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Diamonds are very hard, and graphite is very soft.
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What is a good conductor of heat and electricity anthracite charcoal diamond graphite?
Graphite is a good conductor of heat and electricity, while anthracite, charcoal, and diamond are poor conductors.
Found in these forms charcoal graphite diamond?
If YOU write in this area, your question goes to the "already answered" bucket- Besides its use as jewelry, Diamond is used where anything incredibly hard is needed. Diamond (dust) is used to make saw blades and drill bits that can cut through just about anything. Graphite, while also composed of carbon, has an entirely different crystal structure, and different uses. Graphite is used as an electrical contactor (a brush) in electrical motors. It makes a great dry lubricant for things like locks, and when mixed with clay, forms the "lead" for ordinary pencils.
What are the key differences between the diamond structure and graphite, and how do these variances impact their properties and applications?
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.
What are examples of pure carbon?
I know diamond is, as long as it's clear and doesn't have color tint. I think coal and graphite, the stuff in pencils, is.
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.
Similarities between Graphite and Fullerenes?
difference between diamond graphite and fullrene
What element is used in charcoal graphite and diamond?
Carbon
What is a good conductor of heat and electricity anthracite charcoal diamond graphite?
Graphite is a good conductor of heat and electricity, while anthracite, charcoal, and diamond are poor conductors.
What is the name for bits of unburnt carbon?
charcoal graphite diamond
What is the difference between diamond and grapite?
There is none, diamond has about 60 bonds of graphite inside of it.
Which is more dense diamond or charcoal?
Diamond , nearly twice that of graphite. (charcoal is not a fair comparison it is a porous partially combusted wood product composed mainly of graphite but there are many impurities.)
What is a solid element used in diamonds and graphite?
carbon is in both diamond and graphite along with countless other things like charcoal
What is the structural difference between a diamond and graphite?
The structural difference between diamond and graphite is in their arrangement of carbon atoms. Diamond has a three-dimensional network structure where each carbon atom is bonded to four other carbon atoms in a tetrahedral arrangement. In contrast, graphite consists of layers of carbon atoms arranged in hexagonal rings with each carbon atom bonded to three others in the same plane, allowing for easy slippage between the layers.
Can carbon bond with other carbons?
Yes, it can bond with other cabons . For example, a diamond, graphite (in pencils) and charcoal.
Give examples of pure carbon?
Diamond, graphite, and charcoal are examples of pure carbon. Diamond is a crystalline form of carbon, graphite is composed of layers of carbon atoms, and charcoal is produced by heating organic materials in the absence of oxygen.
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.
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.
