Chemistry for FSC Part 1 (Class 11) is published by the Punjab Education, Curriculum, Training and Assessment Authority (PECTAA). The 2025–26 edition is based on the Updated/Revised National Curriculum of Pakistan 2023 and covers sixteen chapters, from the Periodic Table and Atomic Structure through to Lab Safety and Practical Skills.
For FSC Part 1 students, Chemistry carries heavy weight in both the board exam and entry tests like MDCAT and ECAT. Each chapter’s summary and short-answer questions here are grounded in the book’s actual content, helping students revise reactions, laws, and numerical concepts quickly before the exam.
Book Overview
| Class | 11 (FSC Part 1 / First Year) |
| Subject | Chemistry |
| Category | FSC |
| Board | Punjab Board (PECTAA, Lahore) |
| Curriculum | NCP 2023 (Updated/Revised) |
| Total Chapters | 16 |
| Format |
Chapter List
Chapter 1: Periodic Table and Periodic Properties
This chapter traces the periodic table’s history from Döbereiner’s triads (1829) and Newlands’ law of octaves (1864) to Mendeleev’s 1869 table arranged by atomic mass, and Moseley’s 1913 correction arranging elements by atomic number instead. It covers the modern table’s 118 elements across 7 periods and 18 groups, and the “stair-step line” from boron to polonium that separates metals, metalloids, and nonmetals.
Important Questions:
- Who is considered the father of the Periodic Table, and what did he do? Dmitri Mendeleev, who in 1869 arranged 63 elements by increasing atomic mass and left gaps for undiscovered elements, correctly predicting their properties.
- What correction did Moseley make to Mendeleev’s table in 1913? He used X-ray emission to determine exact atomic numbers and rearranged elements by atomic number instead of atomic mass, fixing earlier discrepancies.
- How many periods and groups does the modern periodic table have? Seven horizontal periods and eighteen vertical groups.
- Where are metalloids positioned in the periodic table? Along the “stair-step line” running from boron (B) to polonium (Po), where they show properties of both metals and nonmetals.
Chapter 2: Atomic Structure
This chapter explains atomic number (Z), mass number (A), and how the number of neutrons is found using N = A − Z, based on Moseley’s 1913 discovery that atomic number is a fundamental property of an element. It covers quantum numbers, electron configuration rules (Aufbau principle, Pauli’s exclusion principle, Hund’s rule), and the shapes of s, p, and d orbitals.
Important Questions:
- How is the number of neutrons in an atom calculated? N = A − Z, where A is the mass number and Z is the atomic number.
- What did Moseley discover about atomic number in 1913? That the square root of the frequency of X-rays produced when elements are bombarded with cathode rays is directly proportional to the atomic number Z, making Z a fundamental property of an element.
- What three rules govern how electrons fill orbitals? The Aufbau principle, Pauli’s exclusion principle, and Hund’s rule.
- How many protons, neutrons, and electrons does the Al³⁺ ion have (from ²⁷₁₁Al)? 13 protons, 14 neutrons, and 10 electrons (13 minus 3 lost electrons).
Chapter 3: Chemical Bonding
This chapter explains ionic bonding (using the Na⁺ and Cl⁻ example), covalent bonding (like the Cl–Cl bond), and dative/coordinate covalent bonds (like H₃O⁺ formation), all based on the Lewis theory that atoms bond to achieve noble-gas-like configurations. It covers VSEPR theory for molecular shapes, hybridization (sp, sp², sp³), molecular orbital theory, van der Waals forces, and hydrogen bonding.
Important Questions:
- How is an ionic bond formed, using Na and Cl as an example? Na (2,8,1) loses its outermost electron to form Na⁺ (2,8), while Cl (2,8,7) gains that electron to form Cl⁻ (2,8,8); the oppositely charged ions are held together by ionic bonding.
- What is a dative (coordinate covalent) bond? A bond formed when the shared pair of electrons is donated entirely by one of the bonding atoms, as when oxygen in H₂O donates a lone pair to H⁺ to form H₃O⁺.
- What does VSEPR theory predict? The shapes and bond angles of molecules, based on the repulsion between electron pairs around a central atom.
- Define electronegativity. The power of an atom to attract electrons to itself within a bond.
Chapter 4: Stoichiometry
This chapter introduces the mole concept, based on Avogadro’s number (6.02 × 10²³, named after Amedeo Avogadro), and shows how to calculate molar mass and number of moles using n = m/M. It covers balanced equations, limiting reagents, and theoretical, actual, and percentage yield calculations, following the law of conservation of mass and the law of definite proportions.
Important Questions:
- What is Avogadro’s number, and who is it named after? 6.02 × 10²³, the number of entities in one mole of a substance, named after Italian scientist Amedeo Avogadro (1776–1856).
