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Introduction 3) To expose the students to various emerging According to NCF 2005, the new and new areas of chemistry and apprise them updated curriculum is introduced at +2 stage. with their relevance in their future studies There is a need to provide the sufficient and their applications in various spheres conceptual background of chemistry which will of chemical sciences and technology. help the students to appear for different common 4) To equip students to face various changes entrance test at the state level and the national related to health, nutrition, environment, level. This new syllabus will make them population, weather, industries and competent to meet the challenges of academic agriculture. and professional courses like medicine, 5) To develop problem solving skills in engineering, technology, etc, after the +2 stage. students. The syllabus is comparable to the international 6) To expose the students to different level. processes used in industries and their The syllabus contains areas like physical, technological applications. organic, inorganic, industrial, analytical and 7) To apprise students with interface of polymer chemistry. The upgraded syllabus has chemistry with other disciplines of science taken care of new formulations and such as physics, biology, geology, nomenclature of elements, compounds and engineering, etc. IUPAC units of physical quantities. New nomenclature, symbols and formulations, Std. XI (Theory) fundamental concepts, modern techniques are given importance. Unit 1: Some Basic Concepts of Chemistry Objectives : General Introduction: Importance and The broad objectives of teaching scope of chemistry. Historical approach to Chemistry at Higher Secondary stage are to particulate nature of matter, laws of help the learners : chemical combination, Dalton’s atomic 1) To promote understanding of basic facts theory : concept of elements, atoms and and concepts in chemistry while retaining molecules. Atomic and molecular masses the excitement of chemistry. mole concept and : Avogadro’s 2) To make students capable of studying law and Avogadro number, percentage chemistry in academic and professional composition, empirical and molecular courses (such as medicine, engineering, formula, chemical reactions, stoichiometry technology) at tertiary level. and calculations based on stoichimetry. 157

Unit 2 :States of matter : Gases and electronegativity, valence. liquids Unit 5: Redox reactions Three states of matter. Intermolecular Concept of oxidation and reduction, redox interactions, type of bonding. Role of gas reactions, oxidation number, Balancing laws in elucidating the concept of the redox reactions, in terms of loss and gain molecule, Boyle’s law, Charles law, Gay of electrons and change in oxidation Lussac’s law. Ideal behaviour, empirical number. derivation of gas equation. Ideal gas Unit 6: Chemical equilibrium equation. Deviation from ideal behaviour, Equilibrium in physical and chemical liquefaction of gases. Critical temperature. processes, dynamic nature of equilibrium, Kinetic energy and molecular speeds law of mass action, equilibrium constant, (elementary idea) Liquid State – Vapour factors affecting equilibrium, Le Chatelier’s pressure, viscosity and surface tension principle. (qualitative idea only, no mathematical Ionic equilibrium: Ionization of acids and derivations). bases, strong and weak electrolytes, degree Unit 3 : Structure of atom of ionization, ionization of polybasic acids, Discovery of electron, proton and neutron; acid strength, concept of pH. Hydrolysis atomic number, isotopes and isobars. of salts (elementary idea). Buffer solutions, Rutherford’s model and its limitations, product, common ion effect (with Bohr’s model and its limitations, concept illustrative examples.) Handerson equation. of shells and subshells, dual nature of Unit 7 : Surface chemistry matter and light, de Broglie’s relationship, Adsorption – physisorption and Heisenberg’s uncertainty principle, concept chemisorption; factors affecting adsorption of orbitals, quantum numbers, shapes of s, of gases on solids; catalysis : homogenous p and d orbitals, rules for filling electrons and heterogeneous, activity and selectivity: in orbitals – Aufbau principle, Pauli’s enzyme catalysis; colloidal state : exclusion principle and Hund’s rule, distinction between true solutions, colloids electronic configuration of atoms, stability and suspensions; Lyophilic, Lyophobic, of half filled and completely filled orbitals. multimolecular and macromolecular Unit 4 : Periodic table colloids; properties of colloids; Tyndall Significance of classification, brief history effect, Brownian movement, of the development of periodic table, electrophoresis, coagulation; emulsion – modern periodic law and present form of types of emulsions. Elementary idea of periodic table, periodic trends in properties nanomaterials. of elements atomic radii, ionic radii. Inert Unit 8 : Nature of chemical bond gas radii nomenclature of elements with Valence electrons, ionic bond, Born Haber atomic number greater than 100.Enthalpy: cycle : covalent bond parameters. Lewis Explanation and definition of term. structure, polar character of covalent bond, Ionization enthalpy, electron gain enthalpy, covalent character of ionic bond, valence 158

