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How do you Propose an explanation for the difference in propertise between diamond and graphite?
The difference in properties between diamond and graphite is primarily due to their distinct atomic structures. In diamond, each carbon atom is tetrahedrally bonded to four other carbon atoms, creating a strong three-dimensional network that results in high hardness and a brilliant luster. In contrast, graphite has a planar structure where each carbon atom is bonded to three others in flat sheets, with weaker van der Waals forces between the layers, allowing them to slide over each other. This structural variation accounts for diamond’s rigidity and brilliance compared to graphite’s softness and conductivity.
A diamond and a pencil are made of what element?
A diamond and a pencil lead (graphite) are both made of carbon. The difference is the crystalline structure of the carbon atoms.
Why diamond and graphite the two allotropic of carbon evolve different amount of heat on combustion?
Diamond and graphite are two allotropes of carbon that exhibit different structures, leading to variations in their combustion heat. Diamond has a rigid crystal lattice, resulting in a higher energy content due to stronger carbon-carbon bonds, while graphite has a layered structure with weaker van der Waals forces between layers. Consequently, when combusted, diamond releases more heat compared to graphite, as it requires more energy to break its stronger bonds during combustion. This structural difference accounts for the variation in the amount of heat each allotrope evolves during the combustion process.
What is the structural difference between diamond and coal?
The difference between graphite and diamond is in the three-dimensionalarrangement of the carbon atoms in the material. Graphite is made of flatsheets of carbon atoms in a hexagonal arrangement. The sheets stack oneover the other, with only weak interactions between sheets. Diamond is notarranged in sheets; instead, each carbon atom is connected to four others ina tetrahedral arrangement. It turns out that this arrangement is not asdifferent from the structure of graphite as it sounds. If the sheets ofgraphite are compressed close enough together, the carbon atoms will be injust about the right position to make the bonds of diamond. In fact, athigh temperatures and pressures, this indeed happens.Richard E. Barrans Jr., Ph.D.Assistant DirectorPG Research Foundation, Darien, Illinoishttp://www.newton.dep.anl.gov/askasci/chem00/chem00349.htm
Differnce between diamond and graphite?
diamonds form a 3 dimensional latice. they also have have four bonds per atom. This makes a very strong material. graphite forms a 2 dimensional latice. it has 3 bonds per atoms (the fourth bond is added to the other three making partial double bonds). it forms sheets. it has excellent 2-d strength: it is what is used in carbon fibers. it also is an excellent lubricant because the sheets slide on one another. fullerenes are like graphite, but the small sheets are wrapped up into small balls or tubes. this gives them 3 d strength on a nano scale. But they lack large scale 3d properties
Similarities between Graphite and Fullerenes?
difference between diamond graphite and fullrene
What is the difference between diamond and grapite?
There is none, diamond has about 60 bonds of graphite inside of it.
Are diamond and graphite different structural forms of carbon?
yes
How do you Propose an explanation for the difference in propertise between diamond and graphite?
The difference in properties between diamond and graphite is primarily due to their distinct atomic structures. In diamond, each carbon atom is tetrahedrally bonded to four other carbon atoms, creating a strong three-dimensional network that results in high hardness and a brilliant luster. In contrast, graphite has a planar structure where each carbon atom is bonded to three others in flat sheets, with weaker van der Waals forces between the layers, allowing them to slide over each other. This structural variation accounts for diamond’s rigidity and brilliance compared to graphite’s softness and conductivity.
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 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 do the structural differences of diamond and graphite suggest?
diamond is the hardest substance known to science at this time, and graphite is a rather weak substance, and they are both made of the same elements. Their only differences are the arrangement of the molecules
What do graphite and charcoal have in common?
Both graphite and diamond are forms of carbon. As such, they are said to be alotropes of carbon. Both occur naturally. Both are mined for industrial purposes, though larger diamonds are sought and used for other things. Both are produced in the earth in geothermal processes. Both can be made artificially. Both are normally solids and highly stable. And they are both difficult to burn, even in an oxygen environment.
A diamond and a pencil are made of what element?
A diamond and a pencil lead (graphite) are both made of carbon. The difference is the crystalline structure of the carbon atoms.
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.
What is the difference between charcoal graphite and diamond?
Diamonds are very hard, and graphite is very soft.
Why diamond and graphite the two allotropic of carbon evolve different amount of heat on combustion?
Diamond and graphite are two allotropes of carbon that exhibit different structures, leading to variations in their combustion heat. Diamond has a rigid crystal lattice, resulting in a higher energy content due to stronger carbon-carbon bonds, while graphite has a layered structure with weaker van der Waals forces between layers. Consequently, when combusted, diamond releases more heat compared to graphite, as it requires more energy to break its stronger bonds during combustion. This structural difference accounts for the variation in the amount of heat each allotrope evolves during the combustion process.
