1. Chapter 1 - Some basic concepts of Chemistry
• Nature of matter
• Mixtures and pure substances
• Homogeneous and heterogeneous mixtures
Chapter 1.1
• Units and measurements
• Mole concept and molar masses
• Solved examples
Chapter 1.2
• Percentage composition
• Molecular formula
• Empirical formula
Chapter 1.3
• Solved examples on molecular formula and empirical formula
Chapter 1.4
• Stoichiometry and stoichiometric Calculations
Chapter 1.5
• Molarity and Molality
Chapter 1.6
• Solved examples on molarity and molality
2. Chapter 2 - Structure of Atom
• Cathode rays
• J.J. Thompson's method for calculating charge to mass ratio of electron
• Millikan's oil drop method for calculating charge of electron
Chapter 2.1
• Protons and neutrons
• Radioactivity
• Alpha, beta and gamma radiations
• X-rays
Chapter 2.2
• Thomson's Atomic model
• Rutherford's Atomic model
Chapter 2.3
• Atomic number and mass number
• Isotopes and isobars
• Solved examples
Chapter 2.4
• Drawbacks of Rutherford model of atom
Chapter 2.5
• Wave nature of electromagnetic radiations
• Electromagnetic spectrum
• Frequency, wavelength and wavenumber
Chapter 2.6
• Particle nature of radiations
• Black body radiation
• Max Planck's Quantum theory
Chapter 2.7
• Photoelectric effect
• Explanation given by Albert Einstein
Chapter 2.8
• Continuous spectrum
• Absorption spectrum
• Emission spectrum
• Line spectrum
• spectroscopy
Chapter 2.9
• Emission spectrum of Hydrogen
• Lyman series
• Balmer series
• Paschen series
• Rydberg constant
Chapter 2.10
• Bohr model of hydrogen atom
• Energy levels
Chapter 2.11
• Explanation for hydrogen spectrum, based on Bohr model
• Hydrogen like species
Chapter 2.12
• Dual nature of matter
• Heisenberg's Uncertainty principle
Chapter 2.13
• Quantum mechanical model of atom
• Principal quantum number
• Azimuthal quantum number
• Magnetic orbital quantum number
Chapter 2.14
• Electron spin quantum number
• Solved examples
Chapter 2.15
• Shapes of orbitals
• Probability of finding electrons
Chapter 2.16
• Radial nodes and Angular nodes
• Solved examples
Chapter 2.17
• Energies of orbitals
• (n+l) rule
Chapter 2.18
• Electronic configuration from hydrogen to neon
• Aufbau principle
• Pauli's exclusion principle
• Hund's rule of maximum multiplicity
Chapter 2.19
• Electronic configuration from sodium to krypton
Chapter 2.20
• Basic pattern of the electronic configuration of elements after krypton
• Core electrons and valence electrons
3. Chapter 3 - Classification of elements
• Nature of matter
• Mixtures and pure substances
• Homogeneous and heterogeneous mixtures
Chapter 1.1
• Units and measurements
• Mole concept and molar masses
• Solved examples
Chapter 1.2
• Percentage composition
• Molecular formula
• Empirical formula
Chapter 1.3
• Solved examples on molecular formula and empirical formula
Chapter 1.4
• Stoichiometry and stoichiometric Calculations
Chapter 1.5
• Molarity and Molality
Chapter 1.6
• Solved examples on molarity and molality
2. Chapter 2 - Structure of Atom
• Cathode rays
• J.J. Thompson's method for calculating charge to mass ratio of electron
• Millikan's oil drop method for calculating charge of electron
Chapter 2.1
• Protons and neutrons
• Radioactivity
• Alpha, beta and gamma radiations
• X-rays
Chapter 2.2
• Thomson's Atomic model
• Rutherford's Atomic model
Chapter 2.3
• Atomic number and mass number
• Isotopes and isobars
• Solved examples
Chapter 2.4
• Drawbacks of Rutherford model of atom
Chapter 2.5
• Wave nature of electromagnetic radiations
• Electromagnetic spectrum
• Frequency, wavelength and wavenumber
Chapter 2.6
• Particle nature of radiations
• Black body radiation
• Max Planck's Quantum theory
Chapter 2.7
• Photoelectric effect
• Explanation given by Albert Einstein
Chapter 2.8
• Continuous spectrum
• Absorption spectrum
• Emission spectrum
