Chemistry of Group 13 and Group 14 Elements - Important Question 2

Slide 1

  • Introduction to Group 13 and Group 14 elements
  • Boron family (Group 13): Boron (B), Aluminium (Al), Gallium (Ga), Indium (In), Thallium (Tl)
  • Carbon family (Group 14): Carbon (C), Silicon (Si), Germanium (Ge), Tin (Sn), Lead (Pb)

Slide 2

  • Electronic configuration and general trends in the periodic table
  • Group 13: ns^2np^1 (except Tl)
  • Group 14: ns^2np^2

Slide 3

  • Physical properties of Group 13 elements
  • Boron: Non-metal, low melting and boiling points
  • Aluminium: Metal, high melting and boiling points
  • Gallium, Indium, Thallium: Soft metals, low melting points, good electrical conductors

Slide 4

  • Chemical properties of Group 13 elements
  • Boron: Forms covalent compounds, doesn’t show typical metallic behavior
  • Aluminium: Exhibits typical metallic behavior, forms covalent and ionic compounds
  • Gallium, Indium, Thallium: Reactivity increases (down the group), form compounds with +1 oxidation states

Slide 5

  • Boron and its compounds
  • Boron trihalides (BX₃): BF₃, BCl₃, BBr₃, BI₃
  • Boranes: BₙHₙ₊₄
  • Diborane (B₂H₆): Structure and properties

Slide 6

  • Aluminium and its compounds
  • Aluminium oxide (Al₂O₃): Structure and properties
  • Aluminium chloride (AlCl₃): Lewis acid, used in Friedel-Crafts reactions

Slide 7

  • Physical properties of Group 14 elements
  • Carbon: Non-metal, exists in various allotropes (diamond, graphite, fullerene)
  • Silicon: Metalloid, used in computer chips
  • Germanium: Metalloid, used in semiconductors

Slide 8

  • Chemical properties of Group 14 elements
  • Carbon: Forms covalent compounds, shows catenation
  • Silicon: Forms covalent compounds, exhibits similar chemical behavior to carbon
  • Germanium: Forms covalent compounds, behaves similarly to silicon

Slide 9

  • Tin and its compounds
  • Metallic tin: Used in soldering, low melting point
  • Tin(II) oxide (SnO): Used as a reducing agent
  • Organotin compounds: Example - Tributyltin (C₄H₉)₃Sn

Slide 10

  • Lead and its compounds
  • Metallic lead: Used in batteries, low melting point
  • Lead oxide (PbO): Red pigment in paints
  • Lead sulfate (PbSO₄): Forms in car batteries

Slide 11

  • Carbon dioxide (CO₂):
    • Greenhouse gas responsible for global warming
    • Produced during combustion and respiration
    • Used in carbonated beverages
  • Carbon monoxide (CO):
    • Poisonous gas, produced during incomplete combustion
    • Binds to hemoglobin, preventing oxygen transport

Slide 12

  • Silicon dioxide (SiO₂):
    • Commonly known as silica
    • Found in quartz and sand
    • Used in glass manufacturing and as a filler in concrete

Slide 13

  • Germanium dioxide (GeO₂):
    • Used in the production of optical fibers
    • Used in the semiconductor industry

Slide 14

  • Tin(IV) oxide (SnO₂):
    • Named as “stannic oxide”
    • Used as a polishing agent and as a glaze in ceramics

Slide 15

  • Lead(II) oxide (PbO):
    • Red pigment in paints, known as “lead red”
    • Used in the production of glass and ceramics

Slide 16

  • Group 13 elements in the periodic table:
    • Boron: Atomic number 5
    • Aluminium: Atomic number 13
    • Gallium: Atomic number 31
    • Indium: Atomic number 49
    • Thallium: Atomic number 81

Slide 17

  • Group 14 elements in the periodic table:
    • Carbon: Atomic number 6
    • Silicon: Atomic number 14
    • Germanium: Atomic number 32
    • Tin: Atomic number 50
    • Lead: Atomic number 82

Slide 18

  • Electronegativity of Group 13 elements:
    • Increases from boron to aluminum
    • Gallium, indium, and thallium have similar electronegativity

Slide 19

  • Electronegativity of Group 14 elements:
    • Carbon: 2.5
    • Silicon: 1.9
    • Germanium: 2.0
    • Tin: 1.8
    • Lead: 2.3

