• Home
  • Courses
  • Online Test
  • Contact
    Have any question?
    +91-8287971571
    contact@dronstudy.com
    Login
    DronStudy
    • Home
    • Courses
    • Online Test
    • Contact

      Class 11 CHEMISTRY – JEE

      • Home
      • All courses
      • Chemistry
      • Class 11 CHEMISTRY – JEE
      CoursesClass 11ChemistryClass 11 CHEMISTRY – JEE
      • 1. Stoichiometry 1
        13
        • Lecture1.1
          Introduction & POAC 30 min
        • Lecture1.2
          Mole Stoichiometric relationship 29 min
        • Lecture1.3
          Successive reaction & Limiting reagent 25 min
        • Lecture1.4
          Gas Stoichiometry 29 min
        • Lecture1.5
          Important Types of Reactions 25 min
        • Lecture1.6
          Avogadro’s No.1 30 min
        • Lecture1.7
          Mole & Number 28 min
        • Lecture1.8
          Atomic, Molecular Wt 26 min
        • Lecture1.9
          Ionic wt, Avg. At. Wt. 15 min
        • Lecture1.10
          Molar wt. 27 min
        • Lecture1.11
          Molar Volume & Gas Analysis 30 min
        • Lecture1.12
          Gas Analysis 17 min
        • Lecture1.13
          Empirical Formula Determination 26 min
      • 2. Stoichiometry 2
        18
        • Lecture2.1
          Acid Base definition 23 min
        • Lecture2.2
          Acidity & Basicity 32 min
        • Lecture2.3
          Acidic Strength 30 min
        • Lecture2.4
          Acidic Strength 23 min
        • Lecture2.5
          Conjugate Acid-Base pair, Basic Strength 48 min
        • Lecture2.6
          Oxidation & Reduction 50 min
        • Lecture2.7
          Calculation of Oxidation Number 46 min
        • Lecture2.8
          O.A. & R.A., Balancing by Oxidation Number Method 01 hour
        • Lecture2.9
          Balancing by Ion Electron Method. 35 min
        • Lecture2.10
          Eq. Wt. 1 – n factor & Eq. Wt. Concept 47 min
        • Lecture2.11
          Eq. Wt. 2 – Eq. Concept 35 min
        • Lecture2.12
          Volumetric Analysis 43 min
        • Lecture2.13
          Volumetric analysis 44 min
        • Lecture2.14
          Titration – Acid Base Titration 49 min
        • Lecture2.15
          Titration – Acid Base Titration, Indicator 56 min
        • Lecture2.16
          Titration – Redox Titration-8 58 min
        • Lecture2.17
          Titration – Redox Titration, volume Strength of H2O2 50 min
        • Lecture2.18
          Titration – Redox Titration, Iodometry, Oleum, Bleaching Powder 49 min
      • 3. Thermodynamics & Thermochemistry
        19
        • Lecture3.1
          Zeroth Law 55 min
        • Lecture3.2
          1st law – System, Properties, State 40 min
        • Lecture3.3
          1st Law, Process, Internal energy, Work 43 min
        • Lecture3.4
          Work done in Irreversible process, Isobaric Process 49 min
        • Lecture3.5
          Isochoric Process & problems TD 42 min
        • Lecture3.6
          Isothermal irreversible Process, Problems on TD 46 min
        • Lecture3.7
          Adiabatic Process 49 min
        • Lecture3.8
          Problems on TD 44 min
        • Lecture3.9
          Thermochemistry & Enthalpy 38 min
        • Lecture3.10
          Hess’s Law, Kirchhoff’s Law 43 min
        • Lecture3.11
          Enthalpy of Formation, combustion 39 min
        • Lecture3.12
          Enthalpy of Hydrogenation, Hydration, dissolution, lattice energy 40 min
        • Lecture3.13
          Enthapy of Neutralisation, atomisation, Bond Energy 47 min
        • Lecture3.14
          Resonance energy & problems 45 min
        • Lecture3.15
          2nd Law, Entropy-positional 40 min
        • Lecture3.16
          TD Entropy, 3rd Law, Entropy change in a reaction 45 min
        • Lecture3.17
          Gibb’s free energy 43 min
        • Lecture3.18
          Efficiency, engine, pump & Carnot engine 39 min
        • Lecture3.19
          Chapter Notes – Thermodynamics & Thermochemistry
      • 4. Atomic Structure
        22
        • Lecture4.1
          Introduction, Cathode rays & Anode rays 41 min
        • Lecture4.2
          J.J. Thomson Model, Millikan Oil Drop Experiment 38 min
