Academic year:
Units and Topics
| # | Unit/Topic | Marks |
|---|---|---|
| 1 | Matter | - |
| 2 | Physical and Chemical Changes | - |
| 3 | Elements, Compounds and Mixtures | - |
| 4 | Atomic Structure | - |
| 5 | Language of Chemistry | - |
| 6 | Chemical Reactions | - |
| 7 | Hydrogen | - |
| 8 | Water | - |
| 9 | Carbon and Its Compounds | - |
| Total | - |
Syllabus
1 Matter
- Main Postulates of Kinetic Molecular Theory of Matter
- Change of State of the Matter on the Basis of Inter Particle Space and Inter Particle Attraction and Collision
- Law of Conservation of Mass Statement and Explanation with Examples)
- Matter
- Interconversion of States of Matter
- Nature of matter
- Main postulates of the kinetic molecular theory of matter.
- Explanation of change of state of the matter on the basis of interparticle space and interparticle attraction and collision.
- Law of conservation of mass. (statement and explanation with examples)
- Interconversion of states of matter.
2 Physical and Chemical Changes
- Concept of Physical Changes
- Meaning of Physical Changes
- Characteristics of Physical Changes
- Examples of Physical Changes
- Physical and Chemical changes
3 Elements, Compounds and Mixtures
- Concept of Elements, Compounds and Mixture
- Separation of the Components of a Mixture
- Emphasis on the Principle of Separation
- Revision of Matter taught in earlier classes.
- Elements, compounds and mixture – a brief explanation.
- Separation of the components of a mixture.
- Emphasis on the principle of separation.
4 Atomic Structure
- Concept of Atom
- Fundamental Subatomic Particles Present in an Atom: Electrons, Protons, Neutrons
- Nucleus and Extra Nuclear Parts
- Concept of Atomic Number
- The Combining Capacity of Elements
- Fundamental subatomic particles present in an atom: electrons, protons, neutrons.
- Nucleus and extra nuclear parts.
- Atomic number and mass number.
- The combining capacity of elements
5 Language of Chemistry
- Concept for Language of Chemistry
- Symbols of Elements
- Formulae of Compounds
- Language of Chemistry - Law of Conservation of Mass
- Balancing Simple Equations
- Relate the Law to the Balancing of Simple Equations
- Information Gathered from a Chemical Equation
- Limitations of a Chemical Equation:Catalyst, Conditions
- Symbols of elements.
- Formulae of compounds.
- Chemical equations (from word equations).
- Law of conservation of mass.
- Balancing simple equations
- Relate the law to the balancing of simple equations.
- Information gathered from a chemical equation.
- Limitations of a chemical equation: Catalyst, conditions for the reaction, state of the reactants and products, nature of the chemical reaction are not gathered from the equation.
6 Chemical Reactions
- Concept of Chemical Reactions
- Chemical Reaction
- Characteristics of Chemical Reaction
- Types of Chemical Reactions
- Combination Reaction
- Combination Reaction
- Experiment: Formation of slaked lime by the reaction of calcium oxide with water
- Decomposition Reactions
- Decomposition Reactions
- Experiment: Correct way of heating the boiling tube containing crystals of ferrous sulphate and of smelling the odour.
-
Experiment: Heating of lead nitrate and emission of nitrogen dioxide (Thermal decomposition reaction).
-
Experiment: Electrolysis of water.
-
Experiment: Silver chloride turns grey in sunlight to form silver metal.
- Displacement Reaction
- Displacement Reaction
- Experiment: Reaction of iron nails with copper sulphate solution.
- Double Displacement Reaction
- Double Displacement Reaction
- Precipitation reaction
-
Experiment: Formation of barium sulphate and sodium chloride.
- Combination Reaction
- Reactivity Series - in Reactivity Series Metals Are Arranged in Order of Their Reactivity
- Reactivity Series - Metal that Displaces the Metal Ion from the Solution is More Reactive.
