CBSE Class 12 Chemistry Syllabus 2017 2018 Term 2 available in Pdf for free download. The latest syllabus for Class 12 Chemistry have been issued by CBSE based on which Grade 12 students will have to prepare for examinations by CBSE, NCERT and KVS in Standard 12. The latest CBSE syllabus has been used to design NCERT book for Class 12 Chemistry based on which exams for Grade 12 Chemistry will be conducted. Refer to MCQ Questions for Class 12 Chemistry with answers and also download more latest study material for all subjects
Chemistry Term 2 Class 12 CBSE Syllabus
Class 12 Chemistry students should refer to the following curriculum for NCERT Class 12 Chemistry Term 2. These CBSE NCERT KVS Syllabus for Grade 12 Chemistry will be very useful for preparing for upcoming exams and help you to score good marks
Chemistry Term 2 CBSE Syllabus Class 12
CBSE Class 12 Chemistry Syllabus 2017-2018. Download the latest syllabus to do your studies as per the latest guidelines issued by CBSE NCERT. The syllabus, weightage of chapters, blue print of question papers and the design of question papers is issued every year for the benefit of students. Access all syllabus for all subjects here.
8. CHEMISTRY (Code No. 043)
Higher Secondary is the most crucial stage of school education because at this juncture specialized discipline
based, content -oriented courses are introduced. Students reach this stage after 10 years of general
education and opt for Chemistry with a purpose of pursuing their career in basic sciences or professional
courses like medicine, engineering, technology and study courses in applied areas of science and technology
at tertiary level. Therefore, there is a need to provide learners with sufficient conceptual background of
Chemistry, which will make them competent to meet the challenges of academic and professional courses
after the senior secondary stage.
The new and updated curriculum is based on disciplinary approach with rigour and depth taking care that
the syllabus is not heavy and at the same time it is comparable to the international level. The knowledge
related to the subject of Chemistry has undergone tremendous changes during the past one decade. Many
new areas like synthetic materials, bio -molecules, natural resources, industrial chemistry are coming in a
big way and deserve to be an integral part of chemistry syllabus at senior secondary stage. At international
level, new formulations and nomenclature of elements and compounds, symbols and units of physical
quantities floated by scientific bodies like IUPAC and CGPM are of immense importance and need to be
incorporated in the updated syllabus. The revised syllabus takes care of all these aspects. Greater emphasis
has been laid on use of new nomenclature, symbols and formulations,teaching of fundamental concepts,
application of concepts in chemistry to industry/ technology, logical sequencing of units, removal of
obsolete content and repetition, etc.
The curriculum of Chemistry at Senior Secondary Stage aims to:
promote understanding of basic facts and concepts in chemistry while retaining the excitement of
make students capable of studying chemistry in academic and professional courses (such as medicine, engineering, technology) at tertiary level.
expose the students to various emerging new areas of chemistry and apprise them with their relevance
in future studies and their application in various spheres of chemical sciences and technology.
equip students to face various challenges related to health, nutrition, environment, population, weather, industries and agriculture.
develop problem solving skills in students.
expose the students to different processes used in industries and their technological applications.
apprise students with interface of chemistry with other disciplines of science such as physics, biology, geology, engineering etc.
acquaint students with different aspects of chemistry used in daily life.
develop an interest in students to study chemistry as a discipline.
integrate life skills and values in the context of chemistry.
CLASS–XI (THEORY) (2017-18)
Total Periods (Theory 160 + Practical 60)
Time: 3 Hours Total Marks 70
Unit No. Title No. of Periods Marks
Unit I Some Basic Concepts of Chemistry 12
Unit II Structure of Atom 14
Unit III Classification of Elements and Periodicity in Properties 08 04
Unit IV Chemical Bonding and Molecular Structure 14
Unit V States of Matter: Gases and Liquids 12
Unit VI Chemical Thermodynamics 16
Unit VII Equilibrium 14
Unit VIII Redox Reactions 06
Unit IX Hydrogen 08
Unit X s -Block Elements 10
Unit XI Some p -Block Elements 14
Unit XII Organic Chemistry: Some basic Principles and Techniques 14
Unit XIII Hydrocarbons 12 18
Unit XIV Environmental Chemistry 06
Total 160 70
Unit I: Some Basic Concepts of Chemistry 12 Periods
General Introduction: Importance and scope of chemistry.
Nature of matter, laws of chemical combination, Dalton's atomic theory: 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.
Unit II: Structure of Atom 14 Periods
Discovery of Electron, Proton and Neutron, 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 completely filled orbitals.
Unit III: Classification of Elements and Periodicity in Properties 08 Periods
Significance of classification, brief history of the development of periodic table, modern periodic
law and the present form of 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.
Unit IV: Chemical Bonding and Molecular structure 14 Periods
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.
Unit V: States of Matter: Gases and Liquids 12 Periods
Three states of matter, intermolecular interactions, types of bonding, melting and boiling points,
role of gas laws in elucidating the concept of the molecule, Boyle's law, Charles law, Gay Lussac's
law, Avogadro's law, ideal behaviour, empirical derivation of gas equation, Avogadro's number,
ideal gas equation. Deviation from ideal behaviour, liquefaction of gases, critical temperature,
kinetic energy and molecular speeds (elementary idea), Liquid State- vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations)
Unit VI: Chemical Thermodynamics 16 Periods
Concepts of System and types of systems, surroundings, work, heat, energy, extensive and intensive properties, 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).
Unit VII: Equilibrium 14 Periods
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, Henderson Equation, hydrolysis of
salts (elementary idea), buffer solution, solubility product, common ion effect (with illustrative examples).
Unit VIII: Redox Reactions 06 Periods
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.
Unit IX: Hydrogen 08 Periods
Position of hydrogen in periodic table, occurrence, isotopes, preparation, properties and uses of
hydrogen, hydrides-ionic covalent and interstitial; physical and chemical properties of water,
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