In Cl_2, the van der Waals radius is 180 pm. | vedclass

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Question

(A) The distance between the two atoms in a $Cl_2$ molecule is the bond length (covalent bond distance).For a homonuclear diatomic molecule like $Cl_2

Vedclass · Accepted Answer

$180$

Vedclass · Answer

(A) The distance between the two atoms in a $Cl_2$ molecule is the bond length (covalent bond distance).For a homonuclear diatomic molecule like $Cl_2$, the bond length is equal to twice the covalent radius.However, the question provides the van der Waals radius.In a $Cl_2$ molecule, the distance between the two nuclei is the covalent bond length, which is typically smaller than the van der Waals radius.If the question implies the distance between two non-bonded $Cl$ atoms in adjacent $Cl_2$ molecules, it would be twice the van der Waals radius $(360 \ pm)$.Assuming the question asks for the distance between the two atoms bonded in the $Cl_2$ molecule, and given the standard relationship where covalent radius is approximately $0.77 	imes$ van der Waals radius, the bond length is $d = 2 	imes r_{covalent}$.Given the context of typical textbook problems, if the value $180 \ pm$ is provided as the van der Waals radius, the distance between the two atoms in the molecule is $99 \ pm$ (covalent radius $\approx 99 \ pm$, bond length $\approx 198 \ pm$).If the question asks for the distance between two atoms in the $Cl_2$ molecule based on the provided value as the covalent radius, the answer is $180 \ pm$.Given the options, the most logical interpretation is that $180 \ pm$ represents the bond length (distance between the two atoms).

In $Cl_2$, the van der Waals radius is $180 \ pm$. What is the distance between the two atoms (in $pm$)?

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