NCERT Solutions for Class 11 Chemistry

Chapter 1 - Some Basic Concepts of Chemistry

General Introduction: Importance and scope of Chemistry. Nature of matter, laws of chemical combination, Dalton's atomic theory: the concept of elements, atoms, and molecules. Atomic and molecular masses, mole concept and molar mass, percentage composition, empirical and molecular formula, chemical reactions, stoichiometry, and calculations based on stoichiometry.

Class 11 NCERT solutions help the students to go through the formulas and concepts easily. Here find the Important formulas of  Chapter 1 - Some Basic Concepts of Chemistry to crack your exams.

1. Mole Concept:

Number of moles (n) = $\frac{Mass (m)}{Molar Mass (M)}$

Number of particles = n × Avogadro's Number

2. Percentage Composition:

$\text{Percentage composition of an element} = \frac{\text{Atomic mass of element}}{\text{Molar mass of compound}} \times 100$

3. Empirical Formula: The empirical formula represents the simplest whole-number ratio of atoms present in a compound.

4. Molecular Formula: The molecular formula represents the actual number of atoms of each element present in a molecule of the compound.

5. Molarity:

$\text{Molarity} = \frac{\text{Number of moles of solute}}{\text{Volume of solution (in liters)}}$

Students can access extra study materials on Some Basic Concepts of Chemistry, These resources are available for download, offering additional support for your studies.

Chapter 2 - Structure of Atom

Discovery of electrons, protons and neutrons, atomic number, isotopes, and isobars. Thomson's model and its limitations. Rutherford's model and its limitations, Bohr's model and its limitations, concept of shells and subshells, dual nature of matter and light, de Broglie's relationship, Heisenberg uNCERTainty principle, concept of orbitals, quantum numbers, shapes of s, p and d orbitals, rules for filling electrons in orbitals - Aufbau principle, Pauli's exclusion principle and Hund's rule, electronic configuration of atoms, stability of half-filled and filled orbitals.

Class 11 NCERT solutions help the students to go through the formulas and concepts easily. Here find the Important formulas of  Chapter 2 - Structure of Atom to crack your exams.

1. de Broglie's Wavelength Equation

• $\lambda = \frac{h}{mv}$

2. Heisenberg UNCERTainty Principle

• $\Delta x \times \Delta p \geq \frac{h}{4\pi}$

• States that it is impossible to simultaneously determine the exact position and momentum of a particle.

3. Quantum Numbers

• Principal Quantum Number (n): Describes the energy level of an electron in an atom.

• Azimuthal Quantum Number (l): Describes the shape of the orbital.

• Magnetic Quantum Number (m): Describes the orientation of the orbital in space. Spin Quantum Number (ms): Describes the spin of the electron.

4. Aufbau Principle, Pauli's Exclusion Principle, and Hund's Rule

• Aufbau Principle: Electrons occupy the lowest energy orbitals available.

• Pauli's Exclusion Principle: No two electrons in an atom can have the same set of four quantum numbers.

• Hund's Rule: Electrons occupy orbitals singly before pairing up, and all electrons in singly occupied orbitals have the same spin.

Students can access extra study materials on the Structure of Atom, These resources are available for download, offering additional support for your studies.

Chapter 3 - Classification of Elements and Periodicity in Properties

Significance of classification, a brief history of the development of the periodic table, modern periodic law and the present form of the periodic table, periodic trends in properties of elements -atomic radii, ionic radii, inert gas radii, Ionization enthalpy, electron gain enthalpy, electronegativity, valency. Nomenclature of elements with atomic number greater than 100. 

Students can access extra study materials on the Classification of Elements and Periodicity in Properties, These resources are available for download, offering additional support for your studies.

Class 11 NCERT solutions help the students to go through the formulas and concepts easily. Here find the Important formulas and concepts of Chapter 3 - Classification of Elements and Periodicity in Properties to crack your exams.

1. Mendeleev's Periodic Table

• Mendeleev arranged elements in order of increasing atomic mass and observed periodic recurrence of properties.

2. Modern Periodic Law

• States that the properties of elements are a periodic function of their atomic numbers.

3. Periodic Trends

• Atomic Radius: Generally decreases across a period and increases down a group.

• Ionization Energy: Generally increases across a period and decreases down a group.

• Electron Affinity: Generally increases across a period and decreases down a group.

• Electronegativity: Generally increases across a period and decreases down a group.

4. Effective Nuclear Charge (Zeff)

• Zeff = Z - S, where Z is the atomic number and S is the shielding constant. It represents the net positive charge experienced by an electron in an atom.

5. Periodic Classification of Elements

• Elements are arranged in periods (horizontal rows) and groups (vertical columns) based on similarities in their properties.

Chapter 4 - Chemical Bonding and Molecular Structure

Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, polar character of covalent bond, covalent character of ionic bond, valence bond theory, resonance, geometry of covalent molecules, VSEPR theory, concept of hybridization, involving s, p and d orbitals and shapes of some simple molecules, molecular orbital theory of homonuclear diatomic molecules(qualitative idea only), Hydrogen bond.