Slide 20

  • Reactivity of Group 13 elements:
    • Boron: Less reactive, mostly forms covalent compounds
    • Aluminium: Reacts with acids, forms ionic compounds
    • Gallium, indium, and thallium: Reactive, exhibit metallic behavior, form compounds with various oxidation states

Slide 21

  • Naming compounds of Group 13 elements:
    • Cation: Named using the element name (e.g., Al^3+ is called aluminum ion)
    • Anion: Named by replacing the ending of the element name with “-ide” (e.g., aluminium chloride)
  • Examples:
    • AlCl₃: Aluminum chloride
    • Ga₂O₃: Gallium oxide
    • TlBr: Thallium bromide

Slide 22

  • Naming compounds of Group 14 elements:
    • Carbon compounds usually named using common names (e.g., methane, ethane)
    • Silicon and germanium compounds named similar to carbon compounds
    • Tin and lead compounds named using the stock system (e.g., SnCl₄: Tin(IV) chloride)
  • Examples:
    • CO: Carbon monoxide
    • SiO₂: Silicon dioxide
    • PbO₂: Lead(IV) oxide

Slide 23

  • Common applications of Group 13 elements:
    • Aluminum: Used in aerospace industry, construction, and packaging
    • Boron: Used in high-strength materials, nuclear reactors, and medicine
    • Gallium: Used in semiconductors, LEDs, and solar cells
    • Thallium: Used in specialized glass, infrared optics, and cancer treatment
  • Examples and equations can be discussed for each application if needed

Slide 24

  • Common applications of Group 14 elements:
    • Carbon: Used in making steel, fuel production, and organic compounds
    • Silicon: Used in computer chips, solar cells, and glass manufacturing
    • Germanium: Used in fiber optics, semiconductors, and infrared optics
    • Tin: Used in soldering, coating for food cans, and organotin compounds
    • Lead: Used in batteries, radiation shielding, and pigments
  • Examples and equations can be discussed for each application if needed

Slide 25

  • Oxidation states of Group 13 elements:
    • Boron: Generally +3, +1 in some compounds (e.g., B₂H₆)
    • Aluminum: +3
    • Gallium: +3
    • Indium: +3
    • Thallium: +1, +3
  • Examples can be given to illustrate the oxidation states in different compounds

Slide 26

  • Oxidation states of Group 14 elements:
    • Carbon: +4, -4 in some compounds (e.g., CH₄)
    • Silicon: +4
    • Germanium: +4
    • Tin: +4, +2 in some compounds (e.g., SnCl₂)
    • Lead: +4, +2 in some compounds (e.g., PbCl₂)
  • Examples can be given to illustrate the oxidation states in different compounds

Slide 27

  • Allotropes of carbon:
    • Diamond: Consists of carbon atoms arranged in a tetrahedral network, extremely hard
    • Graphite: Consists of carbon atoms arranged in layered sheets, conducts electricity, lubricant
    • Fullerene: Consists of carbon atoms arranged in closed-cage structures, used in nanotechnology
    • Carbon nanotubes: Cylindrical structures of carbon atoms, used in electronics and materials science

Slide 28

  • Peculiar properties of carbon:
    • Catenation: Ability to form strong covalent bonds with other carbon atoms, giving rise to a variety of compounds
    • Isomerism: Ability to form isomers, compounds with same molecular formula but different structures
    • Organic chemistry: The branch of chemistry that deals with compounds containing carbon
    • Carbon-based life: The basis for all known life on Earth, due to its unique bonding properties

Slide 29

  • Important compounds in the carbon cycle:
    • Carbon dioxide (CO₂): Produced during respiration and combustion, used in photosynthesis by plants
    • Methane (CH₄): Produced during natural gas formation and decomposition of organic matter
    • Carbonates (e.g., CaCO₃): Found in rocks, shells, and coral reefs
    • Carbonic acid (H₂CO₃): Formed when CO₂ dissolves in water, important in maintaining acid-base balance in oceans

Slide 30

  • Summary of key points covered:
    • Group 13 and 14 elements have distinct physical and chemical properties
    • Naming compounds using systematic rules
    • Common applications of these elements in various industries
    • Oxidation states and allotropes of carbon
    • Carbon cycle and its importance in the environment End of Lecture.