The answer is simple: "C". Attractions between solvent molecules and carbon atoms will never be strong enough to overcome the strong covalent bonds in graphite. The melting points of both graphite and diamond are very high. Graphite is insoluble in water and organic solvents - for the same reason that diamond is insoluble. To distinguish them, we write: diamond: C(s,diamond) graphite: C(s,graphite) The s stands for solid. conducts electricity. Graphite. Graphite has a giant covalent structure in which: makes diamond useful for cutting tools, such as diamond-tipped glass cutters and oil rig drills. Carbon has an electronic arrangement of 2,4. Similarities Carbon Both graphite and diamonds are made out of pure carbon. In fact, when a diamond is exposed to high heat and ion bombardment, it will begin to convert back to graphite, which is a more stable structure for carbon atoms. The delocalized electrons are free to move throughout the sheets. The chemical composition of the two is exactly the same. Graphite also has a lower density (2.266 grams per cubic centimeter) than diamond. Structure and bonding. Graphite (/ ˈ ɡ r æ f aɪ t /), archaically referred to as plumbago, is a crystalline form of the element carbon with its atoms arranged in a hexagonal structure.It occurs naturally in this form and is the most stable form of carbon under standard conditions.Under high pressures and temperatures it converts to diamond.Graphite is used in pencils and lubricants. A diamond consists of a giant three … The planar structure of graphite allows electrons to move easily within the planes.

The structure of diamond. Graphite, diamond and silica Properties of giant covalent structures . In diamond, each carbon shares electrons with four other carbon atoms - forming four single bonds. The giant covalent structure of diamond. Diamond is one form of carbon; the other is graphite. The melting point of graphite is 4200 degrees Kelvin, and diamond's melting point is 4500 degrees Kelvin.

In the diagram some carbon atoms only seem to be forming two bonds (or even one bond), but that's not really the case. There are other exotic allotropes of carbon (graphenes and fullerenes among them) but they are much less common. Both diamond and graphite are allotropes of carbon. We are only showing a small bit of the whole structure. Very high melting points – this is because a lot of strong covalent bonds must be broken.