NIOS Class 12 Syllabus 2023 Chemistry

NATIONAL OPEN SCHOOL
Senior Secondary Curriculum in Chemistry

RATIONALE
According to present scheme of school education at Senior Secondary stage, chemistry emerges out as a
separate discipline. It is this stage where major emphasis is to be laid on providing suitable conceptual foundation
The present chemistry course has been developed basically around the themes: Why do chemical reactions
occur? What is the quantitative relationship among reacting constituents in a chemical reaction? How far
andhow fast will a chemical reaction proceed under a given set of conditions? Can we predict whether a
chemical reaction willoccur or not? What is the relation between the structure of a chemical substance and its
functions/properties? In What way is a chemical reaction relevant for getting new types of substances and
materials for dialylife and chemical industries?
In the present course, there in no compartmentalisation like physical, inorganic and organic chemistry. How-
ever, basic chemical concept considered necessary in the study of descriptive chemistry (inorganic and or-
ganic) are provided in the beginning of the course and an effort has been made to provide a disciplinary
structure to chemistry and, therefore, a logical sequencing of concepts in provided. Applications of chemistry in
daily life have been interwoven with the conceptual themes in such a way that learners can appreciate the
importance of the study of chemistry relevant to daily life and in the economic development of the country.
Some interdisciplinary aspects have also been provided to make the course more meaningful and cunctional.
OBJECTIVES OF THE COURSE
It is expected that a learner will be able to:
 understand the principles, theories and laws of chemistry responsible for various chemical processes/
reactions,
 realise the role of chemistry in production of many elements (metals/non-metals) and compounds useful in
industries and daily life,
 appreciate the chemical nature of inorganic and organic substances around him/her,
 choose various vocational, professional and applied courses of his/her choice based on knowledge of
chemistry gained.
Apart from this, the present course also aims at developing the following capacity in the learner:
 perform chemical calculations to know about the chemical reactions and chemical compounds,
 explain chemical reactions, concepts and phenomenon,
 develop awareness about uses and abuses of chemical substances,
 develop skills arranging/setting aparatus, handling apparatus and chemicals properly, and
 analyse and synthesise simple compounds.
SPECIAL FEATURES OF THE COURSE
The academic standard of the present chemistry course in comparable with the chemistry course of any State
Education Board or Central Board of Secondary Education, New Delhi. Considering the nature of open learning
system, it has not been found desirable to divide the course into class XI and class XII. The rationale behind the
course is that every lesson has a role to play in understanding the holistic view of chemistry.
The course also provides optional modules ‘mostly of applied nature’ out of which a student can choose one
module according to his/her choice of career. Thus, there are seven core modules and two optional modules. A
student appearing for senior secondary examination is expected to offer all the seven core modules, one
Module out of two optional modules, and practicals. All the core and optional modules are listed below:

CORE MODULES
S.No. Module Marks Study
Alloted Hours
1. Atom Molecule and
Chemical Arithmatics 7 14
2. Atomic Structure and Chemical Bonding 12 33
3. States of Matter 12 18
4. Chemical Energetics 8 23
5. Chemical Dynamics 8 19
6. Chemistry of Elements 10 48
7. Chemistry of Organic Compounds 12 48

OPTIONAL MODULES
I. Environmental Chemistry 15
II. Chemistry and Industry 37
Total 80 240

