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Graphite and diamond are different because of their molecular structures. Graphite has layers of carbon atoms arranged in sheets, allowing it to be soft and slippery. Diamond, on the other hand, has a rigid, three-dimensional structure of carbon atoms, making it the hardest natural substance.
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What is the significance of the diamond graphite phase diagram in understanding the structural transformations between these two allotropes of carbon?
The diamond-graphite phase diagram is important because it shows how the structure of carbon can change between diamond and graphite under different conditions like temperature and pressure. This helps us understand the relationship between these two forms of carbon and how they can transform into each other.
Which element makes up a diamond and graphite?
Both diamond and graphite are made up of the element carbon. The difference lies in how the carbon atoms are arranged. In diamond, the carbon atoms are arranged in a rigid, three-dimensional structure, while in graphite, the carbon atoms are arranged in layers that can easily slide past each other.
What are the three forms of the element carbon?
The three forms of the element carbon are diamond, graphite, and fullerenes (such as buckyballs and nanotubes). Each form has distinct properties and structures due to different arrangements of carbon atoms.
Why does diamond have a greater density than graphite?
Diamond has a greater density than graphite because it has a crystal structure where each carbon atom is bonded to four other carbon atoms in a tetrahedral arrangement, making it tightly packed and more dense. In contrast, graphite has a layered structure with weak forces between the layers, resulting in a lower density.
Diamond and graphite are of carbon?
Diamond and graphite are both composed of carbon, but they are physically different from each other. Diamond is the hardest mineral known, is usually transparent and very abrasive. Graphite on the other hand, is soft, opaque and a very good lubricant.
What is found in diamond and graphite?
Carbon. (C)Carbon is present in both diamond and graphite, both contain carbon atoms but they have different structure means carbon atoms are attach with each other in different manner in both diamond n graphite, in graphite three out of four electrons of outer most shell r attached with other electrons of other carbon atoms and one electron is fee that's why graphite is a good conductor of electricity .
Diamond and graphite are both forms of carbon.Diamond is hard Graphite is soft and flaky How could these different properties be explained?
Diamond and graphite have different structures which account for their different properties. Graphite is arranged into sheets which are easily removed. Diamond, on the other hand, is a network solid that has very strong bonds and intermolecular forces holding it together.
Does graphite make diamonds?
No. Graphite and diamond are both allotropes of carbon, each with a different and distinct molecular structure.
How can diamond and graphite be made out of same substance and be so different?
They are so different because of the way the carbon atoms bond to each other. Graphite has layers of very strong bonds, but the layers are very weakly bonded to each other. Diamonds are so strong because all of its carbon atoms are uniformly bonded to one another.
Why is graphite a good lubricant and diamond is an excellent abrasive?
Because graphite forms layers and each layer, each carbon molecule is bonded to three other carbon molecules. The fourth electron to each atom is weakly bonded to the layer next to it. The structure allows the layers to slide past each other, making this element an excellent lubricant.
List in a table the similarities and differences between diamond and graphite including their uses?
Diamond and graphite are allot-ropes of each other. Diamond has a tetrahedral structure where as graphite has an hexagonal arrangement. Both are made of carbon atoms entirely. Diamond is used in jewelry etc. where as graphite is used as in batteries , lubricants etc.
Which is the best reason for the difference between the properties of diamond and graphite?
Graphite and diamonds are both network covalent carbon chains. The only difference is the structure of each. Graphite is very soft and is used as a lubricant, due to the fact that its carbon atoms are bonded together in layers which slide apart easily. Diamond, however, is very abrasive, because its carbons are all bonded to each other in a very rigid fashion.
What is the significance of the diamond graphite phase diagram in understanding the structural transformations between these two allotropes of carbon?
The diamond-graphite phase diagram is important because it shows how the structure of carbon can change between diamond and graphite under different conditions like temperature and pressure. This helps us understand the relationship between these two forms of carbon and how they can transform into each other.
Which element makes up a diamond and graphite?
Both diamond and graphite are made up of the element carbon. The difference lies in how the carbon atoms are arranged. In diamond, the carbon atoms are arranged in a rigid, three-dimensional structure, while in graphite, the carbon atoms are arranged in layers that can easily slide past each other.
What are the three forms of the element carbon?
The three forms of the element carbon are diamond, graphite, and fullerenes (such as buckyballs and nanotubes). Each form has distinct properties and structures due to different arrangements of carbon atoms.
Why is diamond so much harder then graphite?
Diamond is so much harder than graphite because the carbon atoms in diamond are bonded to other carbon atoms tetrahedrally. In graphite, the carbon atoms are only bonded to three other carbon atoms and form sheets. There is one valence electron that wanders the surface which makes graphite a conductor.
Diamond is an insulator while graphite conducts electricity?
Diamond is considered the hardest mineral known to man, while graphite is one of the softest. Diamond is an excellent electrical insulator, while graphite is a good conductor of electricity. This is due to the way the carbon atoms are arranged in each mineral.
