Why are Van der Waals forces weak in liquid argon?

As argon is a monatomic molecule, Van der Waal's forces arise when electrons in the molecule take on specific positions that upset the balance of charge. Since argon has eight electrons in its outer electronic level, it has a high degree of symmetry and stability, so the Van der Waal's forces are negligible.

Van der Waals forces are weak in liquid argon because the atoms in argon have a symmetrical electron distribution, resulting in negligible dipole moments. Additionally, the distance between argon atoms in the liquid phase is relatively large, leading to weak dispersion forces.

Van der Waals forces are weak in liquid argon because argon is a noble gas with a complete outer electron shell, leading to weak intermolecular forces between argon atoms. Additionally, argon atoms are spherical and non-polar, resulting in negligible dipole-dipole interactions. As a result, the only significant intermolecular forces in liquid argon are London dispersion forces, which are weaker compared to other types of intermolecular forces such as hydrogen bonding or dipole-dipole interactions. Therefore, Van der Waals forces are generally weak in liquid argon.