Lecture on Properties of Metals, Non-Metals, and Transition Metals

Metals

• Location in Periodic Table: Bottom left
• Ion Formation: Form positive ions (e.g., Ca^2+)
• Electron Arrangement: Few outer electrons, easy to lose
  • Example: Calcium (group 2) with 2 outer electrons can easily form a positive ion
• Reactivity: Increases towards the bottom
  • Example: Lead (Pb) with 6 shells has outer electrons far from nucleus, thus easily lost
• Physical Properties:
  • Metallic Bonding: Strong bonds
  • Malleability: Can be hammered or bent into shapes
  • Conductivity: Good conductors of heat and electricity
  • High Melting/Boiling Points: Some metals have melting points over 2000°C
  • Appearance and Sound: Shiny and sonorous (ringing sound when hit)

Non-Metals

• Ion Formation: Often form negative ions (e.g., Cl^-) or no ions (e.g., carbon)
• Electron Arrangement: More outer electrons, hard to lose them (high energy required)
  • Example: Chlorine (group 7) with 7 outer electrons
• Physical Properties:
  • Appearance: Dull in color
  • Brittleness: Easily breakable
  • Low Melting/Boiling Points: Many are gaseous at room temperature
  • Conductivity: Poor conductors of electricity
  • Density: Generally lower than metals

Transition Metals

• Location in Periodic Table: Center (marked in green)
• Ion Formation: Can form multiple ions (e.g., Chromium can form Cr^2+, Cr^3+, Cr^6+)
  • Ions often colored (e.g., aqueous forms: blue, green, orange)
• Physical Properties: Same as typical metals
• Catalytic Properties: Excellent catalysts
  • Definition: Substances increasing the rate of chemical reactions without being used up
  • Examples of Use:
    • Iron: Catalyzes Haber process (ammonia production)
    • Nickel: Used in hydrogenation of alkenes (margarine production)

End of Lecture