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      Class 12 CHEMISTRY – JEE

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      • Class 12 CHEMISTRY – JEE
      CoursesClass 12ChemistryClass 12 CHEMISTRY – JEE
      • 1. Solid State
        11
        • Lecture1.1
          Crystalline & Amorphous Solid 50 min
        • Lecture1.2
          Law of Crystallography 01 hour
        • Lecture1.3
          Bravius lattice & Important Terms of solid state 48 min
        • Lecture1.4
          Type of Cubic crystal & Closest packed St. 01 hour
        • Lecture1.5
          Tetrahedral & Octahedral Void 38 min
        • Lecture1.6
          Type of Voids & Radius Ratio 44 min
        • Lecture1.7
          Type of ionic solid 59 min
        • Lecture1.8
          Defect in Solid 48 min
        • Lecture1.9
          Metallic Bonding 52 min
        • Lecture1.10
          Chapter Notes – Solid State
        • Lecture1.11
          NCERT Solutions – Solid State
      • 2. Solution and its C.P
        9
        • Lecture2.1
          Condition of solution formation, TD of Solution, Factors affecting solubility-Henary’s Law 55 min
        • Lecture2.2
          Colligative Properties, Raoult’s Law 49 min
        • Lecture2.3
          Relative lowering of V.P. & Problems 45 min
        • Lecture2.4
          Non ideal solution, Azeotropic Solution 46 min
        • Lecture2.5
          Elevation in B.P., Depression in F.P. 47 min
        • Lecture2.6
          Osmotic Pressure, Abnormal C.P. & Van’t Hoff Factor 59 min
        • Lecture2.7
          Solution – Ostwald Walker Exp. 13 min
        • Lecture2.8
          Chapter Notes – Solution and its C.P
        • Lecture2.9
          NCERT Solutions – Solution and its C.P
      • 3. Chemical Kinetics
        10
        • Lecture3.1
          Rate of reaction 37 min
        • Lecture3.2
          Differential Rate Law 38 min
        • Lecture3.3
          Integrated Rate Law 56 min
        • Lecture3.4
          Integrated Rate problems 53 min
        • Lecture3.5
          Pseudo order Reaction 40 min
        • Lecture3.6
          Reaction Mechanism 47 min
        • Lecture3.7
          Collision Model 34 min
        • Lecture3.8
          Arhenius Equation 34 min
        • Lecture3.9
          Chapter Notes – Chemical Kinetics
        • Lecture3.10
          NCERT Solutions – Chemical Kinetics
      • 4. Electrochemistry
        13
        • Lecture4.1
          Introduction & Galvanic cell 32 min
        • Lecture4.2
          Cell Notation & Cell Reaction 35 min
        • Lecture4.3
          Electrode & Cell Potential 38 min
        • Lecture4.4
          Electrochemical series 39 min
        • Lecture4.5
          The Nernst Equation 39 min
        • Lecture4.6
          Concentration cell, Battery, Corrosion 52 min
        • Lecture4.7
          Electrolysis 20 min
        • Lecture4.8
          Faraday Law 45 min
        • Lecture4.9
          Resistance & Conductance 40 min
        • Lecture4.10
          Molar & Eq. Conductance, Kohlraush’s Law 29 min
        • Lecture4.11
          Problems on Resistance & Conductance 23 min
        • Lecture4.12
          Chapter Notes – Electrochemistry
        • Lecture4.13
          NCERT Solutions – Electrochemistry
      • 5. Surface Chemistry
        11
        • Lecture5.1
          Introduction & Surface tension & surface energy 33 min
        • Lecture5.2
          Adsorption 47 min
        • Lecture5.3
          Factors affecting Adsorption 39 min
        • Lecture5.4
          Catalysis 34 min
        • Lecture5.5
          Type of Catalysis & Enzyme Catalysis 41 min
        • Lecture5.6
          Colloidal Solution 57 min
        • Lecture5.7
          Type of Colloidal Solution 43 min
        • Lecture5.8
          Properties of Colloidal Solution 50 min
        • Lecture5.9
          Protective Colloids 58 min
        • Lecture5.10
          Chapter Notes – Surface Chemistry
        • Lecture5.11
          NCERT Solutions – Surface Chemistry
      • 6. Alcohol & Ether
        8
        • Lecture6.1
