NCERT Solutions Class 11 Chemistry
Class 11 Chemistry NCERT Solutions have been designed to solve all your complicated problems and guide you to score good marks in your examination. Additionally, these solutions can prove to be of enormous support to students in their preparation for Class 11 CBSE Examinations. Proper chapter-wise solutions help students to have a strong grip on the complex concepts with ease.
NCERT Solutions for Class 11 Chemistry are provided here as PDF for free. These solutions are prepared by subject-matter experts in order to develop a deep and conceptual understanding in students. Concepts covered in Class 11 Chemistry curriculum play a very important role in the success of youngsters in competitive exams like NEET and IIT-JEE. Therefore, the students are advised to be attentive towards the chapter-wise pdf of Chemistry Solutions for securing higher ranks in various Competitive Exams. The students can download these chapters from the links provided on this page.
These solutions of Class 11 Chemistry have been prepared in the simplest and easily understandable language along with precise format. Preparing topics from these PDF could help the students to score excellent. Download PDF for free so that you can access these solutions offline as well.
A list of chapters provided in Class 11 NCERT Solutions Chemistry free pdf
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1) NCERT Solutions Class 11 Chemistry Chapter 1 Some Basic Concepts of Chemistry
“Some Basic Concepts of Chemistry” is the first chapter in the Class 11 Chemistry Syllabus. The chapter explains the fine details about the basic concepts of chemistry that will set a foundation for higher education such as the importance of chemistry, atomic masses and molecular masses. Some basic laws and theories in Chemistry such as Dalton’s Atomic Theory, Avogadro Law and the Law of Conservation of Mass are also described in this chapter.
Download free pdf of Class 11 Chemistry Chapter 1 from the link provided by EDUGROSS. Following are the topics of Class 11 Chemistry Chapter 1 ‘Some Basic Concepts of Chemistry’ :-
- Numerical problems in calculating the molecular weight of compounds
- Numerical problems in calculating mass percent and concentration
- Problems on empirical and molecular formulae
- Problems on molarity and molality
Some Important points in ‘Some Basic Concepts of Chemistry’ are as follows –
- Relative atomic mass = Mass of an atom of the element / (1/12) x Mass of an atom of Carbon(C-12)
- Number of gram molecules = W(g) /Gram molecular mass
- Number of gram atoms = W(g) /Gram Atomic Mass(GAM)
- Avogadro’s number, NA = 6.022 X 1023
- Mass of one atom of element = Gram Atomic Mass / NA
- Classification of Matter-
(A) Physical classification
(B) Chemical classification
- Inorganic Compounds are the compounds which are obtained from non-living sources such as rocks and minerals. A few examples are common salt, marble, gypsum, washing soda etc.
- Organic Compounds are the compounds which are present in plants and animals. All the organic compounds have been found to contain carbon as their essential constituent. For example, carbohydrates, proteins, oils, fats etc.
2) NCERT Solutions Class 11 Chemistry Chapter 2 Structure of Atom
“Structure of Atom” is the second chapter in the NCERT Class 11 Chemistry Syllabus. The topics covered under this chapter include subatomic particles, Thomson’s Atomic Model, Rutherford’s Atomic Model, Bohr’s Model and the Quantum Mechanical Model of the atom.
Download free pdf of Class 11 Chemistry Chapter 2 from the link provided by EDUGROSS. Following are the topics of Class 11 Chemistry Chapter 2 ‘Structure of Atom’ :-
- Basic calculations regarding subatomic particles (protons, electrons, and neutrons).
- Numericals based on the relationship between wavelength and frequency.
- Numericals based on calculating the energy associated with electromagnetic radiation.
- Electron transitions to different shells.
- Writing electron configurations.
