Inquiztives!

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

• General Introduction: Importance and scope of Chemistry.
• Nature of Matter: Laws of chemical combination, Dalton’s atomic theory; concepts 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 (14 Periods)

• Discovery of Subatomic Particles: Electron, proton, neutron; atomic number, isotopes, and isobars.
• Atomic Models: Thomson’s model and limitations; Rutherford’s model and limitations; Bohr’s model and limitations.
• Concepts: Shells and subshells; dual nature of matter and light; de Broglie’s relationship; Heisenberg uncertainty principle.
• Quantum Mechanics: Concept of orbitals, quantum numbers; shapes of s, p, and d orbitals.
• Electron Configuration: Rules for filling electrons in orbitals (Aufbau principle, Pauli’s exclusion principle, Hund’s rule); stability of half-filled and completely filled orbitals.

Unit III: Classification of Elements and Periodicity in Properties (08 Periods)

• Significance of Classification: Brief history of the development of the periodic table.
• Modern Periodic Law: Present form of the periodic table; periodic trends in properties of elements:
  • Atomic radii
  • Ionic radii
  • Inert gas radii
  • Ionization enthalpy
  • Electron gain enthalpy
  • Electronegativity
  • Valency
• Nomenclature: Elements with atomic numbers greater than 100.

Unit IV: Chemical Bonding and Molecular Structure (14 Periods)

• Valence Electrons: Ionic bond, covalent bond, bond parameters, Lewis structure.
• Covalent Bond: Polar character; covalent character of ionic bond.
• Valence Bond Theory: Resonance; geometry of covalent molecules; VSEPR theory.
• Hybridization: Concept involving s, p, and d orbitals; shapes of simple molecules.
• Molecular Orbital Theory: Qualitative idea of homonuclear diatomic molecules; hydrogen bond.

Unit V: Chemical Thermodynamics (16 Periods)

• Concepts: System and types of systems; surroundings; work, heat, energy; extensive and intensive properties; state functions.
• First Law of Thermodynamics: Internal energy and enthalpy; heat capacity and specific heat.
• Measurements: Measurement of U and H; Hess’s law of constant heat summation.
• Enthalpy Changes: Bond dissociation, combustion, formation, atomization, sublimation, phase transition, ionization, solution, and dilution.
• Second Law of Thermodynamics: Brief introduction; entropy as a state function; Gibbs energy change for spontaneous and non-spontaneous processes; criteria for equilibrium.
• Third Law of Thermodynamics: Brief introduction.

Unit VI: Equilibrium (14 Periods)

• Equilibrium in Processes: 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.
• Hydrolysis of Salts: Elementary idea; buffer solutions; Henderson Equation; solubility product; common ion effect (with illustrative examples).

Unit VII: Redox Reactions (06 Periods)

• Concepts: Oxidation and reduction; redox reactions; oxidation number.
• Balancing Redox Reactions: In terms of loss and gain of electrons; change in oxidation number.
• Applications: Applications of redox reactions.

Unit VIII: Organic Chemistry – Some Basic Principles and Techniques (14 Periods)

• General Introduction: Methods of purification; qualitative and quantitative analysis.
• Classification and Nomenclature: IUPAC nomenclature of organic compounds.
• Electronic Displacements: Inductive effect, electromeric effect, resonance, and hyperconjugation.
• Fission of Covalent Bonds: Homolytic and heterolytic fission; free radicals; carbocations; carbanions; electrophiles and nucleophiles.
• Types of Organic Reactions: Overview of organic reaction types.

Unit IX: Hydrocarbons (12 Periods)

• Classification of Hydrocarbons:
  • Aliphatic Hydrocarbons:
    • Alkanes: Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions including free radical mechanism of halogenation, combustion, and pyrolysis.
    • Alkenes: Nomenclature, structure of double bond (ethene), geometrical isomerism, physical properties, methods of preparation, chemical reactions (addition of hydrogen, halogen, water, hydrogen halides, ozonolysis, oxidation).
    • Alkynes: Nomenclature, structure of triple bond (ethyne), physical properties, methods of preparation, chemical reactions (acidic character, addition reactions).
  • Aromatic Hydrocarbons: Introduction, IUPAC nomenclature, benzene (resonance, aromaticity), chemical properties (mechanism of electrophilic substitution: nitration, sulphonation, halogenation, Friedel-Craft’s alkylation and acylation, directive influence of functional groups in monosubstituted benzene).
  • Carcinogenicity and Toxicity.

