In nitrogen: $ce 2s^2 2p^3$ In oxygen: $ce 2s^2 2p^4$

This speak me the it should be easier to remove an electron from oxygen than it is because that nitrogen together the electron in oxygen is slightly further away native the nucleus an interpretation lesser nuclear charge.

But why is that harder to remove an electron from oxygen, i.e. Why is the first ionization power of oxygen higher?




You are watching: Why does oxygen have a lower ionization energy than nitrogen

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Oxygen has a lower first ionization energy as the electron the is eliminated is comes from a combine orbital.
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Electrons within the exact same orbital suffer maximum repulsion together the distribution of their wavefunctions is the same, therefore the probability thickness distribution is the same and also the electrons can be thought of together occupying the exact same space. This maximizes your repulsion and also increases the potential power of the electron in that orbital, do the electrons simpler to remove. This is despite the increased reliable nuclear charge experienced by the electron in oxygen and the diminished radius that the orbital.

See: "Physical wgc2010.org", Atkins, P.W. Ar 13.4, p.p.370 (4th edition) - sorry, I have actually an old one!


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You watch from the electronic configurations:

nitrogen: $ce 2s^2 2p^3$ oxygen: $ce 2s^2 2p^4$

In reality, the first ionisation power of nitrogen is better than the an initial ionisation power of oxygen because nitrogen, in a stable fifty percent filled orbit state, is comparatively an ext stable 보다 oxygen. Oxygen, ~ above the various other hand, would have tendency to lose an electron quickly to accomplish it"s more stable half filled orbital state.

Also, as a rule, half filled and fully filled orbital claims are an ext stable as compared to various other configurations since they attribute to maximum exchange energies.


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