Question

Diamond and graphite are the allotropic forms of the
same element but they differ in their characteristics
How will you account for this ?​

Answer 1

Answer:

All the carbon atoms in Graphite are said to have stable chemical bonds with that of the other three carbon atoms, thus making the sheets that look like chicken wire; the weak form of forces hold the sheet quickly. When you are composing with a pencil on the paper, it is these sheets that slide separately to desert the graphite pieces as a blemish on the Paper whereas

All the carbon atoms of Diamond are said to possess strong chemical bonds with that of the four other carbon atoms, thus making a perfect tetrahedron structure and on throughout the crystal. The carbon atoms, here are sp3 hybridized, and the bond lengths of carbon-carbon atom are equal. Hence Diamond forms a three-dimensional network of strong covalent bonds.

iT  basically depends on the bond formation

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Answer 2

Answer:

yes, diamond and graphite are he allotropic form of diamond but they have different characteristics :

because of the free electron.

In graphite there is a free electron so, when it this electron moves by applying potential then current flow into graphite.

graphite is a conductor of electricity.

while diamond is an insulator because it doesn't contains any free electron in it.

Explanation:

Hope, it helps you.