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

Class 9 Tech stream students can download the official Chemistry Tech English 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 covers a broader and more modern syllabus than the older Chemistry curriculum. With 12 chapters including practical lab skills, environmental chemistry, and hydrocarbons, it prepares Tech stream students with both theoretical knowledge and hands-on chemistry skills.

Book Overview

Class	9th Class / Matric Part 1
Subject	Chemistry Tech
Medium	English
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

Matter is grouped here into elements, compounds, and mixtures before the chapter turns to allotropy, the phenomenon where the same element takes more than one physical form. Diamond, graphite, and fullerene are studied as carbon’s allotropes, while sulfur is shown existing as rhombic and monoclinic crystals. Later sections distinguish solutions, colloids, and suspensions by particle size, and describe how rising or falling temperature affects how much solute a solvent can dissolve.

Important Questions:

• Q: Why is graphite a good conductor of electricity while diamond is not? A: Graphite has free-moving electrons between its layered carbon sheets, while diamond’s carbon atoms are all held in fixed covalent bonds.
• Q: Give one difference between a mixture and a compound. A: A compound is chemically combined in fixed proportions, while a mixture is only physically combined and can vary in composition.
• Q: What is a suspension? A: A mixture with visibly large, undissolved particles that settle over time, unlike a solution or colloid.
• Q: Define fullerene. A: A carbon allotrope made of carbon atoms arranged in a hollow, cage-like structure.

Chapter 2: Structure of Atom

Chapter 2 walks through the historical discovery of the three subatomic particles — electron, proton, and neutron — and explains how Bohr’s atomic model placed electrons in fixed energy levels around a central nucleus. Students learn to calculate atomic number and mass number for any element and understand relative atomic mass as a comparison to carbon-12, concepts that form the foundation for the chemical bonding studied later.

Important Questions:

• Q: Which subatomic particle carries no charge? A: The neutron, found in the nucleus alongside protons.
• Q: Why was Bohr’s model an improvement over earlier models? A: It explained that electrons occupy fixed energy levels instead of moving randomly, which accounted for atomic stability.
• Q: How many protons does an atom with atomic number 12 have? A: 12 protons.
• Q: Why is carbon-12 used as the standard for atomic mass? A: It provides a fixed, universally agreed reference point so atomic masses of all other elements can be compared consistently.

Chapter 3: Chemical Bonding

This chapter builds up chemical bonding step by step — starting with ionic bonds, where electrons transfer completely from a metal atom to a non-metal atom, moving to covalent bonds, where atoms share electron pairs, and finishing with coordinate covalent bonds, where only one atom contributes the shared pair. A section on metallic bonding describes the free-electron model that gives metals their conductivity, and a comparison table sets ionic compounds against covalent compounds on melting point, solubility, and electrical behavior.

Important Questions:

• Q: Differentiate between electropositive and electronegative elements. A: Electropositive elements readily lose electrons to form positive ions, while electronegative elements readily gain electrons to form negative ions.
• Q: Why are covalent compounds usually poor conductors of electricity? A: They generally lack free-moving charged particles, since their electrons are shared and held between specific atoms.
• Q: How many electrons are shared in a double covalent bond? A: Four electrons, or two pairs, are shared between the two bonded atoms.
• Q: Why are metals malleable and ductile? A: The free-moving electrons let metal ions slide past each other without breaking the overall metallic bond.

Chapter 4: Stoichiometry

This chapter introduces the mole concept as the central tool of quantitative chemistry, defining it through Avogadro’s number and connecting it to molar mass so that mass, moles, and particle count can all be converted into one another. Students also learn to write empirical and molecular formulas correctly, use the criss-cross method to derive formulas for ionic compounds from valencies, and balance chemical equations before applying mole-ratio calculations to real reaction problems.

Important Questions:

• Q: Why must a chemical equation be balanced before calculations? A: Because the law of conservation of mass requires equal numbers of each atom on both sides, which balancing ensures.
• Q: How do you convert grams of a substance to moles? A: Divide the given mass by the molar mass of the substance.
• Q: What information does a mole ratio give in a reaction? A: It shows the proportion in which reactants combine and products form, based on the balanced equation’s coefficients.
• Q: Write the empirical formula for a compound with molecular formula C6H12O6. A: CH2O, the simplest whole-number ratio of the molecular formula.

Chapter 5: Energetics

This chapter defines a reaction’s system and surroundings before explaining enthalpy change, ΔH, as the energy exchanged between the two. Worked examples show how exothermic reactions like combustion release heat with a negative ΔH value, while endothermic reactions take in heat and carry a positive ΔH. Energy profile diagrams are used to visualize the activation energy needed to reach the transition state, and catalysts are introduced as substances that lower this energy barrier without being consumed in the reaction.

