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      Class 9 Science

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      • Class 09
      • Class 9 Science
      CoursesClass 09ScienceClass 9 Science
      • 01.Matter in Our Surroundings
        9
        • Lecture1.1
          Matter and Its Properties 39 min
        • Lecture1.2
          States of Matter and Compressibility & Rigidity 21 min
        • Lecture1.3
          Moving through, Fluidity, Density, Diffusion, Pressure 26 min
        • Lecture1.4
          Change of State of Matter 56 min
        • Lecture1.5
          Evaporation and Boiling 39 min
        • Lecture1.6
          Cooling Effect of Evaporation Two More States of Matter 22 min
        • Lecture1.7
          Chapter Notes – Matter in Our Surroundings
        • Lecture1.8
          NCERT Solutions – Matter in Our Surroundings
        • Lecture1.9
          Revision Notes Matter in Our Surroundings
      • 02.Is Matter Around Us Pure
        9
        • Lecture2.1
          Elements and Compounds 20 min
        • Lecture2.2
          Mixtures, Homogeneous & Heterogeneous and Chemical & Physical Change 37 min
        • Lecture2.3
          Solution, Suspension, Colloid and Tyndal Effect 48 min
        • Lecture2.4
          Terms related to Solution and Solubility 42 min
        • Lecture2.5
          Separation of Mixtures 47 min
        • Lecture2.6
          Cleaning Drinking Water and Classification of Matter 29 min
        • Lecture2.7
          Chapter Notes – Is Matter Around Us Pure
        • Lecture2.8
          NCERT Solutions – Is Matter Around Us Pure
        • Lecture2.9
          Revision Notes Is Matter Around Us Pure
      • 03.Atoms and Molecules
        7
        • Lecture3.1
          Atom and its Properties, Atomic Mass, Molecule and Molecular Mass 40 min
        • Lecture3.2
          Ions, Valency and Writing the formulae of Compounds 47 min
        • Lecture3.3
          Mole Concept 42 min
        • Lecture3.4
          Calculation of no. of Moles, Percentage of an Element in a Compound and Laws of Chemical Combination 30 min
        • Lecture3.5
          Chapter Notes – Atoms and Molecules
        • Lecture3.6
          NCERT Solutions – Atoms and Molecules
        • Lecture3.7
          Revision Notes Atoms and Molecules
      • 04.Structure of The Atom
        7
        • Lecture4.1
          Charged Particles in Matter and Discovery of Sub – atomic Particles 31 min
        • Lecture4.2
          Atomic Model by J.J Thomson’s Model and Rutherford 57 min
        • Lecture4.3
          Ion, Mass Number, Isotopes, Isobar and Fractional Mass number of Elements 01 hour
        • Lecture4.4
          Electron Distribution in Orbits and Valency 01 hour
        • Lecture4.5
          Chapter Notes – Structure of The Atom
        • Lecture4.6
          NCERT Solutions – Structure of The Atom
        • Lecture4.7
          Revision Notes Structure of The Atom
      • 05.Cell - Fundamental Unit of Life
        7
        • Lecture5.1
          Introduction to Cell and Its Structure – Cell Wall 31 min
        • Lecture5.2
          Cell Membrane, Cytoplasm, Nucleus 32 min
        • Lecture5.3
          Ribosomes, Endoplasmic Reticulum, Golgi bodies, Lisosomes, Mitocondria 38 min
        • Lecture5.4
          Plastids, Vacuole; Types of Cell and Transport through Plasma Membrane 33 min
        • Lecture5.5
          Chapter Notes – Cell – Fundamental Unit of Life
        • Lecture5.6
