Chemistry Class 9 Syllabus ICSE

The Chemistry Class 9  syllabus ICSE  has been designed by academic experts so that students can learn precise details about the topics. The Indian Certificate of Secondary Education is known by the acronym ICSE.

1. The Language of Chemistry Class 9 Syllabus ICSE

(i) The symbol for an element, its valency, radical formulas, and compound formulas, simple chemical equations in balance.

• Definition of a symbol; examples of symbols recurring elements

• Hydrogen definition; valency combinations and valence numbers mono, di, tri, and tetravalent metal and nonmetal electrons Elements.

• Formulas and definitions for Radicals valencies.

• Names and formulas for compounds.Chemical formula definition and examples

chemical equation examples with two or three reactants and one reactant two reactants, three products, and one two reactants, one product, two reactants, two products, and three

or four items; balance

equations (by hit and trial method).

(ii)Relative Atomic Masses (atomic weights) as well as Relative Molecular Masses either conventional H or (molecular weights) or one-twelfth of a carbon-12 atom.

  • Definitions
  • Calculating a compound’s relative molecular mass and percentage composition is one of the.

2. alterations and reactions in chemistry

  • DirectCombination 
  • Decomposition 
  • displacement  
  • double decomposition is among the processes that will be taught, with appropriate chemical equations serving as examples.

(ii) When a chemical change occurs, energy shifts.

Examples of exothermic and endothermic reactions include heat, light, and electricity evolution and absorption.

3. Water

(i) The versatility of water as a solvent

  • Saturated solutions are defined as “mixtures” of solids in water.
  • The effect of temperature on solubility’s characteristics (e.g. solutions of calcium sulphate, potassium nitrate, and sodium chloride in water).

(ii) Hydrated and non-hydrated materials.

(a) Hydrated substances: Definition and instances of Water of Crystallization.

(a) Anhydrous substances: Only definitions and illustrations

(c) Qualities:

  • The efflorescence
  • Deliquescence  
  • Deliquescence

(iii) Agents for drying and dehydrating

Just meaning and examples.

4. Chemical bonding and atomic structure

(i)Atomic structure, mass, atomic number, isotopes, and the octet rule.

An atom is defined as having a nucleus (protons, neutrons) and associated electrons, as well as a mass number and an atomic number.

• The 2n2 rule and Octet rule apply to the electron distribution in orbits. the cause of an atom’s chemical activity.

• Isotope definition and examples (hydrogen, carbon, chlorine).

(ii) Structures of different compounds, orbit structure, and electrovalent and covalent bonding

Atomic orbit structure for the formation of covalent molecules on the basis of duplet and octet of electrons, such as hydrogen, chlorine, oxygen, nitrogen, hydrogen chloride, water, ammonia, carbon tetrachloride, and methane. (a) Electrovalent Bond

• Definition

• Atomic orbit structure for the formation of electrovalent compounds (e.g., NaCl, MgCl2, CaO).

5. The Periodic Table-

Mendeleev’s contributions, Dobereiner’s Triads, Newland’s law of octaves, and modern periodic law and the modern periodic table.

Periods and groups

• A general understanding of Mendeleev’s periodic law, Newland’s law of octaves, and Dobereiner’s triads.

• The atomic number was discovered, and modern periodic law is based on it.

Groups 1 through 18 and periods 1 through 7 of the modern periodic table.

• Specific mention of Group 1 Alkali Metals, Group 2 Alkaline Earth Metals, Group 17 Halogens, and Group 0 (Group 18).

6. Research on Hydrogen, the First Element

Position of the non-metal (Hydrogen) in the periodic table and general group characteristics applicable to the aforementioned element’s valency electrons, burning, and ion production.

(i) Water-derived hydrogen, weak acids, and weak alkalis

(a) The production of hydrogen from water:

• The effects of cold water on calcium, sodium, and potassium.

• How hot water affects magnesium.

• The effects of steam on iron, aluminum, and zinc (iron and steam reactions are reversible).

• Steam’s impact on non-metals (carbon).

In a lab setting, instructors can demonstrate to students how salt and calcium interact with water. For the aforementioned reactions, you must ask them to record their observations and equations.

(c) Hydrogen displacement from alkalis.

The distinctive properties of Al, Zn, and Pb are affected by alkalis ((NaOH, KOH)).

(ii) Using a normal laboratory technique other than electrolysis to prepare and collect hydrogen. The purpose of employing zinc, the contaminants in the gas, their elimination, and the safety measures in the gas collection must all be included in the laboratory preparation.

(iii) The Bosch process for producing hydrogen commercially.

• Primary responses and circumstances.

• Digestion of hydrogen to separate CO2 and CO.

(iv) Reactions of oxidation and reduction.

differences in how oxygen and hydrogen are added to and removed from the mixture.

Source – SpeEdLabs

7. Research into Gas Laws

(i) Boyle’s Law and Charles’ Law; absolute zero; the gas equation; straightforward pertinent calculations; the behavior of gases under changes in temperature and pressure; an explanation in terms of molecular motion (particles, atoms, and molecules);

• The behavior of gases under temperature and pressure variations; molecular motion explanation (particles, atoms, molecules).

• Boyle’s Law: a declarative formula with straightforward calculations.

• Charles’ Law: a declarative formula with straightforward calculations.

• The Kelvin scale of temperature at absolute zero.

• Simple applicable calculations based on the gas equation P1 V1 / T1 = P2 V2 / T2

(ii) The relationship between the Celsius and Kelvin scales of temperature; normal pressure and temperature. temperature measurement conversion from the Celsius scale to the Kelvin scale and vice versa. normalized pressure and temperature. (Easy calculations.


Candidates will be required to watch how reagents and/or heat affect the materials they are given. Simple exercises might involve recognizing and identifying some of the gases listed below.

Gases include nitrogen dioxide, ammonia, water vapour, oxygen, carbon dioxide, chlorine, hydrogen chloride, sulphur dioxide, and hydrogen sulfide.

Candidates must have finished the bare minimal amount of practical work.

simple examinations of

1. The effect of heat on the substances copper carbonate and zinc carbonate, washing soda, copper sulfate crystals, zinc, copper, lead nitrates, ammonium chloride, iodine, and ammonium dichromate.

Make observations, identify the goods, and, if you can draw conclusions.

2. The following compounds are affected by diluted sulfuric acid. (Warm if required)

A metal, a carbonate, a sulfide, a sulfite, or (a) a metal

Make observations, recognize the gas that has developed, and draw conclusions.

3. Use the flame test to determine the metal content of the unidentified substance.

(A) a calcium compound (B) a potassium salt (C) a sodium salt.

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