Bonding
Elements Bonding Structure Examples
Metals Metallic Metallic lattice Na, Cu, Mg, Al
Semi-Metals -- - Si, Ge
Non-Metals
Monoatomic No bonding when Simple covalent He, Ne, Ar, Kr, Xe
gaseous
Covalent Giant Covalent Giant Covalent C (diamond)
(graphite)
Covalent Molecular Covalent Simple covalent NH3, H20, HCL, CO2
Metals
Metallic bonding: Attraction between layers of positive ions and delocalised electrons
Delocalised Electrons: Outer electrons that don’t have fixed positions and move freely
Hardness Strong electrostatic attraction between positive
ions and negative electrons, and a regular
structure
High MP Large amount of energy is required to break the
bonds, which are strong attractions between
positive ions and negative electrons
Good electrical conductivity Delocalised electrons can move and carry
charge
Malleability and ductility Layers of positive ions can slide over each other
without interrupting the bonding
Metallic bond is stronger when there are more delocalised electrons
Ionic Compounds (metal and non-metal)
Ionic bonding: Electrostatic attraction between oppositely charged ions in a regular ionic lattice
Crystalline Regular lattice of positive and negative ions.
Regular arrangement creates crystal structure
High MP Large amount of energy is required to break the
bonds which are strong electrostatic attractions
between ions of opposite charge
Non-conductor when solid Ions are not free to move and cannot carry
charge
Conductor when molten or aqueous Ions are free to move and can carry charge
The smaller the ions and the higher their charge, the stronger the ionic bond.
Covalent Bonding (usually between non-metals, some exceptions e.g. BeCL2)
Covalent Bond: Electrostatic attraction between a shared pair of electrons and the nuclei of bonded
atoms
Octet Rule: Atoms tend to gain, share or lose electrons when bonding in order to achieve 8 in their
outer shell
Elements Bonding Structure Examples
Metals Metallic Metallic lattice Na, Cu, Mg, Al
Semi-Metals -- - Si, Ge
Non-Metals
Monoatomic No bonding when Simple covalent He, Ne, Ar, Kr, Xe
gaseous
Covalent Giant Covalent Giant Covalent C (diamond)
(graphite)
Covalent Molecular Covalent Simple covalent NH3, H20, HCL, CO2
Metals
Metallic bonding: Attraction between layers of positive ions and delocalised electrons
Delocalised Electrons: Outer electrons that don’t have fixed positions and move freely
Hardness Strong electrostatic attraction between positive
ions and negative electrons, and a regular
structure
High MP Large amount of energy is required to break the
bonds, which are strong attractions between
positive ions and negative electrons
Good electrical conductivity Delocalised electrons can move and carry
charge
Malleability and ductility Layers of positive ions can slide over each other
without interrupting the bonding
Metallic bond is stronger when there are more delocalised electrons
Ionic Compounds (metal and non-metal)
Ionic bonding: Electrostatic attraction between oppositely charged ions in a regular ionic lattice
Crystalline Regular lattice of positive and negative ions.
Regular arrangement creates crystal structure
High MP Large amount of energy is required to break the
bonds which are strong electrostatic attractions
between ions of opposite charge
Non-conductor when solid Ions are not free to move and cannot carry
charge
Conductor when molten or aqueous Ions are free to move and can carry charge
The smaller the ions and the higher their charge, the stronger the ionic bond.
Covalent Bonding (usually between non-metals, some exceptions e.g. BeCL2)
Covalent Bond: Electrostatic attraction between a shared pair of electrons and the nuclei of bonded
atoms
Octet Rule: Atoms tend to gain, share or lose electrons when bonding in order to achieve 8 in their
outer shell