- What is the formula for calculating the number of moles? n = m/M, where m is the given mass and M is the molar mass.
- What does the law of conservation of mass state? That matter (mass) can neither be created nor destroyed — the total mass of reactants equals the total mass of products in a balanced equation.
- What is a limiting reagent? The reactant that is completely consumed first in a reaction, limiting the maximum amount of product that can form.
Chapter 5: States and Phases of Matter
This chapter explains the ideal gas equation PV = nRT, derived by combining Boyle’s, Charles’, and Avogadro’s laws, along with the kinetic molecular theory that explains gas pressure as molecular collisions with container walls. It covers liquid properties like viscosity, surface tension, and vapour pressure — including how hydrogen bonding gives water its unusually high boiling point and surface tension — and the difference between amorphous and crystalline solids.
Important Questions:
- What is the ideal gas equation? PV = nRT, where R is the ideal gas constant (0.0821 atm dm³ K⁻¹ mol⁻¹).
- Why does pressure exist in a gas, according to kinetic molecular theory? Because gas molecules constantly collide with the walls of their container.
- How does hydrogen bonding affect water’s properties? It gives water an unusually high boiling point, high surface tension, high specific heat, and high heat of vaporization compared to similar-sized molecules.
- What is the key difference between amorphous and crystalline solids? Crystalline solids have a definite, ordered geometric shape and sharp melting point, while amorphous solids lack a regular internal structure.
Chapter 6: Chemical Energetics
This chapter defines enthalpy change (ΔH) as the heat evolved or absorbed during a reaction, distinguishing exothermic (ΔH negative) from endothermic (ΔH positive) processes. It covers Hess’s Law for calculating enthalpy changes across multiple steps, Born-Haber cycles for ionic solids, lattice energy, entropy, and Gibbs free energy.
Important Questions:
- What is the difference between an exothermic and an endothermic process? An exothermic process releases heat to the surroundings (ΔH negative); an endothermic process absorbs heat from the surroundings (ΔH positive).
- What does Hess’s Law allow chemists to do? Calculate the enthalpy change of a reaction carried out in multiple steps by adding up the enthalpy changes of each step.
- What is entropy? The number of possible arrangements of particles and their energy in a given system, denoted S.
- What is a Born-Haber cycle used for? To calculate the lattice energy of an ionic solid using a cycle of known enthalpy changes.
Chapter 7: Reaction Kinetics
This chapter introduces collision theory, which explains that reactions occur only when particles collide with enough energy (activation energy) and proper orientation. It covers the rate of reaction as change in concentration over time, the effect of temperature via the Boltzmann distribution, and how catalysts speed up reactions by lowering activation energy.
Important Questions:
- What is activation energy? The minimum amount of energy required for an effective collision between reacting particles.
- How is the rate of reaction defined? The change in concentration of a reactant or product divided by the time taken for that change.
- How do catalysts increase reaction rate? By lowering the activation energy needed for the reaction to proceed.
- Give an example each of a very fast and a very slow reaction. The reaction of NaCl with AgNO₃ is very fast; the rusting of iron is a slow process.
Chapter 8: Chemical Equilibrium
This chapter distinguishes irreversible reactions from reversible ones that reach chemical equilibrium, where forward and reverse reaction rates become equal and concentrations stay constant. It covers equilibrium constants (Kc, Kp), Le Chatelier’s Principle, and its industrial applications in the Haber process (ammonia) and the Contact process (sulfuric acid).
Important Questions:
- What is dynamic equilibrium? A state where the forward and reverse reaction rates are equal, so the concentrations of reactants and products remain constant, even though the reaction never actually stops at the molecular level.
- What does Le Chatelier’s Principle state? That when a system at equilibrium is disturbed (by changes in concentration, pressure, or temperature), it shifts to counteract that disturbance and restore equilibrium.
- Give an industrial example where Le Chatelier’s Principle is applied. The Haber process for manufacturing ammonia, and the Contact process for manufacturing sulfuric acid.
- What are macroscopic events, and give an example. Phenomena observable with the naked eye, such as a colour change or the formation of a precipitate.
Chapter 9: Acid-Base Chemistry
This chapter explains the Bronsted-Lowry concept (developed in 1923 by Danish chemist J.N. Bronsted and English chemist T.M. Lowry), where an acid donates a proton and a base accepts it, forming conjugate acid-base pairs. It covers pH, Ka, buffer solutions, the solubility product (Ksp), salt hydrolysis, and how to select indicators for acid-base titrations.
Important Questions:
- Who developed the Bronsted-Lowry concept, and when? Danish chemist J.N. Bronsted and English chemist T.M. Lowry, independently, in 1923.
- According to Bronsted-Lowry theory, what is an acid and what is a base? An acid is a species that donates a proton in a proton-transfer reaction; a base is a species that accepts the proton.
