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(B) Inert gases are monoatomic and non-polar in nature.Since they lack permanent dipoles,the only attractive forces present between their atoms are we

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Instantaneous dipole-induced dipole

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(B) Inert gases are monoatomic and non-polar in nature.Since they lack permanent dipoles,the only attractive forces present between their atoms are weak London dispersion forces,also known as instantaneous dipole-induced dipole forces.These forces arise due to the temporary fluctuation in electron density,which creates a temporary dipole that induces a dipole in the neighboring atom.Therefore,these forces are responsible for the liquefaction of inert gases at very low temperatures.

Gas	$a / (kPa \cdot dm^6 \cdot mol^{-2})$	$b / (dm^3 \cdot mol^{-1})$
$A$	$642.32$	$0.05196$
$B$	$155.21$	$0.04136$
$C$	$431.91$	$0.05196$
$D$	$155.21$	$0.4382$

Which intermolecular force is most responsible for the liquefaction of inert gases?

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Gas $a / (kPa \cdot dm^6 \cdot mol^{-2})$ $b / (dm^3 \cdot mol^{-1})$

$A$ $642.32$ $0.05196$

$B$ $155.21$ $0.04136$

$C$ $431.91$ $0.05196$

$D$ $155.21$ $0.4382$

$a$ and $b$ are van der Waals constants. The correct statement about the gases is:

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