          NCERT Solutions – Cell – Fundamental Unit of Life
        • Lecture5.7
          Revision Notes Cell – Fundamental Unit of Life
      • 06.Tissues
        8
        • Lecture6.1
          Division of Labour, Plant Tissues – Merismatic Tissue 20 min
        • Lecture6.2
          Plant Tissue-Permanent Tissue: Simple Permanent Tissue 34 min
        • Lecture6.3
          Plant Tissue-Permanent Tissue: Complex and Protective Tissue 31 min
        • Lecture6.4
          Animal Tissue- Muscular Tissue and Nervous Tissue 27 min
        • Lecture6.5
          Animal Tissue- Connective Tissue and Epithelial Tissue 42 min
        • Lecture6.6
          Chapter Notes – Tissues
        • Lecture6.7
          NCERT Solutions – Tissues
        • Lecture6.8
          Revision Notes Tissues
      • 07.Diversity in Living Organisms
        8
        • Lecture7.1
          Introduction to Biodiversity and Classification, Nomenclature 35 min
        • Lecture7.2
          The Five Kingdoms 29 min
        • Lecture7.3
          Plantae Kingdom 42 min
        • Lecture7.4
          Animalia Kingdom 01 hour
        • Lecture7.5
          Classification of Chordates and Revision of Animalia Kingdom 33 min
        • Lecture7.6
          Chapter Notes – Diversity in Living Organisms
        • Lecture7.7
          NCERT Solutions – Diversity in Living Organisms
        • Lecture7.8
          Revision Notes Diversity in Living Organisms
      • 08.Motion
        11
        • Lecture8.1
          Straight Line Motion, Position, Vector and Scalar; 23 min
        • Lecture8.2
          Distance & Displacement 48 min
        • Lecture8.3
          Speed and Velocity 57 min
        • Lecture8.4
          Acceleration and Deacceleration, Uniform & Non-uniform Acceleration 47 min
        • Lecture8.5
          Equations of Uniformly Accelerated Motion 58 min
        • Lecture8.6
          Uniform Circular Motion 30 min
        • Lecture8.7
          Graphical representation of Motion 30 min
        • Lecture8.8
          Calculations Using Graph 28 min
        • Lecture8.9
          Chapter Notes – Motion
        • Lecture8.10
          NCERT Solutions – Motion
        • Lecture8.11
          Revision Notes Motion
      • 09.Force and Newtons Laws of Motion
        12
        • Lecture9.1
          Force and Net or Resultant Force 46 min
        • Lecture9.2
          Newton’s 1st Law 46 min
        • Lecture9.3
          Momentum 46 min
        • Lecture9.4
          Newton’s 2nd Law 27 min
        • Lecture9.5
          Newton’s 2nd Law in Terms of Acceleration; 42 min
        • Lecture9.6
          Newton’s 1st Law from 2nd law and Practical Examples of Newton’s 2nd Law 42 min
        • Lecture9.7
          Newton’s 3rd Law and its Practical Examples 35 min
        • Lecture9.8
          Conservation of Momentum 33 min
        • Lecture9.9
          Practical Applications of Conservation of Momentum 29 min
        • Lecture9.10
          Chapter Notes – Force and Newtons Laws of Motion
        • Lecture9.11
          NCERT Solutions – Force and Newtons Laws of Motion
        • Lecture9.12
          Revision Notes Force and Newtons Laws of Motion
      • 10.Gravitation
        9
        • Lecture10.1
          Universal Law of Gravitation and Free Fall 41 min
        • Lecture10.2
          Falling Bodies: case 1 46 min
        • Lecture10.3
          Falling bodies: case 2 and Air Resistance 42 min
        • Lecture10.4
