Question

giving structure of diamond and graphite compare their electrical conductivity and softness??

Answer 1

Electrical conductivity-In graphite each carbon atoms & these forms layers of hexagonal network which are separated by a large distance but in case of diamond it's not happens.

Answer 2

Diamond and graphite are both allotropes of carbon; they are both made entirely of the same element (carbon) but they differ in the way that the atoms bond with each other and arrange themselves in a structure. Each carbon atom has 4 electrons in its outer shell that it can share with other atoms in order to form 4 covalent bonds. Diamond is a giant covalent structure; each valence electron (outer shell electron) of every carbon atom forms a covalent bond, which means that there are no free electrons. Since electrical conductivity relies on the flow of free electrons, diamond is not a good conductor.

Graphite on the other hand, although also only made up of carbon atoms, is the only non-metal that can conduct electricity. This is because only 3 of the available valence electrons form covalent bonds leaving 1 spare electron, which then becomes delocalised. This delocalised electron is no longer associated with one particular carbon atom and it is able to move freely between the carbon layers of graphite and conduct electricity.

Hope it helps.
And plz mark me as brainliest.