TS 1st Year Chemistry Syllabus 2024-25: Download Detailed Class 11 Syllabus PDF For Free!

Chapter and Topics to be covered

Syllabus dictation and discussion of IPE question paper – weightage of marks to each chapter

1.1 Sub-atomic particles

1.2 Atomic models- Rutherford’s nuclear model of the atom

1.3 Developments to Bohr’s model of the atom

1.4 Bohr’s model for the hydrogen atom.

1.5 Towards a quantum mechanical model of the atom.

1.6 Quantum mechanical model of an atom. Important features of the quantum mechanical model of atom-orbitals and quantum numbers-shapes of atomic orbitals-energies of orbitals-filling of orbitals in atoms. Aufbau principle,

Pauli’s exclusion principle and Hund’s rule of maximum multiplicity- Electronic configurations of atoms-Stability of half-filled and filled orbitals.

2.1 Need to classify elements

2.2 Genesis of Periodic Classification

2.3 Modern periodic law and present form of the periodic table

2.4 Nomenclature of elements with atomic number greater than100

2.5 Electronic configuration of elements and the periodic table

2.6 Electronic configuration and types of elements s,p,d and f

2.7 Trends in physical properties-periodic trends chemical properties-Periodic trends and chemical Reactivity

3.1 Kossel – Lewis approach to chemical bonding

3.2 Ionic or electrovalent bond

3.3 Bond Parameters

3.4 The Valence Shell Electron Pair Repulsion (VSEPR) theory.

3.5 Valence bond theory

3.6 Hybridisation

3.7 Coordinate bond

3.8 Molecular orbital theory –bonding in some homonuclear diatomic molecules

3.9 Hydrogen bonding

PRACTICALS: I. Acquinttance with Laboratory Equipment:

1. Bunsen burner, Spirit Lamp Basic Laboratory equipment (Burette, pipette, conical flask, volumetric flask, measuring, cylinder, wash bottle etc.,)

UNIT TEST - I

4.1 Intermolecular forces

4.2 Thermal energy

4.3 Intermolecular forces vs. thermal interactions.

4.4 The gaseous state

4.5 The gas laws

4.6 Ideal gas equation

4.7 Graham’s law of diffusion – Dalton’s law of partial pressures

4.8 Kinetic molecular theory of gases

4.9 Kinetic gas equation of an ideal gas (no derivation)- Deduction of gas laws from kinetic gas equation

4.10 Distribution of molecular speeds – rms, average and most probable speeds-kinetic energy of gas molecules

4.11 Behaviour of real gases – deviation from ideal gas behaviour – compressibility factor Vs pressure diagrams of real gases

4.12 Liquefaction of gases

4.13 Liquid state – properties of liquids in terms of inter-molecular interactions – vapour pressure, viscosity and surface tension (Qualitative idea only, no mathematical derivation)

5.1 Some basic concepts

5.2 Laws of chemical combinations, Gay Lussac’s law of Gaseous volumes, Dalton’s atomic theory, Avogadro's law

5.3 Atomic and molecular masses- mole concept and molar mass concept of equivalent weight

5.4 Percentage composition of compounds and calculations of empirical and molecular formulae of compounds

5.5 Stoichiometry and stoichiometric calculations

5.6 Methods of expressing concentrations of solutions

PRACTICALS: II. Basic Laboratory Techniques

UNIT TEST - II

5.7 Redox reactions

5.8 Oxidation number concept

5.9 Types of redox reactions

5.10 Balancing of redox reactions – oxidation number method-half reaction (ion-electron) method

5.11 Redox reactions in titrimetry

6.1 Thermodynamic terms

6.2 Applications-work-enthalpy-extensive and intensive properties-heat capacity

6.3 Measurement of “U and H”: Calorimetry

6.4 Enthalpy change, ‘rH’ of reactions

6.5 Enthalpies for different types of reactions

6.6 Spontaneity

6.7 Gibbs Energy change and equilibrium

6.8 Absolute entropy and the third law of thermodynamics

Practicals: III. Purification of Chemical substances

UNIT TEST - III

7.1 Equilibrium in physical process

7.2 Equilibrium in chemical process – dynamic equilibrium

7.3 Law of chemical equilibrium - law of mass action and equilibrium constant

7.4 Homogeneous equilibria, equilibrium constant in gaseous systems, the relationship between Kp and Kc

7.5 Heterogeneous equilibrium

7.6 Applications of equilibrium constant

7.7 Relationship between equilibrium constant ‘K’, reaction Quotient ‘Q’ and Gibbs energy ‘G’

7.8 Factors affecting equilibria,-Le-chatelier’s principle application to industrial synthesis of ammonia and sulphur trioxide

