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.