          Value of g, Mass and Weight, Weight on Moon, Circular Motion and Gravitation 48 min
        • Lecture10.5
          Thrust and Pressure and Pressure in fluids 37 min
        • Lecture10.6
          Archimedes Principle; Density 37 min
        • Lecture10.7
          Chapter Notes – Gravitation
        • Lecture10.8
          NCERT Solutions – Gravitation
        • Lecture10.9
          Revision Notes Gravitation
      • 11.Work and Energy
        7
        • Lecture11.1
          Work and Workdone Against Gravity, Oblique Displacement 01 hour
        • Lecture11.2
          Energy and Different Forms of Energy, Derivation of Formulae of K.E. 58 min
        • Lecture11.3
          Transformation of Energy and Law of Conservation of Energy 01 hour
        • Lecture11.4
          Rate of doing Work and Commercial Unit of Energy 43 min
        • Lecture11.5
          Chapter Notes – Work and Energy
        • Lecture11.6
          NCERT Solutions – Work and Energy
        • Lecture11.7
          Revision Notes Work and Energy
      • 12.Sound
        8
        • Lecture12.1
          Production and Propagation of Sound and Medium for Sound 30 min
        • Lecture12.2
          Frequency and Velocity of Sound Wave, Characteristic of Sound 01 hour
        • Lecture12.3
          Sonic Boom, Light faster than Sound, Reflection of Sound, Echo and Reverberation 56 min
        • Lecture12.4
          Types of Sound Based on Frequency 42 min
        • Lecture12.5
          Human Ear and Intensity of Sound 25 min
        • Lecture12.6
          Chapter Notes – Sound
        • Lecture12.7
          NCERT Solutions – Sound
        • Lecture12.8
          Revision Notes Sound
      • 13.Why do We Fall Ill
        7
        • Lecture13.1
          Factors Determining Health, Disease, Look of Disease, Cause of Disease, Types of Diseases 24 min
        • Lecture13.2
          Infectious Diseases, Immune System, Treatment of Diseases 55 min
        • Lecture13.3
          Prevention from Disease, Vaccination – Immunisation 36 min
        • Lecture13.4
          AIDS, Different Modes for Different Diseases 18 min
        • Lecture13.5
          Chapter Notes – Why do We Fall Ill
        • Lecture13.6
          NCERT Solutions – Why do We Fall Ill
        • Lecture13.7
          Revision Notes Why do We Fall Ill
      • 14.Natural Resources
        7
        • Lecture14.1
          Natural Resource-Air and its Pollution 57 min
        • Lecture14.2
          Natural Resource-Water and Soil and its Pollution 49 min
        • Lecture14.3
          Biogeochemical Cycles 33 min
        • Lecture14.4
          Green House Effect, Global Warming and Ozone Layer Depletion 30 min
        • Lecture14.5
          Chapter Notes – Natural Resources
        • Lecture14.6
          NCERT Solutions – Natural Resources
        • Lecture14.7
          Revision Notes Natural Resources
      • 15.Improvements in Food Resources
        7
        • Lecture15.1
          Various Revolution Held in India; Types of Crops; Crop Season; Crop Variety Improvement 31 min
        • Lecture15.2
          Crop Production Improvement 45 min
        • Lecture15.3
          Crop Protection Improvement and Organic Farming 29 min
        • Lecture15.4
          Animal Husbandry 40 min
        • Lecture15.5
          Chapter Notes – Improvements in Food Resources
        • Lecture15.6
          NCERT Solutions – Improvements in Food Resources
        • Lecture15.7
          Revision Notes Improvements in Food Resources

