Talk to Our counsellor: Give a missed call +91 9513850450

NCERT Solutions For Class 11 Chemistry

NCERT Solutions for Class 11 Chemistry is prepared by experts of Physics Wallah. It consists of detail explanation of all the questions asked in NCERT class 11 Chemistry textbook. Theoretical questions are explained with proper use of example and numerical are solved with all required detail steps. Chemistry has been one of the most important subjects in class 11th.

Students looking forward to enhancing their chemistry knowledge can be very effective through NCERT solutions for class 11 chemistry. The team at Physics Wallah comprises of experts with years of experience. We are already acquainted with the appropriate guidelines and parameters that affect student’s marks. The complete NCERT solutions for class 11 chemistry are presented in very systemic and simple solutions.

Chemistry, in general, is a very interesting subject. Whereas many students find it difficult to comprehend. There comes the team of Physics Wallah to resolve the complete problems of students. Students looking forward to enhancing their career must deeply study NCERT Solutions for class 11 chemistry.

Chapter-wise NCERT Solutions for Class 11 Chemistry 

  • Chapter 1 - Some Basic Concepts of Chemistry
  • Chapter 2 - Structure of Atom
  • Chapter 3 - Classication of Elements and Periodicity in Properties
  • Chapter 4 - Chemical Bonding and Molecular Structure
  • Chapter 5 - States of Matter
  • Chapter 6 - Thermodynamics
  • Chapter 7 - Equilibrium
  • Chapter 8 - Redox Reactions
  • Chapter 9 - Hydrogen
  • Chapter 10 - The s-Block Elements
  • Chapter 11 - The p-Block Elements
  • Chapter 12 - Organic Chemistry - Some Basic Principles and Techniques
  • Chapter 13 - Hydrocarbons
  • Chapter 14 - Environmental Chemistry

Why NCERT Solutions for Class 11 Chemistry are important?

It is already known how typical NCERT books are. Many times students are unable to comprehend the language and topics mentioned. Easy solutions and notes which can completely resolve this issue, is none other than Physics Wallah solutions.

We have bifurcated the complete solution into many segments. The NCERT solutions for class 11 chemistry are prepared in the neat, concise and easy readable study material. Students should not fear in any aspect of reading chemistry.

In general NCERT solutions for class 11 chemistry helps students to strengthen their basics. It is crucial for students to crack many of the national level entrance examinations. Whereas Physics Wallah through NCERT solutions for class 11 chemistry helps students to strengthen their logical understanding of the subject.

The complete set of NCERT solutions for class 11 chemistry are prepared under the guidance of experts. The sole aim of creating this study material is to ensure students do not miss any topic. We have formulated NCERT solutions for class 11 chemistry as per latest syllabus of NCERT.

It is necessary for students to adopt a problem-solving approach. The faculties at Physics Wallah has years of experience.

How to Study NCERT solutions for Class 11 Chemistry effectively?

We have trained students to adopt a unique strategy to solve critical questions. We have gone through the number of previous year question papers. In general NCERT books comprises of various unnecessary things.

These things are many times not useful for examinations. Students looking forward to scoring top marks in their examination can always rely upon us.

The complete NCERT solutions for class 11 chemistry are designed in a very concise and simple manner. It is necessary for students to thoroughly go through solutions to clear their doubts. The complete set has been bifurcated into various segments. You can find complete NCERT solutions for class 11 chemistry divided into the number of chapters.

Why Physics Wallah is best for NCERT Solutions for class 11 chemistry?

Since our team deeply believes in serving education to the needy. We have provided NCERT solutions for class 11 chemistry for free on our website. All you need to do is to sign up with us.

Students receiving chemistry solutions can completely rely upon this. Since it is regularly checked for any type of flaws.

The NCERT solutions for class 11 chemistry are the optimum source to revise the complete syllabus. Stringent guidance has been laid to prepare this study material. Study from subject experts by downloading NCERT Solutions for class 11 chemistry.

How to approach Physical chemistry to enhanced your learning

Physical chemistry in class 11  need two thinks one is understating the concept and its applications and second is numerical practising .Start the topic with NCERT book read the theory if required take the help of reference books.Read the theory from Physics Wallah class chemistry sections.

When you feel you have understood the chapter make the mind map of the chapter which consist of all important formula used in the chapters. Proceed to solve the NCERT exercise and take help from NCERT Solutions for Class 11 Chemistry. To solve subjective problem you can refer R.C.Mukherjee or P.Bhadur both are good books for numerical.

