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

Class 9 Tech stream students can download the official Chemistry Tech Urdu Medium textbook here for free. This book is published by Punjab Curriculum and Textbook Board (PCTB) and is based on the Revised National Curriculum of Pakistan 2023.

Chemistry Tech is designed for 9th class Tech stream students and covers a broader and more modern set of topics compared to the older curriculum. With 12 chapters, it includes practical skills, environmental chemistry, and hydrocarbons alongside core chemistry concepts.

Book Overview

Class	9th Class / Matric Part 1
Subject	Chemistry Tech
Medium	Urdu
Stream	Tech (Vocational / Technical)
Board	Punjab Board (PCTB)
Edition	2025-26 (Based on National Curriculum 2023)
Total Chapters	12
Format	PDF (Free Download)

Chapter List

Chapter 1: States of Matter and their Changes

This chapter opens with how matter is classified into elements, compounds, and mixtures, then explains allotropy — how one element can exist in more than one form. Carbon’s three allotropes (diamond, graphite, and fullerene) and sulfur’s two crystalline forms (rhombic and monoclinic) are compared in detail. The chapter also separates true solutions from colloids and suspensions based on particle size and behavior, and shows how the solubility of a solute changes as temperature rises or falls.

Important Questions:

• Q: What is allotropy? A: The existence of an element in more than one physical form; carbon shows this as diamond, graphite, and fullerene.
• Q: Name the two crystalline forms of sulfur. A: Rhombic sulfur and monoclinic sulfur.
• Q: How does a solution differ from a colloid? A: A solution’s particles are small enough to stay fully dissolved, while a colloid has larger dispersed particles that scatter light.
• Q: What happens to solubility when temperature increases? A: For most solid solutes, solubility increases as temperature rises, allowing more solute to dissolve.

Chapter 2: Structure of Atom

This chapter traces how scientists discovered the electron, proton, and neutron, and how each discovery reshaped the atomic model up to Bohr’s version, where electrons orbit the nucleus in fixed energy levels. Atomic number and mass number are defined as ways to identify an element, and relative atomic mass is explained as a comparison against the carbon-12 standard, giving students the basic vocabulary used throughout the rest of the book.

Important Questions:

• Q: Who discovered the electron? A: J.J. Thomson, through his experiments with cathode rays.
• Q: What is the difference between atomic number and mass number? A: Atomic number is the number of protons in an atom; mass number is the total of protons and neutrons.
• Q: What does Bohr’s model say about electrons? A: Electrons move around the nucleus in fixed, defined energy levels or shells.
• Q: Define relative atomic mass. A: The average mass of an atom of an element compared to 1/12th the mass of a carbon-12 atom.

Chapter 3: Chemical Bonding

Bonding is explained through three main types: ionic bonds formed by the transfer of electrons between a metal and non-metal, covalent bonds formed by sharing electron pairs, and coordinate covalent bonds where one atom supplies both electrons. Metallic bonding is covered separately, describing how metal atoms share a “sea” of free electrons. The chapter also compares electropositive and electronegative elements, and lists how ionic and covalent compounds differ in melting point, conductivity, and solubility.

Important Questions:

• Q: What is an ionic bond? A: A bond formed when one atom transfers electrons to another, creating oppositely charged ions that attract each other.
• Q: Give an example of a coordinate covalent bond. A: The ammonium ion (NH4+), where nitrogen donates both electrons of the shared pair to a hydrogen ion.
• Q: Why do ionic compounds have high melting points? A: Because the strong electrostatic attraction between oppositely charged ions requires a large amount of energy to break.
• Q: What holds metal atoms together in metallic bonding? A: A “sea” of delocalized electrons that moves freely around fixed positive metal ions.

Chapter 4: Stoichiometry

Stoichiometry starts by distinguishing molecular formula from empirical formula, then teaches the criss-cross method for writing correct formulas of binary ionic compounds from their valencies. Avogadro’s number (6.022 × 10²³) is introduced to define the mole, linking the mass of a substance to the number of particles it contains through molar mass. The chapter closes with balancing chemical equations and using mole ratios to calculate the amounts of reactants and products involved in a reaction.

Important Questions:

• Q: What is Avogadro’s number? A: 6.022 × 10²³, the number of particles present in one mole of any substance.
• Q: Differentiate between empirical and molecular formula. A: Empirical formula shows the simplest whole-number ratio of atoms; molecular formula shows the actual number of atoms in a molecule.
• Q: How is the criss-cross method used? A: The numerical value of one ion’s charge becomes the subscript of the other ion, giving a neutral overall formula.
• Q: Define molar mass. A: The mass in grams of one mole of a substance, numerically equal to its atomic or molecular mass.

