BOARD OF INTERMEDIATE EDUCATION: A.P. NAMPALLY, HYDERABAD
SYLLABUS (New) – CHEMISTRY I YEAR
Class - XI
1. ATOMIC STRUCTURE PERIODS: 14
1.1 Characteristics of electron, proton and neutron.
1.2 Rutherford model of an atom.
1.3 Nature of electromagnetic radiation,
1.4 Planck's quantum theory.
1.5 Explanation of photo electric effect.
1.6 Features of atomic spectra.
1.7 Characteristics of hydrogen spectrum.
1.8 Bohr's theory of the structure of the atom.
1.9 Bohr's explanation of spectral lines.
1.10 Failure of Bohr's theory.
1.11 Wave-particle nature of electron.
1.12 de Broglie's hypothesis, Heisenberg's uncertainty principle.
1.13 Important features of the quantum mechanical model of an atom.
1.14 Quantum numbers, concept of orbitals, define an atomic orbital in terms of quantum numbers - shapes of s, p and d orbitals, state Aufbau principle, Pauli's exclusion principle and Hund's rule of maximum multiplicity.
1.15 Electronic configurations of atoms. Explanation of stability of half filled and completely filled orbitals.
2. Classification Of Element And Periodicity In Properties: Period 13
2.1 The concept of grouping elements In accordance to their properties.
2.2 The periodic law.
2.3 The significance of atomic number and electronic configuration as the basis for periodic classification.
2.4 Classify elements into s, p, d, f blocks and discuss their main characteristics.
2.5 Periodic trends in physical and chemical properties of elements.
2.6 Periodic trends of elements with respect to atomic radii, ionic radii, inert gas radii, ionization energy, electron gain energy, electro negativity, valence.
2.7 Variation of atomic radii in inner transition elements.
3. CHEMICAL BONDING AND MOLECULAR STRUCTURE: PERIODS 15
3.1 Kossel-Lewis approach to chemical bonding.
3.2 Factors favorable for the formation of ionic bond, energy changes in ionic bond formation.
3.3 Crystal lattice energy - calculation of lattice energy - Bom-Haber cycle.
3.4 Crystal structures of sodium chloride and Caesium chloride.
3.5 Properties of ionic compounds.
3.6 Covalent bond - VSEPR theory and predict the geometry of simple molecules.
3.7 The valance bond approach for the formation of covalent bonds.
3.8 Directional properties of covalent bond.
3.9 Properties of covalent bond.
3.10 Different types of hybridization involving s, p and d orbitals and draw shapes of simple covalent molecules.
3.11 Definition of coordinate covalent bond with examples.
3.12 Description of molecular orbital theory of homonuclear diatomic molecules.
3.13 Bonding, antibonding molecular orbitals, o, n bond orbitals, their symmetry.
3.14 Energy diagrams of molecular orbitals of H2, N2 and 02.
3.15 Concept of hydrogen bond - Types of hydrogen bonds, inter and intra molecular hydrogen bonds.
3.16 Effect of hydrogen bonds on some properties of substances with examples.
3.17 Different states of matter in terms of balance between intermolecular forces, thermal energy of particles.
4. STATES OF MATTER : GASES AND LIQUIDS. PERIODS 14
4.1 Graham's law of diffusion, Dalton's law of partial pressures, Avogadro's law.
4.2 Ideal behavior, empirical derivation of gas equation, ideal gas equation.
4.3 Kinetic molecular theory of gases
4.4 Kinetic gas equation (No derivation) - deduction of gas laws
4.5 Distribution of molecular velocities, types of molecular velocities
4.6 Behavior of real gases, deviation from ideal behavior, Compressibility factor Vs pressure - diagrams of real gases.
4.7 Conditions of liquefaction of gases, critical temperature.
4.8 Liquid state - Properties of liquids in terms of intermolecular attractions.
4.9 Vapor pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations)
5. STOICHIOMETRY: PERIODS 13
5.1 Laws of chemical combination, principles and examples.
5.2 Molar mass, concept of equivalent weight with examples.
5.3 percentage composition of compounds and calculations of empirical and molecular formula of compounds.
5.4 Chemical reactions and equations
5.5 Oxidation number concept.
5.6 Balancing of redox reactions by ion electron method and oxidation number method.
5.7 Types of redox reactions.
5.8 Applications of redox reactions in titrimetric quantitative analysis and redox reactions in electrode process.
5.9 Numerical calculations based on equations.
6. HYDROGEN AND ITS COMPOUNDS: - PERIODS 8
6.1 Position of hydrogen in periodic table.
6.2 Occurrence, Isotopes of hydrogen.
6.3 Hydrogen preparation, properties and uses including as a fuel.
6.4 Reaction of hydrogen with different types of elements leading to ionic, molecular and non-stoichiometric hydrides.
6.5 Physical and Chemical properties of water and heavy water.
6.6 Hydrogen peroxide - preparation methods, physical and chemical properties - oxidation, reduction - decomposition - disproportionation and addition reactions.
