Class 11 NCERT Chemistry Textbook 2026-27 | Free PDF Download

The NCERT Class 11 Chemistry textbook for the 2026-27 session continues to serve as a reliable study material for building a strong foundation in Chemistry. Aligned with CBSE guidelines, it is designed to strengthen conceptual clarity and logical reasoning.

The book covers essential topics such as basic chemical concepts, atomic structure, chemical bonding, thermodynamics, and the fundamentals of organic chemistry. These topics help students build analytical skills and understand how chemistry is applied in real-world situations.

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NCERT Class 11 Chemistry Textbook Part I (2026-27)

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NCERT Class 11 Chemistry Textbook Part II (2026-27)

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NCERT Class 11 Chemistry Overview

The NCERT Class 11 Chemistry book starts with basics like Some Basic Concepts of Chemistry and Structure of Atom, and builds understanding through chapters such as Chemical Bonding and States of Matter.

It further covers key topics like Thermodynamics, Equilibrium, and Organic Chemistry Basics, helping students develop strong concepts for Class 12 and competitive exams like JEE and NEET.

Major Highlights for Chemistry Class 11

The NCERT Class 11 Chemistry book offers several features that make it an essential study resource:

• Based on the latest CBSE syllabus for 2026-27
• Covers physical, inorganic, and organic chemistry basics
• Focuses on concept clarity and numerical application
• Includes solved examples and exercise questions
• Builds foundation for higher studies and competitive exams 

NCERT Chemistry Textbook for Class 11 Chapters

Here is a brief introduction of all chapters included in Class 11 Chemistry syllabus for the 2026-27 session.

Chemistry Part I 

• Chapter 1. Some Basic Concepts of Chemistry: Introduces mole concept, laws of chemical combination, and basic calculations.
• Chapter 2. Structure of Atom: Explains atomic models, quantum numbers, and electron configuration.
• Chapter 3. Classification of Elements and Periodicity in Properties: Covers periodic table trends and element classification.
• Chapter 4. Chemical Bonding and Molecular Structure: Focuses on types of bonds and molecular shapes.
• Chapter 5. Thermodynamics: Covers energy changes, laws of thermodynamics, and heat transfer.
• Chapter 6. Equilibrium: Discusses chemical and ionic equilibrium concepts.

Chemistry Part II

• Chapter 7. Redox Reactions: Explains oxidation-reduction reactions and their applications.
• Chapter 8. Organic Chemistry - Some Basic Principles and Techniques: Covers basic concepts, nomenclature, and purification methods.
• Chapter 9. Hydrocarbons: Explains alkanes, alkenes, alkynes, and aromatic compounds.

Class 11 Chemistry Study Resources 

NCERT Chemistry provides a balanced mix of theory, numericals, and reactions, making it ideal for conceptual clarity.

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Deleted Topics: NCERT Chemistry Class 11 

As per the latest NCERT update, there are no major changes in the Class 11 Chemistry syllabus for the academic session 2026-27. Any other changes or alterations will be seen in the upcoming academic years. 

Most Important Questions from Class 11 Chemistry 

Chapter 1: Some Basic Concepts of Chemistry 

Q1. Calculate the concentration of nitric acid in moles per litre in a sample which has a density,1.41 g mL1 and the mass percent of nitric acid in it being 69%. 

Ans. Given:

Density of solution = 1.41 g per mL

Mass percent of nitric acid = 69 percent

Step 1: Consider 1 litre of solution
1 litre = 1000 mL
Mass of solution = 1.41 multiplied by 1000 = 1410 g

Step 2: Calculate mass of nitric acid
Mass percent = 69 percent
Mass of HNO₃ = 69 by 100 multiplied by 1410
= 972.9 g

Step 3: Convert mass into moles
Molar mass of HNO₃ = 63 g per mol
Number of moles = 972.9 divided by 63
= 15.44 mol

Step 4: Calculate molarity
Molarity = moles per litre
= 15.44 mol per litre

The concentration of nitric acid = 15.44 mol per litre

Q2. How much copper  can be obtained from 100g of copper sulphate (CuSo₄) 

Ans. Given:
Mass of CuSO₄ = 100 g

Step 1: Calculate molar mass of CuSO₄
Cu = 63.5
S = 32
O₄ = 16 multiplied by 4 = 64

Molar mass of CuSO₄ = 63.5 + 32 + 64 = 159.5 g per mol

Step 2: Find moles of CuSO₄
Moles = 100 divided by 159.5
= 0.627 mol

Step 3: Relation between CuSO₄ and Cu
From the formula, 1 mole of CuSO₄ gives 1 mole of Cu

So, moles of Cu = 0.627 mol

Step 4: Convert moles of Cu into mass
Mass = moles multiplied by molar mass of Cu
= 0.627 multiplied by 63.5
= 39.8 g

Amount of copper obtained = 39.8 g

Chapter 4: Chemical Bonding & Molecular Structure 

Q1. Explain the formation of a chemical bond.
Ans.  A chemical bond is defined as an attractive force that holds the constituents (atoms, ions etc.) together in a chemical species. Various theories have been suggested for the formation of chemical bonds such as the electronic theory, valence shell electron pair repulsion theory, valence bond theory, and molecular orbital theory. A chemical bond formation is attributed to the tendency of a system to attain stability.
It was observed that the inertness of noble gases was because of their fully filled outermost orbitals. Hence, it was postulated that the elements having incomplete outermost shells are unstable (reactive). Atoms, therefore, combine with each other and complete their respective octets or duplets to attain the stable configuration of the nearest noble gases. This combination can occur either by sharing of electrons or by transferring one or more electrons from one atom to another. The chemical bond formed as a result of sharing of electrons between atoms is called a covalent bond. An ionic bond is formed as a result of transfer of electrons from one atom to another. 

