ICSE EXAM CLASS 10TH LATEST UPDATE

Finally, wait is over and 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

There will be one paper of two hours duration of 80 marks and an Internal Assessment of practical work carrying 20 marks.

The paper will be divided into two sections, Section I (40 marks) and Section II (40 marks).

Section I (compulsory) will contain short answer questions on the entire syllabus.  

Section II will contain six questions. Candidates will be required to answer any four of these six questions.

Note: All chemical processes/reactions should be studied with reference to the reactants, products, conditions, observation, (balanced) equations and diagrams.

1. Periodic Properties and variations of Properties 

(i) Periodic properties and their variations in groups and periods

Definitions and trends of the following periodic properties in groups and periods should be studied:

• Atomic size

• Metallic character

• Non-metallic character

• Ionisation potential

• Electron affinity

• Electronegativity

(ii) Periodicity on the basis of atomic number for elements

• The study of the modern periodic table upto period 3 (students are to be exposed to the complete modern periodic table but no questions will be asked on elements beyond period 3–Argon);

• Periodicity and other related properties are to be explained on the basis of nuclear charge and shells (not orbitals).

(Special reference to the alkali metals, alkaline earth metals, halogen groups and inert gases).

2. Chemical Bonding

Electrovalent, covalent and co-ordinate bonding, structures of various compounds, Electron dot structure.

(i) Electrovalent bonding:

• Electron dot structure of Electrovalent compounds NaCl, MgCl₂, CaO.

• Characteristic properties of electrovalent compounds – state of existence, melting and boiling points, conductivity (heat and electricity), dissociation in solution and in a molten state to be linked with electrolysis.

(ii) Covalent Bonding:

• Electron dot structure of covalent molecules on the basis of duplet and octet of electrons (example: hydrogen, chlorine, nitrogen, ammonia, carbon tetra chloride, methane.

• Polar Covalent compounds – based on differences in electronegativity:

Examples – HCl and H₂O including structures

• Characteristic properties of Covalent compounds – state of existence, melting and boiling points, conductivity (heat and electricity), ionisation in solution.

Comparison of Electrovalent and Covalent compounds

(iii) Coordinate Bonding:

• Definition

• The lone pair effect of the oxygen atom of the water molecule and the nitrogen atom of the ammonia molecule to explain the formation of H₃H₃O+⁺ and OHOH-  ions in water and NHNH₄+ ion.

The meaning of lone pair; the formation of hydronium ion and ammonium ion must be explained with help of electron dot diagrams.

3. Study of Acids, Bases and Salts

(i) Simple definitions in terms of the molecules and their characteristic properties.

(ii) Ions present in mineral acids, alkalis and salts and their solutions; use of litmus and pH paper to test for acidity and alkalinity.

• Examples with the equation for the ionisation/dissociation of ions of acids, bases and salts.

• Acids form hydronium ions (only positive ions) which turn blue litmus red, alkalis form hydroxyl ions (only negative ions) with water which turns red litmus blue.

• Salts are formed by partial or complete replacement of the hydrogen ion of an acid by a metal. (To be explained with suitable examples).

• Introduction to pH scale to test for acidity, neutrality and alkalinity by using pH paper or a Universal indicator.

(iii) Definition of salt; types of salts.

Types of salts: normal salts, acid salt, basic salt, definition and examples.

(iv) 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).

(v) Methods of preparation of Normal salts with relevant equations. (Details of apparatus or procedures not required). Methods included are:

• Direct combination

• Displacement

• Precipitation (double decomposition)

• Neutralization of insoluble base

• Neutralisation of an al

ICSE EXAM CLASS 10TH LATEST UPDATE

Finally, wait is over and 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

There will be one paper of two hours duration of 80 marks and an Internal Assessment of practical work carrying 20 marks.

The paper will be divided into two sections, Section I (40 marks) and Section II (40 marks).

Section I (compulsory) will contain short answer questions on the entire syllabus.  

Section II will contain six questions. Candidates will be required to answer any four of these six questions.

Note: All chemical processes/reactions should be studied with reference to the reactants, products, conditions, observation, (balanced) equations and diagrams.

1. Periodic Properties and variations of Properties 

(i) Periodic properties and their variations in groups and periods

Definitions and trends of the following periodic properties in groups and periods should be studied:

• Atomic size

• Metallic character

• Non-metallic character

• Ionisation potential

• Electron affinity

• Electronegativity

(ii) Periodicity on the basis of atomic number for elements

• The study of the modern periodic table upto period 3 (students are to be exposed to the complete modern periodic table but no questions will be asked on elements beyond period 3–Argon);

• Periodicity and other related properties are to be explained on the basis of nuclear charge and shells (not orbitals).