        • Lecture4.3
          Rutherford Experiment 51 min
        • Lecture4.4
          Quantum Mechanics, BlackBody Radiation Experiment 41 min
        • Lecture4.5
          Wave 44 min
        • Lecture4.6
          Photoelectric Effect 46 min
        • Lecture4.7
          Problems on Photoelectric Effect 35 min
        • Lecture4.8
          Atomic Structure 44 min
        • Lecture4.9
          Bohr Theory 47 min
        • Lecture4.10
          H – Spectrum 49 min
        • Lecture4.11
          Problems on Bohr’s Theory 40 min
        • Lecture4.12
          Adv. Problems on Bohr Theory & Sommerfeld model 51 min
        • Lecture4.13
          Quantum Mechanical Model for Atomic Structure 47 min
        • Lecture4.14
          Schrodinger wave equation 54 min
        • Lecture4.15
          No. of Orbitals & Quantum no 45 min
        • Lecture4.16
          Orbital Curve, RPD curve, Definition of Node 46 min
        • Lecture4.17
          Calculation of Node, Orbital Picture 43 min
        • Lecture4.18
          Radial Probability curve, MPD, Avg. distance, Screening effect, Zeff 38 min
        • Lecture4.19
          Multielectron system, Electronic configuration 56 min
        • Lecture4.20
          Stability of Elec. Configuration 36 min
        • Lecture4.21
          Chapter Notes – Atomic Structure
        • Lecture4.22
          NCERT Solutions – Atomic Structure
      • 5. Chemical equilibrium
        9
        • Lecture5.1
          Introduction, Eqb constant & Eqb Position 51 min
        • Lecture5.2
          Types of Eqb Constant, Heterogeneous Eqb, Reaction Quotient 45 min
        • Lecture5.3
          Range of Eqb Constant 43 min
        • Lecture5.4
          Problems on Chemical Eqb 41 min
        • Lecture5.5
          Problems on Chemical Eqb 42 min
        • Lecture5.6
          Le-chatelier Principle 42 min
        • Lecture5.7
          Le-Chatelier Principle 35 min
        • Lecture5.8
          Eqb & 2nd Law of TD 26 min
        • Lecture5.9
          NCERT Solutions – equilibrium
      • 6. Ionic Equilibrium
        17
        • Lecture6.1
          Electrolyte, Dissociation of H2O, Nature of Solution 46 min
        • Lecture6.2
          PH scale, Log & Antilog 40 min
        • Lecture6.3
          PH of Strong Acid, Base Solution 51 min
        • Lecture6.4
          PH of Weak Acid, Base solution 41 min
        • Lecture6.5
          PH of mixture of Acids, Bases 46 min
        • Lecture6.6
          PH of Polybasic acids 40 min
        • Lecture6.7
          PH of Salt Solution 1 43 min
        • Lecture6.8
          PH of salt solution 2 52 min
        • Lecture6.9
          Common ion effect, Buffer solution 49 min
        • Lecture6.10
          Buffer Capacity 45 min
        • Lecture6.11
          Titration & PH Curve 1 40 min
        • Lecture6.12
          Titration & PH curve 2 46 min
        • Lecture6.13
          Acid Base indicator 35 min
        • Lecture6.14
          Solubility Equilibrium 47 min
        • Lecture6.15
          Precipitation of Solid, Qualitative analysis of cation 44 min
        • Lecture6.16
          Complex ion equilibrium 23 min
        • Lecture6.17
          Chapter Notes – Equilibrium
      • 7. Introduction & Development of Org. Chemistry
        3
        • Lecture7.1
          Introduction & Development Of Organic Chemistry 44 min
        • Lecture7.2
          Introduction & Syllabus 36 min
        • Lecture7.3
          NCERT Solutions – Org. Chemistry
      • 8. Nomenclature of Org. Compounds
        16
        • Lecture8.1
          Alkane 59 min
        • Lecture8.2
          Alkane 31 min
        • Lecture8.3
          Alkyl Group & Types Of Hydrogen 01 hour
        • Lecture8.4
          Alkene 54 min
        • Lecture8.5
          Alkenyl 32 min
        • Lecture8.6
          Alkyne & Alkenyl 47 min
        • Lecture8.7
          Cycloalkane 43 min
        • Lecture8.8
          Cycloalkene 35 min
        • Lecture8.9
          Bicycloalkane & Spirane 35 min
        • Lecture8.10
          Acid & Aldehyde 45 min
        • Lecture8.11
          Ester & Acid Halides 28 min
