CO₂).
Diffusion is the spontaneous movement of particles from a region of higher concentration to lower concentration (example: spreading fragrance of perfume).

Substance	Melting Point (°C)	Boiling Point (°C)
Water	0	100
Ice	0	100
Iron	1538	2862
Sulphur	115	444.6

Atomic Structure, Isotopes, and Modern Periodic Table

An atom is the smallest particle of an element that participates in chemical reactions.
Must knowElectrons (discovered by J.J. Thomson in 1897) carry a relative charge of -1 and reside outside the nucleus; protons (discovered by Ernest Rutherford in 1919) carry +1 charge; neutrons (discovered by James Chadwick in 1932) are neutral (0 charge).
Must knowAtomic Number (Z) is the number of protons in an atom, which uniquely identifies the element.
Mass Number (A) is the sum of protons (Z) and neutrons (N): plain text formula A = Z + N.
Isotopes are atoms with the same atomic number but different mass numbers / neutron counts (e.g., Protium ¹H₁, Deuterium ²H₁, Tritium ³H₁).
Isobars are atoms with the same mass number but different atomic numbers (e.g., ¹⁴C₆ and ¹⁴N₇).
Isotones are atoms that have the same number of neutrons (e.g., ¹⁴C₆ and ¹⁵N₇ both have N = 8).
Must knowThe Modern Periodic Law states that properties of elements are periodic functions of their atomic numbers; the table contains 7 periods and 18 groups.

Chemical Bonding and Classification of Elements

Ionic bonds are formed by the transfer of electrons from a metal (donor, forms cation) to a non-metal (acceptor, forms anion), as seen in sodium chloride (NaCl).
Covalent bonds are formed by mutual sharing of electron pairs between non-metal atoms (examples: H₂, Cl₂).
Polar molecules have asymmetric electron charge distribution (e.g., HCl, H₂O, NH₃), while non-polar molecules have symmetric charge distribution (e.g., H₂, Cl₂, CH₄).
Hydrogen bonding occurs between a hydrogen atom of one molecule and an electronegative atom (F, O, N) of another molecule; it is relatively weak (e.g., water molecules).
Metals are generally solids, ductile, malleable, lustrous, good conductors of heat and electricity, and form basic oxides (e.g., Au, Ag, Fe, Cu, Al).
Non-metals exist as solids, liquids, or gases, are non-ductile, non-malleable, poor conductors, and form acidic oxides (e.g., O₂, N₂, S, P).
Metalloids possess intermediate properties and act as semiconductors (e.g., Boron B, Silicon Si, Germanium Ge, Arsenic As).
In the metal reactivity series, metals placed before hydrogen displace hydrogen from dilute acids, while those placed after do not.

Reactivity	Elements (Decreasing Order)
Most Reactive	K > Na > Ca > Mg > Al
Moderate Reactive	Zn > Fe > Pb > (H)
Least Reactive	Cu > Hg > Ag > Au

Alloys, Ores, and Corrosion

An alloy is a homogeneous mixture of two or more metals, or a metal and a non-metal, designed to increase strength, hardness, and corrosion resistance.
Corrosion is the gradual destruction of metals due to reaction with air, moisture, acids, or salts; rusting of iron is a prime example.
Must knowGalvanization is the process of applying a thin protective coating of zinc (Zn) onto iron objects to prevent rusting.

Alloy	Constituent Elements	Common Uses
Brass (Peetal)	Copper + Zinc	Utensils, decorative items
Bronze (Kansa)	Copper + Tin	Statues, medals, bells
Stainless Steel	Iron + Chromium + Nickel	Utensils, machines, surgical instruments
Duralumin	Aluminium + Copper + Magnesium + Manganese	Aircraft, utensils, machine parts
Solder	Lead + Tin	Joining electrical components
Nichrome	Nickel + Chromium	Heater coils, electric resistance wires
Metal	Ore Name	Chemical Formula
Iron	Haematite	Fe₂O₃
Iron	Magnetite	Fe₃O₄
Copper	Chalcopyrite	CuFeS₂
Aluminium	Bauxite	Al₂O₃·2H₂O
Zinc	Zinc Blende	ZnS
Lead	Galena	PbS

