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      Class 10 Science

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      • Class 10
      • Class 10 Science
      CoursesClass 10ScienceClass 10 Science
      • 01. Chemical Reactions
        8
        • Lecture1.1
          Elements, Compounds, Ions- Formation of Compounds 01 hour
        • Lecture1.2
          Common Observations in Chemical Reactions and Chemical Equation 27 min
        • Lecture1.3
          Balancing 35 min
        • Lecture1.4
          Information from Chemical Reaction, Oxidation & Reduction and Types of Reactions 55 min
        • Lecture1.5
          Some Important Experiments 37 min
        • Lecture1.6
          Chapter Notes – Chemical Reactions
        • Lecture1.7
          NCERT Solutions – Chemical Reactions
        • Lecture1.8
          Revision Notes Chemical Reactions
      • 02. Acids, Bases and Salts
        10
        • Lecture2.1
          Introduction to Acids and Bases 50 min
        • Lecture2.2
          Reactions of Acids and Bases 33 min
        • Lecture2.3
          Acid and Base react with Metal, Carbonate and Bicarbonate, Metal Oxide; Corrosive Nature and Uses of Acids and Bases 30 min
        • Lecture2.4
          pH Scale and Acid Base Indicator 50 min
        • Lecture2.5
          Importance of pH in Everyday Life, Acids and Bases in absence of Water; 25 min
        • Lecture2.6
          Salt, pH of Salt and Water of Crystallization 51 min
        • Lecture2.7
          Common Salt, Sodium Hydroxide, Bleaching Powder, Baking Soda, Washing Soda 36 min
        • Lecture2.8
          Chapter Notes – Acids, Bases and Salts
        • Lecture2.9
          NCERT Solutions – Acids, Bases and Salts
        • Lecture2.10
          Revision Notes Acids, Bases and Salts
      • 03. Metals and Non - metals
        10
        • Lecture3.1
          Physical Properties of Metals & Non-Metals 39 min
        • Lecture3.2
          Chemical Properties of Metals 43 min
        • Lecture3.3
          Chemical Properties of Non-metals and Difference b/w Metals and Non-metals 47 min
        • Lecture3.4
          Electron Distribution in Orbits and Valency 01 hour
        • Lecture3.5
          Electron Dot Structure and Occurrence Extraction of Metals-Low reactivity 01 hour
        • Lecture3.6
          Extraction of Metals of Medium and High Reactivity 46 min
        • Lecture3.7
          Corrosion 27 min
        • Lecture3.8
          Chapter Notes – Metals and Non – metals
        • Lecture3.9
          NCERT Solutions – Metals and Non – metals
        • Lecture3.10
          Revision Notes Metals and Non – metals
      • 04. Periodic Classification of Elements
        6
        • Lecture4.1
          Attempts by Scientist to Classify the Elements 01 hour
        • Lecture4.2
          Atomic Number, Electronic distribution 59 min
        • Lecture4.3
          Modern Periodic Table 02 hour
        • Lecture4.4
          Chapter Notes – Periodic Classification of Elements
        • Lecture4.5
          NCERT Solutions – Periodic Classification of Elements
        • Lecture4.6
          Revision Notes Periodic Classification of Elements
      • 05. Life Processes - 1
        9
        • Lecture5.1
          Life Processes of living Beings, Nutrition, Mode of Nutrition and Nutrition in Plants 47 min
        • Lecture5.2
          Experiments to Show Necessity of Sunlight, chlorophyll, carbon dioxide in Photosynthesis and Nutrition in Heterotrophs 31 min
        • Lecture5.3
          Nutrition in Human Beings, Dental Caries and Heterotrophic Mode of Nutrition 52 min
        • Lecture5.4
          Respiration 29 min
        • Lecture5.5
          Exchange of Gases during Respiration 39 min
        • Lecture5.6
          Exchange of Gases in Other Organisms and Exchange of Gases in Plants 30 min
        • Lecture5.7
          Chapter Notes – Life Processes – 1
        • Lecture5.8
          NCERT Solutions – Life Processes
        • Lecture5.9
          Revision Notes Life Processes
      • 06. Life Processes - 2