        • Lecture8.12
          Amide & Nitrile 28 min
        • Lecture8.13
          Alcohol & Sulphonic Acid 37 min
        • Lecture8.14
          Isonitrile, Amine, Nitroalkane, Halo Compounds 39 min
        • Lecture8.15
          Ketone, Anhydride & Ether 34 min
        • Lecture8.16
          Polyfunctional Group Compounds 41 min
      • 9. GOC 1- Hybridisation, Resonance, Aromaticity
        16
        • Lecture9.1
          Concept Of Hybridisation 42 min
        • Lecture9.2
          Sp3, Sp2 Hybridisation 44 min
        • Lecture9.3
          Sp Hybridisation, Relative Study Of Sp3, Sp2, Sp Orbitals 46 min
        • Lecture9.4
          Effect Of Hybridisation On Bond Length, Planar Nature 59 min
        • Lecture9.5
          Concept Of Resonance 39 min
        • Lecture9.6
          Doing Resonance 18 min
        • Lecture9.7
          Resonance Hybrid, Cannonical St. , Resonance Energy 44 min
        • Lecture9.8
          Condition Of Resonance 40 min
        • Lecture9.9
          Writing Cannonical St. 39 min
        • Lecture9.10
          Relative Stability Of Cannonical St. 37 min
        • Lecture9.11
          Resonance Energy 45 min
        • Lecture9.12
          Effect Of Resonance On Bond Length, Enthalpy Of Hydrogenation 43 min
        • Lecture9.13
          Introduction To Aromaticity 43 min
        • Lecture9.14
          Introduction To Aromaticity 39 min
        • Lecture9.15
          Unsaturation Factor 31 min
        • Lecture9.16
          Chapter Notes – GOC General Organic chemistry
      • 10. GOC 2 - Substituent effect
        5
        • Lecture10.1
          Substituent Effect, Hyperconjugation 48 min
        • Lecture10.2
          Substituent Effect, Hyperconjugation 43 min
        • Lecture10.3
          Substituent Effect, Mesomeric Effect 47 min
        • Lecture10.4
          Substituent Effect, Inductive Effect 46 min
        • Lecture10.5
          Substituent Effect, Electromeric Effect, Staric Effect, Relative M & I Effect 41 min
      • 11. GOC 2 - Reactive Intermediate
        6
        • Lecture11.1
          Reactive Intermediate, Carbocation 45 min
        • Lecture11.2
          Reactive Intermediate, Carbocation, Carbonium Ion Rearrangement 42 min
        • Lecture11.3
          Reactive Intermediate, Carbonium Ion Rearrangement 41 min
        • Lecture11.4
          Reactive Intermediate, Carbanion 36 min
        • Lecture11.5
          Reactive Intermediate, Free Radical 47 min
        • Lecture11.6
          Reactive Intermediate, Carbene & Nitrene 42 min
      • 12. GOC 2 - Acid, base, Electrophile, Nucleophile
        3
        • Lecture12.1
          Acid Base, Electrophile Nucleophile 50 min
        • Lecture12.2
          Acid Base, Electrophile Nucleophile 47 min
        • Lecture12.3
          Hard Acid Base, Electrophilic Nucleophilic Strength 40 min
      • 13. Isomerism
        20
        • Lecture13.1
          Structural Isomers 39 min
        • Lecture13.2
          Tautomerism 37 min
        • Lecture13.3
          Stability Of Tautomers 43 min
        • Lecture13.4
          Factors Affecting Stability, Catalysis In Tautomerism 39 min
        • Lecture13.5
          Geometrical Isomerism 41 min
        • Lecture13.6
          E-z Nomenclature, Properties Of G.i. 43 min
        • Lecture13.7
          No. Of G.i., Interconversion Of G.i. 48 min
        • Lecture13.8
          Optical Isomerism & Its Conditions 50 min
        • Lecture13.9
          Different Types Of Projections, R-s Configuration 57 min
        • Lecture13.10
          Relationship Between Optical Isomers 45 min
        • Lecture13.11
          Dissymmetry In A Molecule 44 min
        • Lecture13.12
          Enantiomers, Mesomers, Diastereomers 39 min
        • Lecture13.13
          Special Case Of Optical Isomerism 47 min
        • Lecture13.14
          No. Of Optical Isomers, Stereoisomers 45 min
        • Lecture13.15
          D,l Configuration, Retention & Inversion 36 min
        • Lecture13.16
          Measurement Of Optical Activity 45 min
        • Lecture13.17
          No. Of Isomers 35 min
        • Lecture13.18
