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normally simple covalent bonded compounds have low melting point. Silicon oxide has high cuz it has a huge covalent bonding structure, with a lot of covalent bonds, which makes it stronger than normal covalent compoundsmy book says, "Silicon oxide melts only at high temperatures. This is because the silicon and oxygen are held tightly together by strong covalent bonds in the network" is this correct? i thought melting point is related to van der waal's forces
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