8.2 Covalent Bonding

• Unshared pairs

  • Lone pairs
  • Non-bonding pairs
• Unshared pairs


  Electron pairs that are not involved in bonding
• Electron dot structures of ammonia molecule (NH3)<b>H - N : H<br>H - : N : H<br>H - H</b>
• Octet rule in covalent bonds

  The tendency of atoms to gain stability by having 8 electrons in their outermost shell
• Halogens


  Elements in Group 17 of the periodic table
• Single covalent bonds


  The sharing of one pair of electrons between two atoms
• Halogens

  • Fluorine
  • Chlorine
  • Bromine
  • Iodine
• Electron dot structures of methane molecule (CH4)<b>H - C : H<br>H - C : H<br>H - C : H<br>H - C - H</b>
• Halogen single bonds

  • F2
  • Cl2
  • Br2
  • I2
• Covalent bonding


  A type of chemical bond where two atoms share electrons in order to gain stability
• Electron dot structures of water molecule (H2O)<b>H : H<br>H : : O : H</b>
• Electron dot structures


  Diagrams that represent the bonding between atoms using dots to show valence electrons
• Triple covalent bond example

  • Nitrogen (N₂)
• Coordinate covalent bonds


  One atom contributes both of the shared electrons in a covalent bond
• Double covalent bonds

  • W
  • B
  • I
  • N
  • C
  • H
  • O
  • F
• One atom contributes both of the shared e-

  One atom contributes both of the shared electrons in a covalent bond
• Double covalent bond example

  • Carbon dioxide (CO₂)
• Triple covalent bonds

  Sharing 6 electrons (or three pairs)
• Double covalent bonds

  Sharing 4 electrons (or two pairs)
• Triple covalent bonds

  • O
  • N
  • E
  • N
• Molecule with a double bond

  • Carbon monoxide
• Coordinate covalent bond example

  • Carbon monoxide