A detailed curriculum is given for your ready reference

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Sr. Secondary Chemistry Curriculum
CORE MODULES  Types of bonds and their characteristics (logic,
MODULE 1:ATOMS MOLECULES AND Covalent, Coordinate, Metallic)
CHEMICAL ARITHMATICS  Shapes of molecules, Introduction to VSEPR
Lesson 1 Mole Concept theory (upto 6 electron pairs only)
 A simple idea of basic SI units  Hybridization of atomic orbitals
 Counting and weighing of atoms and molecules  Multiple covalent bonds (,) e.g. C2H4,C2H2
 Avogadro constant  M.O. Theory, Homonuclear molecule
 Molar quantities (H2,N2,O2,F2), Bond Parameters
 Hydrogen Bonding
Lesson 2 Chemical Arithmetic
MODULE 3: STATES OF MATTER
 Chemical formula and percentage composition Lesson 6 Gaseous State
 Empirical and molecular formulae  Properties
 Mole, Mas, Volume relationships in chemical  Boyle’s Law
reactions  Charles law-Kelvin Temperature Scale
 Limiting reagent concept and percentage yield
 Avogadro’s Law
MODULE 2:ATOMS STRUCTURE AND  Dalton’s law of partial pressures
CHEMICAL ARITHMATICS  Ideal gas equation
Lesson 3 Chemical Arithmaties  The kinetic molecular theory of gases (no
 Fundamental particles of an atom (electron, derivation)
Proton, Neutron)  Graham’s law of diffusion
 Rutherford’s nuclear model  real gases-deviations from ideal gas behavior,
 Electromagnetic spectrum Vansder Waal equation Liquefaction of gases,
 Line spectra of H-atom: Bohr model (no critical Constants
derivation) Lesson 7 Liquid State
 Wave-particle duality: Heisenberg’s  Properties of liquids
uncertainty principle  Vapour pressure
 The wave mechanical model-orbitals  Surface tension
(probability picture may be emphasised),  Viscosity
 Quantum numbers
Lesson 8 Solid State
 Pauli’s exclusion principle
 Properties of solids
 Aufbau Principle-electronic configuration of
atoms  Classification of solids
 Types of orbitals (s,p,d,f): shapes of s,p,d  Unit cell and their types
orbitals  Packing in crystals
 Hund’s rule  Structure of simple ionic compounds
 Imperfections in solids (Frenkel, Schottky
Lesson 4 Periodic Table and Atomic Properties defects)
 Long Form of periodic table and IUPAC
nomenclature for elements with Z > 110 (brief Lesson 9 Solutions
mention)  Solution, solute and solvent
 Variation in atomic properties (size, jonization  Concentration of solutions-molarity, molality,
energy, electron affinity, valency and electro mole fraction, percentage and Strength
negativity)  Types of solutions
 Raoult’s law
Lesson 5 Chemical Bonding
 Why do atoms combine? (potential-energy
 Ideal and non-ideal solutions
diagram)  Colligative properties of solutions
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 Van’t Hoff factor Lesson 14 Ionic Equilibria
Lesson 10 Colloids
 Acid-base equilibrium
 The Colloidal Solution
 lonisation constant of lead acids and bases
 True solution, colloidal solution and suspension
 Ionization of water
 Classification of colloids
 pH value
 Preparation and properties of colloidal solutions
 Common Ion effect
 Applications of colloids
 Buffer solutions, Henderson equation
 Solubility equilibrium, solubility product and its
MODULE 4: CHEMICAL ENERGETICS applications
Lesson 11 Chemical Thermodynamics  Salt Hydrolysis
 System : Isolated, closed and open systems  Acid base titration
 Processes: cyclic, isothermal, adiabatic, Lesson 15 Electrochemistry
reversible and irreversible  Oxidation and Reduction (Electron transfer
 Standard state of a substance concept)
 Exothermic and endothermic reactions  Oxidation number, balancing of Redox reaction
 Thermochemical equations by oxidation number method
 Concept of internal energy and enthalpy change,  Types of cells: Electrolytic and electrochemical
relationship between H and U,  Electrolytic conduction (Conductance,
 Ist law of thermodynamics conductivity molar conductivity, effect of
 Standard enthalpy of reactions dilution, Kohlrausch’s law)
 Enthalpy changes during a reaction: enthalpy  Standard electrode potential
of formation, enthalpy of combustion, enthalpy  Electrochemical series and its applications
of neutralization  Effect of concentration of electrode potentials
 Hess’s law and its applications (Nernst equation)
 Bond enthalpy  Relationship between emf and free energy
Lesson 12 Spontaneity of Chemical Reactions change
 Concept of entropy, entropy change and Lesson 16 Chemical Kinetics
spontaneity  Rate of Reaction: Average and Instantaneous
 IInd law of thermodynamics  Expressions for reaction rates
 Concept of free energy, relationship between  Factors affecting rate of reaction
G,H and S  Rate law
 Free energy change and spontaneity of a  Order of a reaction
chemical reaction  First order reaction
 Standard free energy of formation  Half change period
 Free energy change and chemical equilibrium  Effect of temperature on reaction rate
 IIIrd law of thermodynamics and its significance Lesson 17 Adsorption and Catalysis
(illustrative)  Adsorption-Physical and Chemical
MODULE 5: CHEMICAL DYNAMICS  Adsorption Isotherms (Freundlich and
Lesson 13 Chemical Equilibrium
Langmuir)
 Dynamic nature of equilibrium; Factors
 Catalysis-Homogenous and Heterogeneous
affecting equilibrium
 Activation energy
 Reversible and irreversible reactions
 Types of equilibrium system: Homogeneous and MODULE 6 Chemistry of Elements
heterogeneous systems Lesson 18 Occurrence And Extraction of Metals
 Laws of chemical equilibrium  Occurrence of metals
 Relationship between Kc and Kp  Important ores of some common elements :
 Le Chatelier’s Principle and its applications Na,Al, Sn, Pb, Ti, Fe, Cu, Ag and Zn