- Why is water called amphoteric? Because it can act as either an acid or a base depending on the other reactant — for example, it acts as a base with HCl but as an acid with NH₃.
- What common household bases treat stomach acidity? Baking soda (NaHCO₃), milk of magnesia (Mg(OH)₂), and aluminum hydroxide (Al(OH)₃).
Chapter 10: Electrochemistry
This chapter defines oxidation as loss of electrons and reduction as gain of electrons, together forming redox reactions, and explains how electrolytic cells convert electrical energy into chemical energy. It covers standard electrode potentials measured against the standard hydrogen electrode, galvanic (voltaic) cells like the Cu-Zn cell, and the Nernst equation for predicting electrode potentials at different ion concentrations.
Important Questions:
- What is oxidation, and what is reduction? Oxidation is the loss of one or more electrons; reduction is the gain of one or more electrons.
- What happens at the anode and cathode in an electrolytic cell? Oxidation occurs at the anode, and reduction occurs at the cathode.
- Give an example of a galvanic cell discussed in this chapter. The Cu-Zn galvanic cell, which converts chemical energy from a spontaneous redox reaction into electrical energy.
- Name two everyday redox reactions mentioned in the chapter. Photosynthesis and respiration.
Chapter 11: Hydrocarbons
This chapter divides hydrocarbons into aliphatic (alkanes, cycloalkanes, alkenes, alkynes) and aromatic (benzene-based) classes, and explains alkane nomenclature using the homologous series from methane to decane. It covers alkene structure and reactivity — hydrogenation, halogenation, hydration, and polymerization — along with isomerism and the electrophilic addition mechanism explained through Markovnikov’s rule.
Important Questions:
- What is the general formula for alkanes? CₙH₂ₙ₊₂, with methane (CH₄) as the simplest member.
- What distinguishes aromatic hydrocarbons from aliphatic ones? Aromatic hydrocarbons are cyclic, based on benzene (C₆H₆) or similar compounds, with a high carbon-to-hydrogen ratio; aliphatic hydrocarbons are not aromatic and can be open-chain or cyclic.
- Where does the word “aromatic” come from? The Greek word “aroma,” meaning fragrance, since early aromatic compounds had characteristic odours.
- Name two practical uses of alkanes mentioned in the chapter. Butane is used as fuel in lighters; isobutane is used as a propellant in products like shaving gel.
Chapter 12: Nitrogen and Sulfur
This chapter explains why nitrogen (N₂) is so unreactive — its strong, nonpolar triple bond has a bond enthalpy of +944 kJ/mol — and covers ammonia’s industrial production through the Haber-Bosch process and its basicity as a Bronsted-Lowry base. It also covers sulfur’s variable oxidation states and the properties, production, and industrial uses of sulfuric acid.
Important Questions:
- Why is nitrogen gas (N₂) so unreactive? Because of its strong, nonpolar triple bond with a bond enthalpy of +944 kJ/mol, which requires very high energy to break.
- How is ammonia produced industrially? Through the Haber-Bosch process, reacting N₂ and H₂ under appropriate conditions.
- Why is nitrogen used as a protective blanket for hydrocarbon shipments? Because it is inert and prevents the cargo from reacting with oxygen and moisture.
- How does ammonia behave as a Bronsted-Lowry base? It accepts a proton (H⁺) from an acid to form the ammonium ion (NH₄⁺).
Chapter 13: Halogens
This chapter covers Group 17 elements — fluorine, chlorine, bromine, and iodine — their distinct colours (pale yellow, greenish yellow, reddish-brown, and greyish black), and the trend of decreasing volatility from chlorine to iodine due to increasing London dispersion forces. It explains halide ion tests using silver nitrate, and chlorine’s role in water purification through the formation of HOCl and ClO⁻, which kill bacteria.
Important Questions:
- Where does the word “halogen” come from? The Greek words “halos” (salt) and “gen” (to make), since halogens readily form salts.
- Which halogen was first isolated and recognized as an element? Chlorine.
- How does volatility change from chlorine to iodine, and why? Volatility decreases from chlorine to iodine due to increasing molecular mass and stronger London dispersion forces.
- How does chlorine purify water? It forms active species HOCl and ClO⁻, which kill bacteria in the water.
Chapter 14: Atmosphere
This chapter describes the atmosphere’s composition — mainly nitrogen (78%) and oxygen (21%) — and its four layers: the troposphere (weather events, up to 12 km), stratosphere (containing the ozone layer, 12–50 km), mesosphere (coldest layer, 50–80 km), and thermosphere (hottest layer, 80–600 km). It covers primary and secondary air pollutants, and processes like smog formation, acid rain, and the greenhouse effect.
Important Questions:
- What are the two major components of the atmosphere? Nitrogen (78.00%) and oxygen (21.01%).
