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Definition: Anything that has mass, occupies space, and offers resistance is called matter.Perception: Matter can be perceived by our five senses.Examples: Water, soil, stones, plants, animals, books, pens, bags, shoes, cars, sugar, milk, gold, oxygen, and carbon dioxide.
Mass: The quantity (amount) of matter that an object contains. Matter has a definite mass.Difference between Mass and Weight:Mass: The quantity of matter contained in an object. It remains the same at all places.Weight: The force with which the earth attracts an object towards itself. It changes from place to place.
Volume: The space occupied by an object is called its volume.Example (Air): Blowing air into a balloon increases its size because the air occupies space inside it. Releasing the air decreases its size.
Matter resists external force.Examples: Experiencing difficulty swimming in fast-flowing water, or feeling resistance while walking against a storm.
Definition: Atoms are the basic building blocks or basic units of matter. It is the smallest particle that exhibits all the properties of matter.Existence: Atoms usually do not have an independent existence.Historical Timeline:Ancient View: Everything in the universe is made up of five elements (air, water, earth, sky, and fire).Maharishi Kanad (Indian Philosopher): Proposed that matter is composed of very small particles called parmanu.John Dalton (British Chemist): Proposed the modern concept of the atom.
Definition: The smallest particle of matter that exhibits all the properties of matter and has an independent existence.Composition: A molecule is made up of two or more atoms of the same or different kinds. Both atoms and molecules are too small to be seen with the naked eye or an ordinary microscope.Examples:Oxygen Molecule ( 
): Made of 2 atoms of oxygen ( 
).Nitrogen Molecule ( 
): Made of 2 atoms of nitrogen ( 
).Water Molecule ( 
): Made of 2 atoms of hydrogen and 1 atom of oxygen ( 
).
Particles of matter are so tiny they cannot be seen even with a microscope.Example: A single small drop of water contains about 
molecules of water.
Brownian Motion: The continuous zigzag motion of the particles of matter.Kinetic Energy Connection: Particles move because they possess kinetic energy.With Temperature Increase: Kinetic energy increases, causing particles to move faster.With Temperature Decrease: Kinetic energy decreases, slowing down particle movement.Example: Adding blue ink to a glass of water results in the ink spreading uniformly on its own due to the continuous motion of particles.
The space between the particles of matter is known as interparticle or intermolecular space.Example: Adding a teaspoon of sugar to a beaker of water initially increases the water level. After stirring, the sugar dissolves completely, and the water level recedes to its initial mark. This is because sugar particles break down and get accommodated in the spaces between water particles.
The force holding the particles together is called the intermolecular force of attraction.Types of forces:Cohesive Force: Force of attraction between the same kind of particles (e.g., water-water).Adhesive Force: Force of attraction between different kinds of particles (e.g., water-glass).Relationship with Space: The intermolecular force of attraction depends on the intermolecular space.Less space = Stronger intermolecular force of attraction.More space = Weaker intermolecular force of attraction.Example: A piece of wood does not break easily because it has a stronger intermolecular force of attraction between its particles compared to a piece of chalk, which breaks easily.
Melting (Solid 
Liquid): Occurs on heating (e.g., Ice at 
changing to water).Boiling/Evaporation (Liquid Gas): Occurs on further heating (e.g., Water changing to steam at 
).Condensation (Gas Liquid): Occurs on cooling (e.g., Steam cooling to form water).Freezing (Liquid Solid): Occurs on further cooling (e.g., Water kept in a freezer changing to ice at ).Sublimation (Solid Gas directly): A solid changes directly to gaseous state on heating without becoming a liquid (e.g., camphor, naphthalene, ammonium chloride).Deposition (Gas Solid directly): Vapour changes directly to solid state on cooling.
Increasing Pressure: Compressing certain gases forces the molecules closer together, increasing intermolecular forces and converting them to liquids (e.g., LPG, liquid oxygen, liquid nitrogen).Decreasing Pressure: Releasing pressure allows molecules to move far apart, changing the liquid back to gas.Example: Liquefied Petroleum Gas (LPG) is stored in cylinders as a liquid under high pressure. When the regulator valve is opened, pressure is released, and it exits as a gas.
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Prepared by: learnloophq@gmail.com
Chapter: 01. Matter And Its Composition
Matter and Its Composition: Revision Crash Course
1. What is Matter?
2. Fundamental Properties of Matter
A. Matter Has Mass
B. Matter Occupies Space
C. Matter Offers Resistance
3. Composition of Matter
A. Concept of Atom
B. Concept of Molecule
4. Characteristics of Particles of Matter
1. Extremely Small Size
2. Continuous Random Motion (Brownian Motion)
3. Particles Have Spaces Between Them (Interparticle/Intermolecular Space)
4. Particles Attract Each Other (Intermolecular Force of Attraction)
5. States of Matter (Detailed Comparison Table)
S. No.
Parameter
Solid
Liquid
Gas
1.
Shape
Definite shape
No definite shape; takes the shape of the container
No definite shape
2.
Volume
Definite volume
Definite volume
No definite volume; occupies all available space
3.
Molecular Arrangement
Very closely packed
Loosely packed
Far apart
4.
Intermolecular Space
Almost negligible
Larger than solids
Very large
5.
Intermolecular Force
Very strong
Weak
Weakest / negligible
6.
Position of Molecules
Fixed; molecules only vibrate about their mean positions
Not fixed; free to move within the boundary of liquid
Not fixed; free to move in all directions
7.
Rigidity
Rigid
Not rigid
Not rigid
8.
Compressibility
Incompressible
Slightly compressible
Highly compressible
9.
Fluidity
Does not flow
Flows from higher to lower levels
Flows in all directions (Liquid & Gas are fluids)
10.
Solubility in Water
Some insoluble (sand, wood, mud); some soluble (sugar, common salt)
Miscible (vinegar, alcohol); Immiscible (oil, diesel)
Readily soluble (ammonia, chlorine); Insoluble (hydrogen)
11.
Diffusion
Does not diffuse
Diffuses slowly
Diffuses very fast
6. Interconversion of States of Matter
The process of matter changing from one physical state to another and back to its original state without any change in its chemical composition.
A. Interconversion by Temperature Changes
B. Interconversion by Pressure Changes
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