Start solving the solve questions take the help of solutions and then move to unsolved questions. Physics Wallah provided a free resource of physical chemistry solve the objective and subject questions from Physics Wallah to have better understanding of the chapter you can also go for chapter wise online test for physical chemistry.

How to approach Organic chemistry enhanced your learning

Chemistry in class 11 generally starts from the month of November. Start organic chemistry in class 11. One must have clear concept of chemical read the chemical bonding chapter revise it carefully before moving to organic chemistry.

NCERT books theory part of organic chemistry is awesome so read it carefully make your own notes and solve all questions of exercise and take help from NCERT Solutions for Class 11 Chemistry.Organic chemistry require thinking of how not with why so always try to find out the answer of how not why.

Take the help of reference book to enhanced your learning I.L. Finar vol-1 is good book for theory. Make you own notes do general organic chemistry very carefully understand the concept of inducting effect resonance and hyperconjugations start learning how to apply these concept in questions.

NCERT questions are good solve it by yourself make a short notes on important points. To help you while solving questions of exercise given in NCERT we have prepared detail step by step explanation of NCERT Solutions.

How to approach Inorganic chemistry enhanced your learning

Inorganic chemistry generally fail to create the interest of the students because of the absence of logical reasoning so it must be takes an it’s a subject which require information’s and facts. Notes play a key role to have good understanding of inorganic chemistry NCERT is best available book for inorganic chemistry.

Start with periodic table and s-block elements prepared your own notes solve the questions of NCERT book and take the help NCERT solutions for Class 11 Chemistry.For reference use J.D.Lee.

  • Chapter 1: Some Basic Concepts of Chemistry

Law of chemical combination, Atomic & molecular mass, Mole concept, Determination of molecular formulae, Stoichiometry, Concentration terms.There are a large number of objects around us which we can see and feel. Anything that occupies space and has mass is called matter.

Ancient Indian and Greek philosopher’s believed that the wide variety of object around us are made from combination of five basic elements: Earth, Fire, Water, Air and Sky. The Indian philosopher Kanad (600 BC) was of the view that matter was composed of very small, indivisible particle called “parmanus”.

Ancient Greek philosopher also believed that all matter was composed of tiny building blocks which were hard and indivisible. The Greek philosopher Domocritus named these building blocks as atoms, meaning indivisible. All these people had their philosophical views about matter, these views were never put to experimental test. It was John Dalton who firstly developed a theory on the structure of matter, latter on which was known as Dalton’s atomic theory.

  • Chapter 2: Structure of Atom

Development of structure of Atom and historical Models; Spectrum of hydrogen atom; Bohr model; de Broglie relation, Uncertainty principle, Quantum model; Electronic configuration of elements (upto to atomic number 36); Aufbau principle, Pauli’s exclusion principle and Hund’s rule; shapes of s, p, and d orbitals; Probability Density Curves (Radial and Angular). You will learn the following sub topic in this chapter

  1. Introduction, Dalton’s theory, Discharge tube experiment, Miliken oil drop, Rutherford scattering.
  2. Basic terms of Waves & Circular motion, Electromagnetic spectrum, Planck’s Quantum theory.
  3. Limitation of Rutherford Model, Basic Coloumb’s Law, Bohr’s Model derivation of V,R,E.
  4. Calculation and problems of Bohr Model & Atomic Spectrum.
  5. De-Broglie Hypothesis, Uncertainty principle, Photoelectric Effect.
  6. Drawbacks of Bohr’s Model, Introduction of Quantum Model, Quantum Number.
  7. Shape of orbitals, Probability distribution, Nodes.
  8. Electronic Configuration & Magnetic Properties.
  • Chapter 3: Classification of Elements and Periodicity in Properties

Periodic properties of elements: classification of elements into s, p, d and f block; periodicity in properties with respect to atomic and ionic radii, ionization energy, electron affinity electronegativity, oxidation state, metallic and non-metallic character and trends in reactivity.You will learn the following sub topics in this chapter

  1. Periodic Table & Introduction of different blocks, Shielding Effect.
  2. Atomic, ionic size, Ionisation Energy,
  3. Electron Affinity, Electronegativity, Acidic basic strength, Hydration Energy.
  4. Oxidation states & Redox Balancing.
  5. Definition of Equivalent mass and n-factors, Law of Equivalence, Normality
  • Chapter 4: Chemical Bonding and Molecular Structure

Orbital overlap and covalent bond; Hybridisation involving s, p and d orbitals only; Orbital energy diagrams for homonuclear diatomic species;  Hydrogen bond; Polarity in molecules, dipole moment (qualitative aspects only); VSEPR model and shapes of molecules (linear, angular, triangular, square planar, pyramidal, square pyramidal, trigonal bipyramidal, tetrahedral and octahedral).