Important Questions:

• Q: What is meant by “system” and “surroundings” in energetics? A: The system is the substances taking part in the reaction; the surroundings are everything else around it that can exchange energy with it.
• Q: What does a negative ΔH value indicate? A: The reaction is exothermic and releases heat to the surroundings.
• Q: What is shown at the peak of an energy profile diagram? A: The transition state, the highest-energy, unstable arrangement of atoms during the reaction.
• Q: Why is a catalyst not consumed during a reaction? A: It only provides an alternative lower-energy pathway for the reaction and is regenerated unchanged at the end.

Chapter 6: Equilibria

This chapter distinguishes irreversible reactions, which run to completion, from reversible reactions, which can be pushed forward or backward. Dynamic equilibrium is introduced using hydrated salts as visual evidence — copper sulfate pentahydrate and cobalt chloride hexahydrate both change color when water is added or removed by heating. Factors that disturb this balance — concentration, temperature, pressure, and the presence of a catalyst — are each examined, with the industrial Haber process used to show how these factors are controlled to maximize ammonia yield.

Important Questions:

• Q: Differentiate between a reversible and an irreversible reaction. A: A reversible reaction can proceed in both forward and backward directions; an irreversible reaction goes to completion in one direction only.
• Q: How does cobalt chloride crystal color indicate water content? A: Hydrated cobalt chloride is pink, while the dehydrated (anhydrous) form turns blue, showing whether water is present.
• Q: Does a catalyst shift the equilibrium position? A: No, a catalyst only speeds up how quickly equilibrium is reached; it does not change the final position.
• Q: Why is the Haber process carried out under high pressure? A: Because increased pressure favors the side of the reaction with fewer gas molecules, increasing ammonia yield.

Chapter 7: Acid Base Chemistry

Acid-base chemistry begins with a look at natural organic acids — such as citric acid in citrus fruits and acetic acid in vinegar — and common mineral acids used in industry. The chapter then presents two theories of acids and bases: the Arrhenius theory, based on H+ and OH- ion production in water, and the Bronsted-Lowry theory, which defines acids and bases as proton donors and acceptors and introduces the idea of conjugate pairs. Practical reactions of acids with metals, metal oxides, and carbonates are explained, along with the defining properties of alkalis.

Important Questions:

• Q: How does the Bronsted-Lowry theory define an acid? A: As a substance that donates a proton (H+) to another substance in a reaction.
• Q: What distinguishes a strong acid from a weak acid? A: A strong acid ionizes almost completely in water, while a weak acid only partially ionizes.
• Q: What products form when an acid reacts with a reactive metal? A: A salt and hydrogen gas.
• Q: Name one common mineral acid discussed in this chapter. A: Hydrochloric acid, or sulfuric acid, both widely used mineral acids.

Chapter 8: Periodic Table and Periodicity

This chapter organizes elements into periods and groups and explains the s, p, d, and f block classification based on where the last electron is added during electron configuration. It links group number to the typical ionic charge of elements in that group, then walks through periodic trends one by one — atomic radius, ionization energy, electron affinity, electronegativity, metallic character, and density — supported by comparative data tables that show how each trend behaves moving across a period or down a group.

Important Questions:

• Q: How does metallic character change across a period and down a group? A: It decreases across a period and increases down a group.
• Q: What is electron affinity? A: The energy change when an atom gains an electron to form a negative ion.
• Q: Why does atomic radius increase down a group? A: Because each successive element has an additional electron shell, increasing the distance between the nucleus and outer electrons.
• Q: Which block of the periodic table do transition metals belong to? A: The d-block.

Chapter 9: Group Properties and Periodicity

This chapter looks at three groups of the periodic table in turn. In Group 1, the alkali metals become softer and more reactive down the group, reacting with water to release hydrogen gas and form hydroxides. In Group 17, the halogens exist as diatomic molecules with distinct colors — from pale yellow fluorine to dark grey iodine — and their reactivity and oxidizing power both decrease going down the group, demonstrated through halogen displacement reactions. Group 18’s noble gases are shown to be chemically inert due to their full outer electron shells, and the chapter closes by comparing key physical properties of metals against non-metals.