- Questions related to quantum numbers and their combinations (for electrons)
Some Important points in ‘Structure of Atom’ are as follows –
- Atomic number (Z) = Number of protons in the nucleus of an atom or Number of electrons in a neutral atom
- Mass number (A) = number of protons + number of neutrons
- Number of neutrons = Mass number (A) – Atomic number (Z)
- Speed of light = product of frequency and wavelength of light
c = vλ
- According to Planck’s Quantum Theory
3) NCERT Solutions Class 11 Chemistry Chapter 3 Classification of Elements and Periodicity in Properties
“Classification of Elements and Periodicity in Properties” is the third chapter in the NCERT Class 11 Chemistry Syllabus. This chapter is considered as one of the most essential chapters since it covers concepts that are very important part of the CBSE Curriculum for classes 11 & 12 (CBSE), JEE and NEET.
Download free pdf of Class 11 Chemistry Chapter 3 from the link provided by EDUGROSS. Following are the topics of Class 11 Chemistry Chapter 3 ‘Classification of Elements and Periodicity in Properties’ :-
- Genesis of periodic classification
- Modern periodic law and the present form of the periodic table
- Nomenclatures of elements with atomic number greater than 100
- Electronic configurations of elements and the periodic table
- The s-block, p-block, d-block and f-block elements
- Metals, Non-metals and Metalloids
- Periodic trends in properties of elements
- Trends in physical properties
- Trends in chemical properties
- Trends in chemical reactivity
Some Important points in ‘Classification of Elements’ are as follows –
- Groups – The long form of periodic table also consists of the vertical rows called groups. There are in all 18 groups in the periodic table. Unlike Mendeleev periodic table, each group is an independent group.
- Characteristics of groups:
(i) All the elements present in a group have same general electronic configuration of the atoms.
(ii) The elements in a group are separated by definite gaps of atomic numbers (2, 8, 8,18, 18,32).
(iii) The atomic sizes of the elements in group increase down the group due to increase the number of shells.
(iv) The physical properties of the elements such as m.p., b.p. density, solubility etc., follow a systematic pattern.
(v) The elements in each group have generally similar chemical properties.
- Periods – Horizontal rows in a periodic table are known as periods. There are in all seven periods in the long form of periodic table.
- Characteristics of periods:
(i) In all the elements present in a period, the electrons are filled in the same valence shell.
(ii) The atomic sizes generally decrease from left to right.
- General electronic configuration of s-Block Elements: ns1-2
- General electronic configuration of p-Block Elements: ns2np1-6
- Characteristics of s-block elements :-
(i) All the elements are soft metals.
(ii) They have low melting and boiling points.
(iii) They are highly reactive.
(iv) Most of them impart colours to the flame.
(v) They generally form ionic compounds.
(vi) They are good conductors of heat and electricity.
4) NCERT Solutions Class 11 Chemistry Chapter 4 Chemical Bonding and Molecular Structure
“Chemical Bonding and Molecular Structure” is the fourth chapter in the CBSE Class 11 Chemistry Syllabus. This chapter explain some major and important topics of Class 11 chemistry (such as hybridization and the modern theories on chemical bonding).
Download free pdf of Class 11 Chemistry Chapter 4 from the link provided by EDUGROSS. Following are the topics of Class 11 Chemistry Chapter 4 ‘Chemical Bonding and Molecular Bonding’ :-
- VSEPR theory
- Lewis structures
- Valence bond theory
- The polar character of covalent bonds
- The concept of hybridization
- The molecular orbital theory of homonuclear diatomic molecules
- Hydrogen bonding
- Drawing Lewis dot symbols for atoms, molecules, and polyatomic ions
- Questions on bond parameters
- Expressing resonance with the help of Lewis structures
- Questions related to dipole moment, bond polarity, and polar covalent bonds
- Questions on hybridization
- Questions on VBT, MOT and the VSEPR theory
Some Important points in ‘Chemical Bonding and Molecular Structure’ are as follows –
- The force that holds different atoms in a molecule is called chemical bond.
- Octet Rule – Atoms of different elements take part in chemical combination in order to complete their octet or to attain the noble gas configuration.
- Valence Electrons – It is the outermost shell electron which takes part in chemical combination.
- When the bond is formed between two or more atoms by mutual contribution and sharing of electrons, it is known as covalent bond.
- If the combining atoms are same then the covalent molecule is known as homo-atomic and if they are different then the covalent molecule is known as hetero-atomic molecule.
