Question

oy radioacuvity
5) Explain the difference lecture diamond& graphite​

Answer 1

Diamond is hard due to strong covalent bonds present in it. In a Graphite, carbon atoms are bounded together in a flat layers by an strong covalent bonds in a regular haxagon. These layers are held together by much wealer van der Wall's forces, therefore the crystals of graphite soft and slippery.

Answer 2

Answer:

Diamond: 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

Graphite: 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.

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