Malleable (can be hammered into sheets) 10. In diamond each carbon atom is linked to four other carbon atoms by covalent bonds. That comes at an expense of energy. (c) its density ranges from 1.9 to 2.3 g/cm 3. Ductile (can be drawn into wires) ... Why does graphite have very high melting/boiling points? In graphite, each carbon atom is linked to three other carbon atoms by covalent bonds. Graphite is used as a lubricant in machines because (a) it is a good conductor of electricity. The boiling point of graphite is 4,200 degrees Celsius. Experimental Boiling Point: 500-600 °C (Sublimes) Alfa Aesar 42008, 42007, 39722: Experimental LogP: 13.44 LabNetwork LN01740556: Experimental Flash Point: 94 °C Biosynth W-204191: Experimental Density: 94 g/mL Biosynth W-204191: Predicted Physico-chemical Properties. In order to melt graphite, it isn't enough to loosen one sheet from another. Melting Point (Celcius) Graphite: 3652 - 3697 (sublimes) Diamond: 3550. Graphite. The layers are free to slide over each other because there are no covalent bonds between the layers and so graphite is soft and slippery. Its melting point, on the other hand, is between 3,652 up to 3,697 degrees Celsius. In this case, since the constituent molecules of graphite are held together by a strong covalent force, a high amount of energy is needed to weaken that bond. Answer: (b) it has a high melting point … On the phase diagram, label the graphite phase. (c) If graphite at normal conditions is heated to 2500 K while the pressure is increased to 1010 Pa, it is converted into diamond. (b) it has a high melting point and slippery layers. Boiling Point (Celcius) Graphite:4200. Each carbon atom has sp 3 hybridisation with bond angles of 109.5º (HL only). Strong covalent bonds that require a lot of heat energy to break. High melting point 6. Properties of graphite: Soft The weak Van der Waal’s forces of attraction between the layers are easily overcome and this enables the layers to slide over one another. That explains graphite's high melting point. It has high melting and boiling points and is the hardest naturally occurring substance. You have to break the covalent bonding throughout the whole structure. High melting and boiling point A lot of energy is required to break the numerous strong covalent bonds between the carbon atoms; Conducts electricity A lot of energy is needed to overcome the strong covalent bonds between the carbon atoms. It has a soft, slippery feel, and is used in pencils and as a dry lubricant for things like locks. High boiling point 7. top. Graphite is another naturally occurring allotrope of carbon. Thus, it has high melting and boiling points. (d) it is strong and soft. In graphite, each carbon atom forms three covalent bonds with three other carbon atoms, forming layers of hexagonal rings and so graphite has a high melting point. Graphite has a high melting point, similar to that of diamond. Good conductor of electricity 9. Answer. Graphite: Though little energy is needed to overcome the weak inter-molecular forces between the layers, a lot of energy is still needed to overcome the strong covalent bonds between the carbon atoms. Label the diamond phase. (d) Circle each triple point on the phase diagram. Diamond:4827 So it seems paradoxical that diamond would have a lower melting point. Now melting is essentially turning a highly ordered state of molecules to a disorderly one. Good conductor of heat 8. (b) Graphite is the most stable phase of carbon at normal conditions. 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