Though Argon has d orbital,why it has low ionization energy than Ne?
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Each of the noble gases, in the last column of the periodic table, has its last electron shell ... Ionization Energy ... Neon, Argon, Krypton.
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Calculations of what exactly? Unless you want to start talking about quantum mechanics, there aren’t very many calculations to be had outside of the ones involved with atomic orbital theory, which is far from trivial. Wave functions are not a joke.
Suffice it to say, Argon has all filled orbitals as well as a filled valence shell. As a result, it doesn’t want to lose or gain any electrons. If it were to lose an electron, it would go from having no unfilled orbitals to one unfilled orbital, and from a filled valence shell to an unfilled valence shell. Both of these are unfavorable, which explains the high ionization energy. The same thing would happen if it were to gain an electron, which explains the low electron affinity.
Suffice it to say, Argon has all filled orbitals as well as a filled valence shell. As a result, it doesn’t want to lose or gain any electrons. If it were to lose an electron, it would go from having no unfilled orbitals to one unfilled orbital, and from a filled valence shell to an unfilled valence shell. Both of these are unfavorable, which explains the high ionization energy. The same thing would happen if it were to gain an electron, which explains the low electron affinity.
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