With respect to graphite and diamond, which of the statement(s) given below is(are) correct?a)Graphite is harder than diamond.b)Graphite has higher electrical conductivity than diamond.c)Graphite has higher thermal conductivity than diamond.d)Graphite has higher C—C bond order than diamond.Correct answer is option 'B,C,D'. Can you explain this answer?

Question

With respect to graphite and diamond, which of the statement(s) given below is(are) correct?a)Graphite is harder than diamond.b)Graphite has higher electrical conductivity than diamond.c)Graphite has higher thermal conductivity than diamond.d)Graphite has higher C&mdash;C bond order than diamond.Correct answer is option 'B,C,D'. Can you explain this answer?

Answer

Graphite and Diamond

Introduction
Graphite and diamond are two allotropes of carbon, meaning they are different forms of the same element. Despite being composed of the same element, graphite and diamond have different properties due to their distinct atomic structures.

Comparison of Properties

Hardness
- Graphite is not harder than diamond. In fact, diamond is the hardest known natural substance, while graphite is relatively soft and brittle.

Electrical Conductivity
- Graphite has higher electrical conductivity than diamond. This is because graphite has a unique layered structure, with carbon atoms arranged in sheets of hexagonal rings. The delocalized pi electrons in graphite can move freely within these layers, allowing for the conduction of electricity. In contrast, diamond lacks this layered structure and does not have freely moving electrons, resulting in poor electrical conductivity.

Thermal Conductivity
- Graphite has higher thermal conductivity than diamond. The layered structure of graphite also contributes to its high thermal conductivity. Heat can be transferred more efficiently through the layers of graphite compared to the tightly bonded carbon atoms in diamond.

C-C Bond Order
- Graphite does not have a higher C-C bond order than diamond. Both graphite and diamond consist of carbon atoms bonded together through strong covalent bonds. In diamond, each carbon atom forms four covalent bonds with neighboring atoms, resulting in a three-dimensional network of carbon atoms. In graphite, each carbon atom forms three covalent bonds, creating a two-dimensional network. The bond order is the same in both cases, with each carbon-carbon bond having a bond order of one.

Summary
In summary, the correct statements regarding graphite and diamond are:
- Graphite has higher electrical conductivity than diamond.
- Graphite has higher thermal conductivity than diamond.
These properties arise from the unique layered structure of graphite, which allows for the movement of electrons and efficient transfer of heat. However, graphite is not harder than diamond, and both materials have the same C-C bond order.

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