Students can access extra study materials on Bonding and Molecular Structure, These resources are available for download, offering additional support for your studies.

Class 11 NCERT solutions help the students to go through the formulas and concepts easily. Here find the Important formulas and concepts of Chapter 4 - Chemical Bonding and Molecular Structure to crack your exams.

1. Lewis Dot Structures

• Used to represent the valence electrons of atoms and their bonding patterns in molecules.

• Octet Rule: Atoms tend to gain, lose, or share electrons to achieve a noble gas electron configuration.

2. Ionic Bonding

• Forms between a metal and a non-metal.

• Electrostatic attraction between oppositely charged ions.

3. Covalent Bonding

• Forms between non-metal atoms by sharing of electrons.

• Polar Covalent Bond: Unequal sharing of electrons due to differences in electronegativity.

• Non-polar Covalent Bond: Equal sharing of electrons.

4. Valence Shell Electron Pair Repulsion (VSEPR) Theory

• Predicts the geometry of molecules based on the repulsion between electron pairs.

• Shapes include linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral, among others.

5. Molecular Orbital Theory

• Describes the behavior of electrons in molecules using molecular orbitals formed by the overlap of atomic orbitals.

• Bonding Molecular Orbital: Formed by in-phase overlap of atomic orbitals.

• Antibonding Molecular Orbital: Formed by out-of-phase overlap of atomic orbitals.

Chapter 5 - Chemical Thermodynamics

Concepts of Systems and types of systems, surroundings, work, heat, energy, extensive and intensive properties, and state functions. First law of thermodynamics -internal energy and enthalpy, heat capacity, and specific heat, measurement of U and H, Hess's law of constant heat summation, enthalpy of bond dissociation, combustion, formation, atomization, sublimation, phase transition, ionization, solution, and dilution. Second law of Thermodynamics (brief introduction) Introduction of entropy as a state function, Gibb's energy change for spontaneous and nonspontaneous processes, criteria for equilibrium. Third law of thermodynamics (brief introduction).

Students can access extra study materials on Chemical Thermodynamics, These resources are available for download, offering additional support for your studies.

Class 11 NCERT solutions help the students to go through the formulas and concepts easily. Here find the Important formulas and concepts of Chapter 5 - Chemical Thermodynamics to crack your exams.

1. First Law of Thermodynamics

• $\Delta U = q + w$

2. Enthalpy

• $\Delta H = H_{\text{final}} - H_{\text{initial}}$

• Change in enthalpy represents the heat absorbed or released at constant pressure.

3. Heat Transfer:

• $q = mc\Delta T$

4. Gibbs Free Energy 

• $\Delta G = \Delta H - T\Delta S$

5. Entropy

• $\Delta S = \frac{q_{\text{rev}}}{T}$

• Change in entropy represents the dispersal of energy in a system during a reversible process. 

Chapter 6 - Equilibrium 

Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of mass action, equilibrium constant, factors affecting equilibrium - Le Chatelier's principle, ionic equilibrium- ionization of acids and bases, strong and weak electrolytes, degree of ionization, ionization of poly basic acids, acid strength, concept of pH, hydrolysis of salts (elementary idea), buffer solution, Henderson Equation, solubility product, common ion effect (with illustrative examples). 

Students can access extra study materials on Equilibrium ,These resources are available for download, offering additional support for your studies.

Class 11 NCERT solutions help the students to go through the formulas and concepts easily. Here find the Important formulas and concepts of Chapter 6 - Equilibrium to crack your exams.

1. Equilibrium Constant 𝐾𝑐= $\frac{[C]c \cdot [D]d}{[A]a \cdot [B]b}$

2. Le Chatelier's Principle

• States that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust itself to counteract the effect of the change and establish a new equilibrium.

3. Equilibrium Shifts

• Effect of Concentration: Adding reactants or products will shift the equilibrium in the direction that reduces the concentration change.

• Effect of Temperature: Increasing temperature favors endothermic reactions, while decreasing temperature favors exothermic reactions.

• Effect of Pressure (for gases): Increasing pressure favors the side with fewer moles of gas.

4. Equilibrium Expressions for Heterogeneous Equilibria

• For 𝑎𝐴+𝑏𝐵⇌𝑐𝐶+𝑑𝐷

• aA+bB⇌cC+dD involving solids or liquids, their concentrations are considered constant and not included in the equilibrium expression.

Chapter 7 - Redox Reactions

Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, in terms of loss and gain of electrons and change in oxidation number, applications of redox reactions.

Class 11 NCERT solutions help the students to go through the formulas and concepts easily. Here find the Important formulas and concepts of Chapter 7 -Redox Reactions to crack your exams.

1. Oxidation Number

• The oxidation number is the hypothetical charge that an atom would have if all bonds to atoms of different elements were 100% ionic.

