Chemistry Class 9 ICSE CISCE Topics and Syllabus

• Concept for Language of Chemistry 
• Valency and Its Types 
• Radicals and Its Types 
• Writing Chemical Formulae 
• Naming Certain Compounds 
  1. A metal  and a non-Metal
  2. Two non-metal
  3. Two elements and oxygen
  4. Naming of acid
  5. Trivial names
• Chemical Equation 
• Mass Number (A) or Atomic Mass 
• Molecular Mass 
• Percentage Composition 
• Empirical Formula of a Compound 
• Symbols of Elements 
• Concept of Hydrogen 
  • Discovery
  • occurrence
• Balancing Simple Equations 

Symbol of an element; valency; formulae of radicals and formulae of compounds. Balancing of simple chemical equations.

Symbol - definition; symbols of the elements used often.

Valency - definition; hydrogen combination and number of valence electrons of the metals and non-metals; mono, di, tri and tetra valent elements.

Radicals – definition of radicals; formula and valencies of the radicals and formula of compounds.

Chemical equation – definition and examples of chemical equations with one reactant and two or three products, two reactants and one product, two reactants and two products and two reactants and three or four products; balancing of equations. (By partial equation method and hit and trial method)

• Collision Theory 
  • Condition for a Chemical change 

    Close contact, particles should collide, heat, light, electricity, pressure, catalysts with examples

• Types of Chemical Change or Chemical Reaction 
• Energy Changes in a Chemical Change 

  Exothermic and endothermic reactions with examples - evolution/absorption of heat, light and electricity.

• Burning - Definition and Conditions of Burning 

  combustible substance, supporter of combustion and ignition temperature

• Comparison of Respiration and Burning 
• Burning of Magnesium Or Candle to Show that Substances Gain Weight on Burning 
• Classification of Change: Chemical Changes 

(i) Definitions and distinction between Physical and Chemical changes.

Simple experiments like dissolution of sugar in water, burning of paper should be shown to make the concepts of physical and chemical change clear. More examples of such type may be given.

(ii) Conditions for chemical change.

Close contact, heat, light, electricity, pressure, catalysts with examples.

(iii) Types of chemical change.

Direct combination; decomposition; displacement; double decomposition with examples.

(iv) Energy changes in a chemical change.

Exothermic and endothermic reactions with examples - evolution/absorption of heat, light and electricity.

(v) Burning:- Definition and conditions of burning.

Definition; (Air is used for combustion) conditions for burning (combustible substance, supporter of combustion and ignition temperature); comparison of respiration and burning; burning of magnesium or candle to show that substances gain weight on burning; students to be made aware of how the balance of O₂ and CO₂ is maintained in nature. O₂ and CO₂ Cycle.

• Water, Our Lifeline 
• Chemical Properties of Water 
• Concept of Universal Solvent 
• Solutions as 'Mixtures' of Solids in Water 
• Saturated Solutions 
• Concentration of a Solution 
• Solubility 
• Crystals and Crystallisation 
• Hydrated and Anhydrous Substances, Hygroscopic 
• Properties 
  • Efflorescence
  • Deliquescence
• Drying and Dehydrous Substances 
• Removal of Hardness of Water 
• Soft and Hard Water 
• Water as a Compound and as a Universal Solvent 
• Qualitative Effect of Temperature on Solubility 

  e.g. solutions of calcium sulphate, potassium nitrate, sodium chloride in water

• Introduction of Water Pollution and Its Control 
• Dissolution of Salts in Water 
  • meaning and explanation
• Salts 
• Components of Solutions 
• Water 
  • Hard and Soft Water 

Water as a compound and as a universal solvent; its physical and chemical properties.

Why water is considered a compound? Chief physical properties should include: density, b.p, m.p. Experiment to show that the water we drink, contains dissolved solids and dissolved gases (air); their significance. Solutions as 'mixtures' of solids in water; saturated solutions; qualitative effect of temperature on solubility (e.g. solutions of calcium sulphate, potassium nitrate, sodium chloride in water).

Water Pollution – Causes – household, detergents, sewage, industrial waste, offshore and oil drilling.

Treatment of Water Pollution – Proper collection and disposal of domestic sewage, treatment of industrial waste to yield safe effluents.

Chemical Properties: The action of cold water on sodium and calcium; the action of hot water on magnesium and steam on iron; reversibility of reaction between iron and steam.

Students can be shown the action of sodium and calcium on water in the laboratory; they must be asked to make observations (equations for the above reactions) and form reactivity series based on reactions.

