The atomic size of atoms decreases across a period due to increase in nuclear charge but the atomic size of noble gases is greater than the atomic size of halogen members,WHY???
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The atomic size of atoms decreases across a period due to increase in nuclear charge but the atomic size of noble gases is greater than the atomic size of halogen members,WHY???
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Noble gases have comparatively large atomic sizes as they have vanderwaals radii which is larger than both the ionic and covalent radii.
The Atomic radius is determined using the distance from the nucleus to the outermost electron but since the position of the outermost electron can never be determined, it is assumed to be half the distance between the nuclei of two bonded atoms of the same element. The halogens naturally exist as Br2 and Cl2 and are quite stable because each halogen contributes its unpaired electron in the outermost shell. This means that when both are joined they each have full valence shells. Now noble gases already have full outer shells so the attractions between the atoms is Van der Waals forces which means that the attraction between atoms is much weaker compared to the attraction between halogens. This in conclusion means the assumed atomic radius is larger than halogens. I hope this helped!
The noble gases are more stable because of their fully filled electronic configurationn than the halogens .Across a period in noble gases nuclear charge decreases n their atomic size increases
the extra electron and repulsion forces make it larger