Tripura Board Class 11 Syllabus for Chemistry

Tripura Board of Higher Secondary Education Class XI Syllabus for Chemistry with course structure are given below.

Unit I : Some Basic Concepts of Chemistry (Periods 12)

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, empirical and molecular formula; chemical reactions, stoichiometry and calculations based on stoichiometry.

Unit II: Structure of Atom (Periods 16)

Discovery of electron, proton and neutron; atomic number, isotopes and isobars. Rutherford’s model and its limilations. 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 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 ( Periods 8 )

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. Lonization enthalpy, electron gain enthalpy, electro negativity, valence, Nomenclature of elements with atomic number greater than 100.

Unit IV: Chemical Bonding and Molecular Structure (Periods 16)

Valence electrons, ionic bond, bond parameters, covalent bond: Born Haber Cycle. 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 and hydrogen bond.

Unit V: States of Matter: Gases and Liquids ( Periods 14 )

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, Derivation from ideal behaviour, liquefaction of gases, critical temperature, kinetic energy and molecular speeds (elementary ideal)

Liquid State : Vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations).

Unit VI: Chemical Thermodynamics ( Periods 16 )

Concepts of System, types of systems, surroundings, Work, heat, energy, extensive and intensive properties, state functions.

First law of themodynamics-internal energy change (∆U) and enthalpy change (∆H), Hess’s law of constant heat summation, enthalpy of; bond dissociation, Combustion, formation, atomization, sublimation, phase transformation, ionization, and solution.

Introduction of entropy as a state function, Gibbs energy change for spontaneous and nonspontaneous processes, criteria for equilibrium.

Second and third laws of thermodynamics.

Unit VII : Equilibrium (Periods 20)

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 polybasic acids, acid strength, concept of pH Henderson Equation, Hydrolysis of salts (elementary idea). Buffer solutions, solubility product, common ion effect (with illustrative examples).

Unit VIII: Redox Reactions ( Periods 6 )

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.

Unit IX : Hydrogen ( Periods 8 )

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, heavy water; hydrogen peroxide-preparation, properties, structure and use; hydrogen as a fuel.

Unit X : s-Block Elements (Alkali and Alkaline earth metals) (Periods 12 )

Group 1 and Group 2 elements :

General introduction, electronic configuration, occurrence, 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 hydroxide and sodium hydrogen carbonate, biological Importance of sodium and potassium.

Ca0, CaC03 and industrial use of lime and limestone, biological importance of Mg and Ca.

Unit XI : Some p-Block Elements ( Periods 14 )

General Introduction to p-Block Elements

Group 13 elements; General introduction, electronic configurations, 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 acid, boron hydrides, Aluminium : reactions with acids and alkalies and uses.

Group 14 elements : General introduction, electronic configurations, 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 a few uses; silicon tetrachloride, silicones, silicates and zeolites, their uses and structure of silicates.

Unit XII: Organic Chemistry – Some Basic Principles and Techniques ( Periods 16 )

General introduction, methods of 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 XIII : Hydrocarbons ( Periods 16 )

Classification of hydrocarbons Alkanes – Nomenclature, isomerism, conformations (ethane only), physical properties, chemical reactions including halogenation, free radical mechanism, Combustion and pyrolysis.

Alkenes- Nomemclature, structure of double bond (ethane) 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 perperties: mechanism of electrophilic substitution- nitration sulphonation, halogenation, Friedel Craft’s alkylation and acylation carcinogenicity and toxicity.

Unit XIV : Environmental Chemistry ( Periods 8 )

Environmental pollution – air, water and soil pollution, chemical reactions in atmosphere, smog, 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.

PRACTICAL SYLLABUS

Time : 3 hours

Total Periods : 60

Three Experiments to be given in the examination as follows:

1. Volumetric Analysis 8

i. Standard solution to be provided

ii. One exercise out of the following :

a) Determination of strength of a given solution of sodium Hydroxide by titrating it against standard solution of oxalic acid.

b) Determination of strength of a given solution of hydrochloric acid by titrating it against standard solution of sodium carbonate.

Distribution of 8 marks :

i.   Procedure 3
ii.  Observation including recording of data 2
iii. Calculation 1
iv. Result 2

2. Qualitative Analysis 8 marks :

Salt analysis consisting of one anion and one cation (only water soluble salts and no interfering radical) Distribution of 8 marks :

i. Systematic reporting 4
ii. Correct result
Anion 2
Cation 2

3. One of the following experiments (4)

i. Determination of melting or boiling point of an organic compound

ii. Comparing pH of solutions of strong and weak acid of same concentration.

iii. Study of pH change by common ion effect in the case of a weak acid or a weak base.

iv. Study of shift in equilibrium by increasing/decreasing the concentration of either of the ions in case of:

a) Equilibrium between ferric ions and thiocynate ions. b) [ Co(H2O)6]2+ and Cl- ions.

V. Detection of Nitrogen/Chlorine/Sulphur in organic compounds

List of experiments in chemistry

A. Basic Laboratory Techniques ( Periods 3 )

Experiment -1

a) Cutting glass tube and glass rod

b) Bending a glass tube

c) Drawing out a glass jet

d) Boring a cork

B. Characterization and purification of chemical substances ( Periods 7 )

Experiment – 2

Determination of melting point of an organic compound

Experiment – 3

Determination of boiling point of an organic compound

Experiment – 4

Crystallization of impure sample of anyone of the following : Alum, copper sulphate, Benzoic acid.

C. Experiments related to pH change ( Periods 7)

Experiment – 5

Comparing the pH of solutions of strong and weak acid of same concentration.

Experiment – 6

Study of pH change by common-ion effect in case of weak acids and weak bases.

D. Chemical equilibrium ( Periods 5 )

Experiment – 7 Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either ions.

or

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 ( Periods 18 )

Experiment – 8 Preparation of standard solution of oxalic acid

Experiment – 9 Determination of strength of a given solution of sodium hydroxide by titrating it against standard solution of oxalic acid.

Experiment – 10 Determination of strength of a given solution of hydrochloric acid by titrating it against standard sodium carbonate solution.

F. Qualitative analysis ( Periods 18 )

Experiment – 11 Identification of following cations by systematic analysis

Pb2+,Cu2+, Al3+,Fe3+,Mn2+, Ni2+,Zn2+,

Experiment – 12 Identification of following cations by systematic analysis

Co2+,Ca2+,Sr2+,Ba2+,Mg2+, NH+4

Experiment – 13 Identification of following anions

CO32-, S2-, SO32-, SO42- , NO2 , NO3 ,

Experiment – 14 Identification of following anions

Cl, Bl, l, CH2COO

(Note : Insoluble salts excluded)

Experiment – 15 Detection of nitrogen, sulphur and chlorine in organic compounds ( Periods 12 )

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