• Chemical Bond 
• Sub-atomic Particles of Atom 
  • Electrons (e) 
  • Protons (p) 
  • Nucleus 
  • Neutrons (n) 
• Neil Bohr’s Model of Atom 
• Atom 
• Atomic Number (Z) 
• Bohr-bury Scheme 
  • Distribution of electrons in the orbits
• Valency Electrons 
• Reason for Chemical Activity of an Atom 
• Isotopes 
• Electrovalent (Or Ionic) Bond 
• Covalent (Molecular) Bond 
• Mass Number (A) or Atomic Mass 
• Electrons Distributed in Different Orbits (Shells) 
• Characteristic Properties of Electrovalent Compounds 
  •  state of existence
  • melting and boiling points
  • conductivity (heat and electricity)
  • ionisation in solution
  • Dissociation in solution and in molten state to be linked with electrolysis

Structure of an Atom mass number and atomic number, Isotopes and Octet Rule.

Definition of an element, definition of an atom; constituents of an atom - nucleus (protons, neutrons) with associated electrons; mass number, atomic number. Electron distribution in the orbits - 2n² rule, Octet rule. Reason for chemical activity of an atom. Definition and examples of isotopes (hydrogen, carbon, chlorine).

• Dobereiner’s Triads 
• Newland's Law of Octaves 
• Mendeleev’s Periodic Table 
• Modern Periodic Law 
• The Modern Periodic Table 
• Types of Element: Metals 
• Advantage and Disadvantage of Modern Periodic Table 
• Study of Specific Groups in Periodic Table 
• Uses of Periodic Table 
• Periodic Properties 

Dobereiner’s Triads, Newland’s law of Octaves, Mendeleev’s contributions; Modern Periodic Law, the Modern Periodic Table. (groups and periods)

General idea of Dobereiner’s triads, Newland’s law of Octaves, Mendeleev’s periodic law, Discovery of Atomic Number and its use as a basis for Modern Periodic law, Modern Periodic Table (groups 1 to 18 and periods 1 to 7).

• Position of the Non-metal (Hydrogen) in the Periodic Table 
• Hydrogen from Alkalies 
• Similarities Between Hydrogen and Halogens 
• Concept of Hydrogen 
  • Discovery
  • occurrence
• Preparation of Hydrogen 
• Application of Activity Series in the Preparation of Hydrogen 
  • Displacement of hydrogen from dilute acids
  • Displacement of hydrogen from alkalis
• Laboratory Preparation of Hydrogen 
• Manufacture of Hydrogen 
  • Bosch process
  • By electrolysis of water
• Properties and Uses of Hydrogen 
• Hydrogen - Oxidation and Reduction 
• Hydrogen from Water 
• Hydrogen from Dilute Acids 
• Preparation of Hydrogen, from Water – Electrolysis 

  (Introduction to terms electrode, electrolyte, electrolysis – detailed process not required).

• Preference of Zinc as the Metal to Be Used (With Reasons). 

Position of the non-metal (Hydrogen) in the periodic table and general group characteristics with reference to valency electrons, burning, ion formation applied to the above mentioned element.

(i) Hydrogen from water (ii) hydrogen from dilute acids (iii) hydrogen from alkalies.

Hydrogen from water. Cold water and metals; hot water and metals; steam and metals; steam and non-metals. Application of activity series for the above mentioned preparations. Displacement of hydrogen from dilute sulphuric acid or hydrochloric acid by zinc or iron (no reaction with copper). Displacement of hydrogen from alkalis (NaOH, KOH) by Zn, Al – unique nature of these elements.

(ii)The preparation and collection of hydrogen by a standard laboratory method other than electrolysis.

In the laboratory preparation, the reason for using zinc, the impurities in the gas, their removal and the precautions in the collection of the gas must be mentioned.

Industrial manufacture of hydrogen by Bosch process with main reactions and conditions; separation of CO₂ and CO from it.

