Chemical Bonding

Overview

• Three main types of chemical bonding:
  1. Ionic Bonding
  2. Covalent Bonding
  3. Metallic Bonding

Ionic Bonding

• Occurs between metal and non-metal atoms.
• Example: Sodium (Na) and Chlorine (Cl)
  • Sodium: 1 electron in outer shell (loses this electron)
  • Chlorine: 7 electrons in outer shell (gains one electron)
• Metal atoms (1-3 electrons) and Non-metal atoms (4-8 electrons) aim for full outer shells.
• Process:
  • Metal atom gives up electron, non-metal atom gains electron.
  • Sodium becomes a positive ion, and Chlorine becomes a negative ion.
  • Bonding:
    • Attraction between oppositely charged ions forms the ionic bond.
    • Forms a giant lattice structure.
• Properties of Ionic Compounds:
  • High melting points due to strong ionic bonds in lattice structure.

Covalent Bonding

• Occurs between non-metal atoms.
• Example: Water (H₂O)
  • Oxygen: 6 electrons in outer shell (needs 8)
  • Hydrogen: 1 electron in outer shell (needs 2)
• Process:
  • Atoms share electrons to achieve full outer shells.
  • Oxygen shares one pair of electrons with each hydrogen atom.
  • Bonding:
    • Attraction between shared pairs of electrons (negative) and positive nuclei forms the covalent bond.
• Types of Covalent Compounds:
  • Simple Covalent Compounds (e.g., water):
    • Low boiling points due to weak intermolecular forces despite strong covalent bonds.
  • Giant Covalent Compounds (e.g., diamond):
    • High melting points.

Metallic Bonding

• Occurs between metal atoms (e.g., Iron).
• Metal atoms share electrons in a delocalized "sea of electrons."
• Bonding:
  • Positive nuclei are held together by the sea of delocalized electrons.
  • Acts like a strong glue creating very strong bonds.
• Properties of Metals:
  • Generally high melting points due to strong metallic bonding.

Conclusion

• Understanding these bonding types explains the properties of different substances.
• For more detailed information on covalent compounds, refer to the next video.