Compare and contrast the structures of the following solids. a. diamond versus graphite b. silica versus silicates versus glass

Diamond and graphite are both forms of carbon with different atomic arrangements. Diamond has a tetrahedral crystalline structure with strong covalent bonds, resulting in an extremely hard, transparent material with high thermal conductivity and electrical insulating properties. Graphite has a layered hexagonal structure with weaker van der Waals forces, making it softer, opaque, and electrically conductive. Silica, silicates, and glass share silicon-oxygen tetrahedra in their structures. Silica has a crystalline structure, while silicates are minerals with more complex crystal structures containing additional elements. Glass is an amorphous solid with a non-crystalline atomic arrangement, resulting in transparency and low thermal conductivity. These structural differences give rise to distinct physical properties and uses in various applications, such as quartz crystals, ceramics, and optics.