bond theory, resonance, geometry of configuration, occurrence. Variation of covalent molecules, VSEPR theory, properties, oxidation states, trends in concept of hybridization involving s, p chemical reactivity, anomalous properties and d orbitals and shapes of some simple of first element of the group. Boron- molecules, molecular orbital theory of physical and chemical properties, some homonuclear diatomic molecules important compounds: borax, boric acids, (qualitative idea only), bond. boron hydrides. Aluminium; uses, reactions Unit 9 : Hydrogen with acids and alkalies. Position of hydrogen in periodic table, Group 14 elements : occurrence, isotopes, preparation, General introduction, electronic properties and uses of hydrogen; hydrides- configuration, occurrence, variation of ionic, covalent and interstitial; physical properties, oxidation states, trends in and chemical properties of water, heavy chemical reactivity, anomalous behavior water. Hydrogen peroxide- preparation, of first element. – catenation, properties and structure; hydrogen as a allotropic forms, physical and chemical fuel. Uses of hydrogen peroxide. properties; uses of some important Unit 10: s-Block elements (Alkali and compounds; oxides. Important compounds alkaline earth metals) of silicon and their uses: silicon Group 1 and Group 2 elements : tetrachloride, silicones, silicates and General introduction, electronic zeolites and structure of silicates. configuration, occurrence, anomalous Unit 12: Basic principles and techniques properties of the first element of each in organic chemistry group, diagonal relationship, trends in the General introduction, methods of variation of properties (such as ionization qualitative and quantitative analysis, enthalpy, atomic and ionic radii), trends in Classification and IUPAC nomenclature chemical reactivity with oxygen, water, of organic compounds. and hydrogen and halogens; uses. Preparation boiling point. Electronic displacements in and properties of some important a covalent bond; inductive effect, compounds: Sodium carbonate, sodium electromeric effect, resonance and hyper hydroxide and sodium hydrogen carbonate, conjugation.Homolytic and heterolytic biological importance of sodium and fission of a covalent bond; free potassium. Calcium oxide and calcium radicals,carbocations, carbanions; carbonate and industrial uses of lime and electrophiles and nucleophiles, types of limestone, biological importance of organic reactions. Magnesium and Calcium. Unit 13 : Alkanes Unit 11 : p-Block elements Classification of hydrocarbons – Group Introduction to p-Block elements Nomenclature, isomerism, conformations Group 13 elements : ( only), physical properties, chemical General introduction, electronic reactions including free radical mechanism 159

of halogenation, combustion and pyrolysis. 2. Bending glass tube Unit 14 : Alkenes 3. Drawing out a glass jet Nomenclature, structure of double bond 4. Study of burner (ethane), geometrical isomerism, physical 5. Operating pinch cork properties, methods of preparation. B. Characterization and purification of Chemical reactions; addition of hydrogen, chemical substances halogen, water, hydrogen halides 1. Determination of melting point of an (Markovnikoff’s addition and peroxide organic compound. (p-toludine, effect) ozonolysis, oxidation, mechanism naphthalene, oxalic acid, β-naphthol, of electrophilic addition. resorcinol, benzoic acid.) Unit 15: Alkynes 2. Determination of boiling point of an Nomenclature, structure of triple bond organic compound. (, methyl (ethylene), physical properties. Methods acetate, acetic acid, xylene (o,m,p), water) of preparation, chemical reactions: acidic 3. Crystallization of impure sample of any character of alkynes, addition reaction of one of the following compounds. Alum, – hydrogen, halogens, hydrogen halides, copper sulphate, benzoic acid. water. C. Surface chemistry Unit 16 : Aromatic compounds (a) Preparation of one lyophilic and one Introduction, IUPAC nomenclature; lyophobic sol: Lyophilic sol-starch and benzene; resonance aromaticity; chemical gum. properties; mechanism of electrophilic Lyophobic sol–aluminium hydroxide, ferric substitution. – nitration, sulphonaiton, hydroxide, arseneous sulphide. halogenation, Friedel Craft alkylation and (b) Study of the role of emulsifying agents in acylation; Carcinogenicity and toxicity. stabilizing the emulsion of oil. UNIT-17: Environmental chemistry D. Chemical equilibrium Environmental pollution- air, water and Any one of the following experiments: soil pollution, chemical reactions in (a) Study the shift in equilibrium between atmosphere, smog, major atmospheric ferric ions and thiocyanate ions by pollutants, acid rain, ozone and its changing the concentration of either ion. reactions, effects of depletion of ozone (b) Study the shift in equilibrium between 2+ layer, green house effect and global [Co(H2O)6] and chloride ions by changing warming. Pollution due to industrial the concentration of either of the ions. wastes, green chemistry as an alternative E. Experiments related to pH change tool for reducing pollution, strategy for (a) Any one of the following experiments: control of environmental pollution.  Determination of pH of some solutions obtained from fruit juices, varied Practical Syllabus - Std. XI concentrations of acids, bases and salts A. Basic laboratory techniques using pH paper or universal indicator. 1. Cutting glass tube and glass rod  Comparing the pH solutions of strong and 160