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 General principles involved in the isolation of  Properties-metallic character, oxidation state,
metals from their ores (concentration of the ore, ionic radii, catalytic properties, coloured ions,
reduction and refining) complex formation, magnetic properties,
Lesson 19 Hydrogen and s-Block Elements interstitial compounds alloy formation.
 Unique position of H2 in Periodic  Preparation, properties and applications some
 Properties reactions and uses important compounds:
 Isotopes of hydrogen  KMnO4, K2Cr2O7
 Water structure and aggregation of water  f-Block elements-configuration, properties and
molecules, Heavy Water lanthanide contraction
 Hydrogen peroxide Lesson 24 Coordination Compounds
 Alkali Metals and Alkaline earth metals-  Werner’s theory
occurrence, electronic configuration trends in  Nomenclature
atomic and physical properties, reactivity  Bonding-V.B. Approach
electrode potential,  Applications (qualitative analysis, extraction of
 Reaction with oxygen, hydrogen, halogens and metals and biological systems)
water MODULE 7 CHEMISTRY OF ORGANIC
 Solubility and thermal stability of their oxo salts. COMPOUNDS
Lesson 20 General characteristics of The p-block Lesson 25 Nomenclature and General Principles
elements  Rules of IUPAC Nomenclature
 Occurrence in nature and electronic
 Types of bond fission
configuration, (physical and chemical properties)
 Types of reactions: substitution, addition,
 Inert pair effect
elimination, oxidation/reduction (electrophilic
 Anomalous properties of first element and nucle ophillic)
Lesson 21 p-Block elements and Their  Electron displacement in a covalent bond:
Compounds-I
inductive effect, electromeric effect,
 Boron family-borax, boric acid, boron hydrides,
 resonance and hyperconjugation, steric effect
halides.
 Isomerism–Structural isomerism,
 Carbon family-allotropes (graphite, diamond,
stereoisomerism
elementary idea of fullerens)
 Oxides, carbides, halides Lesson 26 Hydrocarbons
 Nitrogen family-Ammonia, Nitric acid, fertilizer  Definition and types of hydrocarbons (Alkane,
(N,P) and fixation of nitrogen industrial and Alkene, alkyne, Arene)
biological  IUPAC nimenclature
 Nitrogenous and phosphatic fertilisers  Preparation and Properties of Hydrocarbons
Lesson 22 p-Block Elements and their  Physical properties of hydrocarbons
compounds-II  Chemical properties of hydrocarbons (addition,
 Oxygen family-oxxides, acidic, basic and substitution, elimination, oxidation)
amphoteric, Ozone (Oxidizing Properties) Lesson 27 Compounds of Carbon
 Halogens- Hydrides, oxides and oxoacids of ContainingHalogens (Haloalkanes and
chlorine. Haloarenes)
 Bleaching powder-preparation and properties,  IUPAC Nomenclature of halogen compounds
Interhalogen compounds.  Preparation of haloalkanes and haloarenes
 Noble gases-compounds of xenon: xenon  Physical and chemical properties and uses
fluorides, oxides (preparation, structure)
Lesson 23 d-Block and f-Block elements Lesson 28 Alcohol, Phenols and Ethers
 Electronic configuration  Classification
 General trends in the Chemistry of first row  IUPAC Nomenclature
transition elements  Methods of preparation

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 Physical and Chemical properties  Legislative measures for prevention of water
pollution
Lesson 29 Aldehydes, Ketones and Carboxylic
acids. Lesson 35 Heavy Metal Contamination
 Carboxylic Acids and acid derivatives  Heavy metals
 IUPAC Nomenclature  Effects of heavy metal contamination
 Preparation and Properties  Preventive measures
 Interconversion of acid derivations Lesson 36 Radioactive Pollution
Lesson 30 Compounds of Carbon Containing  Radioactive sources
Nitrogen  III effects of radiation
 Nitro compounds, amines  Preventive measures
 Classification of amines  Regulation regarding safety
 IUPAC nomenclature
MODULE 2: CHEMISTRY AND INDUSTRY
 Preparation and properties Lesson 32 Petrochemicals
Lesson 31 Biomolecules  Generations of petrochemicals
 Difference between DNA and RNA  Soaps and detergents
 Biomolecules in biological systems.  Rocket propellants
 Structures of proteins and carbohydrates  Pollutants and Indian Space Programs.
OPTIONAL MODULES Lesson 33 Polymers
MODULE 1: ENVIRONMENTAL  Classification
CHEMISTRY  Teflox, polyester and nylons
Lesson 32 Environment at concerns  Biodegradable polymers
 Idea of environment  Biopolymers
 Threats to environment
Lesson 34 Dyes. Paints and Pigments
 Pollutants
 Composition
Lesson 33 Air Pollution  Classification
 Composition of air  Process of dying
 Respiration, photosynthesis and decay cycle  Applications
 Air pollutants Lesson 35 Drugs and Medicines
 Green house effect  Distinction between drugs and medicines
 Global warming  Classification
 Depletion of ozone layer  Analgesics and antipyretics
 Acid rain  Antibiotics and anaestheties
Lesson 34 Water Pollution Lesson 36 Building Materials
 Water resources  Cement and its manufacture
 Water pollutants  Mortar, Concrete and R.C.C
 Biological oxygen demand  Manufacture of glass
 Prevention of water pollution  Ceramics and day products

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