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diamond and graphite are held together by extremely strong covalent bonds, which results in high sublimation points
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When graphite is subjected to very high temperature and pressure does it change to a diamond?
Graphite has its own atomic structure of its basic carbon atoms. Subjecting it to very high temperature and pressure would not change its structure. Carbon, when subjected to very high temperature and pressure can be crystallized into diamond structures.
Can diamond turn into graphite?
At very high temperatures and pressures, in an inert atmosphere.Another AnswerDiamonds are formed under extreme high temperatures and ultra-heavy pressures far beneath the surface of the earth from carbon, not from graphite.Both diamond and graphite are allotropes of carbon: the molecules are simply attached in different ways.
Why does graphite conduct electricity whereas diamond does not and they are both allotropes?
Diamond and Graphite have 2 different structures, Diamond has a rigid tetrahedral network whereas Graphite has layers which completely changes the properties of both types of carbon. Basically graphite has free delocalised electrons which means electricity can be conducted, diamond however does not have any delocalised electrons which means it cannot conduct electricity. Both diamond and graphite are made up of strong covalent bonds which means they both have high melting points. Graphite is soft though because the layers which it is made up of slide, this makes it soft. Diamond is made up of carbon atoms close to each other and in a 3 layered cube shape which is a lot more rigid and this makes it 'the hardest substance on earth'. Hope this helps, Obrien9
Why does graphite have a high melting point?
As graphite has a giant lattice structure, it is very hard to break apart. Therefore, high temperatures are required to break these strong bonds to turn it into a liquid state. Thus the melting point of graphite is high, same goes for diamonds.Even though it is a covalently bonded compound, these 2 examples are the only ones that have high melting points.The melting point of graphite is 3500 c and 6332 f, specific gravity is 2.25, pounds per cubic inch is .812,
What is the similaritie between diamond and iodine bond?
diamond n iodine have high melting points as they are both ionic compounds
What is differences and similaretes between Diamond and graohite?
Diamond and graphite are both covalent structures. Diamond has a tetrahedral arrangement of 5 carbon atoms. Graphite has a hexagonal structure with each carbon atom connected to three others. Diamond is very hard, while graphite is soft. They both have high melting and boiling points. Diamond is an insulator since it has no mobile electrons. Graphite is a conductor due to having valence electrons that are not all used in covalent bonding. This allows them to be delocalized across the planes of carbon atoms.
Can diamond convert to graphite and vice versa?
Diamond (and also graphite) is pure carbon, without iron. Heating graphite and subjecting it to intense pressure can make small industrial diamonds.
When graphite is subjected to very high temperature and pressure does it change to a diamond?
Graphite has its own atomic structure of its basic carbon atoms. Subjecting it to very high temperature and pressure would not change its structure. Carbon, when subjected to very high temperature and pressure can be crystallized into diamond structures.
Can diamond turn into graphite?
At very high temperatures and pressures, in an inert atmosphere.Another AnswerDiamonds are formed under extreme high temperatures and ultra-heavy pressures far beneath the surface of the earth from carbon, not from graphite.Both diamond and graphite are allotropes of carbon: the molecules are simply attached in different ways.
Why does graphite conduct electricity whereas diamond does not and they are both allotropes?
Diamond and Graphite have 2 different structures, Diamond has a rigid tetrahedral network whereas Graphite has layers which completely changes the properties of both types of carbon. Basically graphite has free delocalised electrons which means electricity can be conducted, diamond however does not have any delocalised electrons which means it cannot conduct electricity. Both diamond and graphite are made up of strong covalent bonds which means they both have high melting points. Graphite is soft though because the layers which it is made up of slide, this makes it soft. Diamond is made up of carbon atoms close to each other and in a 3 layered cube shape which is a lot more rigid and this makes it 'the hardest substance on earth'. Hope this helps, Obrien9
Why does graphite have a high melting point?
As graphite has a giant lattice structure, it is very hard to break apart. Therefore, high temperatures are required to break these strong bonds to turn it into a liquid state. Thus the melting point of graphite is high, same goes for diamonds.Even though it is a covalently bonded compound, these 2 examples are the only ones that have high melting points.The melting point of graphite is 3500 c and 6332 f, specific gravity is 2.25, pounds per cubic inch is .812,
How temperature affect sublimation?
Sublimation is accelerated at high temperature.
What is the similaritie between diamond and iodine bond?
diamond n iodine have high melting points as they are both ionic compounds
What is the graphite?
a form of the element carbon (just like diamond is pure carbon). Graphite is used (with clays) in the lead of pencils, as a lubricant, for crucibles (vessels to hold high temperature molten metals), and a host of other things..
What type of carbon is a diamond?
Diamond is carbon, but the atoms are linked in a rigid, three- dimensional lattice, with 4 covalent bonds at each atom. Since there are no free electrons, diamond is a non- conducter. Graphite is only a two dimensional lattice, with a free electron called the pi- electron, which allows it to conduct electricity. The fact that the atoms are joined in sheets which freely slide over each other makes it a good lubricant.simply diamond is crytalline form of carbon.
What is the difference between Diamonds and graphite?
Diamond and graphite are both pure carbon but graphite's atoms attach to three other carbon atoms and are connected in plates that are parallel to eachother. Diamond's atoms attach to four other carbon atoms in a crystal form, and graphite is a lot softer than diamond.
How many allotropic forms of carbon?
There are two Allotropic Forms of Carbon. They are the following: Diamond & Graphite. Diamond: The Diamond is hardest knwon substance (or Natural Substance). It is in Crystalline state. It's density is 3.51 gram per cubic centimeter. It's Melting Point is 3500 centigrade. It has high refractive index i-e: 2.45. It is a bad conductor of electricity. Pure Diamond is transparent to X-rays that's why we use X-rays to distinguish between real diamond & imitation diamond. It's structure is Tetrahedral structure.