(Special reference to the alkali metals, alkaline earth metals, halogen groups and inert gases).

2. Chemical Bonding

Electrovalent, covalent and co-ordinate bonding, structures of various compounds, Electron dot structure.

(i) Electrovalent bonding:

• Electron dot structure of Electrovalent compounds NaCl, MgCl₂, CaO.

• Characteristic properties of electrovalent compounds – state of existence, melting and boiling points, conductivity (heat and electricity), dissociation in solution and in a molten state to be linked with electrolysis.

(ii) Covalent Bonding:

• Electron dot structure of covalent molecules on the basis of duplet and octet of electrons (example: hydrogen, chlorine, nitrogen, ammonia, carbon tetra chloride, methane.

• Polar Covalent compounds – based on differences in electronegativity:

Examples – HCl and H₂O including structures

• Characteristic properties of Covalent compounds – state of existence, melting and boiling points, conductivity (heat and electricity), ionisation in solution.

Comparison of Electrovalent and Covalent compounds

(iii) Coordinate Bonding:

• Definition

• The lone pair effect of the oxygen atom of the water molecule and the nitrogen atom of the ammonia molecule to explain the formation of H₃H₃O+⁺ and OHOH-  ions in water and NHNH₄+ ion.

The meaning of lone pair; the formation of hydronium ion and ammonium ion must be explained with help of electron dot diagrams.

3. Study of Acids, Bases and Salts

(i) Simple definitions in terms of the molecules and their characteristic properties.

(ii) Ions present in mineral acids, alkalis and salts and their solutions; use of litmus and pH paper to test for acidity and alkalinity.

• Examples with the equation for the ionisation/dissociation of ions of acids, bases and salts.

• Acids form hydronium ions (only positive ions) which turn blue litmus red, alkalis form hydroxyl ions (only negative ions) with water which turns red litmus blue.

• Salts are formed by partial or complete replacement of the hydrogen ion of an acid by a metal. (To be explained with suitable examples).

• Introduction to pH scale to test for acidity, neutrality and alkalinity by using pH paper or a Universal indicator.

(iii) Definition of salt; types of salts.

Types of salts: normal salts, acid salt, basic salt, definition and examples.

(iv) 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).

(v) Methods of preparation of Normal salts with relevant equations. (Details of apparatus or procedures not required). Methods included are:

• Direct combination

• Displacement

• Precipitation (double decomposition)

• Neutralization of insoluble base

• Neutralisation of an alkali (titration)

• Action of dilute acids on carbonates and bi-carbonates.

4. Analytical Chemistry

(i) Action of Ammonium Hydroxide and Sodium Hydroxide on the solution of salts: the 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.

On the solution of salts:

• Colour of salt and its solution.

• Action on the addition of Sodium Hydroxide to the solution of Ca, Fe, Cu, Zn, and Pb salts drop by drop in excess. The formation and colour of the hydroxide precipitated are to be highlighted with the help of equations.

• Action on the addition of Ammonium Hydroxide to the solution of Ca, Fe, Cu, Zn, and Pb salts drop by drop in excess. The formation and colour of the hydroxide precipitated are to be highlighted with the help of equations.

• Special action of Ammonium Hydroxide on solutions of copper salts and sodium hydroxide on ammonium salts.

(ii) Action of caustic alkalis (NaOH, KOH) on aluminium 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

(i) Gay Lussac’s Law of Combining Volumes; Avogadro’s Law.

• Idea of mole – a number just as a dozen, a gross (Avogadro’s number).

• Avogadro’s Law - statement and explanation.

• Gay Lussac’s Law of Combining Volumes. – Statement and explanation.

• Understanding molar volume- “the mass of 22.4 litres of any gas at S.T.P. is equal to its molar mass”. (Questions will not be set on formal proof but may be taught for clear understanding).

• Simple calculations based on the molar volume and Gay Lussac’s law.

(ii) Refer to the atomicity of hydrogen, oxygen, nitrogen and chlorine (proof not required).

The explanation can be given using equations for the formation of HCl, NH₃, and NO.

(iii) Vapour Density and its relation to relative molecular mass.

• Molecular mass = 2 × vapour density (formal proof not required)

• Deduction of simple (empirical) and molecular formulas from:

(a) the percentage composition of a compound. 

