ICSE Class 10 Chemistry study guide and chapter map
ICSE Class 10 Chemistry is the Class 10 science paper that tests chemical facts, observations, balanced equations, calculations and practical understanding. This page keeps the Chemistry book PDF resources from the existing page and adds a study plan, worked solutions, practical notes and common mistakes so that students can use the book instead of only collecting downloads.
ICSE Class 10 Chemistry — Books (Free PDF Download)
| Resource | Download |
|---|---|
| Chapter 1: Periodic Table | Download Chapter 1: Periodic Table PDF |
| Chapter 2: Chemical Bonding | Download Chapter 2: Chemical Bonding PDF |
| Chapter 3: Acids Bases And Salts | Download Chapter 3: Acids Bases And Salts PDF |
| Chapter 4: Analytical Chemistry | Download Chapter 4: Analytical Chemistry PDF |
| Chapter 5: Mole Concept And Stoichimetry | Download Chapter 5: Mole Concept And Stoichimetry PDF |
| Chapter 6: Electrolysis | Download Chapter 6: Electrolysis PDF |
| Chapter 7: Metallurgy | Download Chapter 7: Metallurgy PDF |
| Chapter 8: Hydrogen Chloride | Download Chapter 8: Hydrogen Chloride PDF |
| Chapter 9: Ammonia | Download Chapter 9: Ammonia PDF |
| Chapter 10: Nitric Acid | Download Chapter 10: Nitric Acid PDF |
| Chapter 11: Sulphuric Acid | Download Chapter 11: Sulphuric Acid PDF |
| Chapter 12: Organic Chemistry | Download Chapter 12: Organic Chemistry PDF |
| Chapter 13: Practical Work | Download Chapter 13: Practical Work PDF |
All files are hosted free on this site for study use.
Use this page as a subject hub: first check the chapter map, then use the PDF table for reading, and finally practise the worked examples in the same written style expected in school tests and board-style answers. Textbook chapter order may differ slightly between editions such as Concise/Selina and Frank, so treat the order below as a study map, not as a claim that every school edition uses identical numbering.
Concept snapshot: Think of Class 10 Chemistry as three linked notebooks. The first notebook is patterns, such as periodic trends and chemical bonding. The second is reactions, such as acids, salts, electrolysis and compounds. The third is calculations, especially mole concept and stoichiometry. A good answer usually connects all three: write the fact, support it with the correct equation or observation, and use calculation only when the question asks for quantity.
What chapters are covered in ICSE Class 10 Chemistry?
The ICSE Class 10 Chemistry syllabus is usually studied through chapters on periodic properties, chemical bonding, acids, analytical chemistry, mole concept, electrolysis, metallurgy, specific compounds and organic chemistry. Practical work supports the theory because students must recognise observations, reagents and inferences instead of memorising isolated equations.
| Study area | What to learn | What the examiner usually checks |
|---|---|---|
| Periodic Table and periodic properties | Modern periodic arrangement, groups, periods, atomic size, metallic character, ionisation tendency and electronegativity trends. | Trend with reason, not only the final trend name. |
| Chemical bonding | Electrovalent and covalent bonding, electron-dot structures, properties of compounds and relation between bonding and behaviour. | Correct valency, electron transfer or sharing, and properties linked to the bond type. |
| Acids, bases, salts and analytical chemistry | Definitions, neutralisation, salt preparation, precipitates, gas tests and qualitative analysis. | Reagent, observation and inference written together. |
| Mole concept and stoichiometry | Relative molecular mass, mole, Avogadro number, percentage composition, empirical formula and equation-based calculation. | Balanced equation, mole ratio, unit and final answer. |
| Electrolysis and metallurgy | Electrolytes, electrodes, ions, selective discharge, extraction principles and purification. | Ion movement, electrode product and reason for the product. |
| Study of compounds | Hydrogen chloride, ammonia, nitric acid and sulphuric acid: preparation, properties, tests and uses. | Balanced equations, conditions, observations and safety points. |
| Organic Chemistry | Hydrocarbons, functional groups, IUPAC names, reactions of alkanes, alkenes, alcohols and acids as prescribed by the school text. | Correct structure, homologous series, reaction condition and product. |
| Practical Work | Record file, observations, salt analysis and viva-based understanding. | Neat record, accurate observation and explanation of the experiment. |
For the official board source, students should cross-check the subject outline from the CISCE website. Use the school-prescribed textbook for final chapter order because different schools may follow different editions.
How should students use ICSE Class 10 Chemistry Solutions?
