WebDiamond Graphite - In diamond, each C atom is attached to 4 others. The structure is hard because there are strong covalent bonds throughout the structure. Diamond is therefore used for cutting. In graphite, the C atoms are arranged in layers. There are strong covalent bonds within the layers but only weak intermolecular forces between layers. http://molecularrecipes.com/RyTc/why-does-silicon-nitride-have-a-high-melting-point

How does the structure and properties in diamond and graphite …

WebA giant covalent structure is one in which the atoms are joined up by covalent bonds over huge (but variable) numbers of atoms. It is not a molecule, because the number of atoms joined up in a diamond, say, is … WebAnswer: If you define boiling as a physical process where molecules that are held together by intermolecular forces in the liquid phase which are then broken when it transforms to the gas phase, where the same molecules now are far apart from each other and do not experience those intermolecular ... megadeth roblox id

Giant covalent structures - Structures and properties

WebExplanation: SiO2 is a homologue of CO2, a molecular, room temperature gas. No. Silicon has a very high melting point due to its giant covalent structure; a lot of energy is needed to break the strong covalent bonds throughout the structure. Sulfur trioxide is needed to break the covalent bonds in the material strong covalent between. WebDaltile is America's leader in tile. Best known for our award-winning designs and unmatched quality, we invite your to browse our voluminous collection of superior products. WebBoth graphite and diamond exist at ambient temperatures and pressures, and both are composed of carbon atoms only. Yet these two covalently bonded giant structures are … names that end with ah