Covalent, ionic and metallic bonding - 4.1

non-metal and non-metal

strong electrostatic attraction between a pair of shared electrons and positive nuclei

Low boiling point - weak intermolecular forces require little energy to break Electrical insulator - no charged electron particles free to move

Has more electrons –> has stronger intermolecular forces

metal + non-metal

strong electrostatic attraction between positive and negative ions

giant ionic lattice

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

non-metals

attraction between shared electrons and positive nuclei

giant lattice diamond - each C bonded to 4 others graphite - each C bonded to 3 others silicon dioxide - no intermolecular forces

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

metal + metal

attraction between delocalised electrons and positive metal ions

giant metallic lattice, rows of positive ions and localised electrons

conductor - delocalised electrons can move and carry charge malleable - the layers of positive metal ions can slide over each other

alloys - makes it stronger –> extra element which is a different size so it can disrupt the rows so that they can slide over each other

drill bit