graphite has hexagonal crystals and diamond tetrahedron
A diamond and a pencil lead (graphite) are both made of carbon. The difference is the crystalline structure of the carbon atoms.
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.
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
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
Diamond and graphite are polymorphic because they are composed of pure carbon atoms arranged in different crystal structures. In diamond, carbon atoms are arranged in a three-dimensional network of tetrahedral shapes, resulting in a hard and transparent structure. In graphite, carbon atoms are arranged in layered sheets that are weakly bonded between layers, giving graphite its lubricating properties and ability to conduct electricity.
difference between diamond graphite and fullrene
There is none, diamond has about 60 bonds of graphite inside of it.
yes
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.
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.
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
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 lead (graphite) are both made of carbon. The difference is the crystalline structure of the carbon atoms.
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.
Diamonds are very hard, and graphite is very soft.
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.
The key differences between diamond and graphite lie in their atomic structure and bonding. Diamond has a three-dimensional network of carbon atoms bonded together in a tetrahedral arrangement, making it extremely hard and durable. Graphite, on the other hand, consists of layers of carbon atoms arranged in a hexagonal lattice, allowing for easy sliding between layers. This difference in structure results in diamond being hard and transparent, while graphite is soft and opaque. These variances impact their properties and applications, with diamond being used in cutting tools and jewelry due to its hardness, and graphite being used as a lubricant and in pencils due to its slippery nature.