CBSE NCERT Notes for Class 11 Chemistry Part - 1 - Shikshaforall
CBSE NOTES FOR CLASS 11 CHEMISTRY PART - 1
CBSE NCERT Class 11 Chemistry part - 1 Notes - Free PDF Download
Well-prepared Class 11 Chemistry part - 1 Notes can help students understand the concepts, topics and themes covered in all the chapters. The Revision Notes for Class 11 Chemistry part - 1 offered by Shikshaforall are based on the latest curriculum that is approved by CBSE. Students don't have to stress about finding multiple books to revise during the exam period with such handy notes. The key benefit of these Notes of 11 Chemistry part - 1 is that they cover all the essential pointers, explain diagrams with examples that allow students to score well in the exams.
CHAPTER WISE REVISION NOTES FOR CBSE CLASS 11 CHEMISTRY PART - 1 PDF DOWNLOAD
REVISION NOTES FOR CLASS 11 CHEMISTRY PART - 1
Unit I : Some Basic Concepts of Chemistry
General Introduction: Importance and scope of chemistry. Nature of matter, laws of chemical combination, Dalton’s atomic theory: concept 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
Bohr’s model and its limitations, concept of shells and subshells, dual nature of matter and light, de Broglie’s relationship, Heisenberg uncertainty principle, concept of orbitals, quantum numbers, shapes of s, p and d orbitals, rules for filling electrons in orbitals - Aufbau principle, Pauli’s exclusion principle and Hund’s rule, electronic
configuration of atoms, stability of half-filled and completely filled orbitals.
Unit III : Classification of Elements and Periodicity in Properties
Modern periodic law and the present form of periodic table, periodic trends in properties of elements -atomic radii, ionic radii, inert gas radii, Ionization enthalpy, electron gain enthalpy, electronegativity, valency.
Nomenclature of elements with atomic number greater than 100.
Unit IV : Chemical Bonding and Molecular Structure
Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, polar character of covalent bond, covalent character of ionic bond, valence bond theory, resonance, geometry of covalent molecules,
VSEPR theory, concept of hybridization, involving s, p and d orbitals and shapes of some simple molecules, molecular orbital theory of homonuclear diatomic molecules(qualitative idea only), hydrogen bond.
Unit V : States of Matter: Gases, Liquids and Solids
Three states of matter, intermolecular interactions, types of bonding, melting and boiling points, role of gas laws in elucidating the concept of the molecule, Boyle’s law, Charles law, Gay Lussac’s law, Avogadro’s law, ideal behaviour, empirical derivation of gas equation,
Avogadro’s number, ideal gas equation. Deviation from ideal behaviour, liquefaction of gases, critical temperature, kinetic energy and molecular speeds (elementary idea)
Liquid State: vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations)
Solid state: Classification of solids based on different binding forces: molecular, ionic, covalent and metallic solids, amorphous and crystalline solids (elementary idea). Unit cell in two dimensional and three dimensional lattices, calculation of density of unit cell, packing
in solids, packing efficiency, voids, number of atoms per unit cell in a cubic unit cell, point defects, electrical and magnetic properties.
Unit VI : Chemical Thermodynamics
Concepts of 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, measurement of ΔU and ΔH, Hess’s law of constant heat
summation, enthalpy of bond dissociation, combustion, formation, atomization, sublimation, phase transition, ionization, solution and dilution. Second law of Thermodynamics (brief introduction). Introduction of entropy as a state function, Gibb’s energy change for
spontaneous and non- spontaneous processes, criteria for equilibrium. Third law of thermodynamics (brief introduction).
Unit VII : Equilibrium
Equilibrium in 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 poly basic acids, acid strength, concept of pH, Henderson Equation, hydrolysis of salts (elementary idea), buffer solution, solubility product, common ion effect (with illustrative examples).
CONTENTS OF CHEMISTRY PART ll
Unit VIII Redox Reactions
Unit IX Hydrogen
Unit X s -Block Elements
Unit XI p -Block Elements
Unit XII Organic Chemistry: Some Basic Principles and Techniques
Unit XIII Hydrocarbons
Unit XIV Environmental Chemistry
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