        Chapter Notes – Is Matter Around Us Pure

        Matter

        Anything which has mass and occupies space is called matter. It may be solid, liquid or gas.

        Matter is of 2 types –

        1. Pure Matter

        2. Impure substances

        Pure Matter

        Pure substances may be defined as material which contains only one kind of atoms or molecules.

        Pure substances are of 2 kinds : –

        1. Elements –

        Pure substances which are made up of only one kind of atoms are known as elements. All atoms in an element are identical. Atoms of different elements are different.

        1. Compounds –

        Pure substances which are made up of only one kind of molecules are known as compounds. Atoms constituting are from two or more different elements. The different elements are combined in fixed proportion in a compound.

        Impure Matter

        Impure matters are also called mixture. A mixture is a material which contains two or more different kinds of particles (atoms or molecules) which do not react chemically but are physically mixed together in any proportion.

        Mixtures are of 2 types:

        1. Homogeneous mixtures –

        A mixture is said to be homogeneous if all the components of the mixture are uniformly mixed and there are no boundaries of separation between them. For example- Salt in water etc.

        1. Heterogeneous mixtures –

        A mixture is sad to be heterogeneous if all the components of the mixture are not thoroughly mixed and there are visible boundaries of separation between them. For example- Sand in water etc.

        Before we proceed further we should know the difference between the properties of compounds and mixtures.

        Properties of Compounds –

        1. A compound is a homogeneous substance.

        2. A compound has a definite composition.

        3. A compound has definite melting point or boiling point.

        4. Energy is absorbed or evolved in the form of heat or light during the formation of a compound.

        5. The properties of compound are entirely different from those of its constituents.

        For example – If we mix Iron and Sulphur in a watch glass, we get a mixture. This is then heated till a black mass is formed. This leads to formation of compound called Iron Sulphide.

        On bringing magnet near to it, no Iron is attracted towards it. Also, Sulphur does not dissolve on adding carbon disulphide, thus, not showing the properties of its constituents.

        6. The constituents of a compound cannot be separated by simple physical means.

        Properties of Mixtures –

        1. A mixture may be homogenous or heterogeneous.

        2. The composition of a mixture is variable.

        3. A mixture does not have a definite melting point or boiling point.

        4. Energy is neither absorbed nor evolved during the formation of a mixture.

        5. The properties of mixture are the properties of its constituents.

        For example- If we mix Iron and Sulphur in a watch glass, we obtain a mixture. Now, if we bring a magnet near it, it attracts the iron-filings which is the property of its constituent (Iron) whereas if we dissolve it in carbon disulphide, then Sulphur gets dissolved leaving the iron-filings unchanged, thus showing the property of its constituent (Sulphur).

        6. The constituents of mixture can be separated by simple physical methods.

        Physical and Chemical Changes

        Physical Change –

        Those changes in which only physical properties of the substances change but no new substances are formed are called physical changes.

        For example – Melting of ice to form water, breaking of glass, preparing a solution etc.

        Chemical Change –

        Those changes in which new substances are formed are called chemical changes and chemical properties of a substance gets changed in a chemical change. For example – Rusting of iron, burning a piece of paper etc.

        NOTE: There are many features which distinguish a physical and a chemical change. They are as follows: –

        Physical Change Chemical Change
        1. A physical change brings about change in physical properties such as physical state, shape, size etc. 1. A chemical change brings about change in chemical properties.
        2. There is no change in chemical composition of a substance during physical change. 2. There is always a change in chemical composition of a substance during chemical change.
        3. No new substance is formed. 3. A new substance is always formed.
        4. It is temporary and hence reversible. 4. It is permanent and hence irreversible.

        Tyndall Effect

        If a light is passed through a medium and its path can be seen, then the substance is said to show Tyndall effect.

        Example: – When a beam of sunlight enters a dark room through some hole in the window, path of light becomes visible due to scattering of light by the colloidal dust particles present in the air of cinema hall. This shows Tyndall effect.

        Solutions, Suspensions and Colloids

        Solution –

        A solution is defined as a homogeneous mixture of two or more chemically non-reacting substances whose composition can be varied within limits.

        A solution as 2 components: –

        1. Solute : The component which is dissolved or which is present in small amount is called solute. It is also called dispersive medium.

        2. Solvent : The component which is present in larger amount is called solvent. It is
        also called dispersion medium.

        Types of solutions –

        1. Solid in Liquid : – Like sugar in water, tincture of iodine (in it iodine is dissolved in alcohol) etc.

        2. Liquid in Liquid : – Like alcohol in water etc.

        3. Gas in Liquid : – Like CO2 dissolved in water in cold-drinks.

        4. Solid in Solid : – Like Alloys such as Brass (copper + zinc), Bronze (copper + tin) etc.

        5. Gas in Gas : – Like in air, various gases are mixed such as O2, N2 etc.

        6. Liquid in Solid : – Like copper sulphate in dental amalgam.

        7. Gas in Solid : – Gas is adsorbed over the surface of metal.

        8. Solid in Gas : – Like camphor in air.

        9. Liquid in Gas : – Like clouds and fog.

        Properties of Solutions –

        1. A solution is a homogeneous mixture.

        2. Size of particles is smaller than 1 nm (10–9 m).

        3. The particles cannot be seen by microscope.

        4. It is a stable mixture, solute does not settle down over a period of time.

        5. If solution is passed through filter paper, solute and solvent do not separate.

        6. It does not scatter light i.e. it do not show Tyndall effect.

        Suspensions –

        A suspension is a heterogeneous mixture in which the solute particles do not dissolve but remain suspended throughout the bulk of medium.