(b) the masses of combining elements. 

(iv) Mole and its relation to mass.

• Relating mole and atomic mass; arriving at gram atomic mass and then gram atom; atomic mass is a number dealing with one atom; gram atomic mass is the mass of one mole of atoms.

• Relating mole and molecular mass arriving at gram molecular mass and gram molecule – molecular mass is a number dealing with a molecule, the gram molecular mass is the mass of one mole of molecules.

• Simple calculations based on a relation of the mole to mass, volume and Avogadro’s number.

(v) Simple calculations based on chemical equations

Related to weight and/or volumes of both reactants and products.

6. Electrolysis

(i) Electrolytes and non-electrolytes. Definitions and examples.

(ii) Substances containing molecules only, ions only, both molecules and ions.

• Substances containing molecules only ions only, both molecules and ions.

• Examples: relating their composition with their behaviour as strong and weak electrolytes as well as non-electrolytes.

(iii) Definition and explanation of electrolysis, electrolyte, electrode, anode, cathode, anion, cation, oxidation and reduction (on the basis of loss and gain of electrons).

(iv) An elementary study of the migration of ions, with reference to the factors influencing the 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) illustrated by the electrolysis of:

• Molten lead bromide 

• Acidified water with platinum electrodes

• Aqueous copper (II) sulphate with copper electrodes; electron transfer at the electrodes.

The above electrolytic processes can be studied in terms of electrolyte used, electrodes used, ionization reaction, anode reaction, cathode reaction, and use of selective discharge theory, wherever applicable.

(v) Applications of electrolysis:

• Electroplating with nickel and silver, choice of electrolyte for electroplating.

• Electro refining of copper.

Reasons and conditions for electroplating; names of the electrolytes and the electrodes used should be given. Equations for the reactions at the electrodes should be given for the electroplating, and refining of copper.

7. Metallurgy

(i) Occurrence of metals in nature

• Mineral and ore-meaning only.

• Common ores of aluminium.

(ii) Stages involved in the extraction of metals.

(a) Dressing of the ore – hydrolytic method, magnetic separation, froth flotation method.

(b) Conversion of concentrated ore to its oxide- roasting and calcination (definition, examples with equations).

(c) Reduction of metallic oxides- some can be reduced by hydrogen, carbon and carbon monoxide (e.g. copper oxide, lead (II) oxide, iron (III) oxide and zinc oxide) and some cannot (e.g. Al₂O₃, MgO) - refer to activity series). Active metals by electrolysis e.g. sodium, potassium and calcium. (reference only).

Equations with conditions should be given.

(d) Electro refining – reference only.

(iii) Extraction of Aluminium

(a) Chemical method for purifying bauxite by using NaOH–Baeyer’s Process.

(b) Electrolytic extraction–Hall Heroult’s process:

Structure of electrolytic cell - the various components as part of the electrolyte, electrodes and electrode reactions.

Description of the changes occurring, the purpose of the substances used and the main reactions with their equations.

(iv) Alloys -  Definition, alloys of Aluminium (only constituent elements), properties and uses.

8. Study of Compounds

(i) Hydrogen Chloride

Hydrogen chloride: preparation of hydrogen chloride from sodium chloride; refer to the density and solubility of hydrogen chloride (fountain experiment); reaction with ammonia; acidic properties of its solution.

• Preparation of hydrogen chloride from sodium chloride; the laboratory method of preparation can be learnt in terms of reactants, products, conditions, equations, diagram or setting of the apparatus, procedure, observation, precaution, collection of the gas and identification.

• Simple experiment to show the density of the gas (Hydrogen Chloride) – heavier than air.

• Solubility of hydrogen chloride (fountain experiment); setting of the apparatus, procedure, observation, inference.

• Method of preparation of hydrochloric acid by dissolving the gas in water - the special arrangement and the mechanism by which the back suction is avoided should be learnt.

• Reaction with ammonia

• Acidic properties of its solution-reaction with metals, their oxides, hydroxides and carbonates to give their chlorides; decomposition of carbonates, hydrogen carbonates, sulphides, and sulphites.

• Precipitation reactions with silver nitrate solution and lead nitrate solution. 

(ii) Ammonia

Ammonia: its laboratory preparation from ammonium chloride and collection; ammonium salts. Manufacture by Haber’s Process; density and solubility of ammonia (fountain experiment); an aqueous solution of ammonia; its reactions with hydrogen chloride and with hot copper (II) oxide; lead monoxide (PbO) and chlorine; the burning of ammonia in oxygen; uses of ammonia.

