Class 10 Chemistry: Complete Pillar Guide (2026)
Class 10 Chemistry covers five chapters that build on each other more than they seem to at first glance: reactions and equations set the vocabulary everything else uses, acids and bases show that vocabulary in action, metals and non-metals apply it to real elements, carbon compounds show what happens when one element (carbon) is versatile enough to build millions of compounds on its own, and the periodic table ties every single property back to one number — atomic number.
This pillar page gives you a genuinely complete overview of all five chapters in one place — the core reactions, formulas, and worked examples for each — and will link out to ten in-depth companion guides (two per chapter) as they're published. Bookmark this page: it's designed to be your one-stop map of the entire Class 10 Chemistry syllabus.
📋 Table of Contents
1. Chemical Reactions and Equations
A chemical reaction rearranges atoms from reactants into products, and a chemical equation is the shorthand for that rearrangement. Because atoms are never created or destroyed in a reaction, every balanced equation must have the same number of atoms of each element on both sides — this single rule (the Law of Conservation of Mass) is the whole reason "balancing" exists as a skill.
The Four Main Types of Reactions
| Type | Pattern | Example |
|---|---|---|
| Combination | A + B → AB | CaO + H₂O → Ca(OH)₂ |
| Decomposition | AB → A + B | CaCO₃ → CaO + CO₂ (on heating) |
| Displacement | A + BC → AC + B | Fe + CuSO₄ → FeSO₄ + Cu |
| Double displacement | AB + CD → AD + CB | Na₂SO₄ + BaCl₂ → BaSO₄↓ + 2NaCl |
Oxidation and Reduction
Solved example — Balancing an equation
Balance: Fe + H₂O → Fe₃O₄ + H₂
3Fe + 4H₂O → Fe₃O₄ + 4H₂
2. Acids, Bases and Salts
Acids taste sour, turn blue litmus red, and release H⁺ ions in water. Bases taste bitter, feel soapy, turn red litmus blue, and release OH⁻ ions in water. A salt forms when an acid and a base neutralise each other.
Key Reactions
Acid + Metal carbonate → Salt + Water + CO₂
Acid + Base → Salt + Water (neutralisation)
The pH Scale
Common Salts You Should Know
| Salt | Formula | Common Use |
|---|---|---|
| Baking soda | NaHCO₃ | Cooking, antacid |
| Washing soda | Na₂CO₃·10H₂O | Cleaning agent |
| Bleaching powder | CaOCl₂ | Disinfectant, bleaching |
| Plaster of Paris | CaSO₄·½H₂O | Casts, moulds |
Solved example — pH calculation
Find the pH of a solution with [H⁺] = 10⁻³ mol/L.
3. Metals and Non-Metals
Metals are typically malleable, ductile, sonorous, lustrous, and good conductors of heat and electricity — mercury is the one liquid-at-room-temperature exception. Non-metals are usually brittle, dull, and poor conductors, though graphite (a carbon allotrope) is a notable exception that does conduct electricity.
The Reactivity Series
Extraction of Metals — Matched to Reactivity
| Reactivity | Extraction Method | Examples |
|---|---|---|
| Highly reactive | Electrolysis of molten ore | Na, Al |
| Moderately reactive | Reduction with carbon/CO | Fe, Zn |
| Least reactive | Found free, or simple heating | Au, Ag, Cu |
Solved example — Predicting displacement
Will zinc displace copper from a copper sulphate (CuSO₄) solution?
4. Carbon and Its Compounds
Carbon forms an outsized number of compounds because of two properties working together: tetravalency (it forms four covalent bonds) and catenation (its unique ability to bond with other carbon atoms to build long chains, branches, and rings).
Saturated vs Unsaturated Hydrocarbons
| Series | General Formula | Bond Type |
|---|---|---|
| Alkanes | CₙH₂ₙ₊₂ | Single bonds only (saturated) |
| Alkenes | CₙH₂ₙ | One double bond (unsaturated) |
| Alkynes | CₙH₂ₙ₋₂ | One triple bond (unsaturated) |
Functional Groups
Solved example — Naming a compound
Name and write the structural formula for a 3-carbon chain with an −OH group on the end carbon.
5. Periodic Classification of Elements
Mendeleev arranged elements by increasing atomic mass and famously left gaps that correctly predicted undiscovered elements' properties — but his table struggled with isotopes and had no consistent place for hydrogen. The modern periodic law fixed this by arranging elements by atomic number instead, giving today's 18-group, 7-period table.
Periodic Trends
| Property | Across a Period (→) | Down a Group (↓) |
|---|---|---|
| Atomic size | Decreases | Increases |
| Metallic character | Decreases | Increases |
| Valence electrons | Increases (1→8) | Stays the same |
Solved example — Locating an element
An element X has the electronic configuration 2, 8, 7. Which period and group does it belong to?
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🌐 Trusted External References
- NCERT Official Website — download the official Class 10 Science textbook
- CBSE Academic — official syllabus & sample papers
- Chemical Reaction — Wikipedia
- Periodic Table — Wikipedia
Frequently Asked Questions
What are the main chapters in Class 10 Chemistry?
What are the four main types of chemical reactions?
What is the pH scale and why is it important?
What is the reactivity series of metals?
Why can carbon form so many different compounds?
What did Mendeleev's periodic table get right and wrong?
Conclusion: Five Chapters, One Connected Story
Class 10 Chemistry rewards seeing the connections between chapters as much as memorising each one individually. The reaction types from Chapter 1 show up again in acid-base chemistry and metal extraction; the reactivity series from Chapter 3 explains why some metals need electrolysis and others don't; and the periodic table in Chapter 5 quietly explains why metals and non-metals behave the way Chapter 3 describes. Studying the chapters as one connected system, rather than five separate topics, is what makes the whole syllabus click.
Related Test Series & Practice Sets
Class 10 Foundation Series
Tags: Class 10 Chemistry, Chemical Reactions and Equations, Acids Bases and Salts, Metals and Non-Metals, Carbon and Its Compounds, Periodic Classification of Elements, CBSE 2026