        6
        • Lecture6.1
          Human Circulatory System 59 min
        • Lecture6.2
          Relaxation and Contraction of Heart 27 min
        • Lecture6.3
          Blood, Circulatory System in Some Other Animals and Lymphatic System 34 min
        • Lecture6.4
          Transportation in Plants 58 min
        • Lecture6.5
          Excretion in Humans and in Plants 31 min
        • Lecture6.6
          Chapter Notes – Life Processes – 2
      • 07. Control and Coordination
        9
        • Lecture7.1
          Introduction to Control and Coordination, Receptors, Neurons 27 min
        • Lecture7.2
          Peripheral Nervous System, Voluntary & Involuntary Actions, Reflex Action and Arc 39 min
        • Lecture7.3
          Central Nervous System 22 min
        • Lecture7.4
          Endocrine System and Feedback Mechanism, Nervous vs Endocrine System 01 hour
        • Lecture7.5
          Control & Coordination in Plant, Harmons in Plants and Movement in Plants 21 min
        • Lecture7.6
          Tropism and Nastic Movement 39 min
        • Lecture7.7
          Chapter Notes – Control and Coordination
        • Lecture7.8
          NCERT Solutions – Control and Coordination
        • Lecture7.9
          Revision Notes Control and Coordination
      • 08. How do Organisms Reproduce
        7
        • Lecture8.1
          Introduction to Reproduction and Asexual Reproduction 36 min
        • Lecture8.2
          Sexual Reproduction in Plants 33 min
        • Lecture8.3
          Sexual Reproduction in Humans 40 min
        • Lecture8.4
          Ovulation in Females and Importance of Variation 49 min
        • Lecture8.5
          Chapter Notes – How do Organisms Reproduce
        • Lecture8.6
          NCERT Solutions – How do Organisms Reproduce
        • Lecture8.7
          Revision Notes How do Organisms Reproduce
      • 09. Heredity and Evolution
        7
        • Lecture9.1
          Introduction, Variation during Reproduction and Heredity- Rules of Inheritance 43 min
        • Lecture9.2
          Mendel’s Contributions, Sex Determination, How traits are expressed 40 min
        • Lecture9.3
          Evolution- Illustration , Speciation, Darwin’s Theory 24 min
        • Lecture9.4
          Tracing Evolutionary Relations, Molecular Phylogeny; Evolution by Stages 49 min
        • Lecture9.5
          Chapter Notes – Heredity and Evolution
        • Lecture9.6
          NCERT Solutions – Heredity and Evolution
        • Lecture9.7
          Revision Notes Heredity and Evolution
      • 10. Light (Part 1) : Reflection
        8
        • Lecture10.1
          Light and Reflection of Light 39 min
        • Lecture10.2
          Formation of Image by a Plane Mirror 32 min
        • Lecture10.3
          Terms Related to Spherical Mirror and Reflection of Rays by Concave/ Convex Mirrors 26 min
        • Lecture10.4
          Formation of Image by Concave and Convex Mirror , Distinguishing b/w the 3 Types of Mirror 47 min
        • Lecture10.5
          Uses of Concave Mirror and Convex Mirror; Mirror Formulae; Magnification 50 min
        • Lecture10.6
          Chapter Notes – Light (Part 1) : Reflection
        • Lecture10.7
          NCERT Solutions – Light- Reflection and Refraction
        • Lecture10.8
          Revision Notes Light- Reflection
      • 11. Light (Part 2) : Refraction
        5
        • Lecture11.1
          Introduction to Refraction and Light Ray Passing through Glass Slab 46 min
        • Lecture11.2
          Refraction by Spherical Lens 59 min
        • Lecture11.3
          Lens formulae, Magnification and Power of Lens 28 min
        • Lecture11.4
          Chapter Notes – Light (Part 2) : Refraction
        • Lecture11.5
          Revision Notes Light (Part 2) : Refraction
      • 12. Carbon and Its Compounds
        9
        • Lecture12.1
          Introduction to Carbon and its Allotropes 42 min
        • Lecture12.2
          Compounds of Carbon and Hydrocarbons 40 min
        • Lecture12.3
          Isomers and Homologous Series 51 min