          Preparation 35 min
        • Lecture6.2
          Physical Properties & Oxidation Of Alcohol 29 min
        • Lecture6.3
          Hydrates, Acetal, Ketal 38 min
        • Lecture6.4
          Tests Of Alcohol 47 min
        • Lecture6.5
          Ether Preparation & Its Properties 33 min
        • Lecture6.6
          Thiol & Thioether 16 min
        • Lecture6.7
          Chapter Notes – Alcohol & Ether
        • Lecture6.8
          NCERT Solutions – Alcohol & Ether
      • 7. Aldehyde & Ketone
        10
        • Lecture7.1
          Preparation 33 min
        • Lecture7.2
          Physical Properties, Beckmann Rearrangement, Witting Reaction 46 min
        • Lecture7.3
          Schmidt Reaction, Bayer Villegar Oxidation 22 min
        • Lecture7.4
          Aldol Condensation Reaction 40 min
        • Lecture7.5
          Cannizzaro Reaction 32 min
        • Lecture7.6
          Acyloin, Benzoin, Clasien, Perkin Condensation 28 min
        • Lecture7.7
          Reformasky Reaction, Tischenko Reaction 20 min
        • Lecture7.8
          Tests-8 40 min
        • Lecture7.9
          Chapter Notes – Aldehyde & Ketone
        • Lecture7.10
          NCERT Solutions – Aldehyde & Ketone
      • 8. Acid & derivatives
        4
        • Lecture8.1
          Preparation 31 min
        • Lecture8.2
          Chemical Reactions Of Acids 31 min
        • Lecture8.3
          Arndt Eistert, Curtius, Hvz, Hoffmann Reaction 19 min
        • Lecture8.4
          Acid Derivatives 38 min
      • 9. Nitrogen containing compounds
        4
        • Lecture9.1
          Alkyl Nitrites, Nitro Alkane 27 min
        • Lecture9.2
          Alkane Nitrile & Isonitrile 20 min
        • Lecture9.3
          Amine Preparation 24 min
        • Lecture9.4
          Properties Of Amines 13 min
      • 10. Aromatic Compounds
        7
        • Lecture10.1
          Benzene 41 min
        • Lecture10.2
          Aromatic Hydrocarbon 29 min
        • Lecture10.3
          Aryl Halides 18 min
        • Lecture10.4
          Phenol 40 min
        • Lecture10.5
          Aromatic Aldehyde 39 min
        • Lecture10.6
          Aniline 32 min
        • Lecture10.7
          Phenyl Diazonium Salts 37 min
      • 11. Biomolecules
        14
        • Lecture11.1
          Introduction & Types Of Carbohydrates 47 min
        • Lecture11.2
          D-glucose & D-fructose 50 min
        • Lecture11.3
          Reactions Of D-glucose & D-fructose 32 min
        • Lecture11.4
          Reactions Of D-glucose & D-fructose 23 min
        • Lecture11.5
          Sucrose, Maltose, Lactose 31 min
        • Lecture11.6
          Starch, Cellulose, Glycogen 27 min
        • Lecture11.7
          Reducing Sugar, Mutarotation, Osazone Formation 40 min
        • Lecture11.8
          Problems On Carbohydrates 41 min
        • Lecture11.9
          Amino Acids 48 min
        • Lecture11.10
          Peptides 47 min
        • Lecture11.11
          Proteins 18 min
        • Lecture11.12
          Enzyme & Vitamins 30 min
        • Lecture11.13
          Nucleic Acid 36 min
        • Lecture11.14
          Chapter Notes – Biomolecules
      • 12. Polymer Chemistry
        6
        • Lecture12.1
          Polymerisation Addition Reaction 32 min
        • Lecture12.2
          Coordination Addition, Condensation Reaction 24 min
        • Lecture12.3
          Division Of Polymer 41 min
        • Lecture12.4
          Examples Of Polymer 31 min
        • Lecture12.5
          Examples Of Polymer 31 min
        • Lecture12.6
          Chapter Notes – Polymer Chemistry
      • 13. Practical Organic Chemistry
        4
        • Lecture13.1
          Poc Qualitative Analysis 23 min
        • Lecture13.2
          Poc Qualitative Analysis 20 min
        • Lecture13.3
          Poc Quantitative Analysis 29 min
        • Lecture13.4
          Poc Quantitative Analysis 20 min
      • 14. P block elements II
        13
        • Lecture14.1
          VA – Elemental Properties of N family 51 min
        • Lecture14.2
          VA – Compounds of N family 43 min