Important Questions:

• Q: Write the reaction of sodium with water. A: 2Na + 2H2O → 2NaOH + H2, producing sodium hydroxide and hydrogen gas.
• Q: Which hydrogen halide is the most thermally stable, and why? A: HF, because the short, strong H-F bond requires the most energy to break.
• Q: What is a halogen displacement reaction? A: A reaction where a more reactive halogen displaces a less reactive halogen from its compound, e.g., chlorine displacing bromine from sodium bromide.
• Q: Name one physical property where metals and non-metals typically differ. A: Electrical conductivity — metals conduct electricity well, while most non-metals do not (graphite is an exception).

Chapter 10: Environmental Chemistry

Environmental Chemistry identifies the main pollutants found in air — carbon dioxide, carbon monoxide, oxides of nitrogen and sulfur, hydrocarbons, particulates, and ozone — and links their rising levels mostly to fossil fuel combustion. A dedicated section explains acid rain, showing how sulfur dioxide and nitrogen oxides react with water vapor to form acidic rainfall that erodes soil nutrients, harms aquatic ecosystems, and damages monuments such as the Parthenon. The chapter also explains the greenhouse effect behind global warming and closes with strategies to reduce pollution, including tree planting, catalytic converters, desulphurization of flue gases, switching to renewable energy, and monitoring the Air Quality Index.

Important Questions:

• Q: What causes the greenhouse effect? A: Gases like carbon dioxide and methane trap heat radiated from the Earth’s surface, preventing it from escaping into space and warming the planet.
• Q: Give two effects of acid rain on the environment. A: It strips nutrients from soil and harms aquatic life in rivers and lakes; it also damages buildings and monuments.
• Q: Name two strategies used to reduce sulfur dioxide emissions from power plants. A: Using low-sulfur fuel and flue gas desulphurization, which removes sulfur dioxide from the exhaust gases.
• Q: Why is carbon monoxide dangerous to human health? A: It binds to red blood cells and reduces their ability to carry oxygen around the body, which can be fatal in enclosed spaces.

Chapter 11: Hydrocarbons

This chapter defines organic chemistry as the chemistry of carbon compounds, highlighting catenation — carbon’s ability to bond with itself to form chains and rings — as the reason so many organic compounds exist. Alkanes, represented by the formula CnH2n+2, are named using the IUPAC system’s root, suffix, and prefix parts, with worked examples such as naming butane and its branched isomer methylbutane (isobutane). Students also learn three ways to prepare alkanes — cracking larger hydrocarbons, hydrogenating alkenes or alkynes over a nickel catalyst, and reducing alkyl halides with zinc/HCl — and study alkanes’ two characteristic reactions, substitution with halogens under UV light and combustion.

Important Questions:

• Q: Why are alkanes also called saturated hydrocarbons? A: Because all their carbon-carbon and carbon-hydrogen bonds are single bonds, with no room for more atoms to attach.
• Q: What type of reaction occurs when methane reacts with chlorine in sunlight? A: A photochemical substitution reaction, where a hydrogen atom is replaced by a chlorine atom.
• Q: What products form when an alkane undergoes complete combustion? A: Carbon dioxide and water, along with the release of heat energy.
• Q: What catalyst is used to hydrogenate alkenes into alkanes? A: Nickel (Ni), under heat.

Chapter 12: Laboratory and Practical Chemical Skills

The final chapter focuses on practical lab safety, classifying chemical hazards into flammable/explosive substances, corrosive chemicals, and toxic chemicals, with examples and precautions for each. It covers how to read hazard warning signs and symbols on chemical bottles, what personal protective equipment (PPE) — like goggles, gloves, and lab coats — is required for different tasks, and where fire extinguishers and safety showers should be located in a lab. Clear emergency steps are also outlined for responding calmly and safely if something goes wrong during an experiment.

Important Questions:

• Q: What does a hazard warning sign on a chemical bottle indicate? A: It warns users about the specific danger the chemical poses, such as being corrosive, toxic, or flammable, so proper precautions are taken.
• Q: Why should acid always be added to water, and not water to acid? A: Adding water to concentrated acid can cause a violent, heat-releasing reaction that may splash acid; adding acid to water dilutes it more safely.
• Q: What is a fume cupboard used for? A: To safely carry out reactions that release harmful or toxic vapors, keeping them away from the person working.
• Q: List one step to take during a lab fire emergency. A: Turn off gas valves and equipment immediately, then use a fire extinguisher or evacuate if the fire cannot be controlled.

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Download Chemistry Tech Class 9 English Medium PDF

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

⬇ Download PDF (English Medium)

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Who Should Read This

This book is for 9th class Tech stream students studying Chemistry in English medium under Punjab Board. The English medium edition is ideal for students who want to build scientific vocabulary alongside learning Chemistry, especially useful for those planning to continue into technical or science-related 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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