        • Lecture12.4
          Functional Group 35 min
        • Lecture12.5
          Chemical Properties of Carbon and it’s Compounds 43 min
        • Lecture12.6
          Commercially Important Compounds of Carbon 29 min
        • Lecture12.7
          Chemical Properties of Acetic acid; Soaps & Detergents- Soft and Hard Water 31 min
        • Lecture12.8
          Chapter Notes – Carbon and Its Compounds
        • Lecture12.9
          Revision Notes Carbon and Its Compounds
      • 13. The Human Eye and The Colorful World
        7
        • Lecture13.1
          The Human Eye 38 min
        • Lecture13.2
          Defects of Eye and Correction, Why we have two eyes 50 min
        • Lecture13.3
          Refraction of Light through Prism, Dispersion of Light and its Application, Atmospheric Refraction 47 min
        • Lecture13.4
          Practical Applications of Scattering of Light 35 min
        • Lecture13.5
          Chapter Notes – The Human Eye and The Colorful World
        • Lecture13.6
          NCERT Solutions – The Human Eye and The Colorful World
        • Lecture13.7
          Revision Notes The Human Eye and The Colorful World
      • 14. Electricity
        8
        • Lecture14.1
          Electric Current, Potential Difference and Circuit Diagram 53 min
        • Lecture14.2
          Ohm’s Law and its Verification 46 min
        • Lecture14.3
          Resistance of a system of Resistors in series 31 min
        • Lecture14.4
          Resistance of a system of Resistors in Parallel and Devices in Series & Parallel 01 hour
        • Lecture14.5
          Heating Effect of Current, Electric Power 01 hour
        • Lecture14.6
          Chapter Notes – Electricity
        • Lecture14.7
          NCERT Solutions – Electricity
        • Lecture14.8
          Revision Notes Electricity
      • 15. Magnetic Effect of Current
        10
        • Lecture15.1
          Magnets; Magnetic Compass, Magnetic Field & Field Lines and its Properties 27 min
        • Lecture15.2
          Magnetic Field due to current carrying Straight Wire, Circular Loop, Solenoid; Electromagnet 18 min
        • Lecture15.3
          Magnetic force on Current Carrying Wire placed in magnetic field 38 min
        • Lecture15.4
          Electric Motor 29 min
        • Lecture15.5
          Electromagnetic Induction 32 min
        • Lecture15.6
          Electric Generator (Dynamo) 20 min
        • Lecture15.7
          Domestic Electric Circuits 30 min
        • Lecture15.8
          Chapter Notes – Magnetic Effect of Current
        • Lecture15.9
          NCERT Solutions – Magnetic Effect of Current
        • Lecture15.10
          Revision Notes Magnetic Effect of Current
      • 16. Sources of Energy
        5
        • Lecture16.1
          Good Source of Energy, Fossil Fuels, Energy Production By Power Plants, Wind Energy 40 min
        • Lecture16.2
          Energy from Different Sources 47 min
        • Lecture16.3
          Chapter Notes – Sources of Energy
        • Lecture16.4
          NCERT Solutions – Sources of Energy
        • Lecture16.5
          Revision Notes Sources of Energy
      • 17. Our Environment
        5
        • Lecture17.1
          Types of Living beings, Food Chain, Food Web, Trophic Levels; Flow of Energy, Biological Magnification, Ecosystem 51 min
        • Lecture17.2
          Our Effect on Environment and Ozone Layer Depletion 23 min
        • Lecture17.3
          Chapter Notes – Our Environment
        • Lecture17.4
          NCERT Solutions – Our Environment
        • Lecture17.5
          Revision Notes Our Environment
      • 18. Management of Natural Resources
        4
        • Lecture18.1
          Introduction to Management of Natural Resources, Management of Forest and Wildlife 34 min
        • Lecture18.2
          Management of Water and Fossil Fuel and Reduce, Reuse and Recycle 39 min
        • Lecture18.3
          NCERT Solutions – Management of Natural Resources
        • Lecture18.4
          Revision Notes Management of Natural Resources