• Laboratory preparation from ammonium chloride and collection; (the preparation to be studied in terms of, setting of the apparatus and diagram, procedure, observation, collection and identification)

• Ammonia from ammonium salts using alkalies.

The reactions are to be studied in terms of reactants, products, conditions and equations.

• Manufacture by Haber’s Process.

• Density and solubility of ammonia (fountain experiment).

• The burning of ammonia in oxygen.

• The catalytic oxidation of ammonia (with conditions and reaction)

• Its reactions with hydrogen chloride and with hot copper (II) oxide and chlorine (both chlorine in excess and ammonia in excess).

All these reactions may be studied in terms of reactants, products, conditions, equations, and observations.

• Aqueous solution of ammonia-reaction with sulphuric acid, nitric acid, hydrochloric acid and solutions of iron (III) chloride, iron (II) sulphate, lead nitrate, zinc nitrate and copper sulphate.

(iii) Nitric Acid

one laboratory method of preparation of nitric acid from potassium nitrate or sodium nitrate. Large-scale preparation. Nitric acid as an oxidizing agent.

• Laboratory preparation of nitric acid from potassium nitrate or sodium nitrate; the laboratory method to be studied in terms of reactants, products, conditions, equations, setting up of apparatus, diagram, precautions, collection and identification.

• Manufacture of Nitric acid by Ostwald’s process (Only equations with conditions where applicable).

• As an oxidising agent: its reaction with copper, carbon, and sulphur.

(iv) Sulphuric Acid

Its behaviour as an acid when dilute, as an oxidizing agent when concentrated - oxidation of carbon and sulphur; as a dehydrating agent-dehydration of sugar and copper (II) sulphate crystals; its non-volatile nature.

• Its behaviour as an acid when dilute-reaction with metal, metal oxide, metal hydroxide, metal carbonate, metal bicarbonate, metal sulphite, and metal sulphide.

• Concentrated sulphuric acid as an oxidizing agent - the oxidation of carbon and sulphur.

• Concentrated sulphuric acid as a dehydrating agent - (a) the dehydration of sugar (b) Copper (II) sulphate crystals.

• Non-volatile nature of sulphuric acid-reaction with sodium or potassium chloride and sodium or potassium nitrate.

9. Organic Chemistry

(i) Introduction to Organic compounds

• Unique nature of Carbon atom–tetravalency, catenation.

• Formation of single, double and triple bonds, straight chain, branched chain, and cyclic compounds (only benzene).

(ii) Structure and Isomerism

• Structure of compounds with single, double and triple bonds.

• Structural formulae of hydrocarbons. The structural formula must be given for: alkanes, alkenes, and alkynes up to 5 carbon atoms.

• Isomerism – structural (chain, position).

(iii) Homologous series – characteristics with examples

Alkane, alkene, and alkyne series and their gradation in properties and the relationship with the molecular mass or molecular formula.

(iv) Simple nomenclature

Simple nomenclature of the hydrocarbons with simple functional groups–(double bond, triple bond, alcoholic, aldehydic, carboxylic group) longest chain rule and smallest number for functional groups rule–trivial and IUPAC names (compounds with only one functional group).

(v) Hydrocarbons: alkanes, alkenes, alkynes

• Alkanes - general formula; methane (greenhouse gas) and ethane, Complete combustion of methane and ethane, the reaction of methane and ethane with chlorine through substitution.

• Alkenes – (unsaturated hydrocarbons with a double bond); ethene as an example.

• Alkynes - (unsaturated hydrocarbons with a triple bond); ethyne is an example of alkyne.

Only main properties, particularly addition products with hydrogen and halogen namely Cl₂, Br₂ and I₂ pertaining to alkenes and alkynes.

(vi) Alcohols: ethanol – preparation, properties and uses.

• Preparation of ethanol by hydrolysis of alkyl halide.

• Properties – Physical: Nature, Solubility, Density, Boiling Points. Chemical: Combustion, action with sodium, ester formation with acetic acid, dehydration with con. Sulphuric acid to prepare ethene.

• Denatured and spurious alcohol.

• Important uses of Ethanol.

(vii) Carboxylic acids (aliphatic - monocarboxylic acid): Acetic acid – properties and uses of acetic acid.

• Structure of acetic acid.

