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TN State Board 11th Chemistry Tuition

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What will you learn in this course?
    • Promote understanding of basic facts and concepts in chemistry while retaining the excitement of chemistry.
    • Make students capable of studying chemistry in academic and professional courses (such as medicine, engineering, technology) at tertiary level.
    • Expose the students to various emerging new areas of chemistry and apprise them with their relevance in future studies and their application in various spheres of chemical sciences and technology.
    • Equip students to face various challenges related to health, nutrition, environment, population, weather, industries and agriculture.
    • Develop problem solving skills in students.
    • Expose the students to different processes used in industries and their technological applications.
    • Apprise students with the interface of chemistry with other disciplines of science such as physics, biology, geology, engineering etc.
    • Acquaint students with different aspects of chemistry used in daily life.
    • Develop an interest in students to study chemistry as a discipline.

    Integrate life skills and values in the context of chemistry

₹ 12000
Course Teacher
Course Information
Category
Duration
Hours
Price
₹ 12000

* Exclusive of 18% GST

Includes
    • Assignments every week
    • 200+ MCQs
    • Courseware prepared by experts
    • Assessments to give you the level of improvement

Class 11th Chemistry becomes a mystical journey for kids who rack their brains to comprehend ideas, from equations to explanations. We assist students in making the mysterious magic by breaking down topics into easy-to-understand bite size chunks so that they may grasp subject material. They give SCERT Solutions for Tamilnadu State Board 11th Chemistry in a chapter-wise format and help students understand the concepts in each area.

The courses have been created based on Class 11th Tamilnadu State Board Board Exam pattern.Make the most of your practise time by using questions tailored to your specific requirements. The subject experts deliver live lectures in this course. A thorough curriculum with study materials prepared by subject experts is provided. You may also take part in the live doubt sessions, as well as one-on-one doubt solutions. 

Course Features

120 hours of Live Classes
200+ MCQ Test Series
Live Doubt Resolution
Individual Attention

Course Structure

Units Topics
I Basic concepts of chemistry and chemical calculations
II Quantum mechanical model of the atom
III Elements and periodic classification
IV Hydrogen and water
V Alkaline and alkaline earth metals
VI Chemical Bonding
VII Thermodynamics
VIII Gaseous state
IX Solutions
X Chemical equilibrium
XI Organic Chemistry – Basic principles and technique
XII Organic reactions and their mechanism
XIII Hydrocarbons
XIV Halo-alkanes and haloarenes
XV Environmental chemistry

Course Lessons

Importance of Chemistry; Classification of matters; Elements and compounds; Atomic and molecular masses; equivalent mass, empirical and molecular formula; mole concept; stoichiometric calculations; Limiting reagents, redox reactions, competitive electron transfer reactions, oxidation number; types of redox reactions and balancing redox reactions

A brief introduction to various atom models; Dual behavior of matter; Debroglie relation, Heisenberg’s uncertainty principle; Quantum mechanical model of atom; Schrodinger equation, Quantum numbers; Atomic orbitals – shapes, energy, Aufbau principle, Pauli exclusion principle, Hund’s rule; Electronic configuration of atoms, stability of completely filled and half-filled orbitals

Need for classification of elements; Modern periodic law and the periodic table; Nomenclature of elements with atomic numbers greater than 100; Classification of elements based on electronic configurations; Periodic trends in properties - atomic radius, ionic radius, ionization enthalpy, electron affinity, electronegativity; Periodic trends in chemical properties, periodicity of valence/oxidation states, Anomalous properties of second-period elements, Diagonal relationship

Position of hydrogen in the periodic table, isotopes of hydrogen, ortho and para hydrogen; Preparation of hydrogen: laboratory and commercial production; Physical and chemical properties of hydrogen, uses of hydrogen; Hydrides: classification; Physical and chemical properties of water, heavy water; hardness of water and its removal; Hydrogen peroxide: Preparation, structure, physical and chemical properties, uses.

Alkali metals: General characteristics, chemical properties and uses; general characteristics; physical, chemical properties and uses; compounds of alkali metals: oxides, hydroxides, halides, salts of oxoacids – general characteristics; Biological importance of sodium and potassium. Alkaline earth metals: general characteristics, physical, chemical properties and uses; compounds of alkaline earth metals: oxides, hydroxides, halides, salts of oxoacids – general characteristics; important compounds of calcium: quick lime, slake lime, gypsum, and plaster of paris; Biological importance of magnesium and calcium.

