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