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Title: The statement that the first ionization energy for an oxygen atom is lower than the first ionization ... Post by: nomi on Mar 21, 2021 The statement that the first ionization energy for an oxygen atom is lower than the first ionization energy for a nitrogen atom is: ▸ consistent with the general trend relating changes in ionization energy across a period from left to right, because it is easier to take an electron from an oxygen atom than from a nitrogen atom. ▸ consistent with the general trend relating changes in ionization energy across a period from left to right, because it is harder to take an electron from an oxygen atom than from a nitrogen atom. ▸ inconsistent with the general trend relating changes in ionization energy across a period from left to right, due to the fact that the oxygen atom has two doubly-occupied 2p orbitals and nitrogen has only one. ▸ inconsistent with the general trend relating changes in ionization energy across a period from left to right, due to the fact that oxygen has one doubly-occupied 2p orbital and nitrogen does not. ▸ incorrect. Title: The statement that the first ionization energy for an oxygen atom is lower than the first ionization ... Post by: Zee68 on Mar 21, 2021 Content hidden
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