        Chapter Notes – Chemical Reactions

        Chemical Reactions and Equations

        Chemical Reaction – The transformation of chemical substance into another chemical substance is known as Chemical Reaction. For example: rusting of iron, burning of coal, burning of candle, burning of paper, setting of milk into cottage cheese or ghee, digestion of food etc.

        In chemical reaction new substance is formed which is completely different in properties from the original substance, so in a chemical reaction chemical change takes place.

        Experiment 1 –

        The burning of magnesium in air to form magnesium oxide is an example of a chemical reaction.

        Magnesium + Oxygen –heat–>Magnesium oxide

        (As ribbon)   (From air)               (White powder)

        • Take about 2cm long magnesium ribbon and clean it by rubbing its surface with sand paper.
        • Hold it with a pair of tongs. Burn it using a burner.
        • The magnesium ribbon starts burning with a dazzling white flame.
        • Hold the burning magnesium ribbon over a watch glass so that the magnesium oxide powder being formed collects in the watch glass.

        Note: Before burning in air, the magnesium ribbon is cleaned by rubbing with a sand paper. This is done to remove the protective layer of basic magnesium carbonate from the surface of magnesium ribbon so that it may readily combine with the oxygen of air.

        Experiment 2 –

        Formation of a precipitate:

        Some chemical reactions are characterized by the formation of precipitate. A precipitate is a ‘solid product’ which separates out from the solution during a chemical reaction.

        The chemical between potassium iodide and lead nitrate is characterized by the formation of a yellow precipitate of lead iodide.

        • Take some lead nitrate solution in test tube.
        • Add potassium iodide solution to it.
        • A yellow precipitate of lead iodide is formed at once.
        • A change in colour also takes place in this chemical reaction.

        Experiment 3 –

        Evolution of a Gas:

        Some chemical reactions are characterized by the evolution of a gas.

        The chemical reaction between zinc and dilute sulphuric acid is characterized by the evolution of hydrogen gas.

        • Take some zinc granules in a conical flask.
        • Add dilute sulphuric acid over zinc granules.
        • We will see the bubbles of hydrogen gas being formed around zinc granules.
        • If we touch the conical flask with our hand, we will find that it is somewhat hot. So, a change in temperature also occurs in this chemical reaction.

        Experiment 4 –

        Change in colour :

        Some chemical reactions are characterized by a change in colour.

        The chemical reaction between citric acid and purple coloured potassium permanganate solution is characterized by a change in colour from purple to colourless.

        • Take some dilute potassium permanganate solution in a test tube. It has purple colour.
        • Add some lemon juice (it contains citric acid) to it with the help of a dropper and shake the test tube.
        • The purple colour of potassium permanganate solution goes on fading and ultimately it becomes colourless.

        Experiment 5 –

        Change in temperature:

        Some chemical reactions are characterized by a change in temperature.

        The chemical reaction between quicklime and water to form slaked lime is characterized by a change in temperature.

        • Take a little of quicklime in a hard-glass beaker.
        • Add water to it slowly.
        • Touch the beaker.
        • The beaker feels to be quite hot.

        Experiment 6 –

        Change in state:

        Some chemical reactions are characterized by a change in state.

        • When wax is burned (in the form of wax candle,) then water and carbon dioxide are formed.
        • Now, wax is a liquid whereas carbon dioxide is a gas. This means that during the combustion reaction of wax, the physical state changes from solid to liquid and gas.

         

        Common observations in a chemical reaction –

        1. Change of state of substance.
        2. Change in colour of substance.
        3. Evolution of gas.
        4. Change in temperature.

        Chemical Equation – 

        Reactant: Substances which take part in a chemical reaction are called reactants.

        Product: New substance formed after a chemical reaction is called product.

        Representation of chemical reaction using symbols of substances is called chemical equation.