Chemical Bond is the physical process responsible for the attractive interactions between atoms and molecules, and that which confers stability to diatomic and polyatomic chemical compounds. The explanation of the attractive forces is a complex area that is described by the laws of quantum electrodynamics.

In general, strong chemical bonding is associated with the sharing or transfer of electrons between the participating atoms.The study on the “nature of forces that hold or bind atoms together to form a molecule” is required to gain knowledge of the following

  1. To know about how atoms of same element form different compounds combining with different elements.
  2. To know why particular shapes are adopted by molecules.
  3. To understand the specific properties of molecules or ions and the relation between the specific type of bonding in the molecules.
  • Chapter 5: States of Matter

Absolute scale of temperature, ideal gas equation; Deviation from ideality, van der Waals equation.Kinetic theory of gases, average, root mean square and most probable velocities and their relation with temperature; Law of partial pressures; Vapour pressure; Diffusion of gases.

The various kinds of substance that make up matter can be divided roughly into three categories, namely, gases, liquids and solids. These are called as three states of matter. These states can be considered to arise as a result of competition between two opposing molecular forces, namely, the force of attraction which tends to hold the molecules together, and the disruptive force due to the thermal energy of molecules.

If the disruptive forces due to thermal energy are much greater than the forces of attraction, then we have matter in its gaseous state. Molecules in the gaseous state move with very large speeds and the forces of attraction amongst them are not sufficient to bind the molecules at one place, with the result that the molecules move practically independent of one another. Because of this feature, gases are characterized by marked sensitivity of volume change with change of temperature and pressure.

There exists no boundary surface and, therefore, gases tend to fill completely any available space, i.e. they do not possess a fixed volume. If the forces of attraction are greater than the disruptive forces due to thermal energy, we have matter in the liquid state. Molecules in the liquid state too have kinetic energy but they cannot go very far away because of the larger forces of attraction amongst them.

Due to this feature, liquids have definite volume, but they do not have definite shape. They take the shape of the vessel in which they are placed. In general, liquids are denser and less compressible than gases. If the forces of attraction between molecules are much greater than the disruptive forces due to thermal energy, the positions of the molecules remain fixed and we have the solid state of matter.

The molecules in the solid state, therefore, do not possess any translational energy, but have only vibrational energy since they can vibrate about their mean positions. Extremely large forces of attraction exist amongst them. That is why solids differ markedly from liquids and gases in respect of size, shape and volume. Solids, in general, have definite size, shape and volume.

  • Chapter 6: Thermodynamics

First law of thermodynamics; Internal energy, work and heat, pressure-volume work; Enthalpy, Hess's law; Heat of reaction, fusion and vapourization. Second law of thermodynamics; Entropy; Free energy; Criterion of spontaneity. The term ‘thermodynamics’ implies flow of heat. Thermodynamics deals with energy changes associated with all types of physical and chemical processes.

Thermodynamics is based on three important generalizations called first, second and third laws of thermodynamics. All the laws of thermodynamics are based on human experience. There is no formal proof for any of these laws. But nothing contrary to these laws has been known to happen whenever we consider the behaviour of matter in bulk.

Thermodynamics helps us to predict whether a given process or a chemical reaction is feasible under given conditions temperature, pressure and concentration. Thermodynamics does not tell anything about the rate at which a given process may proceed.

  • Chapter 7: Equilibrium

Law of mass action; equilibrium constant; exothermic and endothermic reactions; Le Chatelier’s Principle and its applications - It is an experimental fact that most of the process including chemical reactions, when carried out in a closed vessel, do not go to completion.

Under these conditions, a process starts by itself or by initiation, continues for some time at diminishing rate and ultimately appears to stop. The reactants may still be present but they do not appear to change into products any more.

A reaction is said to be reversible if the composition of reaction mixture on the approach of equilibrium at a given temperature is the same irrespective of the initial state of the system, i.e. irrespective of the fact whether we start with reactants or the products.

  • Chapter 8: Redox Reactions

Those reactions in which the process of reduction and oxidation takes place simultaneously are called redox reaction. Electronic concept-Loss of electrons is oxidation while gain of electrons is known as reduction. You will learn how to balance the redox reaction by two methods.

