Course Content
CHAPTER 3: CLASSIFICATION OF ELEMENTS
Section Name Topic Name 3 Classification of Elements and Periodicity in Properties 3.1 Why do we Need to Classify Elements ? 3.2 Genesis of Periodic Classification 3.3 Modern Periodic Law and the present form of the Periodic Table 3.4 Nomenclature of Elements with Atomic Numbers > 100 3.5 Electronic Configurations of Elements and the Periodic Table 3.6 Electronic Configurations and Types of Elements: s-, p-, d-, f – Blocks 3.7 Periodic Trends in Properties of Elements
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CHAPTER 7: EQUILIBRIUM
Section Name Topic Name 7 Equilibrium 7.1 Equilibrium in Physical Processes 7.2 Equilibrium in Chemical Processes – Dynamic Equilibrium 7.3 Law of Chemical Equilibrium and Equilibrium Constant 7.4 Homogeneous Equilibria 7.5 Heterogeneous Equilibria 7.6 Applications of Equilibrium Constants 7.7 Relationship between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G 7.8 Factors Affecting Equilibria 7.9 Ionic Equilibrium in Solution 7.10 Acids, Bases and Salts 7.11 Ionization of Acids and Bases 7.12 Buffer Solutions 7.13 Solubility Equilibria of Sparingly Soluble Salts
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CHAPTER 10: S-BLOCK ELEMENTS
Section Name Topic Name 10 The s-Block Elements 10.1 Group 1 Elements: Alkali Metals 10.2 General Characteristics of the Compounds of the Alkali Metals 10.3 Anomalous Properties of Lithium 10.4 Some Important Compounds of Sodium 10.5 Biological Importance of Sodium and Potassium 10.6 Group 2 Elements : Alkaline Earth Metals 10.7 General Characteristics of Compounds of the Alkaline Earth Metals 10.8 Anomalous Behaviour of Beryllium 10.9 Some Important Compounds of Calcium 10.10 Biological Importance of Magnesium and Calcium
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CHAPTER 12: CHARACTERIZATION OF ORGANIC COMPOUND
Section Name Topic Name 12 Organic Chemistry – Some Basic Principles and Techniques 12.1 General Introduction 12.2 Tetravalence of Carbon: Shapes of Organic Compounds 12.3 Structural Representations of Organic Compounds 12.4 Classification of Organic Compounds 12.5 Nomenclature of Organic Compounds 12.6 Isomerism 12.7 Fundamental Concepts in Organic Reaction Mechanism 12.8 Methods of Purification of Organic Compounds 12.9 Qualitative Analysis of Organic Compounds 12.10 Quantitative Analysis
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Chemical properties of group 13

  • Out of all elements of this group, Boron is non-reactive. This is because of its small size as it has high ionization energy .So, reactivity increases down the group.

            B               <        Al                  <     Ga            <     In                 <       Tl

Boron                                     aluminum                              Gallium                         indium                                thallium

  • In this Boron is least reactive because of its small size and high ionization energy and Thallium is most reactive because of its low ionization energy.
  • Aluminum: When react initially, it keeps reacting .But after some time, a layer of its oxide is formed over its surface. This layer prevent it from further reacting .So, it becomes passive after some time.
  • Most of the compounds of this group are electron deficient that is their octet is not complete. So, they behave as Lewis acids.

            Example: BX3 (only 6 electrons in valence shell of Boron).

            Therefore, it forms coordinate bond.

                       BX3 + NH3–>[NH3–>BF3]coordinate bond

                                                  Boron halide   ammonia

  • That means, they have tendency to take electrons. Or, we can say they are Lewis acids. But down the group, acidic character decreases (that is tendency to attract incoming electron decreases).

BX3>               AlX3 >          GaX3           >InX3                 >TlX3

boron halide    aluminum halide    gallium halide   indium halide         thallium halide

  • Lewis acid strength decreases because size increases .As a result, attraction towards incoming electron decreases.
  1. Reactivity towards oxygen : Forms oxides
  • Boron does not react with oxygen at ordinary temperature due to small size and high ionization energy.
  • If we react Al with oxygen, it reacts at normal temperature. With time it forms a protective layer of oxide on its surface. This layer makes it non reactive.

                Al   +3O2 –>2Al2O3

                                                    aluminum   oxygen   aluminum oxide

  • They react with nitrogen gas also, to form compound with formula EN.

Example: 6Al +3N2–>6AlN

                    aluminum      nitrogen     aluminum nitride

  • If we see acidic strength of oxides, then it decreases down the group.

BeO             Al2O3           GaO                   InO             TlO

beryllium oxide     aluminum oxide     gallium oxide             indium oxide             thallium oxide

                  (acidic)                     (amphoteric)                                        (all are basic)

  1. Reaction with water: Hydroxides are formed of type E(OH)
  • Boron does not react with water.
  • Aluminum reacts with cold water that is :

Al  + H2O –> Al(OH)3 + H2

                     Aluminium  water   aluminium hydroxide  hydrogen gas

  • Gallium and indium neither react with cold water nor with hot water.
  • Thallium reacts with water but form protective layer which make it passive.
  1. 3. Reactivity towards acids and bases:
  • Boron doesn’t react with acids and bases at normal temperature, but reacts with strong acids.
  • Aluminum reacts with acid and base because it is amphoteric in nature.