Chapter 5: Energetics

Energetics separates a chemical reaction into the system (the reacting substances) and the surroundings (everything else), then defines enthalpy change as the heat absorbed or released during a reaction. Exothermic reactions, such as combustion, release heat and have a negative ΔH, while endothermic reactions absorb heat and have a positive ΔH — both shown through worked numerical examples. Energy profile diagrams illustrate activation energy and the transition state, and the chapter explains how catalysts speed up reactions by lowering this activation energy barrier.

Important Questions:

• Q: What is the difference between exothermic and endothermic reactions? A: Exothermic reactions release heat to the surroundings (negative ΔH); endothermic reactions absorb heat from the surroundings (positive ΔH).
• Q: Define activation energy. A: The minimum energy needed for reactants to reach the transition state and form products.
• Q: Give one example of an exothermic reaction. A: Combustion of fuel, which releases heat and light.
• Q: How does a catalyst affect a reaction’s activation energy? A: It lowers the activation energy required, allowing the reaction to proceed faster without being used up itself.

Chapter 6: Equilibria

Equilibria opens by separating reversible reactions, which can proceed in both directions, from irreversible ones that go to completion. Dynamic equilibrium is demonstrated through color-changing hydrated salts — blue copper sulfate crystals (CuSO4·5H2O) turning white on heating, and pink cobalt chloride crystals (CoCl2·6H2O) changing color as water is lost or gained. The chapter then explains how concentration, temperature, pressure, and catalysts shift the position of equilibrium, using the industrial Haber process for ammonia as a worked example.

Important Questions:

• Q: What is dynamic equilibrium? A: A state in a reversible reaction where the forward and backward reaction rates are equal, so concentrations stay constant.
• Q: What color change occurs when hydrated copper sulfate is heated? A: It turns from blue to white as it loses its water of crystallization.
• Q: Name four factors that can shift a reaction’s equilibrium position. A: Concentration, temperature, pressure, and the addition of a catalyst.
• Q: What is the Haber process used to produce? A: Ammonia, made industrially from nitrogen and hydrogen gas.

Chapter 7: Acid Base Chemistry

This chapter opens with organic acids found in everyday foods — citric acid in citrus fruits, acetic acid in vinegar — before covering mineral acids like sulfuric and hydrochloric acid. Arrhenius theory defines acids as substances producing H+ ions and bases as substances producing OH- ions in water, while Bronsted-Lowry theory extends this to proton donors and acceptors, introducing conjugate acid-base pairs. Reactions of acids with reactive metals, metal oxides, and carbonates are covered alongside the general properties of alkalis.

Important Questions:

• Q: According to Arrhenius theory, what is an acid? A: A substance that produces hydrogen ions (H+) when dissolved in water.
• Q: Give one example of an organic acid and its natural source. A: Citric acid, found in citrus fruits such as lemons and oranges.
• Q: What happens when an acid reacts with a metal carbonate? A: It produces a salt, water, and carbon dioxide gas.
• Q: Define a conjugate acid-base pair. A: Two species that differ from each other by a single proton — an acid and the base formed after it donates that proton.

Chapter 8: Periodic Table and Periodicity

The modern periodic table is introduced through its horizontal periods and vertical groups, with elements classified into s-block, p-block, d-block, and f-block based on their electron configuration. The chapter shows how an element’s group number relates to the charge of the ion it typically forms. Using data tables, it then works through the major periodic trends — atomic radius, ionization energy, electron affinity, electronegativity, metallic character, and density — explaining how each property changes across a period and down a group.

Important Questions:

• Q: What determines whether an element belongs to the s, p, d, or f block? A: The sub-shell in which its last (outermost) electron is placed.
• Q: How does atomic radius change across a period? A: It generally decreases from left to right, as increasing nuclear charge pulls electrons closer.
• Q: What happens to ionization energy down a group? A: It generally decreases, because outer electrons are farther from the nucleus and more shielded.
• Q: Define electronegativity. A: The tendency of an atom to attract shared electrons towards itself in a covalent bond.

Chapter 9: Group Properties and Periodicity

Group 1 alkali metals are shown to get softer and more reactive going down the group, reacting vigorously with both water and chlorine to form hydroxides and chlorides — lithium reacts gently, while potassium reacts almost explosively. Group 17 halogens are covered next, from pale yellow fluorine gas to grey solid iodine, with reactivity decreasing down the group and displacement reactions used to show which halogen is the stronger oxidizing agent. The chapter ends with the largely unreactive Group 18 noble gases and a side-by-side comparison of metal and non-metal physical properties.