• Study of Gas Laws 
• Gases and Its Characteristics 
• Molecular Motion : Relationship of Temperature, Pressure and Volume 
• The Gas Laws 
• Fundamental Laws of Gases 
  • Pressure and Volume Relationship or Bolye's Law 
  • Temperature - Volume Relationship or Charles's Law 
• Absolute Zero 
• Temperature 
• Scales of Thermometers 
• Gas Equation 
• Standard Temperature and Pressure 
• The Effect of Moisture and Pressure 
• Derivation of Boyle’s Law 

  statement, mathematical form, simple calculations

• Relative Molecular Mass of Non-volatile Substances 
  • Van’t Hoff- Charles’ Law 

    statement, mathematical form, simple calculations

• Molar Volume of a Gas at S.T.P 
  • Understanding molar volume- “the mass of 22.4 litres of any gas at S.T.P. is equal to its molar mass”. 
• Mole Concept 

(i) The behaviour of gases under changes of temperature and pressure; explanation in terms of molecular motion (particles, atoms, molecules); Boyle’s Law and Charles’ Law; absolute zero; gas equation; simple relevant calculations.

The behaviour of gases under changes of temperature and pressure; explanation in terms of molecular motion (particles, atoms, molecules). Boyle’s Law (statement, mathematical form, simple calculations).

Charles’ Law; (statement, mathematical form, simple calculations). Absolute zero; Kelvin scale of temperature. Gas equation P₁ V₁ / T₁ = P₂ V₂ / T₂; simple relevant calculations based on gas equation.

(ii) Relationship between Kelvin Scale and Celsius Scale of temperature; Standard temperature and pressure.

Conversion of temperature from Celsius Scale to Kelvin scale and vice versa. Standard temperature and pressure. (simple calculations).

• Atmospheric Pollution 
• Air Pollution and Its Causes 
• Acid Rain - Composition, Cause and Its Impact 
• Meaning of Global Warming 
• Effect of Global Warming 
• Ozone Layer Depletion 
• Sources of Greenhouse Gases and Ways of Reducing Their Presence in the Atmosphere 

(a) Acid rain – composition, cause and its impact.

Sulphur in fossil fuels giving oxides of sulphur when burnt. High temperatures in furnaces and internal combustion engines produce oxides of nitrogen. (Equations to be included). Acid rain affects soil chemistry and water bodies.

(b) Global warming:-

Greenhouse gases – their sources and ways of reducing their presence in the atmosphere.

(water vapour, carbon dioxide, methane and oxides of nitrogen)

(c) Ozone depletion

Formation of ozone – relevant equations

Function in the atmosphere.

Destruction of the ozone layer – chemicals responsible for this to be named but reactions not required.

• Differences Between Elements, Compounds, and Mixtures 
• Types of Mixtures: Homogeneous and Heterogeneous Mixture 
• Mixture 
• Separation of Mixtures 
• Use of Solvent and Filtration 

  e.g. sodium chloride + sand, (water as solvent), carbon and sulphur (Carbon tetra chloride as solvent

• Change of State of Matter 
  • Concept of Evaporation 
• Methods of Separation 
  • Distillation Method 
  • Distillation Method 
  • Chromatography Method 
  • Centrifugation Method 
  • Solvent Extraction (Using a Separating Funnel Method) 

(i) General characteristics and differences between elements, compounds and mixtures.

Reasons for considering a substance as an element, compound or mixture may be given to make the concepts clear.

(ii) Types of mixtures: of two solids, a solid and a liquid, two liquids, liquid and gas, two gases.

Definition of mixture; each type of mixture should be shown to the students (including both homogeneous and heterogeneous types) – true solution, suspension and colloidal solution to make the concepts clear.

(iii) Separation of mixtures involving - use of a solvent, filtration, evaporation and distillation, fractional distillation, simple paper chromatography Centrifugation immiscible liquid.

The following examples should be used to illustrate the principles of separation of mixtures by using following methods

(a) use of solvent and filtration (e.g. sodium chloride + sand, (water as solvent), carbon and sulphur (Carbon tetra chloride as solvent)

(b) evaporation e.g. sodium chloride from its aqueous solution

(c) distillation e.g. purification of water containing dissolved solids.

(d) fractional distillation involves the difference in boiling points of liquids e.g. benzene + toluene.

(e) simple paper chromatography (limited to separation of colouring matter in ink);

(f) Centrifugation (involving separation of cream from milk).

(g) immiscible liquids (separating funnel e.g water + carbon tetra chloride).

• Change of State of Matter 
• Inter-particle Space and Interparticle Attraction and Collision 
• Laws of Chemical Combination 
  • Law of Conservation of Mass 

(i) Explanation of change of state of matter on the basis of Kinetic Theory of Matter.

Main postulates of Kinetic Theory of Matter and explanation of change of state on the basis of. Inter-particle space and Interparticle attraction and collision.

(ii) Law of Conservation of Mass:- Statement and explanation with examples.