Choose the correct statements about allotropes of carbon I. Graphite has layered structure II. Buckminster fullerene is not aromatic in nature III. The distance between two adjacent layers in graphite is 141.5 pm IV. The hybridization of carbons in graphite and Buckminster fullerene is same

Question

$\textbf{Reduction potential of ions are given below:}$
\[ \begin{array}{ccc} \text{ClO}_4^- & \text{IO}_4^- & \text{BrO}_4^- \\ E^\circ = 1.19 \, \text{V} & E^\circ = 1.65 \, \text{V} & E^\circ = 1.74 \, \text{V} \\ \end{array} \]
The correct order of their oxidising power is:

Answer 1

The question asks us to choose the correct statements about the allotropes of carbon. Let's evaluate each statement:

Graphite has a layered structure.
This statement is correct. Graphite is known for its layered structure where each layer is composed of carbon atoms bonded together in a hexagonal lattice. The layers are held together by weak van der Waals forces which allow them to slide over each other easily, making graphite a good lubricant.
Buckminster fullerene is not aromatic in nature.
This statement is also correct. Although Buckminster fullerene (C₆₀) has a structure resembling aromatic compounds (due to alternating single and double bonds), it does not exhibit traditional aromatic stability typical of benzene-like compounds. Its bonding is more localized, and it does not display the resonance associated with aromaticity.
The distance between two adjacent layers in graphite is 141.5 pm.
This statement is incorrect. The distance between two adjacent layers in graphite is approximately 335 pm, not 141.5 pm. 141.5 pm would refer more closely to the bond length between two carbon atoms within the same layer.
The hybridization of carbons in graphite and Buckminster fullerene is the same.
This statement is incorrect. In graphite, the carbon atoms are sp² hybridized, resulting in a planar structure for each layer. In contrast, in Buckminster fullerene, the carbon atoms are also sp² hybridized; however, the overall geometry is a spherical shape, not planar. Despite the same hybridization, the resulting structures are quite different.

Therefore, the correct statements are I and II. Thus, the correct answer is I & II.

Answer 2

The question asks us to choose the correct statements about the allotropes of carbon. Let's evaluate each statement:

Graphite has a layered structure.
This statement is correct. Graphite is known for its layered structure where each layer is composed of carbon atoms bonded together in a hexagonal lattice. The layers are held together by weak van der Waals forces which allow them to slide over each other easily, making graphite a good lubricant.
Buckminster fullerene is not aromatic in nature.
This statement is also correct. Although Buckminster fullerene (C₆₀) has a structure resembling aromatic compounds (due to alternating single and double bonds), it does not exhibit traditional aromatic stability typical of benzene-like compounds. Its bonding is more localized, and it does not display the resonance associated with aromaticity.
The distance between two adjacent layers in graphite is 141.5 pm.
This statement is incorrect. The distance between two adjacent layers in graphite is approximately 335 pm, not 141.5 pm. 141.5 pm would refer more closely to the bond length between two carbon atoms within the same layer.
The hybridization of carbons in graphite and Buckminster fullerene is the same.
This statement is incorrect. In graphite, the carbon atoms are sp² hybridized, resulting in a planar structure for each layer. In contrast, in Buckminster fullerene, the carbon atoms are also sp² hybridized; however, the overall geometry is a spherical shape, not planar. Despite the same hybridization, the resulting structures are quite different.

Therefore, the correct statements are I and II. Thus, the correct answer is I & II.

Choose the correct statements about allotropes of carbon I. Graphite has layered structure II. Buckminster fullerene is not aromatic in nature III. The distance between two adjacent layers in graphite is 141.5 pm IV. The hybridization of carbons in graphite and Buckminster fullerene is same

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The Correct Option is B

Solution and Explanation

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