Bonding

Bonding

 

Metal + Electrons = Metallic Bonding
Metal + Non-Metal = Ionic Bonding
Non-Metal + Non-Metal = Covalent Bonding

 

Metallic Bonding:

 

  • Metallic Bond is the attraction between the metal ions and the delocalised electrons
  • Too many atoms to count, unlike small molecules like H2O
  • Number of delocalised electrons = number of electrons in out shell of element
  • Metals conduct electricity because the electrons can move
  • Metals are easily shaped (malleable) because cat-ions are in compact layers and can move

Metallic Lattice – the regular arrangement in metal ions in solid metals

 

Ionic Bonding:

 

  • Ionic Bond is the electrostatic attraction between positive and negative ions
  • Only show valence electrons in
  • Show transfer of electrons with arrow
  • Write the correct formula
  • Both atoms should end up with full valence shells

Polyatomic ions – ions containing more than one atom. Brackets must be used to write formulae involving more than one of these ions. E.g. Al2(SO4)3; SO4 is a polyatomic ion

Covalent Bonding

  • Covalent bond is the sharing between atoms to gain full valence shells
  • Only show valence electrons on diagrams
  • No arrows
  • Atoms will be connected