SATHEE: Chemistry 11

Chemistry 11 Chemistry 11

UNIT I: SOME BASIC CONCEPTS OF CHEMISTRY

Matter and its nature

Dalton’s atomic theory

Concept of atom

Molecule

UNIT II: STRUCTURE OF ATOM

Discovery of Electron, Proton and Neutron, atomic number, isotopes and isobars

Thomson’s model and its limitations

Rutherford’s model and its limitations, Bohr’s model and its limitations

Nature of electromagnetic radiation

photoelectric effect

Spectrum of the hydrogen atom

Bohr model of a hydrogen atom - its postulates

derivation of the relations for the energy of the electron and radii of the different orbits

limitations of Bohr’s model

Dual nature of matter

de Broglie’s relationship

Heisenberg uncertainty principle

Elementary ideas of quantum mechanics, quantum mechanics, the quantum mechanical model of the atom, its important features

Concept of atomic orbitals as one-electron wave functions: Variation of 𝚿 and 𝚿2 with r for ls and 2s orbitals

various quantum numbers (principal, angular momentum, and magnetic quantum numbers) and their significance

shapes of s, p, and d - orbitals

electron spin and spin quantum number

Rules for filling electrons in orbitals - Aufbau principle

Pauli’s exclusion principle and Hund’s rule

electronic configuration of elements, extra stability of half-filled and completely filled orbitals

UNIT III: CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

Significance of classification

Modem periodic law and present form of the periodic table, s, p, d and f block elements, periodic trends in properties of elements atomic and ionic radii, ionization enthalpy, electron gain enthalpy, valence, oxidation states, and chemical reactivity

UNIT IV: CHEMICAL BONDING AND MOLECULAR STRUCTURE

Kossel - Lewis approach to chemical bond formation, the concept of ionic and covalent bonds

Ionic Bonding: Formation of ionic bonds

factors affecting the formation of ionic bonds; calculation of lattice enthalpy

Covalent Bonding

concept of electronegativity

Fajan’s rule, dipole moment

valence Shell Electron Pair Repulsion (VSEPR) theory and shapes of simple molecules

Quantum mechanical approach to covalent bonding: Valence bond theory - its important features

the concept of hybridization involving s, p, and d orbitals

Resonance

Molecular orbital Theory - Its important features. LCAOs, types of molecular orbitals (bonding, antibonding), sigma and pi-bonds, molecular orbital electronic configurations of homonuclear diatomic molecules, the concept of bond order, bond length, and bond energy

Elementary idea of metallic bonding

Hydrogen bonding and its application

UNIT V: STATES OF MATTER : GASES AND LIQUIDS

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)

UNIT VI: THERMODYNAMICS

Fundamentals of thermodynamics: system and surroundings, extensive and intensive properties, state functions, types of processes

The first law of thermodynamics

concept of work, heat internal energy

enthalpy

heat capacity, molar heat capacity

Hess’s laws of constant heat summation

Enthalpies of bond dissociation, combustion formation, atomization, sublimation, phase transition, hydration, ionization, and solution

The second law of thermodynamics - Spontaneity of processes: ΔS of the universe and ΔG of the system as criteria for spontaneity

ΔG° (Standard Gibbs energy change)

equiliribrium constant

UNIT VII: EQUILIBRIUM

Meaning of equilibrium, the concept of dynamic equilibrium

Equilibria involving physical processes: Solid-liquid, liquid - gas and solid-gas equilibria

Henry’s law

General characteristics of equilibrium involving physical processes

Equilibrium involving chemical processes: Law of chemical equilibrium

equilibrium constants ($K_P$ and $K_C$) and their significance

the significance of ΔG and ΔG° in chemical equilibrium

factors affecting equilibrium - concentration, pressure

temperature, the effect of catalyst

Le Chatelier’s principle

Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenius, Bronsted - Lowry and Lewis) and their ionization, acid-base equilibria (including multistage ionization)

ionization constants, ionization of water. pH scale, common ion effect

hydrolysis of salts and pH of their solutions

the solubility of sparingly soluble salts

solubility products

buffer solutions

UNIT VIII: REDOX REACTIONS

Electronic concepts of oxidation and reduction

redox reactions

oxidation number, rules for assigning oxidation number

balancing of redox reactions

Electrolytic and metallic conduction, conductance in electrolytic solutions

molar conductivities and their variation with concentration

Kohlrausch’s law and its applications

Electrochemical cells

Electrolytic

Galvanic cells

different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions, emf of a Galvanic cell and its measurement