• Rules for assigning oxidation numbers help determine whether a species undergoes oxidation or reduction in a reaction.

2. Balancing Redox Reactions

• Half-Reaction Method: Involves balancing the reduction and oxidation half-reactions separately.

• Ion-Electron Method (or Oxidation-Reduction Method): Balances the redox reaction by dividing it into oxidation and reduction half-reactions and balancing the number of electrons transferred.

3. Oxidizing Agent and Reducing Agent

• Oxidizing Agent: Substance that gains electrons and undergoes reduction, causing another substance to be oxidized.

• Reducing Agent: Substance that loses electrons and undergoes oxidation, causing another substance to be reduced.

Students can access extra study materials on Redox Reactions , These resources are available for download, offering additional support for your studies.

Chapter 8 - Organic Chemistry - Some Basic Principles and Techniques 

General introduction, methods of purification, qualitative and quantitative analysis, classification, and IUPAC nomenclature of organic compounds. Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance, and hyperconjugation. Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions, electrophiles and nucleophiles, types of organic reactions.

Class 11 NCERT solutions help the students to go through the formulas and concepts easily. Here find the Important formulas and concepts of  Chapter 8 -Organic Chemistry -Some Basic Principles and Techniques to crack your exams.

1. Nomenclature

• IUPAC (International Union of Pure and Applied Chemistry) rules are used for naming organic compounds systematically based on their structure and functional groups.

• Prefixes, suffixes, and numbering systems are employed to denote substituents, parent chains, and functional groups.

2. Reactivity of Organic Compounds

• Organic compounds exhibit diverse reactivity patterns based on functional groups and structural features.

• Common reactions include addition, elimination, substitution, oxidation, and reduction reactions.

3. Isomerism

• Isomers are compounds with the same molecular formula but different structural arrangements or spatial orientations.

Students can access extra study materials on Organic Chemistry -Some Basic Principles and Techniques, These resources are available for download, offering additional support for your studies.

Chapter 9 -  Hydrocarbons 

Classification of Hydrocarbons Aliphatic Hydrocarbons: Alkanes - Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions including free radical mechanism of halogenation, combustion, and pyrolysis. Alkenes - Nomenclature, structure of double bond (ethene), geometrical isomerism, physical properties, methods of preparation, chemical reactions: addition of hydrogen, halogen, water, hydrogen halides (Markovnikov's addition and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition. Alkynes - Nomenclature, structure of triple bond (ethyne), physical properties, methods of preparation, chemical reactions: acidic character of alkynes, addition reaction of - hydrogen, halogens, hydrogen halides, and water. Aromatic Hydrocarbons: Introduction, IUPAC nomenclature, benzene: resonance, aromaticity, chemical properties: mechanism of electrophilic substitution. Nitration, sulphonation, halogenation, Friedel Craft's alkylation and acylation, directive influence of the functional group in monosubstituted benzene. Carcinogenicity and toxicity.

Class 11 NCERT solutions help the students to go through the formulas and concepts easily. Here find the Important formulas and concepts of  Chapter 9 -  Hydrocarbons to crack your exams.

1. Classification of Hydrocarbons

• Hydrocarbons are organic compounds consisting of only carbon and hydrogen atoms.

• They are classified into two main groups: aliphatic hydrocarbons (open-chain or cyclic) and aromatic hydrocarbons (containing benzene ring or its derivatives).

2. Structural Isomerism

• Structural isomers have the same molecular formula but different structural arrangements.

3. IUPAC Nomenclature

• The International Union of Pure and Applied Chemistry (IUPAC) system is used to systematically name hydrocarbons based on their structure and functional groups.

• Rules include identifying the longest continuous carbon chain (parent chain), numbering the chain to give substituents the lowest possible locants, and naming substituent groups based on prefixes.

4. Types of Hydrocarbons

• Alkanes: Saturated hydrocarbons containing only single bonds between carbon atoms.

• Alkenes: Unsaturated hydrocarbons containing at least one carbon-carbon double bond.

• Alkynes: Unsaturated hydrocarbons containing at least one carbon-carbon triple bond.

• Aromatic Hydrocarbons: Contain one or more benzene rings or derivatives.

5. Reactions of Hydrocarbons

• Combustion: Hydrocarbons burn in the presence of oxygen to produce carbon dioxide and water.

• Substitution: Alkanes undergo substitution reactions, where one or more hydrogen atoms are replaced by other atoms or groups.

• Addition: Alkenes and alkynes undergo addition reactions, where atoms or groups are added to the carbon-carbon double or triple bonds.

Students can access extra study materials on Hydrocarbons, These resources are available for download, offering additional support for your studies.

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1. Quality of Solutions

• Study material formulated to aid problem-solving approach.

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• Solutions designed by experienced teachers.

• Solutions cover important parts and chapters, based on past years' question papers.

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• Solutions designed in easy language for clear understanding.

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