AHSEC 1st Year Syllabus Chemistry

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CHEMISTRY
SYLLABUS FOR HIGHER SECONDARY FIRST YEAR COURSE

Rationale :
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 higher 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, applications of concepts in chemistry to industry/ technology, logical
sequencing of units, removal of obsolete content and repetition etc.
Objectives :
The broad objectives of teaching Chemistry at Senior Secondary Stage are to help the learners :
 to promote understanding of basic facts and concepts in chemistry while retaining the excitement of
chemistry .
 to make students capable of studying chemistry in academic and professional courses (such as
medicine, engineering, technology) at tertiary level.
 to expose the students to various emerging new areas of chemistry and apprise them with their
relevance in their future studies and their application in various spheres of chemical sciences and
technology .
 to equip students to face various changes related to health, nutrition. environment, population,
weather, industries and agriculture .
 to develop problem solving skills in students .
 to expose the students to different processes used in industries and their technological applications
 to apprise students with interface of chemistry with other disciplines of science such as physics.
biology, geology, engineering etc .
 to acquaint students with different aspects of chemistry used in daily life.
 to develop an interest in students to study chemistry as a discipline.

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CHEMISTRY
SYLLABUS FOR HIGHER SECONDARY FIRST YEAR COURSE

One Paper (Theory Three Hours Marks : 70
Unitwise distribution of marks and periods :
Unit No. Title Marks Periods
Unit-l Some Basic concepts of chemistry 03 14
Unit-2 Structure of Atom 06 16
Unit-3 Classification of Elements and Periodicity in Properties 04 08
Unit-4 Chemical Bonding and molecular Structure 05 16
Unit-5 States of Matter : Gases and Liquids 04 14
Unit-6 Thermodynamics 06 16
Unit-7 Equilibrium 06 16
Unit-8 Redox Reactions 03 06
Unit-9 Hydrogen 03 08
Unit-10 S-Block Elements 05 14
Unit-11 Some P-Block Elements 07 16
Unit-12 Organic Chemistry: some basic Principles and Techniques 07 14
Unit-13 Hydrocarbons 08 16
Unit-14 Environmental Chemistry 03 06
Total Marks : 70 180

Unitwise Distribution of Course contents :
Unit-I: Some Basic concepts of chemistry
General Introduction : Importance and scope of chemistry. Historical approach to particulate
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 and
empirical and molecular formula; chemical reactions, stoichiometry and calculations based on stoichiometry
Unit-2 : Structure of Atom
Discovery of electron, proton and neutron; atomic number, isotopes and isobars. Thompson'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-3 : Classification of Elements and Periodicity in Properties
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 -Periodic Trend and
chemical reactivity atomic radii, ionic radii, inert gas radii, ionization enthalpy, electron gain enthalpy,
electronegativity, valency.

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Unit-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.
Unit-5 : States of Matter: Gases and Liquids
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.
Liquid State- Vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical
derivations).
Unit-6 : Thermodynamics
Concepts of system, types of systems, surroundings, work, heat, energy, extensive and intensive
propoerties, 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 and dilution.
Introduction of entropy as a state function, free energy change for spontaneous and nonspontaneous
process, equilibrium.
Unit-7: 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, concept of pH. Hydrolysis of salts
(elementary idea), buffer solutions, solubility product, common ion effect (with illustrative examples).
Unit-8 : Redox Reactions
Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reaction,
applications of redox reactions.
Unit-9 : Hydrogen
Position of hydrogen in periodic table, occurence, isotopes, preparation, properties and uses of
hydrogen; hydrides- ionic, covalent and interstitial; physical and chemical propoerties of water, heavy
water, hydrogen peroxide- preparation, reaction and structure; hydrogen as a fuel.
Unit-10 : s-Block Elements
Group 1 and Group 2 elements :
General introduction, electronic configuration, occurence, anomalous properties of the first element
of each group, diagonal relationship, trends in the variation of properties (such as ionization enthalpy,
atomic and ionic radii), trends in chemical reactivity with oxygen, water, hydrogen and halogens; uses.
Preparation and properties of some important compounds :
Sodium carbonate, sodium chloride, sodium hydroxide and sodium hydrogen carbonate, biological

