Chemistry Class 9 English Medium PDF Download – Punjab Board (PCTB)

Class 9 students studying Chemistry in English medium can download the official Punjab Board textbook here for free. The book is approved by the Federal Ministry of Education and published by Caravan Book House under a print licence from Punjab Textbook Board for free distribution in government schools across Punjab.

For 9th class board exam preparation, this English medium edition covers all 8 fundamental Chemistry units, from the basics of matter and atomic structure through to electrochemistry and chemical reactivity. Studying key terms in English builds the scientific vocabulary needed for FSC Chemistry, MDCAT, and ECAT.

Book Overview

Class	9th Class / Matric Part 1
Subject	Chemistry
Medium	English
Board	Punjab Board (PCTB)
Authors	Dr. Jaleel Tariq, Dr. Irshad Ahmad Chatha
Publisher	Caravan Book House, Lahore
Total Units	8
Format	PDF (Free Download)

Chapter List

Unit 1: Fundamentals of Chemistry

This unit introduces chemistry’s main branches: physical, organic, inorganic, biochemistry, industrial, nuclear, environmental, and analytical chemistry. It defines matter, substances, and mixtures, then explains elements, compounds, and mixtures with real examples, along with atomic number, mass number, and relative atomic mass on the carbon-12 scale. It closes with empirical and molecular formulas, ions, molecular ions, free radicals, Avogadro’s number, and mole-based chemical calculations.

Important Questions:
• What is the difference between an element, a compound, and a mixture? An element is made of one type of atom and can’t be broken down further; a compound is two or more elements chemically combined in a fixed ratio; a mixture is substances combined physically with no fixed ratio, separable by physical means.
• What is Avogadro’s number and how does it relate to a mole? It is 6.02 × 10²³ particles (atoms, molecules, or formula units) — a mole of any substance contains exactly this many particles.
• Differentiate between empirical formula and molecular formula. Empirical formula shows the simplest whole-number ratio of atoms; molecular formula shows the actual number of atoms of each element in one molecule, and is a whole-number multiple of the empirical formula.
• What is the relative atomic mass of an element? The average mass of its atoms compared with 1/12th the mass of one atom of carbon-12.

Unit 2: Structure of Atoms

This unit traces the theories and experiments behind atomic structure, from the discovery of protons (canal rays) and electrons (cathode rays) to Rutherford’s nuclear model and Bohr’s atomic theory with quantized electron orbits. It covers writing electronic configurations for the first 18 elements across K, L, and M shells and subshells, and explains isotopes — atoms of the same element with different numbers of neutrons — along with their medical and industrial uses.

Important Questions:
• Who discovered the proton and how? Eugene Goldstein discovered protons in 1886 through canal rays — positively charged particles produced in a discharge tube.
• What is an isotope? Atoms of the same element having the same atomic number but different mass numbers, due to a different number of neutrons.
• What are the defects of Rutherford’s atomic model? It could not explain why orbiting electrons don’t lose energy and spiral into the nucleus, nor account for the line spectrum of hydrogen.
• How many subshells does the M shell consist of? Three subshells — s, p, and d.

Unit 3: Periodic Table and Periodicity of Properties

This unit explains how the modern periodic table arranges elements into periods and groups by increasing atomic number, replacing Mendeleev’s mass-based arrangement. It covers periodic trends across periods and down groups — atomic radius, shielding effect, ionization energy, electron affinity, and electronegativity — and explains why each property rises or falls as you move through the table.

Important Questions:
• What was Mendeleev’s Periodic Table based on? The increasing atomic mass of elements.
• State the modern periodic law. Properties of elements are a periodic function of their atomic numbers.
• Why does atomic radius decrease across a period? Nuclear charge increases while electrons are added to the same shell, pulling the outer electrons closer to the nucleus.
• Define ionization energy and its trend. The energy needed to remove the most loosely held electron from an isolated gaseous atom; it increases across a period and decreases down a group.

Unit 4: Structure of Molecules

This unit explains why atoms react — to attain a stable noble gas configuration — and covers the main types of chemical bonds: ionic, covalent (including dative/coordinate covalent), polar versus non-polar covalent, and metallic bonding. It also introduces intermolecular forces such as dipole-dipole interactions and hydrogen bonding, and links bond type to the physical properties of ionic compounds, covalent compounds, and metals.

Important Questions:
• Why do atoms react with each other? To attain a stable noble gas electronic configuration by completing their octet.
• Differentiate between an ionic bond and a covalent bond. An ionic bond forms by transfer of electrons between an electropositive and an electronegative atom; a covalent bond forms by sharing of electron pairs between two non-metal atoms.
• Why does ice float on water? Hydrogen bonding arranges water molecules into an open hexagonal lattice in ice, making it less dense than liquid water.
• What is a coordinate covalent bond? A covalent bond in which both shared electrons are donated by only one of the two bonding atoms.