• Line spectrum
• spectroscopy
Chapter 2.9
• Emission spectrum of Hydrogen
• Lyman series
• Balmer series
• Paschen series
• Rydberg constant
Chapter 2.10
• Bohr model of hydrogen atom
• Energy levels
Chapter 2.11
• Explanation for hydrogen spectrum, based on Bohr model
• Hydrogen like species
Chapter 2.12
• Dual nature of matter
• Heisenberg's Uncertainty principle
Chapter 2.13
• Quantum mechanical model of atom
• Principal quantum number
• Azimuthal quantum number
• Magnetic orbital quantum number
Chapter 2.14
• Electron spin quantum number
• Solved examples
Chapter 2.15
• Shapes of orbitals
• Probability of finding electrons
Chapter 2.16
• Radial nodes and Angular nodes
• Solved examples
Chapter 2.17
• Energies of orbitals
• (n+l) rule
Chapter 2.18
• Electronic configuration from hydrogen to neon
• Aufbau principle
• Pauli's exclusion principle
• Hund's rule of maximum multiplicity
Chapter 2.19
• Electronic configuration from sodium to krypton
Chapter 2.20
• Basic pattern of the electronic configuration of elements after krypton
• Core electrons and valence electrons
3. Chapter 3 - Classification of elements
• History of the development of periodic table
• Mendeleev's periodic table
• Long form of the periodic table
• IUPAC rules for naming a new element
Chapter 3.1
• Relation between electronic configuration and periods
• Transition elements
• Inner transition elements
Chapter 3.2
• Comparing elements within Groups
• Same 'number of valence electrons'
• Similar 'valence orbitals'
• Similar 'physical and chemical properties'
Chapter 3.3
• Various blocks in the periodic table
• General electronic configuration for each block
• Main group elements (Representative elements)
• Families in the periodic table
Chapter 3.4
• Classification into metals, non-metals and metalloids
• Position of elements in the periodic table
• Solved examples
Chapter 3.5
• Advantages of learning Periodic trends
• Periodic trends in atomic radius
Chapter 3.6
• Periodic trends in ionic radius
• Isoelectronic species
Chapter 3.7
• Periodic trends in ionization enthalpy
• Anomalies at boron and oxygen
• Solved examples
Chapter 3.8
• Periodic trends in electron gain enthalpy
• Anomalies at oxygen and fluorine
• Solved examples
Chapter 3.9
• Periodic trends in electronegativity
• Metallic and non-metallic characters
• Solved examples
Chapter 3.10
• Basics about oxidation states
• Oxidation state of oxygen in O2F
• Oxidation state of oxygen in Na2O
Chapter 3.11
• Valence
• Periodic trends in valence
• Solved examples
Chapter 3.12
• Chemical reactivity
• Periodic trends (along periods) in Chemical reactivity
Chapter 3.13
• Comparing oxides
• Periodic trends (along groups) in Chemical reactivity
4. Chapter 4 - Chemical bonding and Molecular structure
• Lewis-Kossel model of molecules
• Lewis symbols
• Postulates put forward by Kossel
• Basic study of ionic compounds
• Mendeleev's periodic table
• Long form of the periodic table
• IUPAC rules for naming a new element
Chapter 3.1
• Relation between electronic configuration and periods
• Transition elements
• Inner transition elements
Chapter 3.2
• Comparing elements within Groups
• Same 'number of valence electrons'
• Similar 'valence orbitals'
• Similar 'physical and chemical properties'
Chapter 3.3
• Various blocks in the periodic table
• General electronic configuration for each block
• Main group elements (Representative elements)
• Families in the periodic table
Chapter 3.4
• Classification into metals, non-metals and metalloids
• Position of elements in the periodic table
• Solved examples
Chapter 3.5
• Advantages of learning Periodic trends
• Periodic trends in atomic radius
Chapter 3.6
• Periodic trends in ionic radius
• Isoelectronic species
Chapter 3.7
• Periodic trends in ionization enthalpy
• Anomalies at boron and oxygen
• Solved examples