        Example:

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction1.GIF

        In this equation, A and B are called reactants and C and D are called products. Arrow shows the direction of chemical reaction. Condition, if any, is written generally above the arrow.

        When hydrogen reacts with oxygen, it gives water. This reaction can be represented by following chemical equation.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction2.GIF

        In first equation, words are used and in second, symbols of substances are used to write the chemical equation. For convenience, symbol of substance is used to represent chemical equations.

        Chemical Equation is a way to represent the chemical reaction in concise and informative way.

        Chemical equation can be divided into two types –

        1. Balanced Chemical Equation
        2. Unbalanced Chemical Equation.

        Balanced Chemical Equation – A balanced chemical equation has number of atoms of each element equal on both sides.

        Example:

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction3.GIF

        In this equation, numbers of atoms of zinc, hydrogen and sulphate are equal on both sides, so it is a balanced chemical equation.

        According to Law of Conservation of Mass, mass can neither be created nor destroyed in a chemical reaction. To obey this law, the total mass of elements present in reactants must be equal to the total mass of elements present in products or we can say that initial number of atoms of an element should be equal to final number of atoms.

        Unbalanced Chemical Equation – If the number of atoms of each element in reactants is not equal to the number of atoms of each element present in product, then the chemical equation is called unbalanced chemical equation.

        Example:

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction4.GIF

        In this example number of atoms of elements are not equal on two sides of the reaction. For example, on the left hand side only one iron atom is present, while three iron atoms are present on the right hand side. Therefore, it is an unbalanced chemical equation.

         

        Balancing a chemical equation –

        To balance any chemical equation, we have to follow these steps:

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction5.GIF

        (1) Write the number of atoms of elements present in reactants and in products in a table; as shown here.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction6.GIF

        (2) Attack on the problem.

        In above equation, number of elements of iron and oxygen are not equal on two sides.

        Let’s take oxygen first.

        (3) Attack the side where there is less number of atoms of that particular element.

        In above equation, number of oxygen atom is minimum on LHS.

        (4) Thus to balance the equation, we need to multiply the oxygen by 4 on LHS.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction7.GIF

        (5) Now again check the number of atoms of each element present in reactants and in products.

        You can see that the number of hydrogen atoms becomes 8 on the LHS; which is more than that on the RHS. To balance it, one needs to multiply the hydrogen on the RHS by 4.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction8.GIF

        (6) After that number of oxygen and hydrogen atoms becomes equal on both sides. The number of iron is one on the LHS, while it is three on the RHS. To balance it, multiply the iron on the LHS by 3.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction9.GIF

        (7) Now the number of atoms of each element becomes equal on both sides. Thus, this equation becomes a balanced equation.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction10.GIF

        After balancing, the above equation can be written as follows.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction11.GIF

        Q.1 Balance the given equations.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction12.GIF

        Making Chemical Equation More Informative –

        1.By writing the physical states of substances a chemical equation becomes more informative –

        Gaseous state is represented by symbol ‘g’.

        Liquid state is represented by symbol ‘l’.

        Solid state is written by symbol ‘s’.

        Aqueous solution(substance dissolved in water) is written by symbol ‘aq’.

        2.Exothermic and Endothermic Reaction –

        Reactions which produce energy are called exothermic reaction.

        Reactions which absorb/require energy are called endothermic reaction.

        Respiration is a exothermic reaction as in respiration process energy is released. When quick lime (calcium carbonate) is added to water, it decomposes and releases energy. So it is also an example of exothermic reaction.

        Cooking involves chemical reactions which are endothermic as cooking is possible because of heating. Similarly in process of photosynthesis, sunlight is required so it is also an example of endothermic reaction.

        3.Writing the condition in which reaction takes place –

        The condition is generally written above and/or below the arrow of a chemical equation.

                                                 340 atm.

        CO2(g) + 2H2(g) ————-> CH3OH(l)

        • Catalyst is a chemical substance which is neither a reactant nor a product but the reactions takes place only in its presence or the reaction speeds up in its presence.