ICSE Class 10 Chemistry Solutions are useful only when they train you to write the answer, not when they replace the textbook. Read the concept first, try the question without looking, then compare your steps with the solution. If your answer misses the condition, observation or balanced equation, rewrite it once in full.
Four-step method for using solutions
- Step 1: Read the question command. Words such as explain, distinguish, give reason, calculate and identify demand different answer styles.
- Step 2: Write the chemistry first. For reactions, write the correct formula and balanced equation before adding prose.
- Step 3: Add the observation or reason. In analytical chemistry, colour and solubility changes matter. In periodic properties, the reason must mention atomic size, nuclear pull or shielding where relevant.
- Step 4: Check the final line. A numerical answer needs a unit; a test needs an inference; a preparation answer needs the condition if the reaction depends on it.
A practical way to revise is to keep an error notebook with three columns: wrong formula, missing condition and wrong observation. Most Chemistry marks are lost through these repeated mistakes rather than through difficult theory.
ICSE Class 10 Chemistry book PDF resources
The table below preserves the Chemistry PDF links available on this page. Each link opens in a new tab. Some chapter titles appear in two forms because the existing page contains more than one PDF entry for the same broad chapter; keep both if your teacher has asked you to use a particular file.
| No. | Chapter title on the existing page | |
|---|---|---|
| 1 | Ch 01 Periodic Table | Download |
| 2 | Ch 01 Periodic Table Periodic Properties and Variat | Download |
| 3 | Ch 02 Chemical Bonding | Download |
| 4 | Ch 03 Acids Bases and Salts | Download |
| 5 | Ch 03 Study of Acids Bases and Salts | Download |
| 6 | Ch 04 Analytical Chemistry | Download |
| 7 | Ch 04 Analytical Chemistry | Download |
| 8 | Ch 05 Mole Concept and Stoichimetry | Download |
| 9 | Ch 05 Mole Concept and Stoichiometry | Download |
| 10 | Ch 06 Electrolysis | Download |
| 11 | Ch 06 Electrolysis | Download |
| 12 | Ch 07 Metallurgy | Download |
| 13 | Ch 07 Metallurgy | Download |
| 14 | Ch 08 Hydrogen Chloride | Download |
| 15 | Ch 08 Study of Compounds Hydrogen Chloride | Download |
| 16 | Ch 09 Ammonia | Download |
| 17 | Ch 09 Study of Compounds Ammonia | Download |
| 18 | Ch 10 Nitric Acid | Download |
| 19 | Ch 10 Study of Compounds Nitric Acid | Download |
| 20 | Ch 11 Sulphuric Acid | Download |
| 21 | Ch 12 Organic Chemistry | Download |
| 22 | Ch 12 Organic Chemistry | Download |
| 23 | Ch 13 Practical Work | Download |
Worked examples from Chemistry chapters
The following model answers are original practice examples based on standard ICSE Class 10 Chemistry treatment. They show the written method a student should follow: formula, balanced equation, observation or mole ratio, and final answer.
Example 1: Explain the manufacture of sulphuric acid by the Contact Process
Step 1: Produce sulphur dioxide by burning sulphur in oxygen, or by roasting iron pyrites.
\mathrm{S} + \mathrm{O}_2 \rightarrow \mathrm{SO}_2
4\mathrm{FeS}_2 + 11\mathrm{O}_2 \rightarrow 2\mathrm{Fe}_2\mathrm{O}_3 + 8\mathrm{SO}_2
Step 2: Oxidise sulphur dioxide to sulphur trioxide in the presence of vanadium pentoxide catalyst. This step is reversible and is the main reaction controlled in the process.
2\mathrm{SO}_2 + \mathrm{O}_2 \rightleftharpoons 2\mathrm{SO}_3 + \text{heat}
Step 3: Do not dissolve \mathrm{SO}_3 directly in water because the reaction is highly exothermic and produces a fine mist of acid that is difficult to condense. Instead, absorb it in concentrated sulphuric acid to form oleum.
\mathrm{SO}_3 + \mathrm{H}_2\mathrm{SO}_4 \rightarrow \mathrm{H}_2\mathrm{S}_2\mathrm{O}_7
Step 4: Dilute oleum carefully with water to obtain sulphuric acid of the required concentration.
\mathrm{H}_2\mathrm{S}_2\mathrm{O}_7 + \mathrm{H}_2\mathrm{O} \rightarrow 2\mathrm{H}_2\mathrm{SO}_4
Final answer: The Contact Process prepares sulphuric acid through production of \mathrm{SO}_2, catalytic oxidation to \mathrm{SO}_3, absorption in concentrated \mathrm{H}_2\mathrm{SO}_4 to form oleum, and controlled dilution of oleum.
