The first ionization energy of oxygen is less than that of nitrogen. Which of the following is/are the incorrect reason(s) for this observation ?

Lesser effective nuclear charge of oxygen than nitrogen

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Lesser atomic size of oxygen than nitrogen

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Greater inter-electron repulsion between two electrons in the same p-orbital counter balances the increase in effective nuclear charge on moving from nitrogen to oxygen

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Greater effective nuclear charge of oxygen than nitrogen

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Solution

The correct options are
B Lesser atomic size of oxygen than nitrogen
D Greater effective nuclear charge of oxygen than nitrogen
The first ionization energy of oxygen is less than that of nitrogen because as we from left to right the atomic size decreases. Therefore ionization energy will be increased. But in case of oxygen and nitrogen the greater inter-electron repulsion between two electrons in the same p-orbital counter balances the increase in effective nuclear charge on moving from nitrogen to oxygen.
Hence options B & D are correct.

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