  • Chapter 9: Hydrogen

Hydrogen is the first element in the periodic table and is also the lightest element known. Its atomic form exists only at high temperatures. In the normal element form, it exists as a diatomic molecule, i.e. . Position of Hydrogen in the Periodic Table.Hydrogen, the first element in the periodic table, has the simplest atomic structure of all the elements, and consists of a nucleus of charge + 1 and one orbital electron.

The alkali metals also have a single outer orbital electron, but they tend to lose this electron in reactions and form positive ions; by contrast, hydrogen has little tendency to lose this electron but a great tendency to pair the electron and form a covalent bond. The halogens 17, like hydrogen, are one electron short of an inert gas structure.

In many reactions the halogens gain an electron and so form negative ions, although hydrogen can only do this in reactions with highly electropositive metals. This behaviour is explained by the atomic structure, the extremely small size of hydrogen atoms and the low electronegativity value.

These unique properties make it difficult to place hydrogen in the periodic table, since its properties differ from those of both Group 1 and group 17 elements, and although it is included in both groups in the tables in this book, it could well be put in a group on its own.

  • Chapter 10: The s-Block Elements

S-block consists of group 1 (alkali metals) and group 2 (alkaline earth metals) elements. You will learn physical and chemical properties of both the group. The group 1 of the periodic table contains six elements, namely lithium (Li), sodium (Na),potassium (K), rubidium (Rb), caesium (Cs) and francium (Fr). All these elements are typical metals.

These are usually referred to as alkali metals since their hydroxides forms strong bases or alkalies.The group 2 of the periodic table consists of six metallic elements. These are beryllium (Be),magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba) and radium (Ra). These (except Be) are known as alkaline earth metals as their oxides are alkaline and occur in earth crust.

  • Chapter 11: The p-Block Elements

Group 13 to 18 elements (except helium), in which the last electron enters the p-orbitals, constitute the p-block. In this chapter will be study systematic group wise details of p-block elements.In the s-block, group I elements are univalent and group II elements are divalent. In group III we would expect the elements to be trivalent.

In most of their compounds this is the case, but some of the elements show lower valency states as well. There is an increasing tendency to form univalent compounds on descending the group. Compounds with Ga(I), In(I) and Tl(I) are known. With Ga and In the (I) oxidation state is less stable than the (III) state.

However, the stability of the lower oxidation state increases on descending the group. Tl(I) thallous compounds are more stable than Tl(III) thallic compounds.How and why does monovalency occur in group III? The atoms in this group have an outer electronic configuration of s2p1. Monovalency is explained by the s-electrons in the outer shell remaining paired and not participating in bonding.

This is called the ‘inert pair effect’. If the energy required to unpair them exceeds the energy evolved when they form bonds, then the s-electrons will remain paired. The strength of the bonds in MX3 compounds decreases down the group. The mean bond energy for chlorides are GaCl3 = 242, InCl3 = 206 and TlCl3 = 153 kJ mol-1. Thus the s-electrons are most likely to be inert in thallium.

The inert pair effect is not the explanation of why monovalency occurs in group III. It merely describes what happens, i.e. two electrons do not participate in bonding. The reason that they do not take part in bonding is energy.The univalent ions are much larger than the trivalent ions and (I) compounds are ionic and are similar in many ways to group I elements.

The inert pair effect is not restricted to group III, but also occurs among the heavier elements in other groups in the p-block. Examples from group IV are Sn2+ and Pb2+ and examples from group V are Sb3+ and Bi3+. The lower oxidation state becomes more stable on descending the group.

Thus, Sn2+ is a reducing agent but Pb2+ is stable and Sb3+ is a reducing agent but Bi3+ is stable. When the s-electrons remain paired, the oxidation state is always two lower than the usual oxidation state for the group. Thus, in the s-block, groups I and II show only the group valency.

Groups in the p-block show variable valency, differing in steps of two. Variable valency also occurs with elements in the d-block. This arises from using different number of d-electrons for bonding, so in this case the valency can change in steps of one (e.g. Cu+ and Cu2+, Fe2+ and Fe3+).

  • Chapter 12: Organic Chemistry – Some Basic Principles & Techniques

Nomenclature of organic compounds-Organic chemistry is the study of hydrocarbons and their derivatives. The term nomenclature means the system of naming of organic compounds. In case of aliphatic compounds, two systems of nomenclature are generally used.

