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  •  Assertion 2: Graphite is a good conductor of electricity, while diamond is not. Reasoning 2: In graphite, each carbon atom is sp2 hybridized and covalently bonded to three other car

 Assertion 2: Graphite is a good conductor of electricity, while diamond is not.

Reasoning 2: In graphite, each carbon atom is sp2 hybridized and covalently bonded to three other carbon atoms of the same layer by single bonds, forming a layer of hexagonal rings. At each carbon atom, the fourth valence electron is available free, which moves among different layers and provides good electrical conducting nature to graphite. On the other hand, diamond has a fully occupied valence band and an empty conduction band, and hence, no free electrons are available for electrical conduction.

 

Option: 1

Both the assertion and reasoning are true, and the reasoning is the correct explanation for the assertion.

 


Option: 2

Both the assertion and reasoning are true, but the reasoning is not the correct explanation for the assertion.


Option: 3

The assertion is true, but the reasoning is false.


Option: 4

The assertion is false, but the reasoning is true.


Answers (1)

best_answer

The assertion that "Graphite is a good conductor of electricity, while diamond is not" is true. Graphite is an excellent conductor of electricity, while diamond is an electrical insulator. The reasoning that "In graphite, each carbon atom is sp2 hybridized and covalently bonded to three other carbon atoms of the same layer by single bonds, forming a layer of hexagonal rings. At each carbon atom, the fourth valence electron is available free, which moves among different layers and provides good electrical conducting nature to graphite. On the other hand, diamond has a fully occupied valence band and an empty conduction band, and hence, no free electrons are available for electrical conduction" is also true and is the correct explanation for the assertion. In graphite, each carbon atom is covalently bonded to three other carbon atoms of the same layer by single bonds, forming a layer of hexagonal rings. The fourth valence electron of each carbon atom is available free and is delocalized over the entire layer, which results in the formation of a "sea" of free electrons that can move freely among different layers of graphite. This delocalization of electrons is responsible for the good electrical conducting nature of graphite. In contrast, diamond has a fully occupied valence band and an empty conduction band. This means that no free electrons are available for electrical conduction, and hence diamond is an insulator. The valence electrons in diamond are tightly held by the strong covalent bonds between the carbon atoms and are not available for electrical conduction.

 

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