Why are diamonds and graphite so different if they are made of the same element carbon?

Both diamond and graphite are made entirely out of carbon, as is the more recently discovered buckminsterfullerene (a discrete soccer-ball-shaped molecule containing carbon 60 atoms). The way the carbon atoms are arranged in space, however, is different for the three materials, making them allotropes of carbon.

Why are diamonds and graphite so different if they are both made up of only carbon?

Both have Giant Covalent Structures, resulting in very high melting temperatures. However each carbon atom in Diamond has 4 covalent bonds with other Carbons, making it extremely strong and hard. On the other hand, each carbon in graphite is bonded to three carbons, and therefore graphite is formed in layers.

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Why are carbon and diamonds different?

The key difference between carbon and diamond is that carbon is a chemical element whereas diamond is an allotrope of carbon. … These structures contain only carbon as the chemical element but the spatial arrangement of the carbon atoms is different from each other. Diamond is also a type of allotrope.

What about the atoms makes graphite and diamond different?

In diamond, the carbon atoms have solid bonds in three measurements, makings it hard. In graphite the bonds create in level layers with carbon atoms having solid bonds on the very same layer with weaker layers above as well as below that makes this graphite weak.

What is the reason for the difference in properties between diamond and graphite?

The difference between the properties of diamond and graphite are the following : 1. Diamonds are formed due to covalent bonds which forms a strong three-dimensional network whereas graphite are formed due Van der Waal force which is weak. Thus, Graphite are formed of flat carbon atoms layers one upon other.

Why is diamond hard and graphite not note that diamond and graphite are both composed of carbon atoms?

While there are strong covalent bonds between carbon atoms in each layer, there are only weak forces between layers. This allows layers of carbon to slide over each other in graphite. … In this rigid network atoms cannot move. This explains why diamonds are so hard and have such a high melting point.

How are diamonds and graphite the same How are they different quizlet?

How are diamonds and graphite the same? How are they different? Both diamonds and graphite are made entirely out of carbon. They are different because the carbon atoms are arranged differently with a more three-dimensional structure in diamonds and flat layers in graphite.

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What is the main difference between diamond and graphite?

Although there are many differences between these two substances, the main difference between diamond and graphite is that diamond is made out of sp3 hybridized carbon atoms whereas graphite is made out of sp2 hybridized carbon atoms.

How are carbon and diamond similar and different?

Carbon. Both graphite and diamonds are made out of pure carbon. The chemical composition of the two is exactly the same. … The difference lies in how all the carbon atoms align and connect to one another.

How do diamond and graphite differ in their structures Is there any effect of structures on the nature of these?

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.

Why is graphite an electrical conductor but diamond is not?

Graphite can conduct electricity because of the delocalised (free) electrons in its structure. These arise because each carbon atom is only bonded to 3 other carbon atoms. … However, in diamond, all 4 outer electrons on each carbon atom are used in covalent bonding, so there are no delocalised electrons.

Why is diamond hard and graphite is not?

However, diamond is harder than graphite because of the carbon atoms in a diamond form 4 covalent bonds in the form of tetrahedral structure. While the carbon atoms in the graphite form 4 covalent bonds in the form of hexagonal structure. … This is the reason why diamond is harder than graphite.

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How does diamond and graphite differ in terms of electrical conductivity and hardness?

Graphite, for example, has a melting point of more than 3,600°C. Variable electrical conductivity – diamond does not conduct electricity, whereas graphite contains free electrons so it does conduct electricity. Silicon is a semi-conductor – it is midway between non-conductive and conductive.