Multiple Choice
The statement that the first ionization energy for an oxygen atom is lower than the first ionization energy for a nitrogen atom is
A) 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
B) 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
C) 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
D) 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
E) incorrect
Correct Answer:
Verified
Correct Answer:
Verified
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