Acids, Bases, Salts, and Indicators

Acids taste sour, have a pH less than 7, and turn blue litmus paper red.
Bases taste bitter, feel slippery, have a pH greater than 7, and turn red litmus paper blue.
Neutralization is the reaction between an acid and a base producing a salt and water: Acid + Base -> Salt + Water.
The pH scale ranges from 0 to 14, where 7 indicates a neutral solution (such as pure water), values below 7 indicate acidity, and values above 7 indicate alkalinity.
Common daily life acids: citric acid (lemons, oranges), acetic acid (vinegar), hydrochloric acid (stomach digestive fluid), sulfuric acid (lead-acid batteries).
Common daily life bases: sodium hydroxide (soap manufacturing), calcium hydroxide (whitewash/lime), ammonium hydroxide (glass cleaning solutions).
Common salts: sodium chloride (cooking salt), sodium bicarbonate (baking soda/powder), alum/phitkari (water purification).

Indicator	Color in Acidic Medium	Color in Basic Medium
Blue Litmus	Red	Blue (no change)
Red Litmus	Red (no change)	Blue
Phenolphthalein	Colorless	Pink
Methyl Orange	Red	Yellow
Turmeric (Haldi)	Yellow	Red-Brown

Everyday Chemistry: Plastics, Glass, Cement, and Fibers

Thermoplastics soften on heating and harden upon cooling repeatedly (examples: polythene, PVC, nylon, teflon, acrylic, polypropylene, polystyrene).
Must knowThermosetting plastics set permanently after being molded once and do not soften on reheating (examples: Bakelite, melamine, formica).
Types of glass include soda-lime glass (bottles, window panes), borosilicate glass (heat-resistant labware), flint glass (lenses, optical prisms), and Crookes glass (UV-protective eyeglasses).
Types of cement include Ordinary Portland Cement (OPC, general construction), Portland Pozzolana Cement (PPC, durable structures), white cement (decorative works), and rapid hardening cement.
Fibers are divided into natural fibers (cotton, jute, wool, silk, flax) and synthetic fibers (rayon, nylon, polyester, acrylic, terylene).
Fertilizers replenish soil nutrients: Urea (nitrogenous), DAP (diammonium phosphate - nitrogen and phosphorus), NPK (nitrogen, phosphorus, potassium).
Pesticides control pests: DDT, BHC (lindane), malathion, chlorpyrifos, carbendazim.
Washing soda is sodium carbonate (Na₂CO₃); baking soda is sodium bicarbonate (NaHCO₃).

Carbon, Allotropes, and Hydrocarbons

Carbon (symbol C, atomic number 6, valency 4) forms covalent bonds and extensive chains (catenation), serving as the foundation of organic chemistry.
Must knowThe three major allotropes of carbon are diamond (tetrahedral structure, hardest known natural substance, non-conductor), graphite (hexagonal layered structure, conductor of electricity, pencil lead/lubricant), and fullerene (spherical buckyball C₆₀).
Hydrocarbons contain only carbon and hydrogen atoms, classified into saturated and unsaturated forms.
Complete combustion of fuel in excess oxygen yields carbon dioxide (CO₂), water (H₂O), heat, and light.
Incomplete combustion due to insufficient oxygen yields carbon monoxide (CO), carbon soot, water, and heat.
Parts of a candle flame: outer non-luminous zone (hottest, complete combustion, blue), middle zone (moderately hot, partial combustion, yellow), inner zone (coolest, unburnt fuel vapors, dark/blue).

