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When silicon dioxide changes state, are the covalent bonds being broken (ie. the intramolecular forces) or is it the intermolecular forces?

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    $\begingroup$ Intermolecular forces don't break $\endgroup$ Aug 22, 2016 at 9:42
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    $\begingroup$ The very words "intermolecular" and "intramolecular" don't quite apply to $\ce{SiO2}$. They imply it is made of molecules, which is not so. $\endgroup$ Aug 22, 2016 at 10:08

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$\ce{SiO_2}$ is a network covalent compound that has an extremely high melting and boiling point, because many silicon-oxygen bonds have to be broken in order for it to achieve the necessary freedom. To clarify, SiO2, which has a tetrahedra network lattice formation, shows that each silicon is actually bonded to 4 oxygens; each oxygen is bonded to 2 silicon. These excess bonds aside from the ones of SiO2 are broken.

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