          Resolution Of Optical Isomers, Syn, Anti Addition, Elimination. 28 min
        • Lecture13.19
          Conformational Isomers 51 min
        • Lecture13.20
          Conformers Of Propane, Butane, Cyclohexane & Problems 44 min
      • 14. Reaction Mechanism
        21
        • Lecture14.1
          Introduction, Types Of Organic Reactions 35 min
        • Lecture14.2
          Nucleophilic Substitution Reaction 40 min
        • Lecture14.3
          Sn1 & Sn2 Reaction, Sni Pathway 53 min
        • Lecture14.4
          Reactivity In Sn1 & Sn2 Path 42 min
        • Lecture14.5
          Reactivity In Sn1 & Sn2 Path 36 min
        • Lecture14.6
          Reactivity In Sn1 & Sn2 Path 30 min
        • Lecture14.7
          Reactivity In Sn1 & Sn2 Path 41 min
        • Lecture14.8
          Elimination Reaction 53 min
        • Lecture14.9
          E1 & E2 Reaction, Isotopic Effect 46 min
        • Lecture14.10
          Orientation In Elimination Reaction 45 min
        • Lecture14.11
          Problems On Elimination Reaction 48 min
        • Lecture14.12
          Elimination Vs Substitution 34 min
        • Lecture14.13
          Addition Reaction 51 min
        • Lecture14.14
          Problems On Addition Reaction 46 min
        • Lecture14.15
          Electrophilic Aromatic Substitution Reaction 49 min
        • Lecture14.16
          Orientation In Electrophilic Aromatic Substitution 53 min
        • Lecture14.17
          Reactivity In Electrophilic Aromatic Substitution Reaction 30 min
        • Lecture14.18
          Examples Of Electrophilic Aromatic Substitution Reaction 37 min
        • Lecture14.19
          Examples Of Electrophilic Aromatic Substitution Reaction 37 min
        • Lecture14.20
          Nucleophilic Aromatic Substitution 44 min
        • Lecture14.21
          Benzyne Pathway 27 min
      • 15. Alkane
        7
        • Lecture15.1
          Alkane Preparation 49 min
        • Lecture15.2
          Alkane Preparation & Selective Hydrogenation 31 min
        • Lecture15.3
          Alkane Preparation 40 min
        • Lecture15.4
          Alkane Preparation 38 min
        • Lecture15.5
          Alkane Preparation 32 min
        • Lecture15.6
          Alkane Properties 55 min
        • Lecture15.7
          Alkane Properties & Problems 39 min
      • 16. Alkene
        7
        • Lecture16.1
          Alkene Preparation 45 min
        • Lecture16.2
          Alkene Preparation 36 min
        • Lecture16.3
          Alkene Properties 53 min
        • Lecture16.4
          Alkene Properties 40 min
        • Lecture16.5
          Alkene Properties 42 min
        • Lecture16.6
          Alkene Properties & Ozonolysis 41 min
        • Lecture16.7
          Alkene Properties, Oxidation, Substitution 38 min
      • 17. Alkyl Halides
        4
        • Lecture17.1
          Preparation 38 min
        • Lecture17.2
          Properties 49 min
        • Lecture17.3
          Haloform Reaction 28 min
        • Lecture17.4
          Grignard Reagent 29 min
      • 18. Chemical Bonding
        32
        • Lecture18.1
          Introduction, definition, Concept & Type of Bonding 53 min
        • Lecture18.2
          Ionic Bonding, covalent bonding 50 min
        • Lecture18.3
          Ionic Character in Covalent Bonding, Electronegativity 34 min
        • Lecture18.4
          Dipole Moment 42 min
        • Lecture18.5
          Fajan’s Rule 34 min
        • Lecture18.6
          Model for Covalent Compound, V.B.T. – Lewis St. Model 56 min
        • Lecture18.7
          Lewis Structure Model 45 min
        • Lecture18.8
          Formal Charge 46 min
        • Lecture18.9
          Formal Charge Rule 44 min
        • Lecture18.10
          Resonance 43 min
        • Lecture18.11
          Merits & Demerits of Lewis St. Model 44 min
        • Lecture18.12
          Drawing Lewis St. 30 min
        • Lecture18.13
          VSEPR 1 49 min
        • Lecture18.14
          VSEPR 2 51 min
        • Lecture18.15
          VSEPR 3 51 min
        • Lecture18.16
          VSEPR 4 33 min
        • Lecture18.17
          BackBonding 38 min
        • Lecture18.18
