Explain noble gases have exceptionally high values of ionization energies but their electron affinities are zero why
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ionisation energy means the energy required to remove one electron in the gaseous state......
no noble gas would like to lose one electron as their stable electronic configuration would be disturbed.... hence we need to give very very high energy for this purpose.... so ionisation energy is high....
on the other hand electron affinity describe how much attracted is an element towards an electron..... this attraction would be zero for a noble gas because it already has a stable electronic configuration..... and it does not need any other extra electron....
hope this helps you....
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no noble gas would like to lose one electron as their stable electronic configuration would be disturbed.... hence we need to give very very high energy for this purpose.... so ionisation energy is high....
on the other hand electron affinity describe how much attracted is an element towards an electron..... this attraction would be zero for a noble gas because it already has a stable electronic configuration..... and it does not need any other extra electron....
hope this helps you....
plz mark it as brainliest
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Answer:
Explanation:
Since inert gases are in their most stable form, it is more unfavorable to remove their valence electrons than those of any other atom in the same period. As a result, more energy (ionization energy) is required to "pull" a valence electron away from inert gases.
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