| ICSE Class 9 Chemistry Syllabus 2025 |
| Chapters |
Topics |
| 1. The Language of Chemistry |
(i) Valency, radical and compound formulas, as well as an element's symbol. Balancing of simple chemical equations.
- Symbol – definition; symbols of the elements used often.
- Valency - definition; hydrogen combination and several valence electrons of the metals and non-metals; mono, di, tri, and tetravalent elements.
- Radicals – definition; formulae and valencies.
- Compounds – name, and formulae.
- A chemical equation's meaning, instances of equations with one substance reacting and forming two or three substances, cases with two substances leading to one product, situations where two substances yield two products, and scenarios with two substances producing three or four products, along with the balancing of equations, are typically explained below, often using the trial-and-error method.
(ii) Relative Atomic Masses (atomic weights) and Relative Molecular Masses (molecular weights): either - standard H atom or 1/12th of carbon 12 atom.
- Definitions
- Calculation of Relative Molecular Mass and percentage composition of a compound.
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| 2. Chemical changes and reactions |
(i) Types of chemical changes.
- Direct combination
- Decomposition
- Displacement;
- Double decomposition
- (The above is to be taught with suitable chemical equations as examples).
(ii) Energy changes in a chemical change.
- Exothermic and endothermic reactions with examples – evolution/absorption of heat, light, and electricity.
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| 3. Water |
(i) Water as a universal solvent.
- Mixtures' of solids in liquids; saturated solutions.
- Qualitative effect of temperature on solubility (e.g. solutions of calcium sulphate, potassium nitrate, and sodium chloride in water).
(ii) Hydrated and anhydrous substances.
- (a) Hydrated substances:
- The water of Crystallisation – meaning and examples.
- (b) Anhydrous substances:
- Meaning and examples only
- (c) Properties:
- Efflorescence
- Deliquescence
- Hygroscopy
- Removal of hardness
- (i) By boiling
- (ii) By the addition of washing soda
- (Definition and examples of each of the above).
- (iii)Drying and Dehydrating Agents Definition and examples only.
- (iv) Soft water and Hard water
- Meaning, (in terms of action of soap)
- hard and soft water's advantages and disadvantages.
- Types and causes of hardness
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| 4. Atomic Structure and Chemical Bonding |
(i) Structure of an Atom, mass number, and atomic number, Isotopes, and Octet Rule.
- Definition of an atom
- The atom consists of an atomic number, mass, and a nucleus composed of protons and neutrons, along with electrons.
- Electron distribution in the orbits - 2n2 rule, Octet rule. what causes an atom to be chemically active.
- An explanation of isotopes, including hydrogen, carbon, and chlorine examples.
(ii) Structures of different compounds, orbit structure, and electrovalent and covalent bonding
- (a) Electrovalent Bond
- Definition
- Atomic orbit structure for the production of electrovalent compounds (e.g. NaCl, MgCl2, CaO);
- (b) Covalent Bond
- Definition
- Atomic orbitals play a role in creating covalent molecules, following the duplet and octet rules for electrons. Examples include hydrogen, chlorine, oxygen, nitrogen, hydrogen chloride, water, ammonia, carbon tetrachloride, and methane.
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| 5. The Periodic Table |
- Mendeleev made important contributions, Dobereiner introduced Triads, Newland proposed the law of octaves, and the modern periodic law and table are significant.
- There is a wide understanding of Dobereiner's triads, Newland's law of octaves, and Mendeleev's periodic law. The discovery of the atomic number led to the establishment of the modern periodic law.
- The modern periodic table consists of groups 1 to 18 and periods 1 to 7. It is important to focus on specific groups like Group 1 (Alkali Metals), Group 2 (Alkaline Earth Metals), Group 17 (Halogens), and Group 18 (Zero Group).
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| 6. Study of the First Element-Hydrogen |
- The place of the non-metal (Hydrogen) on the periodic table and the overall group traits related to valence electrons, burning, and ion creation relate to the element mentioned above.
(i) Hydrogen is produced by water, weak acids, and alkalis.
- (a) Hydrogen from water:
- How calcium, sodium, and potassium behave in cold water.
- What happens when hot water interacts with magnesium.
- How aluminium, zinc, and iron react to steam; (how iron and steam can react in both directions).
- How steam affects non-metals, like carbon.
- In the lab, students can observe how sodium and calcium react with water. They need to write down their observations and create equations for these reactions. The activity series is employed for the mentioned reactions.
- (b) Displacement of hydrogen from dilute acids.
- Sulfuric acid or hydrochloric acid in a weakened form reacts with the metals Mg, Al, Zn, and Fe. (To comprehend the reasons for not utilising different metals and diluting nitric acid.)
- (c) Displacement of hydrogen from alkalis.
- The effect of alkalis like NaOH and KOH on aluminium (Al), zinc (Zn), and lead (Pb) - the unique nature of these elements.
- (ii) Using a regular lab method, not electrolysis, to make and gather hydrogen is essential.
- The lab preparation should cover why zinc is used, how the gas pollutants are removed, and the safety steps taken during gas collection.
(iii) Industrial manufacture of hydrogen by Bosch process.
- Main reactions and conditions.
- Hydrogen is generally separated from CO2 and CO.
- (iv) Oxidation and reduction reactions.
- differences in how oxygen/hydrogen is added to and removed.
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| 7. Study of Gas Laws |
(i) How gases act when temperature and pressure change; described by how tiny particles move (particles, atoms, molecules). Boyle's Law and Charles' Law are included, along with absolute zero, gas equation, and straightforward calculations.
- How gases behave with shifts in temperature and pressure; explained by the motion of tiny particles (particles, atoms, molecules).
- Boyle's Law is presented with an uncomplicated formula for easy calculations.
- Charles' Law: a statement, a mathematical form, and some basic computations.
- Absolute zero Kelvin scale of temperature.
- Gas equation P1 V1 / T1 = P2 V2 / T2; simple relevant calculations based on a gas equation.
(ii) Relationship between Kelvin scale and Celsius Scale of temperature; Standard temperature and pressure.
- temperature measurement conversion from the Celsius scale to the Kelvin scale and vice versa. Standard temperature and pressure. (Simple calculations).
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| 8. Atmospheric pollution |
- (a) The composition, origin, and effects of acid rain.
- When fossil fuels burn, sulphur in them creates sulphur oxides. Oxides of nitrogen form at high temperatures in furnaces and internal combustion engines. This leads to acid rain, impacting the chemistry of soil and water bodies. (Equations will be included).
- (b) Global warming:
- Greenhouse gases - where they come from and methods to decrease their amount in the air. (Water vapour, carbon dioxide, methane, and nitrogen oxides)
- (c) Ozone depletion
- Formation of ozone – relevant equations
- Function in the atmosphere.
- The ozone layer's harm – we need to identify the chemicals causing it, but we don't need to explain the reactions.
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