Explain the following: (i) Why is the atomic size of noble gases comparatively larger? (ii) Being almost equal in electronegativity, Nitrogen forms hydrogen bond while chlorine does not.

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> [!TLDR]
> Noble gases show larger atomic radii because their radius is measured as a van der Waals (non-bonded) radius; nitrogen forms hydrogen bonds while chlorine (of similar electronegativity) does not because nitrogen is a much smaller atom with a compact, high-charge-density lone pair.
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> **(i) Larger atomic size of noble gases:** Noble gases are monatomic and do not form covalent bonds, so their atomic radius cannot be a covalent radius. It is instead the **van der Waals radius**, which is measured up to the point of closest non-bonded approach and is always larger than a covalent radius. Since the radii of neighbouring elements are quoted as covalent radii, the noble gases appear to have anomalously large atomic sizes.
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