          Bond Angle determination 47 min
        • Lecture18.19
          Concept of Hybridisation 44 min
        • Lecture18.20
          Sp3, Sp2 Hybridisation 44 min
        • Lecture18.21
          SP hybridisation, Relative study of SP, SP2, SP3 Hybridisation 46 min
        • Lecture18.22
          Hybridsation involving D-orbitals 39 min
        • Lecture18.23
          Hybridsation with D-orbitals, Limitation of Hybridisation 41 min
        • Lecture18.24
          Calculation of Hybridisation of Central Atom, Problems 43 min
        • Lecture18.25
          Merits & demerits of VBT, Introduction to MOT 33 min
        • Lecture18.26
          MO formation, Bond Order 43 min
        • Lecture18.27
          MO with P-orbitals, B2, Magnetic Character 43 min
        • Lecture18.28
          MO of Diatomic Species, Hetroatomic Species 51 min
        • Lecture18.29
          Secondary Bondings 39 min
        • Lecture18.30
          H Bonding 37 min
        • Lecture18.31
          Metallic Bonding 52 min
        • Lecture18.32
          Chapter Notes – Chemical Bonding
      • 19. Periodic Table
        10
        • Lecture19.1
          Development of P.T. 43 min
        • Lecture19.2
          Mandeelev P.T. & Mosley, Modern P.T. 43 min
        • Lecture19.3
          Modern P.T. & Periodic Properties 27 min
        • Lecture19.4
          Atomic Volume & Radius 49 min
        • Lecture19.5
          Atomic Radius, Ionisation Energy 28 min
        • Lecture19.6
          Ionisation Energy 48 min
        • Lecture19.7
          Electron Affinity, Hydration Energy 52 min
        • Lecture19.8
          Electronegativity, Lattice Energy 46 min
        • Lecture19.9
          Oxidising & Reducing Power, Nature of oxides 38 min
        • Lecture19.10
          M.P. & B.P., Density, Bond Energy, Diagonal relationship, Inert Pair Effect 25 min
      • 20. Metallurgy
        7
        • Lecture20.1
          Introduction, Concentration of ore 49 min
        • Lecture20.2
          Roasting, Calcination, smelting 41 min
        • Lecture20.3
          Refining of metal 29 min
        • Lecture20.4
          Pyrometallurgy, electrometallurgy, Hydrometallurgy 32 min
        • Lecture20.5
          Ellingham Diagram 43 min
        • Lecture20.6
          Extraction of Cu & Fe 22 min
        • Lecture20.7
          Extraction of Al & Zn 26 min
      • 21. Hydrogen and its Compounds
        7
        • Lecture21.1
          preparation, properties & Type of Hydrogen 57 min
        • Lecture21.2
          Compounds of Hydrogen, Hydrides, Water, Hydrates 56 min
        • Lecture21.3
          Hardness of Water, H2O2 56 min
        • Lecture21.4
          Problems 48 min
        • Lecture21.5
          Problems 28 min
        • Lecture21.6
          Chapter Notes – Hydrogen and its Compounds
        • Lecture21.7
          NCERT Solutions – Hydrogen
      • 22. S block metals
        8
        • Lecture22.1
          IA 1 – elemental Properties of Alkali metals& its Compounds 57 min
        • Lecture22.2
          IA 2 – Na & its compounds 01 hour
        • Lecture22.3
          IA 3 – Na & its Compounds, Use of Na & K 27 min
        • Lecture22.4
          IIA 1 – Elemental Properties 41 min
        • Lecture22.5
          IIA 2 – Compounds of IIA Metals 53 min
        • Lecture22.6
          IIA 3 – Compounds of Ca 48 min
        • Lecture22.7
          Chapter Notes – S block metals
        • Lecture22.8
          NCERT Solutions – S block metals
      • 23. p block elements
        8
        • Lecture23.1
          Introduction to P – Block & IIIA – elemental properties 51 min
        • Lecture23.2
          IIIA – General properties of compounds & B-compounds 40 min
        • Lecture23.3
          IIIA – Boron compounds, Use of B and Al 35 min
        • Lecture23.4
          IVA – Elemental Properties of C family 46 min
        • Lecture23.5
          IVA – Allotropes of C & compounds of C 01 hour
        • Lecture23.6
          IVA – Compounds of Si 48 min
        • Lecture23.7
          Chapter Notes – p block elements
        • Lecture23.8
          NCERT Solutions – p block elements

