Slide 1

  • Introduction to p-Block Elements
  • Group 13 Elements
  • Boron as a member of Group 13

Slide 2

  • Physical properties of Boron
    • Atomic number: 5
    • Atomic mass: 10.81 amu
    • Melting point: 2076°C
    • Boiling point: 3927°C

Slide 3

  • Chemical properties of Boron
    • Boron reacts with hydrogen to form hydrides
    • Reaction of Boron with Hydrogen
    • Formation of Diborane (B2H6)

Slide 4

  • Diborane
    • Structure of Diborane
    • Lewis structure and hybridization
    • Preparation of Diborane
    • Properties of Diborane

Slide 5

  • Uses of Diborane
    • As a reducing agent
    • In the synthesis of boron compounds
    • As a rocket propellant

Slide 6

  • Boron Hydrides
    • Types of Boron Hydrides
      • Diborane, B2H6
      • Borane, BH3
      • Borohydrides, MBH4 (Where M is a metal)

Slide 7

  • Diborane (B2H6)
    • Properties of Diborane
    • Reactions of Diborane
      • Hydrolysis of Diborane
      • Oxidation of Diborane
      • Addition reactions of Diborane

Slide 8

  • Preparation of Diborane
    • Direct synthesis from Boron and Hydrogen
    • Alumino-thermic reduction of Boric acid
    • Reaction of Sodium Borohydride with Boron Trifluoride

Slide 9

  • Uses of Diborane
    • As a reducing agent in organic synthesis
    • In the production of high-purity boron
    • In the manufacture of boron-based ceramics

Slide 10

  • Borane (BH3)
    • Structure of Borane
    • Preparation of Borane
    • Properties of Borane
    • Reactions of Borane Sure! Here are slides 11 to 20 in markdown format: ``markdown
  1. Chemistry of p-Block Elements- Group 13 - Reaction of Boron with Hydrogen
  • Boron reacts with hydrogen gas to form hydrides.
  • The reaction can be represented as follows:
    • Boron + Hydrogen → Boron Hydride
  • Example: Boron + 3 Hydrogen → Borane (BH3)
  1. Boron Hydrides
  • Boron forms various hydrides, such as boranes and borohydrides.
  • These hydrides are important reagents in organic synthesis and materials chemistry.
  • Example: Diborane (B2H6), Borane (BH3), Sodium Borohydride (NaBH4)
  1. Diborane (B2H6)
  • Diborane has a molecular formula B2H6.
  • It has a bridged structure with two boron atoms sharing four electrons.
  • Diborane is a versatile reducing agent and is used in various organic reactions.
  • Example: Diborane reacts with aldehydes and ketones to form alcohols.
  1. Preparation of Diborane
  • Diborane can be prepared by the reaction of boron trifluoride (BF3) with lithium aluminum hydride (LiAlH4).
  • Another method is the reaction of boron trichloride (BCl3) with sodium borohydride (NaBH4).
  • Example: 6 NaBH4 + 2 BCl3 → B2H6 + 6 NaCl + 3 H2
  1. Properties of Diborane
  • Diborane is a colorless gas with a pungent odor.
  • It is highly reactive and can spontaneously ignite in air.
  • Diborane is unstable and decomposes at elevated temperatures.
  • Example: Diborane reacts with water to form boric acid and hydrogen gas.
  1. Uses of Diborane
  • Diborane is used as a reducing agent in organic synthesis.
  • It is used in the manufacture of boron-based ceramics.
  • Diborane is used as a rocket propellant.
  • Example: Diborane is used in the production of high-purity boron.
  1. Borane (BH3)
  • Borane (BH3) is a boron hydride compound.
  • It exists in various forms, such as borane-dimethyl sulfide (BH3·SMe2) and borane-THF complex (BH3·THF).
  • Borane is used as a reducing agent in organic synthesis.
  • Example: Borane reduces alkenes to alkanes.
  1. Preparation of Borane
  • Borane can be prepared by the reaction of boron trihalides (BCl3, BBr3) with lithium aluminum hydride (LiAlH4).
  • Another method is the reaction of boron trichloride (BCl3) with sodium borohydride (NaBH4).
  • Example: BCl3 + 3 LiAlH4 → 2 BH3 + 3 LiCl + 3 AlCl3
  1. Properties of Borane
  • Borane is a colorless gas with a pungent odor.
  • It is a powerful reducing agent and reacts readily with organic compounds.
  • Borane easily forms adducts with Lewis bases, such as ethers and amines.
  • Example: Borane forms an adduct with tetrahydrofuran (THF) to give borane-THF complex.
  1. Reactions of Borane
  • Borane reacts with alkenes to form alkylboranes.
  • It reduces aldehydes and ketones to alcohols.
  • Borane can also react with acids to form boronate esters.
  • Example: Borane reacts with ethene to form borane-ethylene complex.

