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Chemistry (55) 156 Chemistry (55) 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 molar mass : 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, solubility 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), hydrogen 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. Carbon – 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. Melting point 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 : (ethane 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. (acetone, 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.
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