- Depending upon the type of overlapping, the covalent bonds are of two types, known as sigma (σ ) and pi (π) bonds.
- Lattice energy of an ionic compound depends upon following factors:
- Size of the ions: Smaller the size, greater will be the lattice energy.
- Charge on the ions: Greater the magnitude of charge, greater the inter-ionic attraction and hence higher the lattice energy.
- Size of the ions: Smaller the size, greater will be the lattice energy.
5) NCERT Solutions Class 11 Chemistry Chapter 5 States of Matter
“States of Matter” is the fifth chapter in the NCERT Class 11 Chemistry Syllabus. This chapter includes various basic concepts related to intermolecular forces and their effects on the physical state of any substance. It also explains about some fine details and deep concepts related to the liquid and gaseous states of matter, in the easiest possible way.
Download free pdf of Class 11 Chemistry Chapter 5 from the link provided by EDUGROSS. Following are the topics of Class 11 Chemistry Chapter 5 ‘States of Matter’ :-
- Numerical problems based on Boyle’s law, Charles’s law, Gay-Lusscac’s law, and Avogadro’s law.
- Numerical problems on calculating partial pressure.
- Questions on critical temperature and pressure.
Some Important points in ‘States of Matter’ are as follows –
- Intermolecular forces are the forces of attraction and repulsion between interacting particles have permanent dipole moments.
- This interaction is stronger than the London forces but is weaker than ion-ion interaction because only partial charges are involved.
- Ion-induced Dipolar Interactions is the type of interaction that permanent dipole of the polar molecule induces dipole on the electrically neutral molecule by deforming its electronic cloud. Interaction energy is proportional to 1/r6 where r is the distance between two molecules.
- A gas which does not follow ideal gas behaviour under all conditions of temperature and pressure is called real gas.
- Boyle’s law: P1V1 = P2V2 (at constant T)
- Charles’ law: V1/T1 = V2/T2 (at constant P)
- Avogadro’s law: V = kn (at constant T and P)
- Ideal gas equation: PV = nRT
- Combined gas equation: P1V1 / T1 = P2V2 / T2
- Dalton’s law of partial pressures: PTotal = P1 + P2 + P3 +⋯
- Partial pressure in terms of mole fraction, Pi = xi Ptotal
- Ven der Waals equation: (P+an2/V2)(V−nb) = nRT
- Compressibility factor, Z = PV / RT (for 1 mole of gas)
6) NCERT Solutions Class 11 Chemistry Chapter 6 Thermodynamics
“Thermodynamics” is the sixth chapter in the NCERT Class 11 Chemistry Syllabus. Thermodynamics is a branch of Science that focuses on the relation between the heat and another forms of energy. A part of the universe where observations are made is called system and the surrounding of a system is the part of the universe that does not contain the system. Based on the exchange of energy and matter, there are three types of thermodynamic systems : closed system, open system, and an isolated system.
Download free pdf of Class 11 Chemistry Chapter 6 from the link provided by EDUGROSS. Following are the topics of Class 11 Chemistry Chapter 6 ‘Thermodynamics’ :-
- Thermal equilibrium
- Zeroth law of Thermodynamics
- Heat, internal energy and work
- First law of thermodynamics
- Specific heat capacity
- Thermodynamic state variables and the equation of state
- Thermodynamic processes
- Heat engines
- Refrigerators and heat pumps
- The second law of thermodynamics
- Reversible and irreversible processes
- Carnot Engine
Some Important points in ‘Thermodynamics’ are as follows –
- ΔU = qv ; qv – Heat exchange at constant volume
- ΔH = qp ; qp – Heat exchange at constant pressure
- Enthalpy, H=U + pV
- Heat Capacity, C = qΔTC = qΔT
- Specific heat capacity, Cs = qm ΔT
- Molar heat capacity, Cn = qnΔT
- First law of thermodynamics: ΔU=q+W
- Relation between ΔH and ΔU
- ΔH = ΔU + pΔV or
- ΔH = ΔU + (Δn) RT
7) NCERT Solutions Class 11 Chemistry Chapter 7 Equilibrium
“Equilibrium” is the seventh chapter in the NCERT Class 11 Chemistry Syllabus. Various essential concepts such as equilibrium constants, buffer solutions and the common-ion effect is explained deeply in this chapter. Detailed explanations are provided in easily understandable language to help students learn and understand the key points related to the chemical equilibrium.
