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nomi nomi
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9 months ago
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.
Textbook 

Chemistry: An Atoms First Approach


Edition: 3rd
Authors:
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Zee68Zee68
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9 months ago
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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.
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