Chemistry bonding

• Ionic bonding involves strong electrostatic forces of attraction (ionic bonds) between oppositely charged ions
• In ionic bonding, when molten ions can move, they carry charge throughout the whole structure in a giant ionic lattice
• Giant ionic lattices contain lots of ions and, therefore, lots of ionic bonds, requiring lots of energy to overcome
• Covalent bonding consists of shared pairs of electrons between atoms
• In covalent bonding between non-metals, weak intermolecular forces between molecules don't require much energy to overcome
• Metallic bonding involves strong electrostatic forces of attraction (metallic bonds) between metal ions and the sea of delocalised electrons
• In metallic bonding, ions are arranged in a regular pattern, all the same size, allowing layers to slide over each other
• In metallic bonding, delocalised electrons are free to move and carry charge throughout the whole structure
• In diamond, there are 4 x strong covalent bonds per C-atom, resulting in lots of bonds and lots of energy needed to overcome them
• In diamond, all electrons within bonds mean there are no free electrons to carry charge throughout the structure
• Metals are malleable because in metallic bonding, layers of ions can slide over each other
• Metallic bonds occur between metal atoms, with delocalized electrons held together by electrostatic forces.
• Covalent bonds form when atoms share pairs of electrons.
• Ionic compounds are formed by the transfer of electrons from one atom to another.