11th class chemistry notes pdf

 
    Contents
  1. Chemistry Notes Class XI
  2. Class 11 Chemistry Revision Notes for Chapter 7 - Equilibrium
  3. CBSE Revision Notes for class 11 Chemistry
  4. Class 11 Chemistry Revision Notes for Chapter 6 - Thermodynamics

class 11, chemistry, cbse board, ncert notes, physical chemistry notes, organic chemistry notes, analytic chemistry notes, download notes, free ncert notes, cbse . Free PDF download of Class 11 Chemistry revision notes and short key-notes to score more marks in exams, prepared by expert Chemistry teachers from the. Free PDF download of Class 11 Chemistry revision notes & short key-notes for Chapter 1 - Some Basic Concepts of Chemistry to score high marks in exams, prepared by expert Chemistry teachers from latest edition of CBSE(NCERT) books. Chapter 4 - Chemical Bonding and Molecular.

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11th Class Chemistry Notes Pdf

Chemistry Notes Class XI. As Per CBSE (NCERT) Books. Chapter Wise-Notes PDF (Board Level). Syllabus. Chapter 1 - Some Basic Concepts of Chemistry. Chemistry Notes PDF for class 11 are available here. You can easily download the PDF only at BYJU's. Here you can find the PDF for the different notes for the. Class 11 Chemistry Notes. Basic Concepts of Chemistry · Atomic Structure · Classification of Elements and Periodicity of Properties · States of Matter · Chemical.

General Introduction: Importance and scope of chemistry. Nature of matter, laws of chemical combination, Dalton's atomic theory: Atomic and molecular masses, mole concept and molar mass, percentage composition, empirical and molecular formula, chemical reactions, stoichiometry and calculations based on stoichiometry. 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.

Importance and scope of chemistry. Nature of matter, laws of chemical combination, Dalton's atomic theory: Atomic and molecular masses, mole concept and molar mass, percentage composition, empirical and molecular formula, chemical reactions, stoichiometry and calculations based on stoichiometry.

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.

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.

Chemistry Notes Class XI

Nomenclature of elements with atomic number greater than 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.

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 behavior, liquefaction of gases, the critical temperature, kinetic energy and molecular speeds elementary idea Liquid State: First law of thermodynamics -internal energy and enthalpy, heat capacity and specific heat, measurement of AU and AH, Hess's law of constant heat summation, enthalpy of bond dissociation, combustion, formation, atomization, sublimation, phase transition, ionization, solution, and dilution.

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.

Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, in terms of loss and gain of electrons and change in oxidation number, applications of redox reactions.

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 peroxide-preparation, reactions and structure, and use; hydrogen as a fuel. The s-Block Elements 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, water, hydrogen and halogens, uses.

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, Aluminium: Reactions with acids and alkalies, uses.

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Class 11 Chemistry Revision Notes for Chapter 7 - Equilibrium

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CBSE Revision Notes for class 11 Chemistry

Question Papers. Previous Year Question Paper. Quick Links. Toll Free: It is denoted by Vm.

One mole of all gaseous substances at K and 1 atm pressure occupies a volume equal to CH is the empirical formula of benzene. The molecular formula shows the exact number of different types of atoms present in a molecule of a compound.

C6H6 is the molecular formula of benzene. The substances that react among themselves to bring about the chemical changes are known as reactants, whereas the substances that are produced as a result of the chemical change, are known as products Limiting Reagent- The reactant which gets consumed first or limits the amount of product formed is known as limiting reagent Reactions in Solutions-- The concentration of a solution can be expressed in any of the following ways. Mass Percent is the mass of the solute in grams per grams of the solution.

Volume percent is the number of units of volume of the solute per units of the volume of solution.

Molarity of the solution is defined as the number of moles of solute dissolved per litre dm3 of the solution. It isdenoted by the symbol M. Measurements in Molarity can change with the change in temperature because solutionsexpand or contract accordingly.

Molality- Molality is defined as the number of moles of solute dissolved per g 1 kg of solvent. Molality is expressed as 'm'. Mole Fraction is the ratio of number of moles of one component to the total number of moles solute and solvents present in the solution.

Class 11 Chemistry Revision Notes for Chapter 6 - Thermodynamics

It is expressed as 'x'. We are not responsible for any type of mistake in data. All pdf files or link of pdf files are collected from various Resources Or sent by Students.

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