                                    300 atm., 300oC

        CO + 2H2 ——————–>CH3OH

                                          ZnO + CrO2

        Thus, by writing the symbols of the physical state of substances and condition under which reaction takes place, a chemical equation can be made more informative.

         

        Example:

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction13.GIF

        Oxidation and Reduction Reactions

        Oxidation: Addition of oxygen or non-metallic element or removal of hydrogen or metallic element from a compound is known as oxidation.

        Elements or compounds in which oxygen or non-metallic element is added or hydrogen or metallic element is removed are called to be oxidized.

        Oxidizing agent: Compounds which can add oxygen or a non-metallic compound or remove hydrogen or metallic element are known as oxidizing agents.

        Reduction: Addition of hydrogen or metallic element or removal of oxygen or non-metallic element from a compound is called reduction. The compound or element which goes under reduction is called to be reduced.

        Reducing agent: Compounds or elements which can cause reduction are called reducing agents.

        In a chemical reaction oxidation and reduction both take place simultaneously and such reactions are also known as REDOX REACTIONS. In the word REDOX, ‘Red’ stands for reduction and ‘Ox’ stands for oxidation.

        Example:

        When iron reacts with air, it forms iron oxide (rust).

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction34.GIF

        In this reaction, oxygen is added to iron, thus, iron is oxidized. Here oxygen is oxidizing agent.

        When cupric oxide reacts with hydrogen, it gives copper and water.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction35.GIF

        In this reaction, oxygen is removed from copper and oxygen is added to hydrogen. So, cupric oxide is reduced to copper and hydrogen is oxidized to water. Cupric oxide is oxidizing agent and hydrogen is reducing agent.

        When sodium hydroxide reacts with hydrochloric acid, it gives sodium chloride and water.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction36.GIF

        In this reaction, sodium hydroxide is reduced to sodium chloride since hydrogen is removed from sodium hydroxide. Hydrochloric acid is oxidized to water, since oxygen is added to hydrogen chloride and non-metallic element chloride is removed. Sodium hydroxide is oxidising agent and hydrochloric acid is reducing agent.

        In this reaction oxidation and reduction both takes place simultaneously, thus it is an example of redox reaction.

        Effects of Oxidation –

        1. Respiration is oxidation reaction in which food is oxidized to produce energy.

        2. Iron gets oxidized to form rust; which leads to corrosion of iron in the long run.

        3. Most of the metals react with atmospheric oxygen and it leads to formation of a layer on the metal article. The metal gets corroded in the long run.

        4. Rusting of iron can be prevented by painting the iron article. This can also be prevented by applying a layer of zinc over iron article. This process is known as galvanization.

        5. Fried food gets oxidized when exposed to air. This spoils the taste of the food and the food becomes unfit for consumption. The spoiling of fried food because of oxidation is called rancidity. Fried food is often packed in airtight packets to prevent rancidity.

        6. We are able to utilize various types of fuel because of oxidation. Oxidation of fuel helps in producing energy.

        Types of Chemical Reaction –

        Chemical reactions can be classified in following types:-

        a. Combination Reactions

        b. Decomposition Reactions

        c. Displacement Reactions

        d. Double Displacement Reactions

        a. Combination Reaction – Reactions in which two or more reactants combine to form one product are called combination reactions.

        A general combination reaction can be represented by the chemical equation given here.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction14.GIF

        Example:

        When magnesium is burnt in air (oxygen), magnesium oxide is formed. In this reaction, magnesium is combined with oxygen.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction15.GIF

        When carbon is burnt in oxygen (air), carbon dioxide is formed. In this reaction, carbon is combined with oxygen.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction16.GIF

        When hydrogen reacts with chlorine, hydrogen chloride is formed.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction17.GIF

        When calcium oxide reacts with water, calcium hydroxide is formed

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction18.GIF

        When carbon monoxide reacts with oxygen, carbon dioxide is formed.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction19.GIF

        b. Decomposition Reaction – Reactions in which one compound decomposes in two or more compounds or element are known as decomposition reaction. Decomposition reaction is just opposite of combination reaction.