Download free pdf of Class 11 Chemistry Chapter 7 from the link provided by EDUGROSS. Following are the topics of Class 11 Chemistry Chapter 7 ‘Equilibrium’ :-
- Solid-liquid Equilibrium
- Equilibrium In Chemical Processes – Dynamic Equilibrium
- Law Of Chemical Equilibrium And Equilibrium Constant
- Homogeneous Equilibria
- Heterogeneous Equilibria
- Applications Of Equilibrium Constants
- Ionic Equilibrium In Solution
- Acids, Bases And Salts
- Ionization Of Acids And Bases
- Buffer Solutions
- Solubility Equilibria Of Sparingly Soluble Salts
Some Important points in ‘Equilibrium’ are as follows –
- Henry’s law – The solubility of a gas in a liquid at a certain temperature is governed by Henry’s law. It states that the mass of a gas that dissolves in a given mass of a solvent at any temperature is proportional to the pressure of the gas above the surface of the solvent.
- Equilibrium in Chemical Processes – Like equilibria in physical systems, it can also be achieved in chemical process involving reversible chemical reactions carried in closed container.
- Equilibrium in Homogeneous System – When in a system involving reversible reaction, reactants and products are in the same phase, then the system is called as homogeneous system.
- Law of Chemical Equilibrium – At a constant temperature, the rate of a chemical reaction is directly proportional to the product of the molar concentrations of the reactants each raised to a power equal to the corresponding stoichiometric coefficients as represented by the balanced chemical equation. Let us consider the reaction
- Le Chatelier’s Principle – If a system under equilibrium is subjected to a change in temperature, pressure or concentration, then the equilibrium shifts in such a manner as to reduce or to counteract the effect of change.
- Effect of Change of Concentration – When the concentration of any of the reactants or products in a reaction at equilibrium is changed, the composition of the equilibrium changes so as to minimise the effect.
8) NCERT Solutions Class 11 Chemistry Chapter 8 Redox Reactions
“Redox Reactions” is the eighth chapter in the NCERT Class 11 Chemistry Syllabus. This chapter is one of the most important chapters in the CBSE Class 11 Chemistry curriculum. The topics given in this chapter are also a part of the JEE and NEET Syllabus.
Download free pdf of Class 11 Chemistry Chapter 8 from the link provided by EDUGROSS. Following are the topics of Class 11 Chemistry Chapter 8 ‘Redox Reactions’ :-
- Classical Idea Of Redox Reactions – Oxidation And Reduction Reactions
- Redox Reactions In Terms Of Electron Transfer Reactions
- Oxidation Number
- Redox Reactions And Electrode Processes
Some Important points in ‘Redox’ are as follows –
- Oxidation is defined as the addition of oxygen/electronegative element to a substance or removal of hydrogen/ electropositive element from a substance
- Reduction is defined as the removal of oxygen/electronegative element from a substance or addition of hydrogen or electropositive element to a substance
- Oxidising agent: Acceptor of electrons
- Reducing agent: Donar of electrons
- When zinc rod is dipped in copper sulphate solution redox reaction begins hence, zinc is oxidised to Zn2+ ions and Cu2+ ions are reduced to metal.
- Redox reaction are the reactions in which oxidation and reduction occur simultaneously are called redox reactions.
- Electrochemical cell is a device in which redox reaction is carried indirectly and decrease in energy gives electrical energy.
- According to electronic concept, every redox reaction consists of two steps known as half reactions.
(i) Oxidation reaction: Half reactions that involve loss of electrons are called oxidation reactions.
(ii) Reduction reaction: Half reactions that involve gain of electrons are called reduction reactions.
9) NCERT Solutions Class 11 Chemistry Chapter 9 Hydrogen
“Hydrogen” is the ninth chapter in the NCERT Class 11 Chemistry Syllabus. NCERT Solutions for Class 11 Chemistry Chapter 9 Hydrogen contains all the essential topics with thoroughly explained solutions that aims to help students in understanding the concepts in a better way.