6.7 Detection of hydrogen peroxide. Structure of H202, uses of H20,.
7. ALKALI AND ALKALINE EARTH METALS: PERIODS 12
7.1 General Introduction, electronic configuration, occurrence,
7.2 Anomalous properties of the first element in each group.
7.3 Diagonal relationship.
7.4. Trends in properties like Ionization enthalpy, atomic and ionic radii, reactivity with oxygen, hydrogen, halogens and water, uses.
7.5. Preparation and properties of some important compounds: Sodium hydroxide, salts of oxo acids, sodium carbonate and sodium hydrogen carbonate. Sodium chloride.
7.6 Biological importance of sodium and potassium.
7.7 CaO, CaCO3 and CaSO4 preparation and uses.
7.8 Industrial use of lime and lime stone.
7.9 Biological importance of Mg and Ca.
8. p-BLOCK ELEMENTS: GROUP 13 ELEMENTS(IIIA GROUP ELEMENTS): PERIODS 6
8.1 General introduction, electronic configuration, occurrence,
8.2 variation of properties, oxidation states, trends in chemical reactivity.
8.3 anomalous properties of first clement of the group.
8.4 Boron- physical and chemical properties and uses,
8.5 Some important compounds: borax, boric acids, boron hydrides.
8.6 Aluminum: uses, reactions with acids and alkalis,
8.7 Potash alum.
9. GROUP 14 ELEMENTS: (IVA GROUP ELEMENTS): PERIODS 9
9.1 General introduction, electronic configuration, occurrence.
9.2 variations of properties, oxidation states, trends in chemical reactivity.
9.3 Anomalous behaviour of first element.
9.4 Carbon - catenation, allotropic forms, physical and chemical properties and uses;
9.5 Similarities between carbon and silicon, uses of oxides of carbon;
9.6 Important compounds of silicon, silicon dioxide and a few uses of silicon
tetrachloride, silicones, silicates and zeolites( Elementary ideas)
9.7 Fuel gases - producer gas and water gas manufacture and uses.
10. GROUP 18 ELEMENTS: (ZERO GROUP ELEMENTS) PERIODS 6
10.1 General introduction, electronic configuration, occurrence, isolation
10.2 Trends in physical and chemical properties, uses.
10.3 Compounds of xenon oxides and halides (Structures only).
11. Environmental Chemistry PERIODS 9
11.1 Definition of terms: Air, water and soil pollution.
11.2 Oxides of carbon, Carbon monoxide,
11.3 oxides of nitrogen and sulphur, chlorofluoro carbons.
11.4 Chemical reactions in atmosphere, smog's, major atmospheric pollutants, acid rain,
11.5 ozone and its reactions, effects of depletion of ozone layer.
11.6 Green house effect and global warming.
11.7 Pollution due to industrial wastes. 11.8 Green chemistry as an alternative tool for reducing pollution with two examples.
12. ORGANIC CHEMISTRY-SOME BASIC PRINCIPLES AND TECHNIQUES: PERIODS 24
12.1 General introduction, methods of purification, qualitative and quantitative analysis,
12.2 classification and IUPAC nomenclature of organic compounds.
12.3 Electronic displacements in a covalent bond: inductive effect, electromeric effectresonance and hyper conjugation.
12.4 Fission of a covalent bond: Homolytic and heterolytic fissions.
12.5 Types of reagents: Electrophiles, nucleophiles and free radicals - examples, reactive intermediates.
12.6 Common types of organic reactions- substitution, addition, elimination and rearrangement reactions with examples.
HYDROCARBONS:
12.7 Classification of hydrocarbons
12.8 Alkanes - Nomenclature, isomerism, conformations (ethane only)
12.9 Methods of preparation of ethane.
12.10 Physical properties, chemical reactions Including free radical mechanism of halogenation, combustion and pyrolysis of ethane.
12.11 Cycloalkanes, preparation and properties of cyclohexane.
12.12 Alkenes - Nomenclature, structure of double bond (ethene), geometrical isomerism, physical properties
12.13 Methods of preparation of ethylene.
12.14 Physical properties, chemical reactions: addition of hydrogen, halogen, water, hydrogen halides (Markovnikov's addition and peroxide effect), ozonolysis,oxidation, mechanism of electrophilic addition.
12.15 Alkynes - Nomenclature, structure of triple bond (acetylene), methods of preparation of acetylene
12.16 Physical properties, chemical reactions: acidic character of acetylene, addition reaction of - hydrogen, halogens, hydrogen halides and water.
12.17 Aromatic hydrocarbons: Introduction, IUPAC nomenclature; Benzene: resonance, aromaticity.
12.18 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 toxlclty.
12.19 Stereo chemistry: Introduction of Isomerism and recapitulation of geometrical isomerism and conformations.
12.20 optical activity-discovery, determination using a polarimeter, specific rotation, chirality-chiral objects, chiral molecules.
12.21 configuration and Fischer projections,
12.22 asymmetric carbon, elements of symmetry,
12.23 compounds containing one chiral centre, enantiomers,
12.24 D-L and R-S nomenclature, racemic forms, racemisation.
12.25 Compounds containing two chiral centers, diastereoisomers, mesoform, resolution, importance of stereochemistry.