Important Questions:

• Q: Why does reactivity increase down Group 1? A: The outer electron is held less tightly as atomic size increases, so it is lost more easily in reactions.
• Q: What color is chlorine gas? A: Pale green, compared to fluorine’s pale yellow, bromine’s red-brown liquid, and iodine’s grey solid.
• Q: Why does halogen reactivity decrease down Group 17? A: Increasing atomic size makes it harder for the atom to attract and gain an extra electron.
• Q: Why are noble gases unreactive? A: Their outer electron shells are already completely full, giving them little tendency to gain, lose, or share electrons.

Chapter 10: Environmental Chemistry

This chapter lists the seven major air pollutants — carbon dioxide, carbon monoxide, nitrogen oxides, sulfur oxides, hydrocarbons, particulate matter, and ozone — and traces most of them back to burning fossil fuels. It explains how sulfur dioxide and nitrogen oxides combine with atmospheric moisture to form acid rain, damaging soil, plants, aquatic life, and even historic buildings like the Taj Mahal. The greenhouse effect and global warming are covered next, followed by practical reduction strategies: afforestation, catalytic converters in vehicles, flue gas desulphurization at power plants, renewable energy sources, and personal precautions like checking the Air Quality Index and wearing N95 masks.

Important Questions:

• Q: Name the seven major air pollutants covered in this chapter. A: Carbon dioxide, carbon monoxide, nitrogen oxides, sulfur oxides, hydrocarbons, particulate matter, and ozone.
• Q: How does acid rain form? A: Sulfur dioxide and nitrogen oxides released into the air react with water vapor to form sulfuric and nitric acid, which fall as acid rain.
• Q: What is the role of a catalytic converter in a car? A: It converts harmful exhaust gases like carbon monoxide, unburnt hydrocarbons, and nitrogen oxides into less harmful substances before they leave the exhaust.
• Q: What does a high Air Quality Index value mean? A: The air is more polluted and unsafe to breathe, especially for children, the elderly, and people with heart or lung conditions.

Chapter 11: Hydrocarbons

Organic chemistry is introduced as the chemistry of carbon, whose unique ability to form strong covalent bonds with itself — called catenation — lets it build long chains and rings found in saturated and unsaturated compounds. The chapter focuses on alkanes, given by the general formula CnH2n+2, and teaches IUPAC nomenclature using root, suffix, and prefix, working through examples like butane and methylbutane. Three preparation methods are covered — cracking of larger hydrocarbons, hydrogenation of alkenes and alkynes using a nickel catalyst, and reduction of alkyl halides with zinc and hydrochloric acid — followed by two key reactions: photochemical substitution with halogens and combustion.

Important Questions:

• Q: What is catenation? A: The ability of carbon atoms to form strong covalent bonds with other carbon atoms, creating chains and rings.
• Q: Give the general formula for alkanes. A: CnH2n+2, where n is the number of carbon atoms.
• Q: What is the IUPAC name for a four-carbon straight-chain alkane? A: Butane.
• Q: Name one method used to prepare alkanes. A: Cracking of higher hydrocarbons, or hydrogenation of alkenes/alkynes using a nickel catalyst.

Chapter 12: Laboratory and Practical Chemical Skills

This final chapter covers laboratory safety in detail, starting with the different categories of chemical hazards — flammable and explosive substances, corrosive chemicals that damage skin and eyes, and toxic chemicals that pose serious health risks. It explains the standard hazard warning signs used on chemical containers and lab doors, lists essential personal protective equipment such as lab coats, goggles, and gloves, and describes where fire extinguishers should be kept. The chapter closes with step-by-step emergency procedures to follow if an accident occurs during a practical.

Important Questions:

• Q: Name three categories of chemical hazards discussed in this chapter. A: Flammable/explosive hazards, corrosive hazards, and toxic hazards.
• Q: What PPE should a student wear when handling corrosive chemicals? A: Safety goggles, gloves, a lab coat, and a face shield where necessary.
• Q: What should you do if a corrosive chemical spills on your skin? A: Immediately wash the affected area with soap and plenty of water, and seek medical help if needed.
• Q: Why is it important to know the location of fire extinguishers? A: So that a fire can be controlled quickly in an emergency before it spreads or causes serious harm.

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Download Chemistry Tech Class 9 Urdu Medium PDF

Click the button below to download the official PCTB Chemistry Tech Urdu Medium book for free.

⬇ Download PDF (Urdu Medium)

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Who Should Read This

This book is for 9th class Tech stream students studying Chemistry in Urdu medium under Punjab Board. With 12 chapters and practical lab skills included, it gives Tech stream students a broader understanding of Chemistry relevant to vocational and technical fields.

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Applicable Boards

This PCTB Chemistry Tech textbook is used in all Punjab Board affiliated schools offering the Tech stream — including Lahore Board, Faisalabad Board, Gujranwala Board, Multan Board, Rawalpindi Board, Sargodha Board, DG Khan Board, and Sahiwal Board.

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