Download free pdf of Class 11 Chemistry Chapter 9 from the link provided by EDUGROSS. Following are the topics of Class 11 Chemistry Chapter 9 ‘Hydrogen’ :-
- Position Of Hydrogen In The Periodic Table
- Dihydrogen, H2
- Preparation Of Dihydrogen, H2
- Properties Of Dihydrogen
- Water Ex
- Hydrogen Peroxide (H202)
- Heavy Water, D20
- Dihydrogen as a Fuel
Some Important points in ‘Hydrogen’ are as follows –
- Position of hydrogen in periodic table is not justified because it resembles both alkali metals as well as halogens.
- Hydrogen and alkali metals both shows +1 oxidation state.
- Hydrogen as well as other alkali metals acts as reducing agents.
- Hydrogen and Alkali metals have affinity for electronegative element. For example – Na2O, NaCl, H20, HCl.
- Vapour density of a gas = (molar mass of gas) / (molar mass of H2)
- Molecular weight = 2×(Vapour Density)
- Volume strength of H2O2 = Molarity×11.2 = Normality×5.6
10) NCERT Solutions Class 11 Chemistry Chapter 10 The s-Block Elements
“The s-block elements” is the tenth chapter in the NCERT Class 11 Chemistry Syllabus. This chapter explains about the Group 1 Alkali Metals and Group 2 Alkaline Earth Metals, elements of s- block, their physical properties and chemical properties, General Characteristics of Compounds of the Alkaline Earth Metals, Some Important Compounds of Calcium, Anomalous properties of Lithium and Behaviour of Beryllium. You should go through the NCERT questions, as solving those questions will help them to evaluate themselves.
Students studying in Class 11 are advised to study the chapters of Class 11 properly because the chapters which are taught in Class 11 are the basics of the chapters which will be taught in Class 11.
Download free pdf of Class 11 Chemistry Chapter 10 from the link provided by EDUGROSS. Following are the topics of Class 11 Chemistry Chapter 10 ‘The s-block elements‘ :-
- Group 1 Elements: Alkali Metals
- General Characteristics Of The Compounds Of The Alkali Metals
- Anomalous Properties Of Lithium
- Some Important Compounds Of Sodium
- Biological Importance Of Sodium And Potassium
- Group 2 Elements: Alkaline Earth Metals
- General Characteristics Of Compounds Of The Alkaline Earth Metals
- Anomalous Behaviour Of Beryllium
- Some Important Compounds Of Calcium
- Biological Importance Of Magnesium And Calcium
Some Important points in ‘The s-Block Elements’ are as follows –
- Electronic Configuration of Group 1 Elements i.e. Alkali Metals – ns1
- These elements are called alkali metals because they readily dissolve in water to form soluble hydroxides, which are strongly alkaline in nature.
- Atomic and Ionic Radii of alkali metals increase on moving down the group i.e. they increase in size going from Li to Cs.
- Alkali metals form monovalent cations by losing one valence electron. Thus, Cationic radius is less as compared to the parent atom.
- The ionization enthalpies of the alkali metals are generally low and decrease down the group from Li to Cs. Since alkali metals possess large atomic sizes as a result of which the valence s-electron (ns1) can be easly removed. These values decrease down the group because of decrease in the magnitude of the force of attraction with the nucleus on account of increased atomic radii and screening effect.
- Hydration Enthalpy – Smaller the size of the ion, more is its tendency to get hydrated hence more is the hydration enthalpy.
- Hydration enthalpies of alkali metal ions decrease with increase in ionic sizes.
- Li+> Na+ > K+ > Rb+ > Cs+
- General Electronic Configuration of s-Block Elements
- For alkali metals (noble gas) ns1
- For alkaline earth metals [noble gas] ns2
- For alkali metals (noble gas) ns1
11) NCERT Solutions Class 11 Chemistry Chapter 11 The p-Block Elements
“The p-block elements” is the eleventh chapter in the NCERT Class 11 Chemistry Syllabus. The p-block elements are between the Group 13 and the Group 18 in the periodic table.