- Which atmospheric layer contains the ozone layer? The stratosphere, which extends 12–50 km above the Earth’s surface.
- Which is the coldest layer of the atmosphere? The mesosphere, where temperature drops to about −93°C.
- What is the difference between primary and secondary air pollutants? Primary pollutants are directly emitted (like volcanic ash or vehicle exhaust CO); secondary pollutants form later through chemical reactions of primary pollutants.
Chapter 15: Basic Separation Techniques
This chapter covers five physical methods for separating mixtures — filtration, crystallization, simple distillation, fractional distillation, and paper chromatography — explaining key terms like solute, solvent, solution, residue, and filtrate along the way. It also explains how the Rf value is used to identify unknown substances by comparing them with known substances in paper chromatography.
Important Questions:
- Name the five separation methods covered in this chapter. Filtration, crystallization, simple distillation, fractional distillation, and paper chromatography.
- In a solution of salt and water, which is the solute and which is the solvent? Salt is the solute; water is the solvent, since it is present in excess.
- What is filtration used for? Separating an insoluble solid component from a liquid in a heterogeneous mixture.
- What does the Rf value help determine in paper chromatography? It helps identify unknown substances by comparing their movement on chromatography paper with known substances.
Chapter 16: Lab Safety and Practical Skills
This practical chapter covers general lab safety rules — wearing lab coats and safety goggles, never working alone, and never tasting or smelling chemicals — along with the three categories of lab hazards: physical, chemical, and biological. It also covers proper chemical waste disposal following EPA regulations, acid-base titration technique using a burette and indicator, and qualitative tests for identifying common anions and cations.
Important Questions:
- What are the three categories of lab hazards covered in this chapter? Physical, chemical, and biological hazards.
- Name two basic safety rules students must follow in the lab. Always wear a lab coat and safety goggles, and never work alone in the lab without an instructor present.
- Why shouldn’t chemical waste be poured down the drain? It must follow proper disposal rules set by the Environmental Protection Agency (EPA) to avoid environmental harm.
- What equipment is used in an acid-base titration? A burette, a volumetric pipette, and a suitable indicator to identify the end point.
Download Chemistry Class 11 Book PDF
Two editions are available below. Click the button for the edition you need — each opens in a new tab and is ready to read or save on any device.
2025–26 Edition (NCP 2023 — PECTAA)
⬇ Download PDF (2025–26)E-Learn Punjab Edition
⬇ Download PDF (E-Learn Punjab)Who Should Read This
This book is for FSC Part 1 (First Year) science students preparing for the Punjab Board annual exam. It is also essential for students planning for MDCAT and ECAT, as Chemistry from Class 11 is heavily tested in both entry tests. Topics like atomic structure, stoichiometry, equilibrium, acid-base chemistry, and hydrocarbons are directly part of the MDCAT and ECAT syllabus.
Applicable Boards
This textbook is published by PECTAA and is used in Punjab Board colleges. Students from the Federal Board (FBISE) and AJK Board can also use it for reference, as the FSC Chemistry syllabus is largely the same across these boards. Students from Sindh and KPK boards will also find most chapters relevant.
FAQs
Is this the latest Chemistry book for FSC Part 1 Punjab Board?
Yes. The 2025–26 edition is the latest, published by PECTAA and based on the Updated/Revised National Curriculum of Pakistan 2023.
How many chapters are in Chemistry Class 11?
There are 16 chapters, from Periodic Table and Periodic Properties to Lab Safety and Practical Skills.
Is this book helpful for MDCAT and ECAT preparation?
Yes. Chemistry from FSC Part 1 is a major part of both MDCAT and ECAT. Topics like atomic structure, stoichiometry, chemical bonding, equilibrium, and electrochemistry are directly tested.
What is the difference between the 2025-26 and E-Learn Punjab editions?
Both follow the same NCP 2023 curriculum. The E-Learn Punjab edition is the digital version from the Punjab government’s e-learning platform. The 2025–26 edition is the latest printed version approved by PECTAA.
Can Federal Board students use this book?
Yes. The FSC Chemistry syllabus is very similar for Punjab and Federal boards. Federal Board students can use this book for additional practice and reference.
Is the PDF free to download?
Yes. Both editions of the Chemistry Class 11 book PDF are completely free to download and read on any device.
Related Books
- Chemistry 2nd Year FSC Book
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- Mathematics 1st Year FSC Book
- English 2nd Year FSC Book
- English Grammar & Composition 2nd Year FSC Book
Study Resources for Chemistry 1st Year
Free exam-preparation resources for Chemistry 1st Year from the Freebooks.pk Editorial Team — chapter-wise notes (definitions, short & long questions and MCQs), the latest paper pairing scheme. Study online or download.