PART-2

Unit II: Solutions (10 Periods)

• Types of Solutions: Expression of concentration of solutions of solids in liquids.
• Solubility: Solubility of gases in liquids; solid solutions.
• Raoult’s Law: Introduction and applications.
• Colligative Properties:
  • Relative lowering of vapour pressure.
  • Elevation of boiling point.
  • Depression of freezing point.
  • Osmotic pressure.
• Determination of Molecular Masses: Using colligative properties; abnormal molecular mass; Van’t Hoff factor.

Unit III: Electrochemistry (12 Periods)

• Redox Reactions: Basics and significance.
• Electromotive Force (EMF): EMF of a cell; standard electrode potential.
• Nernst Equation: Application to chemical cells.
• Gibbs Energy and EMF: Relation between Gibbs energy change and EMF of a cell.
• Conductance in Electrolytic Solutions: Specific and molar conductivity; variations of conductivity with concentration; Kohlrausch’s Law.
• Electrolysis: Introduction and law of electrolysis (elementary idea).
• Electrolytic Cells: Dry cells, Galvanic cells, lead accumulator, fuel cells, corrosion.

Unit IV: Chemical Kinetics (10 Periods)

• Rate of Reaction: Average and instantaneous rates.
• Factors Affecting Rate: Concentration, temperature, catalyst.
• Order and Molecularity: Definition and distinction; rate law and specific rate constant.
• Integrated Rate Equations: Half-life (only for zero and first-order reactions).
• Collision Theory: Concept (elementary idea, no mathematical treatment).
• Activation Energy: Arrhenius equation.

Unit VIII: d and f Block Elements (12 Periods)

• General Introduction: Electronic configuration; occurrence and characteristics of transition metals.
• Trends in Properties: First row transition metals – metallic character, ionization enthalpy, oxidation states, ionic radii, color, catalytic property, magnetic properties, interstitial compounds, alloy formation.
• Preparation and Properties: K₂Cr₂O₇ and KMnO₄.
• Lanthanoids: Electronic configuration, oxidation states, chemical reactivity, lanthanoid contraction and its consequences.
• Actinoids: Electronic configuration, oxidation states, comparison with lanthanoids.

Unit IX: Coordination Compounds (12 Periods)

• Introduction: Coordination compounds, ligands, coordination number.
• Properties: Color, magnetic properties, and shapes.
• IUPAC Nomenclature: Mononuclear coordination compounds.
• Bonding Theories: Werner’s theory, VBT, and CFT.
• Structure and Stereoisomerism: Importance of coordination compounds (in qualitative analysis, extraction of metals, and biological systems).

Unit X: Haloalkanes and Haloarenes (10 Periods)

• Haloalkanes: Nomenclature, nature of C–X bond, physical and chemical properties, optical rotation, mechanism of substitution reactions.
• Haloarenes: Nature of C–X bond, substitution reactions (directive influence of halogen in monosubstituted compounds).
• Uses and Environmental Effects: Of dichloromethane, trichloromethane, tetrachloromethane, iodoform, freons, DDT.

Unit XI: Alcohols, Phenols and Ethers (10 Periods)

• Alcohols: Nomenclature, methods of preparation, physical and chemical properties (of primary alcohols only), identification of primary, secondary, and tertiary alcohols, mechanism of dehydration, uses (special reference to methanol and ethanol).
• Phenols: Nomenclature, methods of preparation, physical and chemical properties, acidic nature, electrophilic substitution reactions, uses of phenols.
• Ethers: Nomenclature, methods of preparation, physical and chemical properties, uses.

Unit XII: Aldehydes, Ketones and Carboxylic Acids (10 Periods)

• Aldehydes and Ketones: Nomenclature, nature of carbonyl group, methods of preparation, physical and chemical properties, mechanism of nucleophilic addition, reactivity of alpha hydrogen in aldehydes, uses.
• Carboxylic Acids: Nomenclature, acidic nature, methods of preparation, physical and chemical properties; uses.

Unit XIII: Amines (10 Periods)

• Amines: Nomenclature, classification, structure, methods of preparation, physical and chemical properties, uses, identification of primary, secondary, and tertiary amines.
• Diazonium Salts: Preparation, chemical reactions, and importance in synthetic organic chemistry.

Unit XIV: Biomolecules (12 Periods)

• Carbohydrates: Classification (aldoses and ketoses), monosaccharides (glucose and fructose), D-L configuration, oligosaccharides (sucrose, lactose, maltose), polysaccharides (starch, cellulose, glycogen); importance of carbohydrates.
• Proteins: Elementary idea of amino acids, peptide bond, polypeptides, proteins; structure of proteins (primary, secondary, tertiary, and quaternary structures – qualitative idea only); denaturation of proteins; enzymes.
• Hormones: Elementary idea excluding structure.
• Vitamins: Classification and functions.
• Nucleic Acids: DNA and RNA.