        • Lecture14.3
          VA – N & Its compounds 45 min
        • Lecture14.4
          VA – Oxides & Oxyacids of Nitrogen 55 min
        • Lecture14.5
          VA – P & its compounds 31 min
        • Lecture14.6
          VA – Oxides & Oxyacids of P 31 min
        • Lecture14.7
          VIA 1 – Elemental Properties of O-Family 36 min
        • Lecture14.8
          VIA 2 – compounds of VIA elements 41 min
        • Lecture14.9
          VIA 3 – Oxygen & Ozone 47 min
        • Lecture14.10
          VIA 4 – Sulphur & oxides of Sulphur 37 min
        • Lecture14.11
          VIA 5 – Sulphuric Acid 25 min
        • Lecture14.12
          Chapter Notes – P block elements
        • Lecture14.13
          NCERT Solutions – P block elements
      • 15. P block elements III
        5
        • Lecture15.1
          VIIA 1 – elemental properties of Halogen 40 min
        • Lecture15.2
          VIIA 2 – Compounds of Halogen 49 min
        • Lecture15.3
          VIIA 3 – Chlorine & its Compounds 41 min
        • Lecture15.4
          VIIIA 1 – Properties of Noble Gas 34 min
        • Lecture15.5
          VIIIA 2 – Compounds of Noble Gas 34 min
      • 16. D block metals
        8
        • Lecture16.1
          D block – Elemental Properties 55 min
        • Lecture16.2
          Elemental Properties 01 hour
        • Lecture16.3
          Elemental Properties 53 min
        • Lecture16.4
          KMnO4 & K2Cr2O7 47 min
        • Lecture16.5
          Problems 40 min
        • Lecture16.6
          Problems 20 min
        • Lecture16.7
          Chapter Notes – The d-and f-Block Elements
        • Lecture16.8
          NCERT Solutions – The d-and f-Block Elements
      • 17. F block metals
        3
        • Lecture17.1
          Lanthanoids 52 min
        • Lecture17.2
          Actinoids 48 min
        • Lecture17.3
          Problems 42 min
      • 18. Co-ordination compounds
        17
        • Lecture18.1
          Introduction of Complex Compound, Ligands 42 min
        • Lecture18.2
          Classification of Ligands, Denticity 35 min
        • Lecture18.3
          Nomenclature of Complex Compounds 46 min
        • Lecture18.4
          Nomenclature of Complex Compounds 2 40 min
        • Lecture18.5
          Bonding in Complex Compound, Primary & Secondary Valency 44 min
        • Lecture18.6
          Concept of EAN 29 min
        • Lecture18.7
          VBT in Complex Compounds 58 min
        • Lecture18.8
          Examples on VBT in complex compounds 31 min
        • Lecture18.9
          CFT in Complex Compounds 43 min
        • Lecture18.10
          CFT for Octahedral & Tetrahedral Complex 35 min
        • Lecture18.11
          Colour & Stability of Complex Compounds 28 min
        • Lecture18.12
          Structural Isomerism in Complex Compounds 49 min
        • Lecture18.13
          Geometrical Isomerism in Complex Compounds 43 min
        • Lecture18.14
          Optical Isomerism in Complex Compounds, use of Complex 01 hour
        • Lecture18.15
          Organometallic Compounds 29 min
        • Lecture18.16
          Chapter Notes – Co-ordination compounds
        • Lecture18.17
          NCERT Solutions – Co-ordination compounds
      • 19. Environmental Chemistry
        4
        • Lecture19.1
          Introduction & Air Pollution 35 min
        • Lecture19.2
          Air Pollution 20 min
        • Lecture19.3
          Water Pollution 23 min
        • Lecture19.4
          Soil Pollution, Prevention of Pollution 16 min

        Chapter Notes – The d-and f-Block Elements

        1. The elements lying in the middle of Periodic Table between s-block and p-block elements (i.e between group 2 and 13) are known as d-block or transition elements.
        2. There are three transition series each of 10 elements:
        (i) First transition series: It involves filling of 3d-orbitals. It starts from scandium (Z = 21) and goes upto zinc (Z = 30).
        (ii) Second transition series: It involves filling of 4d-orbitals. It starts from yittrium (Z=39) to cadmium (Z = 48).