Please note that the slide numbers have been omitted, as per your request. Sure! Here are slides 21 to 30 in markdown format:markdown

  1. Oxidation of Borane
  • Borane can be oxidized to form boric acid (H3BO3) or boron trioxide (B2O3).
  • The reaction can be represented as follows:
    • 2 BH3 + 3 O2 → B2O3 + 3 H2O
  • Example: Borane reacts with oxygen to form boric acid.
  1. Addition reactions of Borane
  • Borane can undergo addition reactions with various compounds.
  • Addition of borane to alkenes forms alkylboranes.
  • Addition of borane to carbonyl compounds forms borohydrates.
  • Example: Addition of borane to ethylene forms borane-ethylene complex.
  1. Borohydrides (MBH4)
  • Borohydrides are compounds with the formula MBH4, where M is a metal.
  • Borohydrides are important reducing agents in organic synthesis.
  • Examples: Sodium borohydride (NaBH4) and lithium borohydride (LiBH4).
  1. Sodium Borohydride (NaBH4)
  • Sodium borohydride is a white crystalline solid.
  • It is a powerful reducing agent and is used in various reactions.
  • NaBH4 reduces carbonyl compounds to alcohols.
  • Example: NaBH4 reduces acetophenone to give 1-phenylethanol.
  1. Lithium Borohydride (LiBH4)
  • Lithium borohydride is a white crystalline powder.
  • It is a very strong reducing agent and is used in organic synthesis.
  • LiBH4 reduces esters to alcohols.
  • Example: LiBH4 reduces ethyl acetate to give ethanol.
  1. Chemistry of Aluminum (Al)
  • Aluminum is a member of Group 13 of the periodic table.
  • It is a silvery-white metal with atomic number 13.
  • Aluminum is a lightweight and malleable metal.
  • Example: Aluminum is used in the production of aircraft.
  1. Reactivity of Aluminum
  • Aluminum is a reactive metal.
  • It reacts with oxygen to form a protective oxide layer.
  • Aluminum reacts with acids to produce hydrogen gas.
  • Example: Aluminum reacts with hydrochloric acid to form aluminum chloride and hydrogen gas.
  1. Uses of Aluminum
  • Aluminum is used in the production of various alloys, such as aluminum-magnesium alloys.
  • It is used in the manufacture of cans for beverages.
  • Aluminum is used in construction due to its strength and resistance to corrosion.
  • Example: Aluminum is used in the production of window frames.
  1. Chemistry of Gallium (Ga)
  • Gallium is a member of Group 13 of the periodic table.
  • It is a soft, silvery metal with atomic number 31.
  • Gallium has a low melting point and is a liquid near room temperature.
  • Example: Gallium is used in the production of semiconductors.
  1. Reactivity of Gallium
  • Gallium is less reactive compared to aluminum.
  • It reacts with oxygen to form gallium(III) oxide.
  • Gallium reacts with acids to produce gallium(III) salts and hydrogen gas.
  • Example: Gallium reacts with sulfuric acid to form gallium sulfate and hydrogen gas. Please note that the line was added to prevent premature formatting; please remove it before using the slides.