Ionic Bonding- between metals and non metals - transfer of electrons - 2 charged particles produced - attraction via electrostatic forces on the compound
always exist as a lattice of alternating charged particles
solid at room temp - giant structures - conduct electricity when molten or dissolved
brittle and shatter easily due to the alternatingly charged ions
Mettalic Bonding- between metals- sea of delocalised electrons so able to carry charge
greater charge = stronger metal
smaller ion = stronger metal
malleable(beaten into shape) and ductile (pulled into wires)
high melting points
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