weak acid of same concentration. fluoride, chloride etc. depending upon the  Study the pH change in the titration of a regional variation in drinking water and strong base using universal indicator. the study of causes of presence of these (b) Study of pH change by common ion effect ions above permissible limit (if any). in case of weak acids and bases. 4 Investigation of the foaming capacity of F. Quantitative estimation different washing soaps and the effect of  Using a chemical balance. addition of sodium carbonate on them.  Preparation of standard solution of oxalic 5 Study of the acidity of different samples acid. of the tea leaves.  Determination of strength of a given 6 Determination of the rate of evaporation solution of sodium hydroxide by titrating of different liquids. it against standard solution of oxalic acid. 7 Study of the effect of acids and bases on  Preparation of standard solution of sodium the tensile strength of fibers. carbonate. 8 Analysis of fruit and vegetable juices for  Determination of strength of a given their acidity. solution of hydrochloric acid by titrating it Note: against standard sodium carbonate solution. Any other investigatory project can be G. Qualitative analysis chosen with the approval of the teacher. Determination of one cation and one anion in a given salt: Std. XII (Theory) Cations – Pb2+, Cu2+, Al3+, Fe3+, Mn2+, Unit 1: Solid State Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, Classification of solids based on different + NH4 forces; molecular, ionic, covalent and 2- 2- 2- - - – Anions – CO3 SO3 SO4 NO2 NO3 Cl , metallic solids, amorphous and crystalline – – 3- 2- - Br , I , PO4 C2O4 CH3COO solids (elementary idea), unit cell in two (Note: Insoluble salts excluded) dimensional and three dimensional lattices, H. Detection of nitrogen, sulphur, chlorine, calculation of density of unit cell, packing bromine and in an organic in solids, voids, number of atoms per unit compound. cell in a cubic unit cell, point defects, PROJECT electrical and magnetic properties, Band Scientific investigations involving theory of metals, conductors and laboratory testing and collecting semiconductors and insulators and n information from other sources. and p type semiconductors. A few suggested Projects Unit 2 : Solutions and colligative 1 Checking the bacterial contamination in properties drinking water by testing sulphide ion. Types of solutions, expression of 2 Study of the methods of purification of concentration of solids in liquids, solubility water. of gases in liquids, solid solutions, 3 Testing the hardness, presence of iron, colligative properties –relative lowering 161

of vapor pressure,Raoult’s law elevation reaction; concentration, temperature, of boiling point, depression of freezing catalyst; order and molecularity of a point, osmotic pressure, determination of reaction; rate law and specific rate constant, molecular masses using colligative integrated rate equations and half life (only properties, abnormal molecular mass.Van’t for zero and first order reactions); concept Hoff factor and calculations involving of collision theory (elementary idea, no it. mathematical treatment). Activation Unit 3 :Chemical thermodynamics and energy, Arrhenius equation. energetic Unit 6 :General principles and processes Concepts of system, types of systems, of isolation of elements surroundings. Work, heat, energy, extensive Principles and methods of extraction – and intensive properties, state functions. concentration, oxidation, reduction First law of thermodynamics – internal electrolytic method and refining; energy and enthalpy, Hess’ law of constant occurrence and principle of extraction of heat summation, enthalpy of bond aluminium, copper, and iron dissociation, combustion, formation, Unit 7: p-Block elements atomization, sublimation. Phase transition, Group 15 elements: ionization and solution and dilution General introduction, electronic Introduction of entropy as a state function, configuration, occurrence, oxidation states, free energy change for spontaneous and trends in physical and chemical properties; non spontaneous processes, and nitrogen – preparation, properties and uses; equilibrium constant. Second and third compounds of nitrogen; preparation and law of thermodynamics properties of ammonia and nitric acid, Unit 4: Electrochemistry oxides of nitrogen (structure only); Redox reactions, conductance in Phoshorous-allotropic forms; compounds electrolytic solutions, specific and molar of phosphorous; preparation and properties

