ICSE EXAM LATEST UPDATE
The Class 9 exams depend on the schools, as they decide when to conduct the exams. Usually, the Class 9 exams are held a few months before the final board exams. This gives you the opportunity to prepare for the final board exams and also mentally prepare for them. Therefore, it is better to contact your school regarding the Class 9 exams, and also take advantage of the complete information provided here for the final board exam.
The Council for the Indian School Certificate Examinations (CISCE) has officially released the date sheet for ICSE (Class 10) board examinations for 2025. This year class 10th board exam will be started from 18 February 2025 and will last upto 27 March 2025, it will take around 38 days to complete the class 10th board exam. The first exam will be held on 18 February 2025 for English subject and the last exam will be held on 27 March 2025 for Environmental Science subject. The Indian School Certificate Examination results will be declared in the month of May.
Official Syllabus
The syllabus will consist of one paper of two hours duration.
Theory - 80 Marks
Practical - 20 Marks
The theory paper will be divided into two sections-
Section I - Section I will consist of short answer-type questions on the entire syllabus. (40 marks)
Section II - Section II will have six questions. Candidates will have to answer any four of these six questions. (40 marks)
Note: All chemical processes/reactions should be studied in terms of reactants, products, conditions, observations and (balanced) equations.
1. The Language of Chemistry
(i) 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 the number of valence electrons of the metals and non-metals; mono, di, tri and tetra valent elements.
• Radicals – definition; formulae and valencies.
• Compounds – name and formulae.
• 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 hit and trial 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.
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.
3. Water
(i) Water as a universal solvent
• Solutions as 'mixtures' of solids in water; 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
(Definition and examples of each of the above).
(iii) Drying and Dehydrating Agents
Meaning and examples only.
4. Atomic Structure and Chemical bonding
(i) Structure of an Atom, mass number and atomic number, Isotopes and Octet Rule.
• 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 the chemical activity of an atom.
• Definition and examples of isotopes (hydrogen, carbon, chlorine).
(ii) Electrovalent and covalent bonding, structures of various compounds – orbit structure
(a) Electrovalent Bond
• Definition
• Atomic orbit structure for the formation of Electrovalent compounds (e.g. NaCl, MgCl2, CaO);
(b) Covalent Bond
...
ICSE EXAM LATEST UPDATE
The Class 9 exams depend on the schools, as they decide when to conduct the exams. Usually, the Class 9 exams are held a few months before the final board exams. This gives you the opportunity to prepare for the final board exams and also mentally prepare for them. Therefore, it is better to contact your school regarding the Class 9 exams, and also take advantage of the complete information provided here for the final board exam.
The Council for the Indian School Certificate Examinations (CISCE) has officially released the date sheet for ICSE (Class 10) board examinations for 2025. This year class 10th board exam will be started from 18 February 2025 and will last upto 27 March 2025, it will take around 38 days to complete the class 10th board exam. The first exam will be held on 18 February 2025 for English subject and the last exam will be held on 27 March 2025 for Environmental Science subject. The Indian School Certificate Examination results will be declared in the month of May.
Official Syllabus
The syllabus will consist of one paper of two hours duration.
Theory - 80 Marks
Practical - 20 Marks
The theory paper will be divided into two sections-
Section I - Section I will consist of short answer-type questions on the entire syllabus. (40 marks)
Section II - Section II will have six questions. Candidates will have to answer any four of these six questions. (40 marks)
Note: All chemical processes/reactions should be studied in terms of reactants, products, conditions, observations and (balanced) equations.
1. The Language of Chemistry
(i) 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 the number of valence electrons of the metals and non-metals; mono, di, tri and tetra valent elements.
• Radicals – definition; formulae and valencies.
• Compounds – name and formulae.
• 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 hit and trial 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.
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.
3. Water
(i) Water as a universal solvent
• Solutions as 'mixtures' of solids in water; 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
(Definition and examples of each of the above).
(iii) Drying and Dehydrating Agents
Meaning and examples only.