Unit 5: Physical States of Matter

This unit covers the typical properties of gases (diffusion, effusion, pressure, compressibility, density) along with Boyle’s Law and Charles’s Law, then moves to liquids (evaporation, vapour pressure, boiling and freezing point) and solids (melting point, rigidity, density, crystalline versus amorphous solids, and allotropy). It builds a complete comparison of how particles behave differently in each physical state of matter.

Important Questions:
• State Boyle’s Law. At constant temperature, the volume of a fixed mass of gas is inversely proportional to its pressure.
• What is diffusion? The spontaneous mixing of molecules of two or more substances due to their random motion, like the smell of perfume spreading through a room.
• Differentiate between crystalline and amorphous solids. Crystalline solids have an ordered geometric arrangement of particles and a sharp melting point (e.g. sugar); amorphous solids lack regular internal structure and soften gradually over a temperature range (e.g. glass, rubber).
• What is vapour pressure and how does temperature affect it? The pressure exerted by a liquid’s vapour in equilibrium with the liquid at a given temperature; it increases as temperature rises.

Unit 6: Solutions

This unit defines solutions, solutes, and solvents, then explains saturated, unsaturated, and supersaturated solutions and how solutions are diluted. It covers concentration units including percentage (mass/mass, mass/volume, volume/volume) and molarity, along with factors affecting solubility such as temperature. It ends by comparing true solutions, colloids, and suspensions, including the Tyndall effect.

Important Questions:
• What is molarity? The number of moles of solute dissolved per dm³ (litre) of solution.
• Differentiate between a saturated and an unsaturated solution. A saturated solution holds the maximum solute that can dissolve at a given temperature; an unsaturated solution can still dissolve more solute at that temperature.
• What is the Tyndall effect and which mixtures show it? The scattering of a beam of light passing through a mixture — shown by colloids, but not by true solutions.
• How does temperature generally affect the solubility of a solid in a liquid? Solubility of most solids increases with temperature, since more kinetic energy helps overcome solute-solute attractive forces.

Unit 7: Electrochemistry

This unit covers oxidation-reduction reactions in terms of electron loss and gain, oxidation states and the rules for assigning them, and oxidizing versus reducing agents. It explains electrochemical cells — both electrolytic cells (like the Downs cell and Nelson’s cell) and galvanic cells (like the Daniel cell) — their industrial applications, and corrosion, covering how iron rusts and how galvanizing, painting, alloying, and electroplating prevent it.

Important Questions:
• Define oxidation and reduction in terms of electrons. Oxidation is the loss of electrons by a substance; reduction is the gain of electrons by a substance.
• What is the difference between a galvanic cell and an electrolytic cell? A galvanic cell converts spontaneous chemical energy into electrical energy; an electrolytic cell uses electrical energy to drive a non-spontaneous chemical reaction.
• Why is oxygen necessary for rusting? Rusting is an oxidation reaction where iron reacts with oxygen and moisture to form hydrated iron oxide (rust) — without oxygen it can’t occur.
• What is electroplating? Depositing a thin layer of metal onto another metal’s surface using electrolysis, to improve appearance or prevent corrosion.

Unit 8: Chemical Reactivity

This unit compares the reactivity of metals, especially alkali and alkaline earth metals, in terms of electropositive character, ionization energy, and reactions with water, oxygen, and acids. It then covers non-metals, focusing on the halogens’ reactivity trend and their reactions with hydrogen, water, and other substances, along with the broader significance of non-metals in the earth’s crust, oceans, atmosphere, and living things.

Important Questions:
• Why does the reactivity of alkali metals increase down the group? Atomic size increases down the group, so the outermost electron sits farther from the nucleus and is held less tightly, making it easier to lose.
• Why are silver and gold the least reactive metals? They have high ionization energies and stable electronic configurations, making them very reluctant to lose electrons.
• Compare the general reactivity trend of halogens. Reactivity as oxidizing agents decreases down the group, from fluorine (most reactive) to iodine (least reactive).
• Why can graphite conduct electricity unlike most non-metals? Its layered structure bonds each carbon atom to only three others, leaving one delocalized electron per atom free to move and carry current.

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Download Chemistry Class 9 English Medium PDF

Click the button below to download the official Chemistry Class 9 English Medium book for free.

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Who Should Read This

This book is for all 9th class students studying Chemistry in English medium under Punjab Board. It is especially useful for pre-medical and pre-engineering students who want to prepare in English from the start, as FSC Chemistry and entry tests like MDCAT and ECAT are also in English.

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Applicable Boards

This textbook is used across all Punjab Board affiliated schools — Lahore Board, Faisalabad Board, Gujranwala Board, Multan Board, Rawalpindi Board, Sargodha Board, DG Khan Board, and Sahiwal Board.

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