        Chapter Notes – S block metals

        ➣  Groups (1 & 2) belong to the s-block of the Periodic Table.
        ➣  Group 1 consists of : lithium, sodium, potassium, rubidium, caesium and francium and collectively known as the alkali metals.
        ➣   Group 2 include : beryllium, magnesium,calcium, strontium, barium and radium. Except Beryllium they are known as alkalinev

        Physical properties-

        a) Large atomic radii: The atomic radii of alkali metals are the largest in their respective periods. These increase as we travel down the group.

        b) Large ionic radii: The ionic radii increase as we move down the group due to the addition of a new energy shell with each succeeding element.

        c) Low ionization enthalpy: The ionization enthalpies  decrease as we move down the group.The ionization enthalpies of the alkali metals are the lowest due to loosely held s- electron.

        d) Hydration enthalpy: It decreases with the increase in ionic radii.The hydration enthalpy of Li ion is the maximum and the hydration enthalpy of Cs ion is the minimum.

        e) Oxidation  state:  The  alkali  metals  exhibit  oxidation  state  of  +1  in  their compounds and are strongly electropositive in character. The electropositive character increases from Li to Cs.

        f) Metallic character: The metallic character increases down the group.

        g) Melting point and boiling point:: The m p and b p  of alkali metals are very low and decrease with increase in atomic number.

        h) Nature of bonds formed: These metals form ionic bonds. The ionic character increases as we down the group.

        i) Flame colouration: All the alkali metals impart a charactersistic colour to the flame.

        j) Photoelectric effect: Alkali metals (except Li) exhibits photoelectric effect.

