Download NCERT Chemistry Textbook for Class 11 PDF: Updated for 2020-21
Class 11 Chemistry NCERT Book PDF Download 2020-21
Chemistry is one of the most important subjects for students who aspire to pursue a career in science, engineering, medicine, or pharmacy. It is also a fascinating subject that deals with the composition, structure, properties, and reactions of matter. To master chemistry, one needs to have a clear understanding of the basic concepts, principles, and techniques.
One of the best sources of learning chemistry is the NCERT book for class 11 chemistry. NCERT stands for National Council of Educational Research and Training, which is an autonomous organization that publishes textbooks for all subjects from classes 1 to 12. These textbooks are based on the latest syllabus prescribed by CBSE (Central Board of Secondary Education) and follow a simple, lucid, and engaging style of writing.
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If you are looking for a PDF version of the class 11 chemistry NCERT book, you can download it from to read online or download any NCERT book for any class or subject.
Chapter-wise Summary of Class 11 Chemistry NCERT Book
Chapter 1: Some Basic Concepts of Chemistry
This chapter introduces you to some fundamental concepts of chemistry such as laws of chemical combination, Dalton's atomic theory, mole concept, stoichiometry, empirical and molecular formulae, chemical reactions, etc. You will learn how to:
Define chemistry and its scope.
State and apply various laws of chemical combination.
Explain Dalton's atomic theory and its limitations.
Differentiate between atoms and molecules.
Calculate atomic and molecular masses Define and use the concept of mole and molar mass.
Perform calculations involving percentage composition and empirical and molecular formulae.
Balance chemical equations using the law of conservation of mass.
Classify chemical reactions based on different criteria.
Chapter 2: Structure of Atom
This chapter deals with the structure of atom and the various models and experiments that led to its discovery. You will learn how to:
Describe the salient features of Thomson's, Rutherford's, and Bohr's models of atom.
Explain the limitations and drawbacks of these models.
State the postulates of quantum mechanical model of atom.
Define and use the terms such as orbitals, quantum numbers, shapes, and orientations of orbitals.
Write the electronic configuration of atoms using the aufbau principle, Pauli's exclusion principle, and Hund's rule of maximum multiplicity.
Differentiate between isotopes, isobars, and isotones.
Chapter 3: Classification of Elements and Periodicity in Properties
This chapter covers the classification of elements based on their properties and periodic trends. You will learn how to:
Explain the historical development of periodic table by Dobereiner, Newlands, Mendeleev, and Moseley.
State the modern periodic law and describe the salient features of the modern periodic table.
Define and use the terms such as atomic number, atomic radius, ionization energy, electron affinity, electronegativity, valency, etc.
Predict the periodic trends in these properties across periods and groups.
Relate these properties with the electronic configuration of elements.
Identify and explain the anomalies and exceptions in these trends.
Chapter 4: Chemical Bonding and Molecular Structure
This chapter explains the concept of chemical bonding and molecular structure. You will learn how to:
Define chemical bond and its types such as ionic, covalent, coordinate, metallic, hydrogen, etc.
Explain the formation of ionic bond using electrostatic force, lattice energy, solvation energy, etc.
Explain the formation of covalent bond using Lewis dot structure, valence bond theory, hybridization, etc.
Predict the shape and polarity of molecules using VSEPR theory and dipole moment.
Explain the formation of coordinate bond using examples.
Describe the characteristics of metallic bond using electron sea model, band theory, etc.
Explain the formation and properties of hydrogen bond using examples.
Chapter 5: States of Matter
This chapter discusses the three states of matter: solid, liquid, and gas. You will learn how to:
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Differentiate between solid, liquid, and gas based on their intermolecular forces, shape, volume, density, etc.
Classify solids into crystalline and amorphous based on their structure and properties.
Determine the type of unit cell and calculate the number of atoms per unit cell in different types of cubic crystals.
Define and use the terms such as close packing, packing efficiency, coordination number, etc. in relation to solids.
Explain the kinetic molecular theory of gases and derive various gas laws from it.
Solve numerical problems involving ideal gas equation (PV = nRT).
Distinguish between ideal and real gases based on their deviation from ideal behavior at high pressure and low temperature.
Chapter 6: Thermodynamics
This chapter introduces you to thermodynamics which is the study of energy changes in physical and chemical processes. You will learn how to:
Define thermodynamics and its various terms such as system, surroundings, boundary, state variables, state functions, etc.
Differentiate between open, closed, and isolated systems based on their exchange of matter and energy with surroundings.
Differentiate between intensive and extensive properties based on their dependence on mass or amount of substance.
Differentiate between isothermal, adiabatic, isobaric, isochoric processes based on their change in temperature or pressure or volume or heat transfer.
State and apply the first law of thermodynamics which relates heat change (q), work done (w), and internal energy change (ΔU) in a system.
Solve numerical problems involving heat capacity (C ), specific heat capacity (Cs), molar heat capacity (Cm), etc.
Define and calculate enthalpy change (ΔH) for various types of reactions such as formation, combustion, neutralization, etc.
State and apply Hess's law of constant heat summation to calculate the enthalpy change of a reaction using the enthalpy changes of other related reactions.
Explain the concept of spontaneity and non-spontaneity of a process using the second law of thermodynamics.
Define and calculate entropy change (ΔS) for a system and its surroundings.
Define and calculate Gibbs free energy change (ΔG) for a process and relate it with the spontaneity, equilibrium, and feasibility of the process.
Chapter 7: Equilibrium
This chapter deals with the concept of equilibrium in physical and chemical processes. You will learn how to:
Define equilibrium and its characteristics such as dynamic nature, reversibility, constancy of observable properties, etc.
Differentiate between homogeneous and heterogeneous equilibrium based on the phases of reactants and products involved.
Differentiate between physical and chemical equilibrium based on the nature of change involved.
State and apply the law of mass action and the law of chemical equilibrium to express the equilibrium constant (Kc) for a given reaction.
Relate the equilibrium constant with the extent of reaction and the direction of reaction.
Solve numerical problems involving the calculation of equilibrium constant, concentration, pressure, degree of dissociation, etc. for various reactions.
Explain the effect of temperature, pressure, concentration, and catalyst on the equilibrium position and equilibrium constant using Le Chatelier's principle.
Define and use the terms such as acid, base, salt, pH, pOH, etc. in relation to aqueous solutions.
State and apply the ionization constant of water (Kw) to calculate the concentration of H and OH ions in a solution.
State and apply the ionization constant of weak acids (Ka) and weak bases (Kb) to calculate the degree of ionization and pH of their solut