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importance of sodium and potassium,
CaO, CaCO3 and industrial use of lime and limestone, biological importance of Mg and Ca.
Unit-11 : Some p-Block Elements
General Introduction to p-Block Elements :
Group 13 elements : General introduction, electronic configuration, occurrence, variation of properties,
oxidation states, trends in chemical reactivity, anomalous properties of first element of the group; Boron-
physical and chemical properties, some important compounds: borax, boric acids, boron hydrides. Aluminium
: uses, reactions with acids and alkalies.
Group 14 elements : General introduction, electronic configuration, occurrence, variation of
properties, oxidation states, trends in chemical reactivity, anomalous behaviour of first element. Carbon-
catenation, allotropic forms, physical and chemical properties; uses of some important compounds :
oxides.
Important compounds of silicon and few uses : silicon tetrachloride, silicones, silicates and zeolites.
Unit-12 : 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
hyper conjugation.
Homolytic and heterolytic fission of a covalent bond : free radicals, carbocations, carbanions;
electrophiles and nucleophiles, types of organic reactions.
Unit-13 : Hydrocarbons
Classification of hydrocarbons :
Alkanes : Nomenclature, isomerism, conformations (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 functional group in mono-substituted benzene;
carcinogenicity and toxicity.
Unit-14 : Environmental Chemistry
Environmental pollution: Air, water and soil pollution, chemical reactions in atmosphere, smogs,
major atmospheric pollutants; acid rain, ozone and its reactions, effects of depletion of ozone layer,
greenhouse effect and global warming- pollution due to industrial wastes; green chemistry as an alternative
tool for reducing pollution, strategy for control of environmental pollution.

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SYLLABUS FOR CHEMISTRY PRACTICAL
Total Marks-30 Total Periods-60

Micro-chemical methods are available for several of the practical experiments. Wherever possible
such techniques should be used.
A. Basic Laboratory Techniques
1. Cutting glass tube and glass rod
2. Bending a glass tube
3. Drawing out a glass jet
4. Boring a cork
B. Characterisation and Purification of Chemical Substance
1. Determination of melting point of organic compound
2. Determination of boiling point of organic compound,
3. Crystallization involving impure sample of anyone of the following:
Alum, Copper sulphate, Benzoic acid.
C. Experiments Related to pH Change
(a) Anyone of the following experiments:
 Determination of pH of some solutions obtained from fruit juices, solutions of known and
varied concentrations of acids, bases and salts using pH or universal indicator .
 Comparing the pH of solutions of strong and weak acid of some concentration .
 Study the pH change in the titration of a strong acid with a strong base using universal
indicator.
(b) Study of pH change by common-ion effect in case of weak acids and weak bases.
D. Chemical Equilibrium
One of the following experiments:
(a) study the shift in equilibrium between ferric ions and thiocynate ions by increasing decreasing
the concentration of either ions.
(b) Study the shift in equilibrium between [Co(H2O)6]2+ and chloride ions by changing the
concentration of either of the ions.
E. Quantitative Estimation
 Using a chemical balance .
 Preparation of standard solution of oxalic acid .
 Determination of strength of a given solution of sodium hydroxide by titrating it against standard
solution of oxalic acid .
 Preparation of standard solution of sodium carbonate .
 Determination of strength of a given solution of hydrochloric acid by titrating it against standard
sodium carbonate solution.
E. Qualitative Analysis
Detection of one anion and one cation in a given salt
Cations-Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4+

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Anions-CO32–, S2–, SO32–, SO42–, NO2–, NO3–, Cl+, Br, I–, PO43–, C2O42–, CH3COO–
(Note: Insoluble salts excluded)
G. Project
Scientific investigation involving laboratory testing and collecting information from other sources.
A few suggestion projects
 Checking the bacterial contamination in drinking water by testing sulphide ions .
 Study of the methods of purification of water .
 Testing the hardness, presence of iron, fluoride, chloride etc. depending upon the regional variation in
drinking water and the study of causes of presences of these ions above permissible limit (if any)
 Investigation of the foaming capacity of different washing soaps and the effect of addition of sodium
Carbonate on them.
 Study of the acidity of different samples of the tea leaves .
 Determination of the rate of evaporation of different liquids .
 Study of the effect of acids and bases on the tensile strength of fibers .
 Analysis of fruit and vegetable juices for their acidity.

Note : Any other investigatory project, which involves about 10 periods of work, can be chosen with
the approval of the teacher.