conductivity, variations of conductivity of phosphine, halides (PCl3,PCl5) and with concentration, Kohlrausch’s Law, oxoacids (elementary idea only). electrolysis and laws of electrolysis Group 16 elements: (elementary idea), dry cell –electrolytic General introduction, electronic and galvanic cells; lead accumulator, EMF configuration, oxidation states, occurrence, of a cell, standard electrode potential, trends in physical and chemical properties; Nernst equation and its application to dioxygen; preparation, properties and uses; chemical cells, fuel cells; corrosion. Classification of oxides, simple oxides; Relation between Gibb’s energy change Ozone. and emf of a cell. Sulphur – allotropic forms; compounds of Unit 5: Chemical kinetics sulphur; preparation, properties and uses Rate of reaction (average and of sulphur dioxide; sulphurc acid; industrial instantaneous), factors affecting rate of process of manufacture, properties and 162

uses, oxoacids of sulphur (structures only). VBT, CFT. isomerism, (structural and Group 17 elements: stereo) importance of coordination General introduction, electronic compounds (in qualitative analysis, configuration, oxidation states, occurrence, extraction of metals and biological trends in physical and chemical properties; systems). compounds of halogens; preparation, Unit 10 : Halogen derivatives of alkanes properties and uses of chlorine and (and arenes) hydrochloric acid, interhalogen Haloalkanes : compounds, oxoacids of halogens Nomenclature, nature of C-X bond, (structure only). physical and chemical properties, Group 18 elements: mechanism of substitution reactions. General introduction, electronic Stability of carbocations,R-S and d-l configuration. Occurrence, trends in configuration physical and chemical properties, uses. Haloarenes : Unit 8 : d and f Block Elements Nature of C-X bond, substitution reactions d-Block Elements - (directive influence of halogen for General introduction, electronic monosubstituted compounds only) stability configuration, occurrence and of carbocations, R-S and d-l characteristics of transition metals, general configurations. Uses and environmental trends in properties of the first row effects of – dichloromethane, transition metals – metallic character, thrichloromethane, tetrachloromethane, ionization enthalpy, oxidation states, ionic iodoform, freons, DDT. radii, colour, catalytic property, magnetic Unit 11 : , phenols and ethers properties, interstitial compounds, alloy Alcohols : formation preparation and properties of Nomenclature, methods of preparation,

K2Cr2O7 and KMnO4. physical and chemical properties (of f-Block elements- primary alcohols only); identification of Lanthanoids – Electronic configuration, primary, secondary and tertiary alcohols; oxidation states, chemical reactivity and mechanism of dehydration, uses of lanthanoid contraction and its methanol and . consequences. Actinoids – Electronic Phenols: configuration, oxidation states. Nomenclature, methods of preparation, Comparison with lanthanoids. physical and chemical properties, acidic Unit 9: Coordination compounds nature of phenol, electrophillic substitution Coordination compounds – Introduction, reactions, uses of phenols. ligands, coordination number, colour, Ethers : magnetic properties and shapes, IUPAC Nomenclature, methods of preparation, nomenclature of mononuclear coordination physical and chemical properties, uses. compounds, bonding; Werner’s theory, Unit 12 : Aldehydes, and 163

