Which of the following orders is not correct?

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(B) $1$. Density: The density of $Diamond$ $(3.51 \ g/cm^3)$ is greater than that of $Graphite$ $(2.26 \ g/cm^3)$. Thus,$Diamond > Graphite$ is correc

Vedclass · Accepted Answer

$Graphite < Diamond$ ($C-C$ bond strength)

Vedclass · Answer

(B) $1$. Density: The density of $Diamond$ $(3.51 \ g/cm^3)$ is greater than that of $Graphite$ $(2.26 \ g/cm^3)$. Thus,$Diamond > Graphite$ is correct.$2$. $C-C$ bond strength: In $Diamond$,all $C-C$ bonds are single bonds ($sp^3$ hybridization). In $Graphite$,there is partial double bond character due to resonance ($sp^2$ hybridization). Therefore,$Graphite$ has higher bond strength than $Diamond$. The order $Graphite $3$. Thermodynamic stability: $Graphite$ is the most stable allotrope of carbon at room temperature and pressure. Thus,$Graphite > Diamond$ is correct.$4$. Heat conductivity: $Diamond$ is a better conductor of heat than $Graphite$ at room temperature. Thus,$Diamond > Graphite$ is correct.Conclusion: Option $B$ is the incorrect order.

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