Chapter 3.8
• Periodic trends in electron gain enthalpy
• Anomalies at oxygen and fluorine
• Solved examples
Chapter 3.9
• Periodic trends in electronegativity
• Metallic and non-metallic characters
• Solved examples
Chapter 3.10
• Basics about oxidation states
• Oxidation state of oxygen in O2F
• Oxidation state of oxygen in Na2O
Chapter 3.11
• Valence
• Periodic trends in valence
• Solved examples
Chapter 3.12
• Chemical reactivity
• Periodic trends (along periods) in Chemical reactivity
Chapter 3.13
• Comparing oxides
• Periodic trends (along groups) in Chemical reactivity
4. Chapter 4 - Chemical bonding and Molecular structure
• Lewis-Kossel model of molecules
• Lewis symbols
• Postulates put forward by Kossel
• Basic study of ionic compounds
Chapter 4.1
• Octet rule
• Covalent bonds
• Lewis dot structures
Chapter 4.2
• Steps for drawing Lewis dot structures of polyatomic molecules
• Examples
Chapter 4.3
• Steps for drawing Lewis dot structures of polyatomic ions
• Examples
Chapter 4.4
• Steps for finding formal charges in atoms of polyatomic molecules and ions
• Examples
Chapter 4.5
• Limitations of octet rule
• Examples
Chapter 4.6
• Ionic or electrovalent bonds
• Lattice enthalpy
Chapter 4.7
• Bond length
• Bond angle
• Bond enthalpy
Chapter 4.8
• Bond order
Chapter 4.9
• Resonance structures
Chapter 4.10
• Polarity of bonds
• Dipole moments
Chapter 4.11
• Dipole moment in NH3
• Dipole moment in NF3
Chapter 4.12
• Partial covalent character in ionic bonds
• Fajans' rules
Chapter 4.13
• VSEPR theory
• Linear structure
• Trigonal planar structure
Chapter 4.14
• VSEPR theory
• Tetrahedral structure
Chapter 4.15
• VSEPR theory
• Trigonal bipyramidal structure
Chapter 4.16
• VSEPR theory
• Octahedral structure (square bipyramidal structure)
Chapter 4.17
• VSEPR theory related to lone pairs
• Bent structure
Chapter 4.18
• VSEPR theory related to lone pairs
• Trigonal pyramidal structure
• T-shape
Chapter 4.19
• VSEPR theory related to lone pairs
• Seesaw shape
• Square planar shape
Chapter 4.20
• VSEPR theory related to lone pairs
• Square pyramidal shape
Chapter 4.21
• Postulates in the VSEPR theory
• Explanations and applications of the Postulates
• Solved example
Chapter 4.22
• Valence bond theory
• Formation of hydrogen molecule
Chapter 4.23
• Orbital overlap concept
Chapter 4.24
• Hybridization
• Hybrid orbitals
Chapter 4.25
• Structure of Methane molecule
• Structure of Ethane molecule
• Sigma bond
Chapter 4.26
• Structure of Ethene (ethylene) molecule
• Pi bond in a double bond
Chapter 4.27
• Structure of Ethyne (acetylene) molecule
• Pi bonds in a triple bond
Chapter 4.28
• Structure of Ammonia molecule
• Structure of Water molecule
Chapter 4.29
• Structure of Trichloro boron
• Structure of Beryllium chloride
Chapter 4.30
• Hybridization involving d orbitals
• Structure of Phosphorus pentachloride (PCl5)
Chapter 4.31
• Hybridization involving d orbitals
• Structure of Sulfur hexafluoride (SF6)
• Salient features of Hybridization
• Conditions for Hybridization
Chapter 4.32
• Molecular orbital theory
• Bonding and -anti-bonding orbitals
• Bond order
• Stability of molecules
Chapter 4.33
• Electronic configuration of
♦ Helium molecule
♦ Hydrogen ion
♦ Helium ion
Chapter 4.34
• Electronic configuration of
♦ Lithium molecule
♦ Beryllium molecule
Chapter 4.35
• Combination of p-orbitals
♦ sigma p-orbitals
♦ pi p-orbitals
Chapter 4.36
• Electronic configuration of
♦ Boron molecule
Chapter 4.37
• Electronic configuration of
♦ Carbon molecule
♦ Nitrogen molecule
Chapter 4.38
• Electronic configuration of
♦ Oxygen molecule
♦ Oxygen ions
Chapter 4.39
• Electronic configuration of
♦ Fluorine molecule
♦ Neon molecule
Chapter 4.40
• Hydrogen bond
♦ Inter-molecular hydrogen bond
♦ Intra-molecular hydrogen bond
• Octet rule
• Covalent bonds
• Lewis dot structures