Q2. Define electronegativity? How does it differ from electron gain enthalpy? 

Ans. Electronegativity is the ability of an atom in a chemical compound to attract a bond pair of electrons towards itself. Electronegativity of any given element is not constant. It varies according to the element to which it is bound. It is not a measurable quantity. It is only a relative number. On the other hand, electron gain enthalpy is the enthalpy change that takes place when an electron is added to a neutral gaseous atom to form an anion. It can be negative or positive depending upon whether the electron is added or removed. An element has a constant value of the electron gain enthalpy that can be measured experimentally. 

Chapter 5: Thermodynamics 

Q1.  In a process, 701 J of heat is absorbed by a system and 394 J of work is done by the system. What is the change in internal energy for the process? 

Ans. Given:
Heat absorbed by system = 701 J
Work done by system = 394 J

 Using First Law of Thermodynamics:
Change in internal energy = Heat supplied − Work done

 Calculation:
Change in internal energy = 701 − 394
= 307 J
The change in internal energy of the system is 307 J.

Q2. For an isolated system, ΔU=0 , what will be ΔS ? 

Ans. ΔS will be positive i.e., greater than zero. Since for an isolated system, ΔU=0 , hence ΔS will be positive and the reaction will be spontaneous. 

Chapter 8: Organic Chemistry: Some Basic Principles & Techniques 

Q1. What are electrophiles and nucleophiles? Explain with examples. 

Ans. An electrophile is a reagent that removes a pair of electrons. In other words, an electrophile (E⁺)  is a reagent that seeks electrons. Electrophiles are electron- deficient and receiver of an electron pair. 

Electrophiles include carbocations and (CH₃ CH⁺²)  functional groups such as the carbonyl group. A reagent that produces an electron pair is known as a nucleophile. A nucleus- seeking reagent is referred to as a nucleophile (Nu:). 

For instance, OH^- , NC^- , carbanions R₃C^- , and so on. 

Because of the presence of a lone pair, neutral molecules such as water and ammonia also serve as nucleophiles. 

Q2. What is the difference between distillation, distillation under reduced pressure and steam distillation? 

Ans.  The difference between distillation, reduced pressure distillation, and stream distillation are shown below. 

• Distillation: It is used to purify chemicals that are related with non-volatile impurities or liquids that do not disintegrate when heated. In other words, distillation is used to separate volatile liquids from nonvolatile contaminants or a mixture of such liquids with significant boiling point difference. This process separates a mixture of fuel and kerosene. 
• Reduced pressure distillation: This procedure is used to purify a liquid that decomposes when heated. Under reduced pressure, the liquid will boil at a lower temperature than its boiling point and so will not decompose. This process is used to purify glycerol. At a temperature of 593 K, it boils with decomposition. It boils at 453 K without breakdown at a lower pressure. 
• Steam distillation: It is used to purify an organic molecule that is steam volatile and water immiscible. The compound is heated by passing steam, and the steam is condensed to water. After some time, the water-liquid mixture begins to boil and flows through the condenser. A separating funnel is then used to separate this condensed mixture of water and liquid. A solution of water and aniline can be separated by this method.

Best Tips to Prepare for Chemistry Class 11 NCERT 

Preparation tips for Class 11 NCERT are given below and can act very effective if used properly: 

• Understand chemical bonding through concepts and visualization: Focus on shapes, hybridisation, and reasoning rather than memorising directly.
• Focus on clarity in thermodynamics: Pay attention to concepts like heat, work, and energy changes to avoid confusion in numericals.
• Build a strong base in organic chemistry: Spend more time on basic concepts before moving to reactions, as this makes later chapters easier.
• Study inorganic chemistry from NCERT carefully: Important lines, trends, and examples are often directly asked in exams.
• Avoid switching between too many topics in one session: Study one type of chemistry at a time for better focus and retention.
• Revise mistakes regularly: Going through incorrect questions helps improve accuracy and understanding.

FAQs 

Q1. How can I improve in Organic Chemistry in Class 11?

Ans. Focus on understanding basic concepts like hybridisation, bond formation, and reaction mechanisms instead of memorising reactions. Practice naming (IUPAC) regularly for better clarity.

Q2. Which chapters require the most numerical practice in Chemistry?

Ans. Chapters like Some Basic Concepts of Chemistry, States of Matter, and Thermodynamics involve extensive numericals and require consistent practice.

Q3. What is the best way to revise Chemistry before exams?

Ans. Revise using short notes, focus on formulas, key reactions, and important concepts, and solve NCERT back questions for quick practice.

Q4. Is Class 11 Chemistry important for Class 12 and competitive exams?

Ans. Yes, Class 11 forms the base for Class 12 topics like organic chemistry, physical chemistry, and inorganic reactions, and is crucial for exams like JEE and NEET.

Q5. How much time should I dedicate to Chemistry daily?
Ans. Ideally, 1-2 hours daily with a mix of theory, numericals, and revision is sufficient for consistent progress.