Kossel – Lewis approach to chemical bonding; octet rule, ionic bond, covalent bond, coordinate bond; bonding in metals; Bond parameters; resonance; polarity of bonds; Hybridisation – Orbital overlap, σ and π bonds, VSEPR theory, shapes of covalent molecules; Valence bond theory (VBT), Molecular Orbital Theory: Bonding in homonuclear diatomic molecules (H2, Li2, B2, C2, N2and O2) and hetero-nuclear diatomic molecules (CO and NO); Hydrogen bond – criteria, types, and significance.

Introduction to thermodynamic terms, System, and surroundings, types and properties of the system: processes: reversible, irreversible, adiabatic, isothermal, isobaric, isochoric, and cyclic processes; Internal energy and work; First law of thermodynamics; Enthalpy: the relationship between ΔH and ΔU; Thermochemical equations; Enthalpy changes for different types of reactions and phase transformations; Measurement of ΔH and ΔU using calorimetry; Hess law of constant heat summation; Lattice enthalpy: Born-Haber cycle; Need for the second law of thermodynamics; various statements of second law; Meaning and significance of entropy; Gibbs free energy and its significance; criteria for spontaneity of a process; Relationship between ΔG and equilibrium constant; Third law of thermodynamics (statement only)

Introduction; Gas laws: Boyle’s law, Charles law, Gay Lussac’s law, Avogadro law; Ideal gas equation and deviation from ideal behavior; Compressibility factor; Vanderwaal’s equation; critical phenomena; Relation between Vander-Waals constants and critical constants; diffusion - Grahams diffusion law; Liquefaction of gases – Joule Thomson effect; isotherms of carbon dioxide

Types of solutions; expressing Concentration of solutions – mass percentage, volume percentage, parts per million (ppm), mole fraction, molarity, molality, and normality; Henry’s law, Vapour pressure of liquid solutions; Raoult’s law for volatile solutes and non-volatile solutes; ideal and non-ideal solutes; factors responsible for deviation from Raoult’s law. Colligative properties; Relative lowering of vapor pressure; depression of freezing point; Elevation of boiling point; Osmosis and osmotic pressure; Reverse osmosis and water purification; Abnormal molecular mass: Dissociation and association, Vant Hoff factor.

Introduction to physical and chemical equilibria; Law of mass action; Equilibrium constants (Kp and Kc); Relation between Kp and Kc; Homogeneous and Heterogeneous equilibrium; Applications of equilibrium constants in predicting the extend and the direction of a reaction; Lechatlier’s principle – effect of concentration, pressure, temperature, catalyst, and inert gas addition; Vant-Hoff equation

Introduction, Classification, and nomenclature of organic compounds; IUPAC rules for naming organic compounds; structural representation; Isomerism – structural isomerism, stereoisomerism: Geometrical and optical isomerism, Detection and estimation of elements (C, H, N, S, X, and P) in organic compounds; Purification of organic compounds – sublimation, crystallization, distillation (fraction, steam and azeotropic), differential extraction, chromatography (absorption, column, thin layer, and partition chromatography)

Fundamental concepts in organic reaction mechanism; Fission of covalent bond; Nucleophiles, electrophiles, and free radicals; Electron displacements effects in covalent bonds – inductive effect, electrometric effect, resonance effect, hyperconjugation, and mesomeric effect; Types of organic reactions: substitution reactions, addition reactions, elimination reactions, oxidation reactions, reduction reactions, molecular rearrangements; Functional group interconversions,

Introduction, classification of hydrocarbons; Preparation and chemical properties of alkanes, alkenes and alkynes; Markovnikov and anti-Markovnikov addition reactions and their mechanism; conformers of alkanes; Aromatic hydrocarbons: Aromaticity and Huckel Rule; Structure of benzene; Preparation of benzene; Aromatic electrophilic substitution reactions and mechanism, influence of the functional group in mono-substituted benzene; toxicity(carcinogenicity)

Halo-alkanes; nature of C–X bond, classification and nomenclature; preparation from alkanes, alkenes, and alcohols; physical properties; chemical properties – nucleophilic substitution reactions, stereochemical aspects (SN1, SN2); Elimination reactions, E1, and E2 mechanisms; organometallic compounds: Introduction, preparation and uses of Grignard reagent; Haloarenes: Preparation of chlorobenzene; Chemical properties of chlorobenzene: nucleophilic and electrophilic substitution reactions, reaction with metals (Wurtz-Fitting and Fitting reactions), Formation of DDT; polyhalogen compounds and uses.

Environmental pollution; Types – air, water, and soil pollution; Particulate pollutants, Greenhouse effect, and global warming; Acid rain and its effect; Ozone hole; Strategies to control environmental pollutions; Green chemistry

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