         

        Chemical features of alkali metals:

        a) Reducing character: As the ionization enthalpies of the alkali metals decrease
        down the  group their reducing character or reactivity in the gaseous state increases down the group. i.e., Li < Na < K < Rb < Cs .

        b) Reaction with dihydrogen: Alkali metals react with dry hydrogen at about 673 K to form crystalline hydrides which are ionic in nature and have high melting points.Alkali metals react with dry hydrogen

        c) Oxides  and  hydroxides:  Alkali  metals  when  burnt  in  air  form  different
        compounds, for example the alkali metals on reaction with limited quantity of oxygen form normal oxides ( M2O) M= Li, Na, K, Rb, Cs

        d) Reaction with halogens: The members of the family combine with halogen to form corresponding halides which are ionic crystalline solids.
        Reactivity of alkali metls with particular halogen increases from Li to Cs.

        e) Reaction with water: Alkali metals react with water and other compounds containing acidic hydrogen atoms such as hydrogen halides, acetylene etc. to liberate hydrogen gas.

        f) Solubility in liquid ammonia: All alkali metals dissolve in liquid ammonia giving deep blue solutions which are conducting in nature.

        g) Reaction with sulphur and phosphorus: Alkali metals react with sulphur and phosphorus on heating to form sulphides and phosphides respectively

        Diagonal relationship between Li and Al

        Li resembles Mg mainly due to similarity in sizes of their atoms and ions.

        The main points of similarity are:

        i)  Both are quite hard.
        ii)  Both LiOH and Mg(OH)2 are weak bases.
        iii) Carbonates of both on heating decompose to produce oxides and carbondioxide.
        iv) Both react with nitrogen to give ionic nitrides.
        v)  Nitrates of both decompose on heating to give oxides.
        vi) Both Li and Mg do not form solid bicarbonates.
        vii Because of covalent character LiCl and MgCl2 are soluble in ethanol.
        viii) The hydroxides, bicarbonates and fluorides of both Li and Mg are sparingly soluble in water.

         

        Biological importance of  Na and K

        i) Sodium ions participate in the transmission of nerve signals.
        ii) Sodium ions also regulate flow of water across the cell membranes and in transport of sugars and amino acids into the cells.
        ii) Potassium ions are the most abundant cations within cell fluids, where they activate many enzymes, participate in oxidation of glucose to produce ATP.
        iv) Potassium ions in combination with sodium  ions are responsible for transmission of nerve signals.
        v) The functional features of nerve cells depend upon the sodium potassium ion gradient that is established in the cell.

        Group 2 elements: Alkaline earth metals

        a) Atomic radii : The atomic radii of alkaline earth metals are fairly large thoughsmaller than the corresponding alkali metals and they increase down the group. This is because on moving down the group, atomic radii increase primarily due to the addition of an extra shell of electrons in each succeeding element.
        (b) Ionic radii: the atoms of these elements form divalent ions which show the same trend of increase in their size down the group.
        (
        c)  Ionization enthalpy:  The  alkaline  earth  metals  have  fairly  low  Ionizations enthalpies though greater than those of the corresponding elements of group 1 and this value decreases down the group.

        (d)  Hydration  enthalpy:  the  Hydration  enthalpies  of  alkaline  earth  metal  ion decrease as the size of the metal ion increases down the Group
        Be2>+ >Mg2+ >Ca2+ >Sr2+ >Ba2+               
        (
        e) Oxidation State: All the members of the family exhibit +2 oxidation state in their compounded and the form divalent cations (M2+)
        (
        f) Electro negativity : The electro negativity values of alkaline earth metals are quite close to those of alkali metals, though slightly more.
        (g) Metallic Character :  Alkaline earth metals have stronger metallic bonds as compared to the alkali metals present in the same period.
        (h) Melting and boiling point : The melting and Boiling points of these metals are higher than those of alkali metals present in the same period.
        (i) Colouration to the flame : With the exceptio9n of beryllium and magnesium, the rest of the elements impart characters in colour to the same flame. For example,

        Be Mg Ca  Sr Ba Ra
        Brick Red  Crimson Grassy  Green  Crimson

        J) Complex formation: Generally the members do not form complexes. However, smaller ions ( Be & Mg Ions) form complexes with the  electron donor species
        k) Formation of  organo-metallic compounds:  Both  beryllium and  magnesium form a number of organo-metallic compounds containing M-C bond with certain organic compounds. For example, magnesium reacts with alkyl halide in the presence of dry ether to give Grignard reagent.