carboxylic acids proteins; enzymes. Aldehydes and ketones : Lipids and hormones (elementary idea) Nomenclature, nature of carbonyl group, excluding structure, their classification and methods of preparation. Physical and functions. chemical properties, mechanism of Vitamins: Classification and functions. nucleophilic addition, reactivity of alpha Nucleic acids: DNA and RNA hydrogen in aldehydes; uses. Unit 15: Polymers Carboxylic acids : Classification - natural and synthetic, Nomenclature, acidic nature, methods of methods of polymerization (addition and preparation, physical and chemical condensation), copolymerization. Some properties; uses. important polymers; natural and synthetic Unit 13: Organic compounds like polythene, nylon, polyesters, bakelite, containing nitrogen and rubber. Biodegradable and non Nitro compounds-General methods of biodegradable polymers. preparation and chemical reactions Unit 16: Chemistry in everyday life : Amines : 1. Chemicals in medicines : analgesics, Nomenclature, classification, structure, tranquilizers, , , methods of preparation, physical and antimicrobials, antifertility drugs, chemical properties, uses, identification of antibiotics, antacids, antihistamines primary, secondary and tertiary amines. elementary idea of antioxidants Cyanides and isocyanides: 2. Chemicals in food : Preservatives, Will be mentioned at relevant places in artificial sweetening agents. context. 3. Cleansing agents : Soaps and detergents, Diazonium salts: cleansing action. Preparation, chemical reactions and importance in synthetic organic chemistry. Practical Syllabus - Std. XII Unit 14: Biomolecules Carbohydrates: A. Chemical Kinetics Classification (aldoses and ketoses), (Any one of the following) : monosaccahrides d-l configuration (a) Effect of concentration and temperature (glucose and fructose), oligosaccharides on the rate of reaction between sodium (sucrose, lactose, maltose), polysaccharides thiosulphate and hydrochloric acid. (starch, cellulose, glycogen), importance. (b) Study of reaction rate of any one of the Proteins: following: Elementary idea of α -amino acids, peptide, (i) Reaction of iodide ion with hydrogen linkage, polypeptides, proteins; structure peroxide at room temperature using of amines-primary, secondary, tertiary different concentration of iodide ions. structure and quaternary structures (ii) Reaction between potassium iodate,

(qualitative idea only), denaturation of KIO3 and sodium sulphite (Na2SO3) 164

using starch solution as indicator G. Tests for the functional groups present (clock reaction). in organic compounds (c) Acid hydrolysis of ethyl acetate. Unsaturation, alcoholic, phenolic, B. Thermochemistry aldehydic, ketonic, carboxylic and amino Any one of the following experiments: (primary) groups. i] Enthalpy of dissolution of copper sulphate H. Characteristic tests of arbohydrates, fats or potassium nitrate. and proteins in pure samples and their ii] Enthalpy of neutralization of strong acid detection in given food stuffs. (HCl) and strong base (NaOH). I. Determinaiton of concentration/molarity

iii] Determination of enthalpy change during of KMnO4 solution by titrating it against interaction (hydrogen bond formation) a standard solution of: between acetone and . (i) Oxalic acid

iv] Heat of displacement of Cu from CuSO4 (ii) Ferrous ammonium sulphate by Zn. (Students will be required to prepare C. Electrochemistry standard solutions by weighing Variation of cell potential in themselves). Zn|Zn2+||Cu2+|Cu with change in J. Qualitative analysis

concentration of electrolytes (CuSO4 or 1) Determination of two cations from a given

ZnSO4) at room temperature mixture of salts. (demonstration). 2) Determination of two anions from a given D. Chromatography (demonstration) mixture of salts. (i) Separation of pigments from extracts of Cations – Pb2+, Cu2+, As3+, Al3+, Fe3+, leaves and flowers by paper Mn2+, Zn2+, Co2+, Ni2+, Ca2+, Sr2+, Ba2+, 2+ + chromatography and determination of Rf Mg ,NH4 , 2- 2- 2- - values. Anions – CO3 , SO3 , SO4 , NO2 NO3, - - - 3- 2- - (ii) Separation of constituents present in an Cl , Br , I , PO4 C2O4 CH3COO inorganic mixture containing two cations (Note : Insoluble salts excluded.) only (constituents having large difference in Rf values to be provided). PROJECT E. Preparation of Inorganic Compounds Scientific investigations involving (i) Preparation of double salt of ferrous laboratory testing and collecting ammonium sulphate or potash alum. information from other sources. (ii) Preparation of potassium ferric oxalate. A few suggested Projects: F. Preparation of Organic Compounds 1 Study of presence of oxalate ions in guava (i) p-Nitrocetanilide fruit at different stages of ripening. (ii) Aniline yellow or 2- Napthol aniline dye. 2 Study of quantity of casein present in (iii) Iodoform different samples of milk. (iv) Phthalic or succinic anhydride. 3 Preparation of soyabean milk and its (v) Di-benzal acetone comparison with the natural milk with 165

respect to curd formation, effect of flour, gram flour, potato juice, carrot juice, temperature, etc. etc. 4 Study of the effect of potassium bisulphate 7 Extraction of essential oils present in Saunf as food preservative under various (aniseed), Ajwain (carum), Illaichi conditions (temperature, concentration, (cardamom). time etc). 8 Study of common food adulterants in fat, 5 Study of digestion of starch by salivary butter, sugar, turmeric powder, chilli amylase and, effect of pH and temperature powder and pepper. on it. 6 Comparative study of the rate of Note : fermentation of following materials: wheat Any investigatory project, can be chosen with the approval of the teacher.