Does SiO2 lattice structure contain any intermolecular attraction forces?

Question

I was told by my teacher that SiO₂ lattice does not contain any intermolecular attraction forces. But if so, how is the lattice kept as it is? And is there any method to exactly know whether a lattice contains intermolecular forces? I do know that graphite has them, then why doesn't SiO₂?

Answer 1

          Silicates do have intermolecular forces but they are on a network level forming a framework of bonds.

Quartz, as a mineral, has a crystal lattice structure which can be mechanically deformed by an outside applied force. Other than this, the only intermolecular attraction force is that which exists as a result of the stable various network/framework of polymorphs which quartz has that makes it up. The edges of these molecular networks are made of closest packed configurations in the family of the Silicates (SiO₄) which has multiple subclasses (Quartz is the subclass of silicates called tectosilicates which is comprised of silicates where the ratio between oxygen and silicon is 2:1.)

          Graphite, on the other hand,  is an allotrope of carbon and therefore different altogether in its lattice structure. It is actually unique in its structure because it is formed like diamonds are formed as a result of extremely high temperatures and pressures in the earth's crust which essentially cause the carbon parts to group together as a result of these outer forces. This causes levels of carbon uniformity in graphite to be extremely uniform and "pure" in structure making the intermolecular structure the strongest and hardest known of all substances. It is actually much different than those of silicates in this sense.

           In a nutshell, silicates are strong due to their geometric, symmetric nature, but graphite is even stronger due to its uniformity and purity.