Download free pdf of Class 11 Chemistry Chapter 11 from the link provided by EDUGROSS. Following are the topics of Class 11 Chemistry Chapter 11 ‘The p-Block Elements’ :-
- Group 13 Elements: The Boron Family
- Important Trends And Anomalous Properties Of Boron
- Some Important Compounds Of Boron
- Uses Of Boron And Aluminium And Their Compounds
- Group 14 Elements: The Carbon Family
- Important Trends And Anomalous Behaviour Of Carbon
- Allotropes Of Carbon
- Some Important Compounds Of Carbon And Silicon
Some Important points in ‘The p-Block Elements’ are as follows –
- Outer Electronic Configuration of p-block elements: ns2np1
- The atomic and ionic radii of group 13 elements are smaller than the corresponding elements of alkali and alkaline earth metals. Reason is that on moving from left to right in a period the effective nuclear charge increases and the outer electrons are pulled more strongly towards the nucleus. This results in decrease in atomic size.
- On moving down the group, both atomic and ionic radii expected to increase due to the addition of a new electron shell with each succeeding element.
- Atomic radius of Ga is less than that of Al due to the presence of poor shedding 10d-electrons in gallium.
12) NCERT Solutions Class 11 Chemistry Chapter 12 Organic Chemistry – Some Basic Principles & Techniques
“Organic chemistry – some basic principles & techniques” is the twelfth chapter in the NCERT Class 11 Chemistry Syllabus. For students of Class 11 who are looking to give their best for the upcoming Class 11 final exams and competitive exams, they need to be accustomed to NCERT Solutions for Class 11 Chemistry Chapter 12.
Download free pdf of Class 11 Chemistry Chapter 12 from the link provided by EDUGROSS. Following are the topics of Class 11 Chemistry Chapter 12 ‘Organic chemistry – some basic principles & techniques’ :-
- General Introduction
- Tetravalence Of Carbon: Shapes Of Organic Compounds
- Structural Representations Of Organic Compounds
- Complete, Condensed And Bond-line Structural Formulas
- Three-dimensional Representation Of Organic Molecules
- Classification Of Organic Compounds
- Nomenclature Of Organic Compounds
- The IUPAC System Of Nomenclature
- Iupac Nomenclature Of Alkanes
- Nomenclature Of Organic Compounds Having Functional Group(S)
- Nomenclature Of Substituted Benzene Compounds
- Fundamental Concepts In Organic Reaction Mechanism
- Methods Of Purification Of Organic Compounds
- Quantitative Analysis
Some Important points in ‘Organic Chemistry Basic Principles & Techniques’ are as follows –
- Organic Chemistry is the branch of chemistry that deals with the study of hydrocarbons and their derivatives.
- Electromeric Effect (E-effect) refers to the polarity produced in a multiple bonded compound when it is attacked by a reagent when a double or a triple bond is exposed to an attack by an electrophile E+(a reagent) the two π electrons which from the π bond are completely transferred to one atom or the other.
- The functional group are atom or group of atoms joined in a specific manner which determines the chemical properties of the organic compound. The examples are hydroxyl group (—OH), aldehyde group (—CHO) and carboxylic acid group (—COOH).
- A covalent bond can undergo fission in two ways :-
- By Homolytic Fission or Homolysis
- By Heterolytic Fission or Heterolysis
- By Homolytic Fission or Homolysis
- In organic or carbon compounds, s and p orbitals are involved in hybridisation. This leads to y three types of hybridisation which are
- sp3(in alkanes) – Tetrahedral in shape
- sp2(in alkenes) – Planar structure
- sp(in alkynes) – Linear molecule
13) NCERT Solutions Class 11 Chemistry Chapter 13 Hydrocarbons
“Hydrocarbons” is the thirteenth chapter in the NCERT Class 11 Chemistry Syllabus. NCERT Solutions for Class 11 Chemistry Chapter 13 Hydrocarbon is one of the important chapters of organic chemistry. CBSE Class 11 Hydrocarbons explains about alkanes, preparation of alkanes from unsaturated hydrocarbons, from alkyl halides, from carboxylic acids, physical and chemical properties of alkanes. Hydrocarbons include deep concepts related to alkenes, the nomenclature of alkenes, isomers, preparation of alkene using alkyne, etc.