Chapter 4.2
• Steps for drawing Lewis dot structures of polyatomic molecules
• Examples
Chapter 4.3
• Steps for drawing Lewis dot structures of polyatomic ions
• Examples
Chapter 4.4
• Steps for finding formal charges in atoms of polyatomic molecules and ions
• Examples
Chapter 4.5
• Limitations of octet rule
• Examples
Chapter 4.6
• Ionic or electrovalent bonds
• Lattice enthalpy
Chapter 4.7
• Bond length
• Bond angle
• Bond enthalpy
Chapter 4.8
• Bond order
Chapter 4.9
• Resonance structures
Chapter 4.10
• Polarity of bonds
• Dipole moments
Chapter 4.11
• Dipole moment in NH3
• Dipole moment in NF3
Chapter 4.12
• Partial covalent character in ionic bonds
• Fajans' rules
Chapter 4.13
• VSEPR theory
• Linear structure
• Trigonal planar structure
Chapter 4.14
• VSEPR theory
• Tetrahedral structure
Chapter 4.15
• VSEPR theory
• Trigonal bipyramidal structure
Chapter 4.16
• VSEPR theory
• Octahedral structure (square bipyramidal structure)
Chapter 4.17
• VSEPR theory related to lone pairs
• Bent structure
Chapter 4.18
• VSEPR theory related to lone pairs
• Trigonal pyramidal structure
• T-shape
Chapter 4.19
• VSEPR theory related to lone pairs
• Seesaw shape
• Square planar shape
Chapter 4.20
• VSEPR theory related to lone pairs
• Square pyramidal shape
Chapter 4.21
• Postulates in the VSEPR theory
• Explanations and applications of the Postulates
• Solved example
Chapter 4.22
• Valence bond theory
• Formation of hydrogen molecule
Chapter 4.23
• Orbital overlap concept
Chapter 4.24
• Hybridization
• Hybrid orbitals
Chapter 4.25
• Structure of Methane molecule
• Structure of Ethane molecule
• Sigma bond
Chapter 4.26
• Structure of Ethene (ethylene) molecule
• Pi bond in a double bond
Chapter 4.27
• Structure of Ethyne (acetylene) molecule
• Pi bonds in a triple bond
Chapter 4.28
• Structure of Ammonia molecule
• Structure of Water molecule
Chapter 4.29
• Structure of Trichloro boron
• Structure of Beryllium chloride
Chapter 4.30
• Hybridization involving d orbitals
• Structure of Phosphorus pentachloride (PCl5)
Chapter 4.31
• Hybridization involving d orbitals
• Structure of Sulfur hexafluoride (SF6)
• Salient features of Hybridization
• Conditions for Hybridization
Chapter 4.32
• Molecular orbital theory
• Bonding and -anti-bonding orbitals
• Bond order
• Stability of molecules
Chapter 4.33
• Electronic configuration of
♦ Helium molecule
♦ Hydrogen ion
♦ Helium ion
Chapter 4.34
• Electronic configuration of
♦ Lithium molecule
♦ Beryllium molecule
Chapter 4.35
• Combination of p-orbitals
♦ sigma p-orbitals
♦ pi p-orbitals
Chapter 4.36
• Electronic configuration of
♦ Boron molecule
Chapter 4.37
• Electronic configuration of
♦ Carbon molecule
♦ Nitrogen molecule
Chapter 4.38
• Electronic configuration of
♦ Oxygen molecule
♦ Oxygen ions
Chapter 4.39
• Electronic configuration of
♦ Fluorine molecule
♦ Neon molecule
Chapter 4.40
• Hydrogen bond
♦ Inter-molecular hydrogen bond
♦ Intra-molecular hydrogen bond
5. Chapter 5 - States of Matter
• London force
• Dipole-dipole force
• Dipole-induced dipole force
• van der Waals forces
• Thermal energy
• London force
• Dipole-dipole force
• Dipole-induced dipole force
• van der Waals forces
• Thermal energy
Chapter 5.2(a)
• Details about Kelvin scale of temperature
• Details about Kelvin scale of temperature
Chapter 5.3
• Gay Lussac law
• Avogadro law
• Details about STP
• Gay Lussac law
• Avogadro law
• Details about STP
Chapter 5.5
• Kinetic molecular theory of gases
• Real gas - Deviation from ideal gas behaviour
• Kinetic molecular theory of gases
• Real gas - Deviation from ideal gas behaviour
Chapter 5.8
• Vapour pressure
• Boiling of liquids
• Boiling points at normal and standard pressures
• Vapour pressure
• Boiling of liquids
• Boiling points at normal and standard pressures
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