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Why is the first ionization energy of nitrogen higher than oxygen?

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So oxygen would readily loose an electron to attain a stable configuration that is half filled configuration. So first Ionization energy of nitrogen is more than first ionization energy of Oxygen. read more

In nitrogen p - subshell is half filled . According to Hund , half filled & full filled orbitals are more stable . Hence it is difficult to remove an electron from 2p, So more amount of energy is required to remove an electron.Therefore IE of nitrogen is higher than oxygen. read more

Elements with low ionization energy tend to be reducing agents and to form salts. As the p orbital is more stable when its completely filled or half filled and in Nitrogen its half filled so p orbital in Nitrogen is more stable than in Oxygen so the ionization energy becomes high in Nitrogen than Oxygen. read more

Well, nitrogen atom has a first ionization energy of "14.53 eV", so it would be (b). But of course, you would not know that off-hand. read more

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