4. Atomic Structure and Chemical bonding
(i) Structure of an Atom, mass number and atomic number, Isotopes and Octet Rule.
• 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 the chemical activity of an atom.
• Definition and examples of isotopes (hydrogen, carbon, chlorine).
(ii) Electrovalent and covalent bonding, structures of various compounds – orbit structure
(a) Electrovalent Bond
• Definition
• Atomic orbit structure for the formation of Electrovalent compounds (e.g. NaCl, MgCl2, CaO);
(b) Covalent Bond
• Definition
• Atomic orbit structure for the formation of Covalent molecules on the basis of duplet and octet of electrons (examples: hydrogen, chlorine, oxygen, nitrogen, hydrogen chloride, water ammonia, carbon tetrachloride, methane.)
5. The Periodic Table
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, and 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).
• Special reference to Alkali metals (Group 1), Alkaline Earth metals (Group 2) Halogens (Group 17) and Zero Group (Group 18).
6. Study of the First Element - Hydrogen
Position of the non-metal (Hydrogen) in the periodic table and general group characteristics with reference to valency electrons, burning, and ion formation applied to the above-mentioned element.
(i) Hydrogen from water, dilute acids and alkalis.
(a) Hydrogen from water:
• The action of cold water on sodium potassium and calcium.
• The action of hot water on magnesium.
• The action of steam on aluminium, zinc, and iron; (reversibility of reaction between iron and steam).
• The action of steam on non-metal (carbon).
Students can be shown the action of sodium and calcium on the water in the laboratory. They must be asked to make observations and write equations for the above reactions.
Application of activity series for the above-mentioned reactions.
(b) Displacement of hydrogen from dilute acids.
The action of dilute sulphuric acid or hydrochloric acid on metals: Mg, Al, Zn and Fe.
(To understand reasons for not using other metals and diluting nitric acid.)
(c) Displacement of hydrogen from alkalis.
The action of Alkalis ((NaOH, KOH) on Al, Zn and Pb – 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.
(iii) Industrial manufacture of hydrogen by Bosch process.
• Main reactions and conditions.
• Separation of CO2 and CO from hydrogen.
(iv) Oxidation and reduction reactions.
Differences in terms of addition and removal of oxygen/hydrogen.
7. Study of Gas Laws
(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 in 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).
8. Atmospheric pollution
(a) Acid rain – composition, cause and its impact.
Sulphur in fossil fuels gives 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
i. Formation of ozone – relevant equations
ii. Function in the atmosphere.
iii. Destruction of the ozone layer – chemicals responsible for this are to be named but reactions are not required.
INTERNAL ASSESSMENT OF PRACTICAL WORK
Candidates will be asked to observe the effect of reagents and/or heat on substances supplied to them. The exercises will be simple and may include the recognition and identification of certain gases listed below.
Gases: Hydrogen, Oxygen, Carbon dioxide, Chlorine, Hydrogen chloride, Sulphur dioxide, Hydrogen sulphide, Ammonia, Water vapour, Nitrogen dioxide.
Candidates are expected to have completed the following minimum practical work.
Simple experiments on:
1. Action of heat on the following compounds:
(a) copper carbonate, zinc carbonate
(b) washing soda, copper sulphate crystals
(c) zinc nitrate, copper nitrate, lead nitrate
(d) ammonium chloride, iodine, ammonium dichromate Make observations, identify the products and make deductions where possible.
2. Action of diluting sulphuric acid on the following substances. (warm if necessary)
(a) a metal
(b) a carbonate
(c) a sulphide
(d) a sulphite Make observations, identify the gas evolved and make deductions.
3. Apply the flame test to identify the metal in the unknown substance.
(a) a sodium salt
(b) a potassium salt
(c) a calcium compound.
4. Simple experiments based on hard water and soft water – identification of hardness – simple softening – by heating the temporary hard water, using washing soda and advantage of using detergents over soap in hard water.
5. Find out the sources of pollution of water bodies in the locality. Suggest preventive steps to control it.
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