  1. Trivial or common system: In the beginning, when the number of carbon compounds were limited, they were named on the basis of their sources, properties and structures eg.
  • From sources: Urea (from urine) Methanol (from wood)(Greek, methu = spirit, hule = wood)
  • From properties: Glucose (from Greek, glykys = sweet), olefin (from French, olefiant = oil forming)
  • From structures: n-petane (from Greek = penta = fuie), methyl chloride (from methyl group + chloride)
  1. IUPAC system
  • Chapter 13: Hydrocarbons

Most important chapter of organic chemistry you will learn chemical and physical properties of alkanes , alkenes ,alkynes , aromatic hydrocarbons and its reactions mechanism. The term ‘hydrocarbon’ is self-explanatory which means compounds of carbon and hydrogen only. Hydrocarbons play a key role in our daily life.

You must be familiar with the terms ‘LPG’ and ‘CNG’ used as fuels. LPG is the abbreviated form of liquified petroleum gas whereas CNG stands for compressed natural gas. Another term ‘LNG’ (liquified natural gas) is also in news these days. This is also a fuel and is obtained by liquifaction of natural gas.

Petrol, diesel and kerosene oil are obtained by the fractional distillation of petroleum found under the earth’s crust. Coal gas is obtained by the destructive distillation of coal. Natural gas is found in upper strata during drilling of oil wells. The gas after compression is known as compressed natural gas.

LPG is used as a domestic fuel with the least pollution. Kerosene oil is also used as a domestic fuel butit causes some pollution. Automobiles need fuels like petrol, diesel and CNG. Petrol and CNG operated automobiles cause less pollution. All these fuels contain mixture of hydrocarbons, which are sources of energy.

Hydrocarbons are also used for the manufacture of polymers like polythene, polypropene, polystyrene etc. Higher hydrocarbons are used as solvents for paints. They are also used as the starting materials for manufacture of many dyes and drugs.

Thus, you can well understand the importance of hydrocarbons in your daily life. In this Booklet, you will learn more about hydrocarbons. “Hydrocarbons are the important sources of energy”

Frequently Asked Question (FAQs)

Q1. How to score good marks in class 11 chemistry with the help of the NCERT textbook?

Ans. Class 11 chemistry consist of equal weightage of all three parts of chemistry like physical chemistry, inorganic chemistry, and organic chemistry.

To score good marks you must give attention in all three parts and must-read the NCERT textbook while reading chapters from the NCERT textbook make sure you prepare your notes and work on numerals and basic concepts. Do solve sample papers and previous year asked questions.

Q2. What is the right approach to reading the NCERT class 11 chemistry Textbook?

Ans. The right approach starts with the strong foundation of the concepts and learning. NCERT textbook theory is sufficient to build strong conceptual learning for chemistry class 11.

Start your preparation of class 11 chemistry with the chapter -1 mole concept do solve questions given in the exercise and write down all formulas mentioned in the textbook for physical chemistry. Give more focus on the chemical bonding chapter and understand the concept of structure.

Q3. What are the right strategies to deal with inorganic chemistry?

Ans. Periodic table and its application are most important to become expert inorganic chemistry. NCERT textbook for Class 11 chemistry consists of few chapters of inorganic chemistry like s-block elements, p-block two-family, and hydrogen all these topics are to be done after a periodic table. Do prepare your notes for all these chapters will help you in the final revision.

Q4. Is NCERT class 11 chemistry text is enough for the competitive entrance exam?

Ans. Yes NCERT textbook is sufficient for JEE Main and NEET entrance exam although for JEE advance you need few reference books.

Q5. What are the most important chapters of class 11 chemistry?

Ans. Class 11 chemistry consist of a few fundamental chapters which are important for class 12 chemistry as well as for your class 11 chemistry final exam. Like in organic chemistry hydrocarbon is very important and it is highly important for class 12 organic chemistry.

All class 12 organic chemistry chapters are related to hydrocarbon. For inorganic chemistry chemical bonding and periodic table need to prepare very well. And in physical chemistry, one must have a very good concept in ionic equilibrium and thermodynamic and thermochemistry.

Q6. How NCERT solutions for class 11 chemistry help me to achieve my goal?

Ans. When you are in class 11 most of the students set there two-goal one is to score good marks in class 11 chemistry and second is to prepare for the competitive entrance exam. NCERT textbook will boost your preparation in both the exam it is highly helpful in class 11 chemistry exams of your school as well as beneficial for competitive exams. 

Q7. Do we need to solve questions from NCERT Exemplar for class 11 chemistry?

Ans. Solving additional questions is always beneficial. NCERT exemplar consists of very good quality of questions that help you to enhance your learning in class 11 chemistry.

Talk to Our counsellor