Covalent, ionic and metallic bonding - 4.1 Flashcards
Simple molecular substances: Types of element
non-metal and non-metal
Covalent Bonding is..
strong electrostatic attraction between a pair of shared electrons and positive nuclei
Simple molecular substances: Properties
Low boiling point - weak intermolecular forces require little energy to break
Electrical insulator - no charged electron particles free to move
Simple molecular substances: special case is fullerene. Why does fullerene have a higher melting point than water?
Has more electrons –> has stronger intermolecular forces
Ionic bonding: Types of element
metal + non-metal
Ionic bonding: Definition
strong electrostatic attraction between positive and negative ions
Ionic bonding: Structure
giant ionic lattice
Ionic bonding: Properties
High MP: because of the strong electrostatic attraction between opposite ions, requires lots of energy to break
Insulator (s): no charged ions are free to move
Conductor (l/aq): charged ions are free to move
Giant covalent substances: Types of element
non-metals
Giant covalent substances: Definition
attraction between shared electrons and positive nuclei
Giant covalent substances: structure
giant lattice
diamond - each C bonded to 4 others
graphite - each C bonded to 3 others
silicon dioxide - no intermolecular forces
Giant covalent substances: properties
Diamond:
High MP - breaking many strong covalent bonds requires a lot of energy
Conductivity - non-conductive, no charged particles that can move
Hardness - hard, lots of strong covalent bonds
Graphite:
High MP - breaking many strong covalent bonds requires a lot of energy
Conductivity - can conduct, each carbon atom has a delocalised electron that can move
Hardness - soft, layers can slide over each other
Metallic bonding: types of element
metal + metal
Metallic bonding: definition
attraction between delocalised electrons and positive metal ions
Metallic bonding: structure
giant metallic lattice, rows of positive ions and localised electrons
