Taylor’s Notes Structures Summary Page
Giant Metallic Structures Bonds
Metals and alloys conduct electricity and heat because the delocalised electrons are free to move through the lattice structure
Metals are malleable because the layers of ions can slide over each other
Alloys are hard because there are different-sized atoms of the mixed metals make the atomic layers less regular, so they cannot
slide as easily
Metals have high melting and boiling points because there are many electrostatic attractions which have to be broken which
takes lots of energy
Giant Ionic Lattice Bonds
Ionic substances have high melting/ boiling points because there are lots of strong electrostatic attractions between oppositely
charged ions They increase with increasing charge on ions Stronger attraction between 2+ and 2- than 1+ and 1-
Ionic substances conduct electricity when molten or when dissolved in water because the ions separate and are free to move
Ionic substances do not conduct electricity when in solid state because the ions cannot move
Simple Molecular Substances Forces of Attraction
Simple molecular substances have low melting points because they have weak intermolecular forces of attraction between
molecules which are easily overcome Do have covalent bonds but are very strong and not broken
Simple molecular substances do not conduct because they do not have any free electrons or an overall charge
The bigger the simple molecular structure the higher the melting and boiling point as there are more intermolecular forces that
needs to be overcome
Giant Covalent
Diamond and silica have very high melting points because there are many strong covalent bonds which have to be overcome
Diamond and silica do not conduct electricity as there are no delocalised electrons and they are usually insoluble
Graphite does conduct electricity as there are delocalised electrons between layers which are free to move
Graphite is soft because the layers can slide over each other as there are weak intermolecular forces
Diamond and silica are hard because there are lots of strong covalent bonds
Simple Molecular Low melting/ boiling point and does not conduct
Giant Ionic Lattice High melting/ boiling point and conduct only
when in solution or molten
Diamond/ Silica High melting/ boiling point but does not conduct
Simple Molecular Low melting/ boiling point and does not conduct
Giant Metallic Structure High melting/ boiling point and conducts
Giant Ionic Lattice High melting/ boiling point but only conducts
when molten or in solution
Giant Metallic Structures Bonds
Metals and alloys conduct electricity and heat because the delocalised electrons are free to move through the lattice structure
Metals are malleable because the layers of ions can slide over each other
Alloys are hard because there are different-sized atoms of the mixed metals make the atomic layers less regular, so they cannot
slide as easily
Metals have high melting and boiling points because there are many electrostatic attractions which have to be broken which
takes lots of energy
Giant Ionic Lattice Bonds
Ionic substances have high melting/ boiling points because there are lots of strong electrostatic attractions between oppositely
charged ions They increase with increasing charge on ions Stronger attraction between 2+ and 2- than 1+ and 1-
Ionic substances conduct electricity when molten or when dissolved in water because the ions separate and are free to move
Ionic substances do not conduct electricity when in solid state because the ions cannot move
Simple Molecular Substances Forces of Attraction
Simple molecular substances have low melting points because they have weak intermolecular forces of attraction between
molecules which are easily overcome Do have covalent bonds but are very strong and not broken
Simple molecular substances do not conduct because they do not have any free electrons or an overall charge
The bigger the simple molecular structure the higher the melting and boiling point as there are more intermolecular forces that
needs to be overcome
Giant Covalent
Diamond and silica have very high melting points because there are many strong covalent bonds which have to be overcome
Diamond and silica do not conduct electricity as there are no delocalised electrons and they are usually insoluble
Graphite does conduct electricity as there are delocalised electrons between layers which are free to move
Graphite is soft because the layers can slide over each other as there are weak intermolecular forces
Diamond and silica are hard because there are lots of strong covalent bonds
Simple Molecular Low melting/ boiling point and does not conduct
Giant Ionic Lattice High melting/ boiling point and conduct only
when in solution or molten
Diamond/ Silica High melting/ boiling point but does not conduct
Simple Molecular Low melting/ boiling point and does not conduct
Giant Metallic Structure High melting/ boiling point and conducts
Giant Ionic Lattice High melting/ boiling point but only conducts
when molten or in solution