7.9 Ionic equilibrium in solutions.

7.10 Acids, bases and salts- Arrhenius, Bronsted-Lowry and Lewis concepts of acids and bases

7.11 Ionisation of acids and bases

7.12 Buffer solutions

7.13 Solubility equilibria of sparingly soluble salts

Solubility product constant-common ion effect on solubility of Ionic salts

8.1 Position of hydrogen in the periodic table

8.2 Dihydrogen-occurrence and isotopes

8.3 Preparation of dihydrogen

8.4 Properties of dihydrogen

8.5 Hydrides: Ionic, covalent, and non- stiochiometric hydrides

8.6 Water: Physical properties; structure of water, ice chemical properties of water; hard and soft water

temporary and permanent hardness of water

8.7 Hydrogen peroxide: Preparation; physical properties; structure and chemical properties; storage and uses.

8.8 Heavy water

8.9 Hydrogen as a fuel

Practicals:

IV. Experiments related to pH change

V. Chemical equilibrium

VI. Quantitative estimation (Volumetric analysis)

MID-TERM HOLIDAYS FROM 06-10-2024 TO 13-10-2024

DATE OF RE-OPENING 14-10-2024

9.1 Alkali metals; Electronic configurations; atomic and ionic radii; ionization enthalpy; hydration enthalpy; physical properties; chemical properties; uses

9.2 General characteristics of the compounds of the alkali metals: oxides; halides; salts of oxyacids

9.3 Anomalous properties of lithium:

9.4 Some important compounds of sodium: Sodium carbonate; sodium chloride; sodium hydroxide; and sodium hydrogen carbonate.

9.5 Biological importance of sodium and potassium.

Group 2 elements

9.6 Alkaline earth elements; Electronic configuration; ionization enthalpy; hydration enthalpy; physical properties; chemical properties; uses

9.7 General characteristics of compounds of the Alkaline earth metals. Oxides, hydroxides, halides, salts of oxyacids (carbonates, sulphates and nitrates)

9.8 Anomalous behaviour of beryllium; its diagonal relationship with aluminium

9.9 Some important compounds of calcium

9.10 Biological importance of calcium and magnesium

10.1 General introduction – Electronic configuration, atomic radii, ionization enthalpy, electro negativity;

physical & chemical properties

10.2 Important trends and anomalous properties of boron

10.3 Some important compounds of boron – borax, orthoboric acid, diborane

10.4 Uses of boron, aluminium and their compounds

11.1 General introduction - Electronic configuration, atomic radii, ionization enthalpy, electro negativity; physical & chemical properties

11.2 Important trends and anomalous properties of carbon

11.3 Allotropes of carbon

11.4 Uses of carbon

11.5 Some important compounds of carbon and silicon – carbon monoxide, carbon dioxide, silica, silicones, silicates and zeolites

HALF-YEARLY EXAMINATIONS

FROM 18-11-2024 TO 23-11-2024

12.1 Definition of terms: Air, Water and Soil Pollutions

12.2 Environmental pollution

12.3 Atmospheric pollution

12.4 Acid rain: Particulate pollutants

12.5 Stratospheric pollution

12.6 Water pollution

12.7 Soil Pollution: Pesticides, industrial wastes.

12.8 Strategies to Control Environmental Pollution

12.9 Green Chemistry

13.1 General introduction

13.2 Tetravalency of Carbon: shapes of organic compounds

13.3 Structural representations of organic compounds

13.4 Classification of organic compounds

13.5 Nomenclature of organic compounds

13.6 Isomerism

13.7 Fundamental concepts in organic reaction mechanisms

13.8 Methods of purification of organic compounds

13.9 Qualitative elemental analysis of organic compounds

13.10 Quantitative elemental analysis of organic compounds

Practicals: VII. Qualitative Analysis

1. Reactions of the following anions with at least one confirmatory test for each anion. Carbonate(CO3 2-) Sulphide(S2-),Sulphite(SO3 2- ) , Sulphate(SO4 2), Nitrite(NO2 -),Nitrate(NO3 -) Chloride(Cl-) Bromide(Br-), Iodide(I-), Phosphate (PO4 3-), Acetate (CH3COO-)

13.11 Classification of hydrocarbons

13.12 Alkanes – Nomenclature, isomerism (structural and conformations of ethane only) preparation of alkanes -properties of alkanes

13.13 Alkenes- Nomenclature, structure of ethane, isomerism (structural and geometrical)- methods of preparation of alkenes-properties of alkenes

13.14 – Nomenclature and isomerism, structure of acetylene methods of preparation of acetylene-physical properties and chemical reactions of alkynes

13.15 Nomenclature and isomerism structure of benzene, resonance and aromaticity-preparation of benzene physical and chemical properties of benzene-directive influence of functional groups in mono substituted benzene. Carcinogenicity and toxicity

Practicals: VII. 2. Reactions of the following cations with

at least one confirmatory test for each cation Lead(Pb2+), Copper (Cu2+), Aluminium(Al3+), Ferric(Fe3+),Manganese (Mn2+), Nickle (Ni2+),

Zinc(Zn2+),Cobalt(Co2+),Calcium(Ca2+),Strontium(Sr2+),

Barium(Ba2+), Magnesium(Mg2+) and Ammonium (NH 4+ )

PRE-FINAL EXAMINATIONS FROM 20-01-2025 TO 25-01-2025

SANKRANTHI HOLIDAYS

FROM 11-01-2025 TO 16-01-2025

REVISION