        Properties of Suspension –

        1. It is a heterogeneous mixture.

        2. Size of the particles is greater than 100 nm.

        3. Particles can be seen by naked eyes.

        4. It is unstable mixture. Solute settles down at the bottom over period of time.

        5. If the solution is passed through filter paper, solute and solvent gets separated.

        6. It scatters light when light is passed through the solution i.e. it shows Tyndall effect.

        Colloids –

        Solutions in which the size of particles lies in between those of true solutions and suspensions are called colloidal solutions or simply colloids.

        Types of colloids –

        Dispersed Phase Dispersion Medium Type Examples
        1. Solid Solid Solid Sol Milky glass
        2. Solid Liquid Sol Muddy water
        3. Solid Gas Solid aerosol. Smoke
        4. Liquid Solid Gel Jelly
        5. Liquid Liquid Emulsion Milk
        6. Liquid Gas Aerosol Fog
        7. Gas Solid Solid foam Pumice stone
        8. Gas Liquid Foam Shaving cream

        Properties of Colloids –

        1. It is a heterogeneous mixture

        2. Size of particles is smaller than suspensions but greater than solutions (1 nm to 100 nm).

        3. Particles can be seen by microscope.

        4. It is a stable mixture. Particles do not settle down at the bottom over a period of time.

        5. When the solution passes through the filter paper, the solute and solvent do not separate.

        6. No Tyndall effect is observed.

        Terms related to Solution

        1. Dilute and concentrated solution –

        Dilute and concentrated are comparative terms. A solution having a small amount of solute in a given solvent is dilute whereas a large amount of solute in that given solvent is concentrated when compared with one another.

        2. Unsaturated and saturated solution –

        – A solution that can dissolve more solute in it at a given temperature is called unsaturated solution.

        – A solution which contains maximum amount of solute dissolved in a given quantity of solvent at the given temperature and which cannot dissolve any more solute at that temperature is called saturated solution.

        3. Solubility –

        The maximum amount of solute that can be dissolved in 100 gm of solvent is called solubility of that solute in that solvent at a particular temperature.

        Alternatively, we can say that

        The amount of solute needed to make saturated solution of 100 gm of solvent is called solubility of that solute in that solvent at a particular temperature.

        4. Effect of Temperature on Solubility –

        (a) Solubility of Solid solute in Liquid:

        – As temperatureincreases, solubility also increases.

        – Saturated solution becomes unsaturated.

        – If saturated solution is cooled down, some dissolved solute separates.

        (b) Solubility of Gas in Liquid:

        – As temperature increases, solubility decreases.

        5. Effect of Pressure on Solubility –

        (a) Solid solute in Liquid:

        – As temperature increases, solubility increases.

        – Pressure has no effect on solubility in case of solid solute in liquid.

        (b) Gas in Liquid:

        – As temperature increases, solubility decreases.

        – As pressure increases, solubility increases.

        This is the reason that cold drinks are packaged at high pressure.

        6. Concentration of Solution –

        (a) Solid in Liquid:

        (b) Liquid in Liquid:

        – Concentration is the measure of amount. It is the amount of solute present in the amount of solution.

        Separation of Mixtures

        The method to be used for separating a mixture depends on the nature of its constituents. Here are few to separate various constituents of mixture –

         

        1. Filtration:

        Filtration is a process in which the solute and the solvent are separated using Filter paper. The difference in the solubility of the constituents is used to separate them in this process.

        Basically, it is used to separate insoluble substances from liquid. The substance which is not soluble and remains behind on the filter paper is called residue while the one which is filtered out is called filtrate.

