Question

1. Difference in structures of diamond and graphite. Explain how this relates their properties. ​

Answer 1

Answer:

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. Thus, graphite's use as a lubricant. The 4th electron isn't involved in bonding and thus is free to move in between layers and is able to carry electricity. Hence, graphite is a weak conductor of electricity.  3. Diamond has stronger intramolecular bonds than graphite. As a result more energy is required to overcome the bonds existing in diamond. Therefore, diamond has a higher boiling point. Also, diamond is used for drilling, cutting, etc which is indicative of it's strength.

Explanation:

Plz mark as brainliest

Answer 2

Here are the key differences in their structures:

• Diamond forms a crystalline lattice whereas graphite has a layers structure.
• In diamond each carbon atom is sp3 hybridised(bonded with four other carbons through a sigma bond) whereas in graphite the carbon atoms are sp2 hybridised(bonded with three other carbon atoms via sigma bond).
• Diamond is made of tetrahedral units whereas graphite has a planar geometry.
• The C-C bond length is 154pm in diamond and that of graphite is 141.5 pm.
• Diamond is difficult to brake(rather the strongest substance) whereas graphite us brittle.

Properties related to structures are:

• Diamond is a bad conductor whereas graphite is a good conductor of electricity: This diffence is due to their structures. As already mentioned above, one carbon atom of diamond is bonded with four other carbon atoms, this means that there is no presence of free electrons, hence it cannot conduct electricity. In graphite, each carbon atom is bonded to three other carbon atoms, this means every carbon has one free electron(presence of free electrons) and hence it can conduct electricity.
• Diamond is hard whereas graphite is brittle: This difference is due to the arrangement of atoms in their structures. Diamond makes a crystalline lattice, which has a rigid covalent bond network, that makes it hard to break. Whereas in graphite, the carbon atoms are present in different layers which are held together by van der waals forces. And these layers can be separated easily. That is why graphite is easy to break.

I hope it is very much clear now....

In case of any query please feel free to contact me.

:)