Question

Compare the structure and Bonding in diamond and graphite. if you will give correct answer I will mark as brilliant but in your own words​

Answer 1

Answer:

Diamond molecules are shaped like perfect tetrahedra and are held together by single atoms forming strong bonds to four other atoms. Their shape makes diamond extra hard and durable to resist compression and broken bonds.

Graphite molecules consist of a single carbon atom attached to three others and gather together with others to form sheets of molecules. Though individual graphite molecules are strongly bonded, the sheets they form are weak and easily broken apart

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Answer 2

Answer:

In diamond, each carbon atom is linked tetrahedrally for four other carbon atoms by sp3 bonds.

Graphite has planar hexagonal layers of carbon atoms held together by weak Van der Waal's forces.

Explanation:

Diamond

Graphite

1. It has crystalline nature
2. It has layered structure
3. Each C is sp3 hybridzed and forms 4 covalent bonds with neighboring C atoms.
4. Each C atom is sp2 hybridized and forms 3 sigma bonds with 3 other C atoms. Fourth electron forms pi bond.
5. The geometry is tetrahedral.
6. The geometry is planar

graphite has a big molecular structure but each atom is only covalently bonded to 3 other carbon atoms compared to diamonds which has 4 , also graphite contains layers of carbon atoms. ... Carbon atoms in graphite form strong bonds on one layer but the diamond has a three dimensional bonding of carbon atoms.

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