        A general decomposition reaction can be represented as follows:

         

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction20.GIF

        Example:

        When calcium carbonate is heated, it decomposes into calcium oxide and carbon dioxide

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction21.GIF

        When ferric hydroxide is heated, it decomposes into ferric oxide and water.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction22.GIF

        Thermal Decomposition:

        When lead nitrate is heated, it decomposes into lead oxide, nitrogen dioxide and oxygen.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction23.GIF

        In the above examples, compound is decomposed because of heating, so, these reactions are called thermal decomposition.

        Electrolytic Decomposition:

        Reactions in which compounds decompose into simpler compounds because of passing of electricity, are known as electrolytic decomposition. This is also known as electrolysis.

        Example:

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction24.GIF

        When electricity is passed in water, it decomposes into hydrogen and oxygen.

        Photolysis or Photo Decomposition:

        Reactions in which a compound decomposes because of sunlight are known as photolysis or photo decomposition.

        Example:

        When silver chloride is put in sunlight, it decomposes into silver metal and chlorine gas.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction25.GIF

        Similarly, when silver bromide is put under sunlight, it decomposes into silver metal and bromine gas.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction26.GIF

        Photographic paper has coat of silver chloride, which turns into grey when exposed to sunlight. It happens because silver chloride is colourless while silver is a grey metal.

        c. Displacement Reaction – Reactions in which atoms or ions move from one compound to other to form new compound are known as displacement reaction. Displacement reaction is also known as Substitution Reaction or Single displacement /Replacement Reaction.

        A general displacement reaction can be represented using chemical equation as follows:

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction27.GIF

        Displacement reaction takes place only when ‘A’ is more reactive than B. If ‘B’ is more reactive than ‘A’, then ‘A’ will not displace ‘C’ from ‘BC’ and reaction will not be taken place.

        Example:

        When zinc reacts with hydrochloric acid, it gives hydrogen gas and zinc chloride.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction28.GIF

        When zinc reacts with copper sulphate, it forms zinc sulphate and copper metal.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction29.GIF

        When silver metal is dipped in copper nitrate, no reaction takes place because silver metal is less reactive than copper.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction30.GIF

        d. Double Displacement Reaction – Reactions in which ions are exchanged between two reactants forming new compounds are called double displacement reactions.

        A general double displacement reaction can be represented using the following general chemical equation.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction31.GIF

        Example:

        When the solution of barium chloride reacts with the solution of sodium sulphate, white precipitate of barium sulphate is formed along with sodium chloride.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction32.GIF

        When sodium hydroxide (a base) reacts with hydrochloric acid, sodium chloride and water are formed.

        http://www.excellup.com/classten/scienceten/ChemicalReaction_image/10_sc_1_ChemicalReaction33.GIF

        Double displacement reaction, in which precipitate is formed, is also known as a precipitation reaction. Neutralisation reactions are also examples of double displacement reaction.

        Prev Some Important Experiments
        Next NCERT Solutions – Chemical Reactions

          7 Comments

        1. Mohit lunawat
          October 2, 2021
          Reply

          Very helpful notes
          Now properly prepared for term 1 exam
          Keep it up
          Please provide me mcqs for more practicing
          And mind maps also

        2. Raj pratap
          October 11, 2021
          Reply

          Please make McQ question papers for preparation term 1 exam .

        3. Abbas Khan
          October 20, 2021
          Reply

          Very helpful Notes ….Thanks From Pakistan..

        4. Sananse akshada
          October 30, 2021
          Reply

          Thank you dron study ….
          After all these practices now I am Full of confidence that I will definitely score 92% + Marks …
          From Maharashtra 🚩…!!

        5. Saloni
          November 11, 2021
          Reply

          Sir please upload MCQs pattern

        6. Sumit Babu
          November 30, 2021
          Reply

          Very helpful

        7. Rajnikant
          October 1, 2022
          Reply

          Thanks I heartily thank Nitin sir. That my half yearly examination got 94/100 marks in science

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