Nernst equation and its applications

Relationship between cell potential and Gibbs’ energy change

Dry cell and lead accumulator

Fuel cells

UNIT IX: HYDROGEN

Position of hydrogen in periodic table

occurrence

isotopes

preparation

properties and uses of hydrogen

hydrides-ionic covalent and interstitial

physical and chemical properties of water

heavy water

hydrogen peroxid-e-preparation

reactions and structure and use

hydrogen as a fuel

UNIT X: s-BLOCK ELEMENTS (ALKALI AND ALKALINE EARTH METALS)

Group 1 and Group 2 Elements: General introduction

electronic configuration

occurrence

anomalous

properties of the first element of each group

diagonal relationship

trends in the variation of properties (such as ionization enthalpy, atomic and ionic radii)

trends in chemical reactivity with oxygen and halogens, uses

Preparation and Properties of Some Important Compounds : Sodium Carbonate, Sodium Chloride, Sodium Hydroxide and Sodium Hydrogencarbonate

Biological importance of Sodium and Potassium

Calcium Oxide and Calcium Carbonate and their industrial uses

biological importance of Magnesium and Calcium

UNIT XI: SOME p- BLOCK ELEMENTS

General Introduction to p- Block Elements Group 13 Elements: General introduction

electronic configuration

occurrence

variation of properties

oxidation states

trends in chemical reactivity

anomalous properties of first element of the group

Boron - physical and chemical properties

some important compounds

Borax

Boric acid

Boron Hydrides

Alumunium : Reactions with acids and alkalies, uses

Group 14 Elements: General introduction

electronic configuration

occurrence

variation of properties

oxidation states

trends in chemical reactivity

anomalous behaviour of first elements

Carbon-catenation

allotropic forms

physical and chemical properties

uses of some important compounds: oxides

Important compounds of Silicon and a few use: Silicon Tetrachloride, Silicones, Silicates and Zeolites, their uses

UNIT XII: ORGANIC CHEMISTRY: SOME BASIC PRINCIPLES AND TECHNIQUES

Tetravalency of carbon: Shapes of simple molecules - hybridization (s and p)

Classification of organic compounds based on functional groups: and those containing halogens, oxygen, nitrogen, and sulphur; Homologous series

Isomerism

structural and stereoisomerism

Nomenclature (Trivial and IUPAC)

Covalent bond fission - Homolytic and heterolytic: free radicals, carbocations, and carbanions; stability of earbocations

free radicals, electrophiles, and nucleophiles

Electronic displacement in a covalent bond - Inductive effect, electromeric effect

resonance, and hyperconjugation

Common types of organic reactions - Substitution, addition, elimination, and rearrangement

UNIT XIII: HYDROCARBONS

Classification, isomerism, IUPAC nomenclature, general methods of preparation, properties, and reactions

Alkanes - Conformations: Sawhorse and Newman projections (of ethane): Mechanism of halogenation of alkanes

Alkenes - Geometrical isomerism: Mechanism of electrophilic addition

addition of hydrogen, halogens, water, hydrogen halides (Markownikoffs and peroxide effect)

Ozonolysis and polymerization

Alkynes - Acidic character: Addition of hydrogen, halogens, water, and hydrogen halides: Polymerization

Aromatic hydrocarbons - Nomenclature, benzene - structure and aromaticity

Mechanism of electrophilic substitution, halogenation, nitration

Friedel - Craft’s alkylation and acylation, directive influence of the functional group in monosubstituted benzene

UNIT XIV: ENVIRONMENTAL CHEMISTRY

Environmental pollution - air

water and soil pollution

chemical reactions in atmosphere

smog

major atmospheric pollutants

acid rain

ozone and its reactions

effects of depletion of ozone layer

greenhouse effect and global warming-pollution due to industrial wastes

green chemistry as an alternative tool for reducing pollution

strategies for control of environmental pollution

Engineering Preparation

Mathematics 11th

Mathematics 12th

JEE Previous Year Questions

JEE Tutorial Sessions

Medical Preparation

NEET Previous Year Questions

NEET Tutorial Sessions

NCERT Books & Solutions

NCERT Books for JEE

NCERT Books for NEET

NCERT Solutions for JEE

NCERT Solutions for NEET

NCERT Exemplar for JEE

NCERT Exemplar for NEET

Important Resources

Physics Formulas

Chemistry Formulas

Mathematics Formulas

Other Resources

Student Help Booklet

SPOC Help Booklet

Syllabus

Mentorship

Mentorship for JEE

Mentorship for NEET

NCERT Video Solution

NCERT Exemplar Video Solutions

NCERT Exercise Video Solution

BETA

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