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Giant ionic lattice: electrostatic forces of attraction between oppositely charged ions
High melting point
Soluble: water’s dipole attracts +/- ions – breaks lattice
Can’t conduct when solid – ions can’t move
Conduct in solution/molten – ions free to move
Giant metallic lattice: electrostatic forces of attraction between cations & delocalised electrons
High melting point: more delocalised electrons = stronger bonding = higher
Insoluble – strength of metallic bonds
Conduct electricity: delocalised electrons can move & carry current
Thermal conductivity: delocalised electrons can pass KE to each other
Simple Molecular: covalently-bonded molecules – held together by intermolecular forces
Low melting point – weak intermolecular forces
Solubility depends on polarity of molecule
Don’t conduct – no charged particles (& electrons in fixed position when solid)
Iodine I2
Regular arrangement of molecules – held together by weak VDW (= low melting point)
Large number of electrons – strong enough VDW to hold molecules together as solid crystal
Macromolecular (giant covalent structure)
High melting point – strong covalent bonds
Insoluble – covalent bonds too strong to break
Diamond – hardest known substance: used in diamond-tipped drills
Tetrahedral – each C form 4 bonds (max)
Good thermal conductivity: vibrations travel easily
Don’t conduct electricity: outer electrons held in localised bonds – not delocalised
Graphite: sheets of hexagons of graphene
Trigonal planar – each C forms 3 bonds + delocalised electron
Lubricant: weak forces between layers – sheets slide over eachother
Low density – large distance between layers
Conduct electricity: free delocalised electrons between layers
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