- Predict the Reactivity of Metals
- Endothermic and Exothermic Processes/ Reactions
- Neutralization Reaction
- Decomposition Reactions to Form Oxides
- Classification of Oxides - Metal Oxides Are Basic
- Classification of Oxides - Nonmetal Oxides Are Acidic in Nature
- Classification of Oxides - Basic Oxides React with Acids
- Amphoteric Oxides - Some Oxides Such as Zno, Pbo React Both with Acids and Bases
- Types of reactions:
- Combination
- Decomposition
- Displacement
- Double displacement.
- Reactivity series:
- In reactivity, series metals are arranged in order of their reactivity.
- The metal that displaces the metal ion from the solution is more reactive.
- Predict the reactivity of metals.
- Endothermic and exothermic processes/reactions.
- Neutralization reaction.
- Decomposition reactions to form Oxides.
- Classification of oxides:
- Metal oxides are basic; nonmetal oxides are acidic in nature.
- Acidic oxides react with base and basic oxides react with acids. some oxides such as ZnO, PbO react both with acids and bases. These are amphoteric oxides.
7 Hydrogen
- Preparation of Hydrogen, from Water – Electrolysis
(Introduction to terms electrode, electrolyte, electrolysis – detailed process not required).
- Preparation of Hydrogen in the Laboratory
- Preference of Zinc as the Metal to Be Used (With Reasons).
- Choice of Dilute Acids (Other than Dil. Nitric Acid)
- Concept of Bosch’S Process
- Properties and Uses of Hydrogen
- Hydrogen - Oxidation and Reduction
- Concept of Hydrogen
- Discovery
- occurrence
- Preparation of hydrogen, from water – electrolysis (Introduction to terms electrode, electrolyte, electrolysis – detailed process not required).
- Preparation of hydrogen in the laboratory.
- Preference of zinc as the metal to be used ( with reasons).
- Choice of dilute acids (other than dil. nitric acid).
- Bosch’s process.
- Properties and uses of hydrogen.
- Oxidation and Reduction.
8 Water
- Concept for Water
- Dissolution of Salts in Water
- meaning and explanation
- Concept of Universal Solvent
- Concept of Suspension
- Suspension
- Properties of a Suspension
- Tyndall effect
- Differentiate Unsaturated/Saturated and Supersaturated Solutions
- Water of Crystallisation
- Hydrated and Anhydrous Substances, Hygroscopic
- Reactivity of Metals with Cold Water, Hot Water and Steam (With Products Formed).
- Hard and Soft Water and Methods of Softening of Hard Water
- Removing hardness of water by boiling or by treating with washing soda
- Dissolution of salts in water – meaning and explanation.
- Universal solvent – meaning.
- Solutions, suspensions, colloids.
- Differentiate unsaturated/saturated and supersaturated solutions.
- Suspensions and colloids.
- Water of crystallisation.
- Hydrated and Anhydrous substances, hygroscopic.
- Reactivity of metals with cold water, hot water and steam ( with products formed).
- Hard and soft water and methods of softening of hard water.
- Disadvantage of using hard water.
- Removing hardness of water by boiling or by treating with washing soda
9 Carbon and Its Compounds
- Concept of Carbon
- Allotropes of Carbon
- Uses of Diamond, Graphite, Coke, Coal, Soot
- Laboratory Preparation, Properties and Uses of Carbon Dioxide
- Physical Properties of Carbon Dioxide
- Chemical Properties of Carbon Dioxide
- Reaction with Lime Water
- Properties and Uses of Carbon Monoxide
- Emphasis on Use as Reducing Agent in the Extraction of Iron
- Emphasize the Harmful Properties of Carbon Monoxide When Inhaled - Asphyxia
- Allotropes of Carbon – definition and explanation.
- Crystalline and amorphous nature of allotropes of carbon.
- Uses of diamond, graphite, coke, coal, soot.
- Laboratory preparation, properties and uses of carbon dioxide
- Physical properties of Carbon dioxide.
- Chemical properties of Carbon Dioxide.
- Acidic nature.
- Reaction with lime water.
- Properties and uses of Carbon monoxide.
- Emphasis on use as reducing agent in the extraction of iron.
- Emphasize the harmful properties of Carbon monoxide when inhaled – Asphyxia.
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