Hydrocarbon Type	Bond Type	General Formula	Examples
Alkanes (Saturated)	Single bond	CnH2n+2	Methane (CH₄), Ethane (C₂H₆)
Alkenes (Unsaturated)	Double bond	CnH2n	Ethene (C₂H₄), Propene (C₃H₆)
Alkynes (Unsaturated)	Triple bond	CnH2n-2	Ethyne (C₂H₂, acetylene), Propyne (C₃H₄)
Fuel Type	Main Composition	Source / Characteristics
LPG	Propane (C₃H₈) + Butane (C₄H₁₀)	Petroleum refining; liquefied in cylinders
CNG	Methane (CH₄)	Compressed natural gas under high pressure
PNG	Methane (CH₄)	Natural gas supplied through pipelines
Biogas	Methane (CH₄) + CO₂	Anaerobic decomposition of animal dung/waste

Types of Chemical Reactions and Rancidity

A chemical reaction occurs when reactants interact to form new products with distinct chemical identities.
Combination reaction: two or more reactants combine to form a single product (A + B -> AB; e.g., 2H₂ + O₂ -> 2H₂O).
Decomposition reaction: a compound breaks down into two or more simpler substances (AB -> A + B; e.g., CaCO₃ -> CaO + CO₂).
Displacement reaction: a more reactive element displaces a less reactive element from its compound (A + BC -> AC + B; e.g., Zn + CuSO₄ -> ZnSO₄ + Cu).
Double displacement reaction: mutual exchange of ions between two compounds (AB + CD -> AD + CB; e.g., AgNO₃ + NaCl -> AgCl + NaNO₃).
Oxidation involves the addition of oxygen or removal of hydrogen; reduction involves the removal of oxygen or addition of hydrogen.
Rancidity is the unpleasant odor and taste resulting from the oxidation of fats and oils in food items; prevented by using antioxidants (BHA, BHT), storing in airtight containers, flushing with nitrogen, or refrigeration.

Key terms

Matter: Anything that has mass, occupies space, and comprises physical objects
Plasma: The fourth state of matter, consisting of ionized gas at extremely high temperatures
Sublimation: The transition of a substance directly from the solid to the gas phase
Isotopes: Atoms of the same element having identical atomic numbers but different mass numbers
Isobars: Atoms of different elements having identical mass numbers but different atomic numbers
Galvanization: The process of coating iron with a protective layer of zinc to prevent rusting
Neutralization: The chemical reaction between an acid and a base producing a salt and water
Thermosetting Plastic: Plastics that permanently set into shape upon heating and cannot be remolded
Allotrope: Different structural forms of the same chemical element exhibiting different physical properties
Rancidity: Aerial oxidation of fats and oils in food marked by foul smell and altered taste

Formulas

A = Z + N: Mass Number equals Atomic Number (protons) plus Number of Neutrons
pH = -log10[H+]: Formula used to determine the acidity or hydrogen ion concentration
CnH2n+2: General formula for saturated hydrocarbons (Alkanes)
CnH2n: General formula for unsaturated hydrocarbons with a double bond (Alkenes)
CnH2n-2: General formula for unsaturated hydrocarbons with a triple bond (Alkynes)

Exam tips and traps

An easy mnemonic to recall subatomic particle discoveries is 'Ita Par Nacho' (E-Ta: Electron - Thomson; Pa-R: Proton - Rutherford; Na-Cho: Neutron - Chadwick).
Baking soda has an 'H' in NaHCO₃, which stands for hydrogen carbonate or sodium bicarbonate (think 'bi' = buy food / bake).

Quick revision

Read these the night before the exam.

The SI unit of mass is the kilogram (kg) while weight is measured in Newtons (N).
In the reactivity series, Potassium (K) is the most reactive metal and Gold (Au) is the least.
Brass is an alloy made of copper and zinc, while bronze is composed of copper and tin.
The modern periodic table contains 7 periods and 18 groups arranged by atomic number.
Diamond has a rigid three-dimensional tetrahedral structure, while graphite has hexagonal layers.
Graphite conducts electricity due to free electrons, whereas diamond is an electrical insulator.
Phenolphthalein turns pink in basic solutions and remains colorless in acidic solutions.
Turmeric indicator changes from yellow to reddish-brown when exposed to a basic substance.
LPG consists predominantly of propane (C₃H₈) and butane (C₄H₁₀).
Bauxite (Al₂O₃·2H₂O) is the primary ore used to extract aluminium.

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