• Properties of Acetic Acid: Physical properties – odour (vinegar), glacial acetic acid (effect of sufficient cooling to produce ice-like crystals). Chemical properties – action with litmus, alkalis and alcohol (the idea of esterification).

• Uses of acetic acid.

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 and ions listed below. The examiners will not, however, be restricted in their choice of substances containing the listed ions.

Gases: Hydrogen, Oxygen, Carbon dioxide, Chlorine, Hydrogen chloride, Sulphur dioxide, Hydrogen sulphide, Ammonia, Water vapour, Nitrogen dioxide.

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:

1. Action of heat on the following substances:

(a) Copper carbonate, zinc carbonate

(b) Zinc nitrate, copper nitrate, lead nitrate Make observations, identify the products and make deductions where possible (equations not required).

2. 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⁺.

3. Supply a solution of dilute acid and alkali. Determine which is acidic and which is basic, giving two tests for each.

EVALUATION

The assignments/project work is to be evaluated by the subject teacher and by an External Examiner. (The External Examiner may be a teacher nominated by the Head of the school, who could be from the faculty but not teaching the subject in the section/class. For example, a teacher of Chemistry of Class VIII may be deputed to be an External Examiner for Class X Chemistry projects.)

The Internal Examiner and the External Examiner will assess the assignments independently.

Award of marks                                     20 Marks

Subject Teacher (Internal Examiner) 10 Marks

External Examiner                                10 Marks

The total marks obtained out of 20 are to be sent to the Council by the Head of the school.

The Head of the school will be responsible for the online entry of marks on the Council’s CAREERS portal by the due date.

TO KNOW MORE

For Official Website: click here

For Time Table: click here

ICSE EXAM CLASS 10TH LATEST UPDATE

Finally, wait is over and 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.

TIME TABLE - CHEMISTRY

TIME TABLE - ALL SUBJECTS

ICSE EXAM CLASS 10TH LATEST UPDATE

Finally, wait is over and 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.

TIME TABLE - CHEMISTRY

TIME TABLE - ALL SUBJECTS

TO KNOW MORE

For Official Website: click here

For Time Table: click here

ICSE EXAM CLASS 10TH LATEST UPDATE

Finally, wait is over and 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 ICSE Analysis

ICSE Chemistry Analysis 2022

ICSE Chemistry Semester 2 Exam 2022 has conducted on May 13, 2022.  Experts Says that the Paper's Difficulty Level was "Easy to difficult"

ICSE Chemistry Semester 2 2022: Exam highlights

Exam Date: Friday, May 13, 2022

Total Exam Timing: 11 am - 12:30 pm

Total Exam Duration: 1.5 hours

Total Marks: 40

ICSE Chemistry Semester 2 2022:  Exam Analysis Facts

1. Several students stated "The Chemistry exam was pretty doable. We solved ICSE specimen papers before coming for the exam as the teacher told us to do. We were not sure if it helped today, but we were happy with this paper."

2. It was a tough paper and some sections were very tricky.

3. According to some students, the chemistry paper was as per their expectations and they may get full marks. 

4. The paper was divided into various sections - A, and B.

5. Section A covered 10 MCQs of one mark each. Section B covered four subjective-type questions carrying ten marks each, out of which three questions were to be attempted.

6. While section A was compulsory and descriptive in nature, other sections gave students internal choices in questions.

ICSE Chemistry Semester 2 2022:  Exam Analysis - Experts and Teacher feedback

Chemistry teachers have stated that "the paper is moderate but manageable". According to experts, "it was a straightforward to average paper."

ICSE Class -10 Chemistry Semester 2 2022: Detailed Exam Analysis 

1. The difficulty level of the ICSE Class 10 Chemistry (Science) paper was from Easy to difficult.

2. Easy Questions - 50%, Moderate  Questions - 35%, Difficult Questions - 15%

3. The average score expected by the students overall is 30 to 32 in the exam.

4. The pattern of the paper is the same as given in the sample paper issued by ICSE

Section A

i. This section was considered to be 100% Easy.

ii. All questions were from the prescribed ICSE Textbook.

iii. In this section, 02 questions were from Metallurgy, 06 questions were from the Study of Compounds, and 02 questions were from Organic chemistry.

iv. No confusing questions in this section.

Section B

i. This section was easy to difficult (40% easy, 40% moderate, and 20% difficult)

ii. All questions were from the prescribed ICSE textbook.

iii. This section covers questions from Metallurgy, the Study of Compounds, and Organic chemistry.