Example 2: State the Brown Ring Test for nitrate ions
Step 1: Take the nitrate solution in a test tube and add freshly prepared ferrous sulphate solution.
Step 2: Add concentrated sulphuric acid slowly along the side of the test tube without shaking, so that two layers form.
Step 3: A brown ring at the junction of the two liquids shows the presence of nitrate ions. The nitric acid formed is reduced to nitric oxide, and nitric oxide forms a brown nitrosoferrous complex with ferrous sulphate.
6\mathrm{FeSO}_4 + 3\mathrm{H}_2\mathrm{SO}_4 + 2\mathrm{HNO}_3 \rightarrow 3\mathrm{Fe}_2(\mathrm{SO}_4)_3 + 2\mathrm{NO} + 4\mathrm{H}_2\mathrm{O}
\mathrm{FeSO}_4 + \mathrm{NO} + 5\mathrm{H}_2\mathrm{O} \rightarrow [katex display="true"]\mathrm{Fe}(\mathrm{NO})(\mathrm{H}_2\mathrm{O})_5\mathrm{SO}_4[/katex]
Final answer: A brown ring confirms nitrate ions. The answer must include the reagent, the careful addition of concentrated \mathrm{H}_2\mathrm{SO}_4, the brown ring observation and the inference.
Example 3: Calculate the mass of calcium carbonate needed to produce 4.4\ \mathrm{g} of carbon dioxide
Step 1: Write the balanced equation for the reaction of calcium carbonate with dilute hydrochloric acid.
\mathrm{CaCO}_3 + 2\mathrm{HCl} \rightarrow \mathrm{CaCl}_2 + \mathrm{H}_2\mathrm{O} + \mathrm{CO}_2
Step 2: Find the molar mass of carbon dioxide.
M_r(\mathrm{CO}_2)=12+2(16)=44
Step 3: Convert the given mass of carbon dioxide to moles.
\text{Moles of }\mathrm{CO}_2=\frac{4.4}{44}=0.1\ \mathrm{mol}
Step 4: Use the equation ratio. From the balanced equation, 1\ \mathrm{mol} of \mathrm{CaCO}_3 gives 1\ \mathrm{mol} of \mathrm{CO}_2. Therefore, 0.1\ \mathrm{mol} of \mathrm{CO}_2 needs 0.1\ \mathrm{mol} of \mathrm{CaCO}_3.
Step 5: Find the molar mass of calcium carbonate.
M_r(\mathrm{CaCO}_3)=40+12+3(16)=100
Step 6: Calculate the required mass.
\text{Mass of }\mathrm{CaCO}_3=0.1 \times 100=10\ \mathrm{g}
Final answer: 10\ \mathrm{g} of \mathrm{CaCO}_3 is required to produce 4.4\ \mathrm{g} of \mathrm{CO}_2.
Example 4: Explain why concentrated sulphuric acid gives hydrogen chloride from sodium chloride
Step 1: Concentrated sulphuric acid is a non-volatile acid. It can displace a more volatile acid from its salt when heated.
Step 2: Sodium chloride contains the chloride ion. When heated with concentrated sulphuric acid, hydrogen chloride gas is formed.
\mathrm{NaCl} + \mathrm{H}_2\mathrm{SO}_4 \xrightarrow{\Delta} \mathrm{NaHSO}_4 + \mathrm{HCl} \uparrow
Step 3: The hydrogen chloride appears as steamy fumes in moist air and gives dense white fumes with ammonia because ammonium chloride is formed.
\mathrm{NH}_3 + \mathrm{HCl} \rightarrow \mathrm{NH}_4\mathrm{Cl}
Final answer: Concentrated sulphuric acid liberates \mathrm{HCl} from \mathrm{NaCl} because it is non-volatile and displaces the volatile acid from its salt.
How to approach ICSE Chemistry practical work
Practical work in Chemistry is not separate from theory. The written paper often expects the same skills used in the laboratory: choosing a reagent, noting an observation and making a correct inference. For example, writing only white precipitate is incomplete if the question asks for a test; the answer must say which reagent gives the precipitate and what it proves.
Practical record file checklist
- Write the aim, apparatus, chemicals, procedure, observations, equations and conclusion for each experiment.
- For salt analysis, learn the colour and solubility of precipitates formed with sodium hydroxide and ammonium hydroxide.
- For gases such as \mathrm{HCl}, \mathrm{NH}_3 and \mathrm{SO}_2, connect smell, solubility, litmus effect and confirmatory test.