        (iii) Third transition series: It involves filling of 5d-orbitals. The first element of this series is lanthanum (Z = 57). It is followed by 14 elements called lanthanides which involve the filling of 4f-orbitals. The next nine elements from hafnium (Z = 72) to mercury (Z = 80) belong to third transition series.
        3. The f-block elements are called inner-transition elements.
        4. All the transition elements are metallic in nature, good conductors, of heat and electricity; show a gradual decrease in electropositive character in moving across a period. Due to strong metallic bonds, these metals are hard, possess high densities, high enthalpies of atomisation, high melting and boiling points and form alloys with other metals.
        5. The melting point of these first increases to maximum and then gradually decreases towards the end of the series. The strength of metallic bonds is roughly related to number of half-filled d-orbitals.
        6. The radii of ions, having the same charge and magnitude, in a given series decreases progressively with increase in atomic number. This is because of poor shielding effect of d-electrons.
        7. Ionisation energies of transition elements are higher than those of s-block elements but lower than p-block elements. It generally increases from left to right in the series.
        8. Transition metals exhibit a variety of oxidation states.
        The variable oxidation states of transition metals are due to involvement of ns and (n – 1 )d- electrons in bonding.
        9. Most of the transition metals are sufficiently electropositive. They react with mineral acids liberating H2 gas.
        10. Transition elements and many of their compounds are paramagnetic,
        11. Formation of coloured compounds (both in solid state as well as in aqueous solution) is another very common characteristics of transition metals. This is due to absorption of some radiation from visible light to cause d-d transition of electrons in transition metal atom.
        12. In contrast to s-and p-block elements, the transition elements have the ability to form complexes. This is because these elements
        (a) have small highly charged ions, and
        (b) contain vacant d-orbitals.
        13. Many of transition metals and their compounds act as catalyst in variety of reactions.
        14. Transition metals form large number of interstitial compounds.
        15. A large number of alloys are formed by transition metals. It is due to their atoms mutually substitute their positions easily in their metal crystal lattices.
        16. The oxides of transition metals in lower oxidation states are generally basic in nature and those in, higher oxidation states are amphoteric or acidic in nature.
        17. The f -block elements have been divided in two series depending upon the fact whether the last electron (differentiating electron) enters 4f- orbitals or 5f-orbitals and accordingly called lanthanides or actinides respectively
        18. Actinides show several oxidation states but + 3 oxidation state is most common. The highest oxidation state shown by actinides is + 7.

        19. Properties of the lanthanides:
        (a) General electronic configuration is [Xe] 4f1-14 5d0-1 6s2.
        (b) The metals are silvery-white in colour. They are malleable, ductile, have low tensile strength and are good conductors of heat and electricity.
        (c) They have relatively high density and possess high melting points.
        (d) The lanthanides exhibit a principle oxidation state of + 3. However, some elements also exhibit + 2 (Eu2+) and + 4 (Ce4+)oxidation states.
        (e) Many of the lanthanide ions are coloured due to the electronic transition between different 4 f-levels.
        (f) The majority of the lanthanide ions exhibit paramagnetism due to the presence of unpaired electrons. The lanthanoid ions that do not exhibit paramagnetism are those with either no 4f-electrons, e. g., La3+ and Ce4+ or with a completed 4f-level, e.g., Yb2+ and Lu3+.
        (g) The lanthanides readily tarnish in air and bum to give trioxides (except cesium, which forms Ce02).
        (h) The oxides and hydroxides of the lanthanides are basic in character.
        (i) The lanthanoid compounds are generally predominantly ionic.
        20. This gradual decrease in atomic size across the first f- transition element series is called lanthanoid contraction.
        21. Properties of actinides:
        (a) General electronic configuration is [Rn] 5f0-14 6ds0-1 7s2.
        (b) The elements are all silvery-white metals.
        (c) The melting points of the actinides are moderately high.
        (d) The ionic size of the actinides decreases gradually along the series.
        (e) The actinides have the ability to exhibit several oxidation states. However, +4 oxidation state is preferred in actinides.
        (f) Some actinoid elements can exist in + 6 oxidation state, e.g., uranium, neptunium and plutonium.
        (g) Many actinoid elements are radioactive. The elements beyond uranium are man-made.
        (h) The actinides have a much greater tendency to form complexes than lanthanides.

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