        For example: Sand and water can be separated by the process of filtration.

        1. Evaporation:

        Evaporation is a process which is used to separate a substance that has dissolved in water(or any other liquid).The use of process of evaporation for separating a mixture is based on the fact that liquids vaporize easily whereas solids do not vaporize easily.

        Evaporation is used for recovering dissolved solid substances from liquid mixtures(or solutions) but the liquid itself cannot be recovered by this method. The liquid vaporizes and get lost to the air. Due to evaporation, ink which is a mixture of dye and water, we can obtain its constituents separately.

         

        1. Crystallization:

        It is a process of cooling a hot, concentrated solution of a substance to obtain crystals is called crystallization. The process of crystallization is used for obtaining a pure solid substance from impure sample. This is done as follows:-

        1. The impure solid substance is dissolved in the minimum amount of water to form a solution.
        2. The solution is filtered to remove insoluble impurities.
        3. The clear solution is heated gently on a water bath till a concentrated or a saturated solution is obtained. Then stop heating.
        4. Allow the hot, concentrated solution to cool slowly.
        5. Crystals of pure solid are formed. Impurities remain dissolved in the solution.
        6. Separate the crystals of pure solid by filtration and dry.

        D:\Diagrams\crystal.JPG

        Crystal of Solution of Copper Sulphate

        Copper Sulphate

        1. Chromatography:

        Chromatography is a technique used for separation of those solutes that dissolve in same solvent in very small quantities, the most common being paper chromatography. This separation is based on the fact that though two or more substances are soluble in same solvent (say water) but their solubility may be different.

        It can be used to separate dye from ink. The method for separation is as follows:– Take a thin and long strip of filter paper. Draw a pencil line on it, about three centimeters from one end.

        – Put a small drop of black ink on filter paper strip at the centre of the pencil line. Let the ink dry.

        – When the drop of ink has dried, the filter paper strip is lowered into a tall glass jar containing some water in its lower part (keeping the pencil line at the bottom). The strip should be held vertical. Please note that though the lower end should dip in water but pencil line should remain above the water level.

        – When the water reaches the top end, the strip is removed from the jar and dried. The paper containing separate coloured spots is obtained.

        1. Sublimation:

        The changing of a solid directly into vapours on heating and of vapours into solid on cooling is called sublimation. The solid which undergoes sublimation is said to sublime. The process of sublimation is used to separate those substances from mixture which sublime on heating. The solid substance obtained by cooling the vapours is known as sublimate. The substances like ammonium chloride, camphor undergo sublimation.

        The process of sublimation is used to separate that component of solid-solid mixture which sublimes on heating (the other component of the mixture being non-volatile).

        Here is an example to show how sublimation helps in separating common salt and ammonium chloride-

        – Take a mixture of common salt and ammonium chloride in a china dish placed on a tripod stand.

        – Cover the china dish with an inverted glass funnel and put a cotton plug on the open end of the funnel to prevent vapours going to the atmosphere.

        – Heat the mixture using burner. On heating, ammonium chloride changes into white vapours which rise up and get converted into solid ammonium chloride on coming in contact with cold inner walls of the funnel.

        – Here, pure ammonium collects on thinner walls of the funnel in the form of the sublimate and can be removed. Since common salt is not prone to sublimation so it remains behind in the china dish.

        1. D:\Diagrams\sublimation.JPGSeparation of Two Immiscible Liquids:

        This process is used to separate 2 liquids which don’t mix into one another. These two immiscible liquids are separated through separating funnel.

        A separating funnel is a type of funnel which has a stopcock in its stem to allow the flow of liquid from it , or to stop the flow of liquid from it. The separation of two immiscible liquids depends on the difference in their densities. Example -Kerosene Oil and water.

        Figure below shows separation of Kerosene oil and water.

        D:\Diagrams\liquid 2.pngKerosene Oil having low density settles to the top of water and water is easily obtained by opening the stopcock of the funnel.

        NOTE: – The principle is that immiscible liquids separate out in layers depending on their densities.

