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The chemical composition of the two is exactly the same. This makes graphite and diamonds allotropes of carbon along with amorphous, which is commonly called soot or carbon black. Allotropes are compounds that have the same chemical makeup but have different structures which results in different properties.
Why does diamond and graphite have the same chemical properties?
It’s because the carbon atoms are rearranged in a specific geometric shape that gives the diamond its properties. Graphite however, is when the carbon atoms bond together in sheets – hexagonal-like lattice. Graphite is formed from the carbon atoms resulting from the metamorphism of minerals such as marble, quartz, etc.
What are the same properties of graphite and diamond?
Explain the difference in properties of diamond and graphite on the basis of their structures. DIAMOND GRAPHITE 1) It has a crystalline structure. 1) It has a layered structure. 2) It is made up of tetrahedral units. 2) It has a planar geometry.
Can a diamond conduct electricity?
Diamond is a form of carbon in which each carbon atom is joined to four other carbon atoms, forming a giant covalent structure. As a result, diamond is very hard and has a high melting point. It does not conduct electricity as there are no delocalised electrons in the structure.
Why is diamond stronger than graphite?
Diamond is harder than graphite because each of its carbon atoms form four covalent bonds in a tetrahedral structure and also due to the presence of strong covalent bonds in it. A chemical bond involving the exchange of electron pairs between atoms is known as a covalent bond.
What are the similarities and differences between graphite and diamond?
Similarities Between Graphite and Diamonds Carbon. Both graphite and diamonds are made out of pure carbon. Covalent Bonds. The bonds that hold the carbon to each other are covalent bonds. High Melting Points. The melting points of both graphite and diamond are very high. Naturally Occuring.
What is the structural difference between graphite and diamond?
Differences 1. Diamond: each carbon atom bonds to 4 other carbon atoms, WHILST, Graphite: each carbon atom bonds to 3 other carbon atoms. Thus, diamond bears more of a tetrahedral structure, whereas graphite takes the form of layers. The presence of layers means that atoms can slide over each other easily.
What is the relationship between graphite and diamond?
In diamond the atoms are arranged in a three dimensional lattice, while in graphite they are joined together in an array of planar six membered rings, arranged in layers. The diamond is very hard while the possible movement of the layers in graphite makes it into an excellent lubricant.
Can acid melt a diamond?
In short, acids do not dissolve diamonds because there simply isn’t an acid corrosive enough to destroy the strong carbon crystal structure of a diamond. Some acids may, however, damage diamonds.
Do Black diamonds conduct electricity?
In case of diamond, each outer shell electron of every carbon atom forms a covalent bond in a tetrahedral arrangement, thus forming a rigid structure which means no free electron for charge transport. This delocalised electron can move move freely between the carbon layers of graphite and conduct electricity.
Why is diamond a bad conductor?
As we know diamond is a giant covalent structure i.e. each carbon atom is covalently bonded with other carbon atoms. So the four outermost electrons, four carbon atoms, are engaged or trapped in the covalent bonds which means that there are no free electrons. So diamond is a bad conductor of electricity.
What is harder than a diamond?
Moissanite, a naturally occurring silicon-carbide, is almost as hard as diamond. It is a rare mineral, discovered by the French chemist Henri Moissan in 1893 while examining rock samples from a meteor crater located in Canyon Diablo, Arizona. Hexagonal boron-nitride is 18% harder than diamond.
Why is a diamond so strong?
The outermost shell of each carbon atom has four electrons. In diamond, these electrons are shared with four other carbon atoms to form very strong chemical bonds resulting in an extremely rigid tetrahedral crystal. It is this simple, tightly-bonded arrangement that makes diamond one of the hardest substances on Earth.
Is graphite stronger than diamonds?
Contrary to common belief, the chemical bonds in graphite are actually stronger than those that make up diamond. While within each layer of graphite the carbon atoms contain very strong bonds, the layers are able to slide across each other, making graphite a softer, more malleable material.
Can we convert graphite into diamond?
It is known that graphite can be converted into diamond when subjected to high pressure and high temperatures. The graphite-diamond transformation can be achieved directly by subjecting graphite to ultra high pressures (> 100 kbar) and temperatures ( > 2000°C).
Why is diamond so hard?
Diamonds are made of carbon so they form as carbon atoms under a high temperature and pressure; they bond together to start growing crystals. That’s why a diamond is such a hard material because you have each carbon atom participating in four of these very strong covalent bonds that form between carbon atoms.
Why is graphite slippery?
Graphite has delocalised electrons, just like metals. The forces between the layers in graphite are weak. This means that the layers can slide over each other. This makes graphite slippery, so it is useful as a lubricant .
Why are diamonds more expensive than graphite?
Diamond is costlier due to the rareness, unique properties and wide varieties of application potentials than graphite. Chemists have figured out that under the right combination of temperature, pressure and time, carbon atoms e.g. from graphite can be converted into diamonds. An expensive process.
Are graphite and diamond isomers?
Definition: Chemical compound that has the same molecular formula – the same number and kinds of atoms – as another compound, but a different structural arrangement of the atoms in space, and, therefore, different properties. For example, graphite (pencil lead) and diamond are isomers of carbon.
Why graphite is less dense than diamond?
Graphite has a lower density than diamond. This is because of the relatively large amount of space that is “wasted” between the sheets. Attractions between solvent molecules and carbon atoms will never be strong enough to overcome the strong covalent bonds in graphite. conducts electricity.
