Metallic bonding and comparing ionic, covalent, and metallic substances
In metallic bonding, metal atoms give up their valence electrons into a shared sea of electrons that moves freely around a lattice of positive metal ions. Those mobile electrons explain why metals conduct electricity and heat well, and why metals are malleable and ductile: the ions can slide past each other without breaking the bond. The type of bonding explains a substance's properties. Ionic compounds, like table salt, form rigid crystals with high melting points that are brittle and conduct electricity only when melted or dissolved. Covalent molecular substances, like sugar or wax, are held together by weaker forces between molecules, so they usually have lower melting points and do not conduct electricity.
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