Question:
In graphite, the C-C bond length within the layer is X pm and the distance between two adjacent layers is Y pm. X and Y respectively are:
In graphite, the C-C bond length within the layer is X pm and the distance between two adjacent layers is Y pm. X and Y respectively are:
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Standard C-C single bond (diamond) is 154 pm. In graphite, the covalent bond is shorter (141.5 pm) because of $sp^2$ hybridization, but the "gap" between sheets is huge (340 pm) because there is no actual bond there.
Updated On: Jun 3, 2026
- 340 , 141.5
- 141.5 , 340
- 141.5 , 154
- 143.5 , 340
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The Correct Option is B
Solution and Explanation
Concept:
Graphite has a unique layered structure consisting of hexagonal rings of carbon atoms. Understanding the bonding within and between these layers explains its physical properties:
• Intra-layer bonding: Carbon atoms within a layer are $sp^2$ hybridized and held together by strong covalent bonds. The bond length is shorter than a standard single bond (154 pm) due to partial double bond character.
• Inter-layer bonding: The planar layers are held together by weak van der Waals forces. This results in a much larger distance between the layers.
Step 1: Determining the intra-layer bond length (X).
In each hexagonal layer of graphite, the C-C distance is significantly shorter because the atoms are closely packed and covalently bonded. This value is standardly measured at141.5 pm.
Step 2: Determining the inter-layer distance (Y).
Because the layers are held by weak forces rather than chemical bonds, they are spread further apart. This large gap allows the layers to slide over each other, making graphite a good lubricant. This distance is340 pm.
Step 3: Arranging in the required order.
The question asks for X (bond length) and Y (layer distance) respectively: \[ X = 141.5 \text{ pm} \] \[ Y = 340 \text{ pm} \] This matches option (B).
• Intra-layer bonding: Carbon atoms within a layer are $sp^2$ hybridized and held together by strong covalent bonds. The bond length is shorter than a standard single bond (154 pm) due to partial double bond character.
• Inter-layer bonding: The planar layers are held together by weak van der Waals forces. This results in a much larger distance between the layers.
Step 1: Determining the intra-layer bond length (X).
In each hexagonal layer of graphite, the C-C distance is significantly shorter because the atoms are closely packed and covalently bonded. This value is standardly measured at141.5 pm.
Step 2: Determining the inter-layer distance (Y).
Because the layers are held by weak forces rather than chemical bonds, they are spread further apart. This large gap allows the layers to slide over each other, making graphite a good lubricant. This distance is340 pm.
Step 3: Arranging in the required order.
The question asks for X (bond length) and Y (layer distance) respectively: \[ X = 141.5 \text{ pm} \] \[ Y = 340 \text{ pm} \] This matches option (B).
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