ICSE class 10 is considered as the first milestone towards the education journey of a student. The marks obtained in class 10 ICSE exam are considered for admission by many schools and later, by colleges and universities. The marks also reflect one’s educational excellence and basic academic skills.
The topics included in the ICSE class 10 syllabus are varying and the students are exposed to a variety of important topics that would be required in the later grades. Subjects like physics, chemistry, maths and biology introduce concepts which are not only important for class 11 and 12 but, also for the competitive exams like JEE and NEET.
ICSE exam is conducted by the Council for the Indian School Certificate Examination (CISCE) and the materials provided here are in accordance with the latest syllabus.
In Class 10 ICSE, While preparing for chemistry, never ignore numerical problems. Most of the times, the questions asked are based on numerical. Remember; if you are a master in numerical problems, be sure of getting good marks in the examination. Chemistry is the one you should write and practice. Balance the equations on your own. Chemistry becomes fairly simple if you have mastered formulae.
Here, the detailed ICSE syllabus for class 10 chemistry is provided for the students to acquaint them with the topics that CISCE has included in the syllabus.
The ICSE Exam Paper for class 10 will be divided into 3 groups. Group A will have 4 compulsory subjects and group B will consist of 2 optional subjects chosen by the students. Whereas, Group C will have 1 optional subject chosen by the students. Apart from that, Group A and Group B will be based on 80% + 20% marking scheme and Group C will be based on 50% + 50% marking criteria. Here, we’re including the official group- wise marking scheme for ICSE Syllabus based on the official notification released by the ICSE Board itself.
1. Periodic Properties and variations of Properties – Physical and Chemical.
Periodic properties and their variations in groups and periods.
Periodicity on the basis of atomic number for elements.
2. Chemical Bonding
3. Study of Acids, Bases and Salts
Simple definitions in terms of the molecules and their characteristic properties.
Ions present in mineral acids, alkalis and salts and their solutions; use of litmus and pH paper to test for acidity and alkalinity.
Definition of salt; types of salts.: Types of salts: normal salts, acid salt, basic salt, definition and examples.
Action of dilute acids on salts. : Decomposition of hydrogen carbonates, carbonates, sulphites and sulphides by appropriate acids with heating if necessary. (Relevant laboratory work must be done).
Methods of preparation of Normal salts with relevant equations. (Details of apparatus or procedures not required).
4. Analytical Chemistry
Action of Ammonium Hydroxide and Sodium Hydroxide on solution of salts: colour of salt and its solution; formation and colour of hydroxide precipitated for solutions of salts of Ca, Fe, Cu, Zn and Pb; special action of ammonium hydroxide on solutions of copper salt and sodium hydroxide on ammonium salts.
Action of alkalis (NaOH, KOH) on certain metals, their oxides and hydroxides. The metals must include aluminium, zinc and lead, their oxides and hydroxides, which react with caustic alkalis (NaOH, KOH), showing the amphoteric nature of these substances.
5. Mole Concept and Stoichiometry
Gay Lussac’s Law of Combining Volumes; Avogadro’s Law.
Refer to the atomicity of hydrogen, oxygen, nitrogen and chlorine (proof not required).
Vapour Density and its relation to relative molecular mass.
Mole and its relation to mass.
Simple calculations based on chemical equations Related to weight and/or volumes of both reactants and products.
Electrolytes and non-electrolytes. : Definitions and examples.
Substances containing molecules only, ions only, both molecules and ions.
Definition and explanation of electrolysis, electrolyte, electrode, anode, cathode, anion, cation, oxidation and reduction (on the basis of loss and gain of electrons).
An elementary study of the migration of ions, with reference to the factors influencing selective discharge of ions (reference should be made to the activity series as indicating the tendency of metals, e.g. Na, Mg, Fe, Cu, to form ions)
Applications of electrolysis
Occurrence of metals in nature
Stages involved in the extraction of metals
Extraction of Aluminium.
Alloys – composition and uses Stainless steel, duralumin, brass, bronze, fuse metal / solder.
8. Study of Compounds
9. Organic Chemistry
Introduction to Organic compounds.
Structure and Isomerism.
Homologous series – characteristics with examples.
Hydrocarbons: alkanes, alkenes, alkynes.
Alcohols: ethanol – preparation, properties and uses.
Carboxylic acids (aliphatic – mono carboxylic acid): Acetic acid – properties and uses of acetic acid.
Internal Assessment of Practical Work
Candidates will be asked to observe the effect of reagents and/or of heat on substances supplied to them. The exercises will be simple and may include the recognition and identification of certain gases and ions listed below. The examiners will not, however, be restricted in their choice to substances containing the listed ions.
Ions: Calcium, Copper, Iron, Lead, Zinc and Ammonium, Carbonate, Chloride, Nitrate, Sulphide, Sulphite and Sulphate.
Knowledge of a formal scheme of analysis is not required. Semi-micro techniques are acceptable but candidates using such techniques may need to adapt the instructions given to suit the size of the apparatus being used.
Candidates are expected to have completed the following minimum practical work:
Action of heat on the following compounds:
Copper carbonate, zinc carbonate
zinc nitrate, copper nitrate, lead nitrate Make observations, identify the products and make deductions where possible. (equations not required)
Make a solution of the unknown substance: add sodium hydroxide solution or ammonium hydroxide solution, make observations and give your deduction. Warming the mixture may be needed. Choose from substances containing Ca2+, Cu2+, Fe2+, Fe3+, Pb2+, Zn2+, NH4+.
Supply a solution of a dilute acid and alkali. Determine which is acidic and which is basic, giving two tests for each.
Add concentrated hydrochloric acid to each of the given substances, warm, make observations, identify any product and make deductions: (a) copper oxide (b) manganese dioxide.
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