Due to the presence of a very stable electronic configuration in their outer she

Question

Due to the presence of a very stable electronic configuration in their outer shells, these elements have very high ionization energies. In a particular period, noble gases have highest ionization energies. In a group, the ionization energies of the noble gases decrease as we move down the group. This is due to increase in the atomic radius and the screening effect.

S.No Element Symbol Atomic number Electronic configuration 1 Helium H 2 1s2 2 Neon Ne 10 [He] 2s2sp6 3 Argon Ar 18 [Ne] 3s23p6 4 Krypton Kr 36 [Ar] 3d104s24p6 5 Xenon Xe 54 [Kr] 4d105s25p6 6 Radon Rn 86 [Xe] 4f145d106s26p6

Explanation / Answer

The following table gives the first ionization energies for the noble gas elements. Using electron configurations, explain why the first atomic number ionization energy decreases with increasing Element He Ne Ar Kr Xe Rn IE (kJ mol 2377 2088 1527 1356 1176 1042

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