ICSE/ISC X Analysis From Other Resources

ICSE EXAM CLASS 10TH LATEST UPDATE

Finally, wait is over and 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 ICSE Analysis

ICSE Chemistry Analysis 2022

ICSE Chemistry Semester 2 Exam 2022 has conducted on May 13, 2022.  Experts Says that the Paper's Difficulty Level was "Easy to difficult"

ICSE Chemistry Semester 2 2022: Exam highlights

Exam Date: Friday, May 13, 2022

Total Exam Timing: 11 am - 12:30 pm

Total Exam Duration: 1.5 hours

Total Marks: 40

ICSE Chemistry Semester 2 2022:  Exam Analysis Facts

1. Several students stated "The Chemistry exam was pretty doable. We solved ICSE specimen papers before coming for the exam as the teacher told us to do. We were not sure if it helped today, but we were happy with this paper."

2. It was a tough paper and some sections were very tricky.

3. According to some students, the chemistry paper was as per their expectations and they may get full marks. 

4. The paper was divided into various sections - A, and B.

5. Section A covered 10 MCQs of one mark each. Section B covered four subjective-type questions carrying ten marks each, out of which three questions were to be attempted.

6. While section A was compulsory and descriptive in nature, other sections gave students internal choices in questions.

ICSE Chemistry Semester 2 2022:  Exam Analysis - Experts and Teacher feedback

Chemistry teachers have stated that "the paper is moderate but manageable". According to experts, "it was a straightforward to average paper."

ICSE Class -10 Chemistry Semester 2 2022: Detailed Exam Analysis 

1. The difficulty level of the ICSE Class 10 Chemistry (Science) paper was from Easy to difficult.

2. Easy Questions - 50%, Moderate  Questions - 35%, Difficult Questions - 15%

3. The average score expected by the students overall is 30 to 32 in the exam.

4. The pattern of the paper is the same as given in the sample paper issued by ICSE

Section A

i. This section was considered to be 100% Easy.

ii. All questions were from the prescribed ICSE Textbook.

iii. In this section, 02 questions were from Metallurgy, 06 questions were from the Study of Compounds, and 02 questions were from Organic chemistry.

iv. No confusing questions in this section.

Section B

i. This section was easy to difficult (40% easy, 40% moderate, and 20% difficult)

ii. All questions were from the prescribed ICSE textbook.

iii. This section covers questions from Metallurgy, the Study of Compounds, and Organic chemistry.

ICSE/ISC X Analysis From Other Resources

ICSE EXAM CLASS 10TH LATEST UPDATE

Finally, wait is over and 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.

KEY HIGHLIGHTS OF THE BOARD EXAM

TIME TABLE

This year Class 10th ICSE Final exams will be conducted for the following subjects:

ICSE EXAM CLASS 10TH LATEST UPDATE

Finally, wait is over and 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.

KEY HIGHLIGHTS OF THE BOARD EXAM

TIME TABLE

This year Class 10th ICSE Final exams will be conducted for the following subjects:

IMPORTANT INSTRUCTIONS

1. In addition to the duration indicated on the timetable for writing the paper, 15 minutes time is given for reading the Question Paper.

2. The Indian School Certificate Year 2025 Examination results will be declared in the month of May 2025.

3. The results will be made available on the official website of the CISCE.

4. For ICSE, the marks of the Practical/Project work Of the subject, already awarded to the candidate in the main examination, Will be carried forward. However, if the candidate was absent earlier either in Practical or during assessment of Project Work of the subject, then, the candidate, in addition to taking the Theory examination, is permitted to submit the Project Work and/or for Practical. which should then be assessed, and marks awarded and submitted.

5. CISCE will not retain answer scripts of the candidates later than 60 days from the day of the declaration of results. The same shall be destroyed thereafter.

6. All candidates who appear for the ICSE Main Examination, are eligible to take the Improvement Examination' conducted in the same year of Examination.

HOW TO CHECK TIME TABLE

Students who are planning to appear for the ICSE Class 10th exam can download their complete timetable by following these simple steps:

Step 1: Visit the official CISCE website: cisce.org

Step 2: On the homepage, find and click on the link for “ICSE Class 10th Time Table”

Step 3: A new page will open displaying the ICSE exam date sheet in PDF format.

Step 4: Carefully review the date sheet to get all the necessary details regarding the ICSE exam.

Step 5: Download and save the timetable. It is also recommended to take a printout for future reference.

TO KNOW MORE

For Official Website: click here

For Time Table: click here