        l)  Reducing character: Alkaline earth metals are weak reducing agent than the corresponding alkali metals which have lower ionization enthalpies and comparatively bigger atomic sizes.

        m) Reaction with oxygen: With the exception of Ba and Ra which form peroxides ( MO2) rest of the metals form normal oxides (MO) on heating with excess of oxygen.

        n) Reaction with  halogens: The  members of the  family combine directly with halogen at appropriate temperature to form corresponding halides.

        o) Reaction with water: The members of this group are less reactive towards water as compared to the corresponding alkali metals because these are less electropositive in nature.

        p) Reaction  with  hydrogen:  The  members  except  Be combine  with  hydrogen directly upon heating to form metal hydrides.

        Uses of some important compounds:–
        Caustic soda:

        It is used: in soap, paper, textile, petroleum industry

        Sodium carbonate

        It is used:

        a)  in glass and soap industry
        b)
         in paper making and textile manufacturing c)  in paint and dye stuffs
        d) in metal refining
        e)  in  production of sodium compounds such as  borax,  caustic  soda,  sodium phosphate etc.

        Quick lime:

        It is used:

        a).  in the preparation of cement, glass and calcium carbide.
        b).  In the purification of sugar
        c).  In softening of hard water
        d). As a flux in the extraction of metal

         

        Lime stone:

        It is used

        a) as building material
        b) in the manufacture of quick lime
        c) in Solvay process to prepare Na2CO3 as it is a source of CO2
        d)
         in metallurgy for the extraction of iron
        e) in toothpaste and certain cosmetics

        Cement:

        It is an important building material. It is used in concrete and reinforced concrete, in plastering and in the construction of bridges, dams and buildings.

         Plaster of paris:

        It is used
        a)
         in making moulds for pottery and ceramics etc.
        b)
         in surgical bandages for setting broken bones of the body
        c) for making statues, models, decorative materials and black board chalk.

        Biological importance of  Ca and Mg

        i)  Magnesium ions are concentrated in animal cells and Calcium ions are concentrated in body fluids, outside the cell.
        ii) All enzymes that utilize ATP in phosphate transfer require magnesium ion as cofactor.
        iii) In green plants magnesium is present in chlorophyll.
        iv) Calcium and magnesium ions are also essential for the transmission of impulses along nerve fibres.
        v) Calcium ions are important in blood clotting and are required to trigger the contraction of muscles.
        vi) Calcium ions also regulate the beating of the heart.

        Prev IIA 3 – Compounds of Ca
        Next NCERT Solutions – S block metals

        Leave A Reply Cancel reply

        Your email address will not be published. Required fields are marked *

        All Courses

        • Backend
        • Chemistry
        • Chemistry
        • Chemistry
        • Class 08
          • Maths
          • Science
        • Class 09
          • Maths
          • Science
          • Social Studies
        • Class 10
          • Maths
          • Science
          • Social Studies
        • Class 11
          • Chemistry
          • English
          • Maths
          • Physics
        • Class 12
          • Chemistry
          • English
          • Maths
          • Physics
        • CSS
        • English
        • English
        • Frontend
        • General
        • IT & Software
        • JEE Foundation (Class 9 & 10)
          • Chemistry
          • Physics
        • Maths
        • Maths
        • Maths
        • Maths
        • Maths
        • Photography
        • Physics
        • Physics
        • Physics
        • Programming Language
        • Science
        • Science
        • Science
        • Social Studies
        • Social Studies
        • Technology

        Latest Courses

        Class 8 Science

        Class 8 Science

        ₹8,000.00
        Class 8 Maths

        Class 8 Maths

        ₹8,000.00
        Class 9 Science

        Class 9 Science

        ₹10,000.00

        Contact Us

        +91-8287971571

        contact@dronstudy.com

        Company

        • About Us
        • Contact
        • Privacy Policy

        Links

        • Courses
        • Test Series

        Copyright © 2021 DronStudy Pvt. Ltd.

        Login with your site account

        Lost your password?

        Modal title

        Message modal