Download free pdf of Class 11 Chemistry Chapter 13 from the link provided by EDUGROSS. Following are the topics of Class 11 Chemistry Chapter 13 ‘Hydrocarbons’ :-
- Aromatic Hydrocarbon
- Carcinogenicity And Toxicity
Some Important points in ‘Hydrocarbons’ are as follows –
- Cyclic compounds in which the ring atoms are of carbon and some other element (For example, N, S, or O) are called heterocyclic compounds.
- Cyclic compounds which consist only of carbon atoms are called alicyclic or carboeyclic compounds.
- Aromatic Hydrocarbon – Benzene and its derivatives are called aromatic compounds.
- Alkenes are hydrocarbons that contain a carbon-carbon double bond (C=C) in their molecule.
- Structural Isomerism – Ethene and Propene have no structural isomers, but there are three structures of Butenes
14) NCERT Solutions Class 11 Chemistry Chapter 14 Environmental Chemistry
“Environmental Chemistry” is the fourteenth chapter in the NCERT Class 11 Chemistry Syllabus. Environmental Chemistry is one of the most important chapters in the NCERT Class 11 Chemistry Book. This chapter topics like like atmospheric pollution, water pollution, soil pollution, and reasons for soil pollution. Apart from these students will get to know about strategies to control environmental pollution like waste disposal, use of pesticides to reduce soil pollution.
Download free pdf of Class 11 Chemistry Chapter 14 from the link provided by EDUGROSS. Following are the topics of Class 11 Chemistry Chapter 14 ‘Environmental Chemistry’ :-
- Environmental Pollution
- Atmospheric Pollution
- Water Pollution
- Soil Pollution
- Industrial Waste
- Strategies To Control Environmental Pollution
- Green Chemistry
Some Important points in ‘Environmental Chemistry’ are as follows –
- Environmental Chemistry – It is the branch of science which deals with the chemical changes in the environment. It includes our surroundings as air, water, soil, forest etc.
- Environmental Pollution – It is the effect of undesirable changes in our surroundings that have harmful effects on plants, animals and human beings.
- Pollutants – A substance, which causes pollution, is known as pollutant. Pollutants can be solid, liquid or gaseous substances. Present in higher concentration, it can be produced due to human activities or natural happenings.
- Troposphere extends to the height of about 10 km from the sea level. It contains air, water vapours, clouds etc. The pollution in this region is caused by some poisonous gases, smoke fumes, smog etc.
- Stratosphere extends from height of 10 km to 50 km above the sea level. Ozone and some other gaseous substances present in this region are responsible for the pollution.
- Tropospheric Pollution is caused by the presence of undesirable gaseous particles like oxides of sulphur, nitrogen and carbon, hydrocarbons along with solid particles like dust, mist, fumes, smoke, etc.
- Oxides of Sulphur – These are produced when coal containing sulphur is burnt.
Advantages of Class 11 NCERT Chemistry Solutions
- Solving these NCERT Solutions will help students clearing all their doubts with the help of materials.
- Students who are preparing for their upcoming exams are advised to practice these NCERT Solutions regularly to score better marks in their exam.
- While studying in CBSE Board Schools, students always get confused while deciding the right study material so you can take help from NCERT Solutions.
- For CBSE students, the best option is NCERT Solutions as it covers the whole CBSE Syllabus for Class 11 Chemistry.
- Students should refer to these NCERT Solutions before their exams because these solutions will help them in clearing the tough concepts by explaining it simply.
- These Class 11 Chemistry NCERT Solutions focus on basics to help students with concepts.
- NCERT Solutions for Class 11 Chemistry not only give significant learning to the students but also help them to upgrade their skills.
- These NCERT Solutions encompassed by the comprehensive step-by-step description using proper explanations, solved examples, etc. of all the exercises given in NCERT Textbooks.
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