           Al + HCl–>AlCl3 + H2

           aluminum hydrogen chloride   aluminum chloride  hydrogen gas

           Al + NaOH –>[NaAl(OH)4]

                                        Aluminum    sodium hydroxide      sodium tetrahydroxoaluminate

  • Al when react with nitric acid, initially it reacts but after same time it became passive.
  1. Reaction with Halogens: Form halides of type EX3

                      2B +3X2–>2BX3

                                    boron    halogen     boron halide

                       B +F2 –>BF3

                                    boron halogen   boron halide

                       Al +Cl2àAlCl3

                       aluminum  chlorine   aluminum chloride

                             All halides are Lewis bases.

Important trends

  1. Formation of Hydrides : EH3
  • Thermal stability of hydrides decrease down the group .Out of all, only BH3 is stable.

BnHn+4 , BnHn+6=  Boranes

Simplest Borane :B2H6(diborane )

  • This diborane has banana bond and it is weak Lewis acid.
  1. Formation of Halides: They form their respective halides. Out of all halides aluminum chloride AlCl3exist as dimer that is Al2Cl(all halides behave as Lewis acids)
  • They will behave as Lewis acids only, if they attract incoming electrons.
  • Trends of strength of Lewis acids :
  • BF3>AlCl3>BBr3>BI3(expected order)
  • BF3<AlCl3>BBr3>BI3(actual)

Explained on the basis of back bonding:

  • In case of BF3, in Boron there is one vacant 2p orbital ( i.e 2s2,2p1)in ground state.
  • In excited state, it will be 2s1, 2pand energy of 2p orbital of B and F are almost similar.
  • As a result, one of the 2p filled orbital overlaps sidewise with the vacant 2p orbital of boron atom resulting in transfer of electrons from Fluorine to vacant 2p orbital.
  • This is called back bonding.
  • Now it doesn’t have fewer electrons therefore, Boron no longer act as a Lewis acid.
  • As size increases, the tendency of back bonding decrease and acidic strength increase.

Uses of Boron

  1. Boron is used as semi conductor for making electrical appliances.
  2. It is used in steel industry for hardening.
  3. Its compounds like borax and boric acid are used in glass industry.
  4. Borax is used for soldering metals.
  5. Borax fibers are used in making bullets.

Uses of Aluminum

  1. It is soft and light metal, non toxic and is used for wrapping food items.
  2. It I used in making electric power cables.
  3. It is used as packaging of food items.
  4. It is used I making cans for cold drink etc.

Alloys of Aluminum

  • Bronze : Aluminum and Copper are its constituents .It is used for making coins ,jewellery etc
  • Magnalium: its constituents are Al and Mg.

           It is used for making pressure cookers, balance beams etc.

  • Duralumin: its constituents are: Al, Cu, Mg and Mn.

It is used for making bodies of air craft’s, helicopters, ships etc.

  • ALNICO: Its constituents are AL, Ni and Cobalt.

It is used in making powerful magnets.

Borax

  1. Borax: Na2B4O7.10H2O
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The p Block Elements

Preparation  

  • From Colemanite ore: It is prepared from Colemanite ore (calcium ore).
  • In this ore is made to react with sodium carbonate.
  • Then it is heated as shown in reaction :

Ca2B6O11 + Na2CO3—> CaCO3 +Na2B4O7 + NaBO2

Colemanite ore   sodium carbonate    calcium carbonate  Borax   sodium metaborate

  • The solution has White precipitate.
  • When these precipitates are filtered, the solution becomes concentrated.
  • Finally, we get crystals of borax on cooling.
  • From Boric acid : In this also boric acid is made to react with Sodium carbonate to form Borax ,carbon dioxide and water as shown below:

H3BO3 + Na2CO3—>Na2B4O7 + CO2 + H2O

Boric acid    sodium carbonate    borax      carbon dioxide     water

PROPERTIES OF BORAX

  • It is white crystalline solid.
  • On heating, it loses water of crystallization and form Na2B4O
  • On further heating, it gives white transparent liquid which further on cooling gives white transparent bead.
  • This bead is made to react with different types of salts.
  • When reacted ,it gives different colour with different metal ions like :

With Ni2+–>brown

With Co2+–>blue

With Cr3+àgreen

With Mn2+–>pink

With Cu2+–>blue

Uses of Borax

  • It is used in laboratory as Borax bead test.
  • It is used in making enamels for pottery.
  • It is used in candle making.
  • It is added in soaps due to its antiseptic properties.
  • It is used in optical glass.
  1. Ortho boric acid

Chemical Formula :- H3BO3 or B(OH)3

The p Block Elements Notes and NCERT Solution For Class 11th Chemistry.
The p Block Elements

Preparation: It is prepared from Borax.

Na2B4O7.10H2O + HCl +H2O–>H3BO3 + NaCl

 Borax                hydrochloric acid      boric acid  sodium chloride

Properties

  • It is white crystalline solid with soapy touch.
  • It is sparingly soluble in cold water but soluble in hot water.
  • At 373k, it forms metaboric acid.
  1. Boron hydrides

The molecular formula is BnH2n+4

The common hydride is :B2H6 that is diborane.

The p Block Elements Notes and NCERT Solution For Class 11th Chemistry.
The p Block Elements
The p Block Elements Notes and NCERT Solution For Class 11th Chemistry.
The p Block Elements
  • Both the Boron will have in total 2 empty d orbital.
  • Each 2p orbital overlaps with 1s orbital of H atoms.
  • The 2 hybrid orbital left on each Boron atom contain an unpaired electron and other is empty.
  • The orbital containing one electron of one boron atom and the other empty orbital of second boron atom form a bond with hydrogen atom simultaneously to give B-H-B bond.
  • Each Boron form 2 covalent bond.
  • Out of 3 unpaired electrons, the left electron of both the boron is 2 and of 2 Hydrogen atom is also 2.
  • Therefore, it forms 3 bonds instead of 2 bonds.
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