        1. Separation of Miscible Liquids / Distillation:

        This process is used to separate 2 liquids which are miscible i.e. they mix into each other in all proportions and form a single layer when put in a container. In this method , we start heating a liquid to form vapour , then cooling the vapour to get back liquid. The liquid obtained by condensing the the vapour is called distillate. This process is used for those liquids which have sufficient difference in their boiling points.

        Figure below shows the process of distillation.

        D:\Diagrams\distillation.JPGThis process is valid only when the difference in boiling point is more than 25 K.

        1. Fractional Distillation:

        Fractional distillation is a process of separating two or more miscible liquids by distillation, the distillate being collected in fractions boiling at different temperatures.

        When the boiling point difference between 2 miscible liquids is less than 25 K, then fractional distillation is used. In this process, except distillation apparatus, a fractionating column is fitted in between distillation flask and the condenser.

        A simple fractionating column has glass beads. These beads provide surface for vapour to cool and condense rapidly.

        Figure above shows the process of Fractional distillation.

        D:\Diagrams\filter.JPG.

        1. Separation of Gases from Air

        Air is a homogeneous mixture of gases and can be separated into its constituents by fractional distillation. The flow diagram shows the steps of process:

        Air

        Compress and cooled by increasing

        pressure and decreasing temperature

        Liquid Air

        Allow to arm up slowly in

        fractional distillation column

        Gases get separated at different heights

        1. Centrifugation:

        If we have a mixture of fine suspended particles in liquid, we can separate it through filtration but that is time consuming .So, we use the process of centrifugation to rapidly separate the mixture. Centrifugation is done by a machine called centrifuge.

        D:\Diagrams\centrifuge.JPGCentrifugation is a method for separating the suspended particles of a substance from a liquid in which the mixture is rotated (or spun) at high speed in a centrifuge.

        As the mixture rotates rapidly, a force acts on heavier suspended particles in it and brings them down to the bottom. The clear liquid being lighter remains on the top. This process is used to separate cream from milk.

        1. Cleaning Water for Drinking

        To have clean water we need to pass the water obtained from lake through a

        long process. It is as follows –

        1. SEDIMENTATION TANK – Heavy impure particles settle down when water is left for some time.
        2. LOADING TANK – Alum is mixed with water. Even small suspended particles settle down.
        3. FILTRATION TANK – It has 3 layers of fine sand, coarse sand & tiny stones. When water passes through them, it is further cleaned.
        4. CHLORINATION TANK – Chlorine is mixed with water in the tank. It kills gems. Now water is sent to home.

        Classification of Matter

        We have studied that matter are of two types – Pure and Impure. Elements are pure matters.

        Around 100 elements exist in nature. Out of those, around 92 are natural and rests are man- made elements. Among them 2 elements are liquid in state – Bromine and Mercury whereas 11 of them exhibit gaseous state like hydrogen , oxygen, nitrogen etc. Thus, most of them are solid in nature.

        Cesium and Gallium are solid at room temperature but tends to change into liquid when temperature increases.

        Properties of metals and non-metals –

        Metals Non-metals
        1. Metals are luster.
        Non-metals do not have luster.
        1. They are generally grey or gold n colour.
        They posses multiple colours.
        1. They conduct heat & electricity.
        They do not conduct heat & electricity.
        1. They are malleable i.e. they can be beaten into thin sheets.
        They are non malleable i.e. they cannot be beaten into thin sheets.
        1. They are ductile i.e. they can be drawn into thin wires.
        They are non ductile i.e. they cannot be drawn into thin wires.
        6. They are sonorous i.e. they produce sound when hit. They are non sonorous i.e. they do not produce sound when hit.

        Metalloids –

        They are those elements which have properties of both metal and non-metal. For example – Germanium, Silicon etc.

        Prev Cleaning Drinking Water and Classification of Matter
        Next NCERT Solutions – Is Matter Around Us Pure

          1 Comment

        1. Arshad
          June 20, 2023
          Reply

          Just amazing notes very helpful thanks ☺️

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