- During viva practice, explain why each reagent is used. Memorising only the final colour is weak preparation.
Examiner’s mindset for Chemistry answers
In ICSE Chemistry, credit is usually awarded for separate answer points: correct formula, balanced equation, observation, condition and inference. A student who writes \mathrm{BaSO}_4 without saying white precipitate, or writes an observation without naming the reagent, may lose the point that proves the chemistry.
For numerical answers, the balanced equation is the start of the solution, not decoration. The mole ratio must come from the equation. For practical-type answers, use this order: reagent → observation → inference. For give reason questions, write the property first and then the example. Example: concentrated sulphuric acid acts as a dehydrating agent because it removes hydrogen and oxygen from a compound in the ratio 2:1, the ratio found in water.
Common mistakes students make in ICSE Chemistry
- Writing unbalanced equations: Always balance atoms on both sides. In stoichiometry, an unbalanced equation gives the wrong mole ratio.
- Confusing drying and dehydrating action: A drying agent removes moisture from a gas; a dehydrating agent removes the elements of water from a compound. Concentrated \mathrm{H}_2\mathrm{SO}_4 cannot dry ammonia because ammonia is basic and reacts with the acid.
- Giving only the colour in analytical chemistry: Write the reagent and solubility change. For example, a precipitate that dissolves in excess reagent may identify a different ion from one that remains insoluble.
- Forgetting reaction conditions: Organic reactions often need sunlight, catalyst, heat or acidified reagent. Missing conditions can make the equation incomplete.
- Using molecular formula where structure is needed: In organic chemistry, \mathrm{C}_2\mathrm{H}_6\mathrm{O} can represent different structures, so draw or name the compound when the question asks for structure or functional group.
- Adding water to concentrated acid: In the laboratory, acid is added slowly to water with stirring. Adding water to concentrated acid can cause splashing due to heat released.
Related ICSE Chemistry resources
After reading the book chapter, use these related pages for structured practice:
- ICSE Class 10 syllabus for checking the overall subject plan.
- ICSE Class 10 Chemistry previous year question papers for timed practice.
- ICSE Class 10 books and solutions for other Class 10 resources.
- ISC Class 12 Chemistry syllabus if you plan to continue Chemistry after ICSE.
Sources and syllabus checks
This replacement page is based on the standard ICSE Class 10 Chemistry syllabus treatment, the existing PDF resource links on icseboard.org, school-level Chemistry texts such as Frank and Concise/Selina where used by schools, and overlapping NCERT Class 10 Science concepts for acids, bases, salts and carbon compounds. For official board updates, use cisce.org. For national textbook reference on overlapping concepts, use NCERT textbooks.
Frequently Asked Questions
How should I study ICSE Class 10 Chemistry from the book?
Study ICSE Class 10 Chemistry by reading one concept, writing its equation or observation, then solving two or three questions without looking at the solution. For calculation chapters, always begin with the balanced equation and use the mole ratio from that equation.
Are ICSE Class 10 Chemistry Solutions enough for exam preparation?
ICSE Class 10 Chemistry Solutions are useful for checking steps, but they are not enough by themselves. You must also read the textbook explanation, practise equations from memory, revise observations in analytical chemistry and solve previous-year style questions under time limits.
Which Chemistry chapters need the most equation practice?
Equation practice is most important in acids, bases and salts, electrolysis, metallurgy, hydrogen chloride, ammonia, nitric acid, sulphuric acid and organic chemistry. In each chapter, learn the reactants, conditions, products and observations together.
How do I avoid mistakes in mole concept questions?
Start with a balanced equation, convert the given mass or volume into moles, use the equation ratio, and convert the answer into the required unit. For example, if 1\ \mathrm{mol} of \mathrm{CaCO}_3 gives 1\ \mathrm{mol} of \mathrm{CO}_2, then 0.1\ \mathrm{mol} of \mathrm{CO}_2 needs 0.1\ \mathrm{mol} of \mathrm{CaCO}_3.
What should I write in analytical chemistry answers?
In analytical chemistry, write the reagent, the observation and the inference. An answer such as white precipitate is incomplete unless it also states which reagent was added and what ion or compound the observation confirms.
Can I use these Chemistry PDFs if my school follows a different edition?
You can use the Chemistry PDFs for revision if the topic matches your school syllabus, but chapter order and wording may vary by edition. Follow your teacher’s prescribed textbook for final homework sequence and use the PDFs here for practice and cross-checking.
Downloads & PDF Resources
Download the related PDFs, question papers, and study resources below.
| equations from previous years’ papers |