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why are metals good conductors of electricity
-the delocalised sea of electrons (valence electrons) are mobile, so can move freely throughout the metallic lattice -these mobile electrons can carry a charge throughout the structure, and the mobile sea of e- move toward the positive terminal of power supply while the positive metal ions remain stationary in their fixed positions
why are metals good conductors of heat
-e- within sea of e- are mobile and so can carry heat energy (as kinetic energy) throughout metal lattice -the vibration of metallic ions also contributes to the flow of heat through the metal lattice
why are metals malleable and ductile
bonding btwn metal ions and sea of e- is non-directional -individual metal cations can move in relation to each other without breaking the bonds between them and the sea of electrons -allowing metal to change shape
why are metals solid at room temperature
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why are ionic solids poor conductors of electricity in the solid phase
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why are ionic compounds good conductors of electricity when molten/(aq)
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why are ionic compounds hard and brittle
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why do ionic compounds have high melting and boiling points
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why are covalent molecular substances non-conductors of electricity in either solid, liquid or aqueous phase
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why are covalent molecular substances soft and weak
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why are covalent network substances non-conductors of heat or electricity
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