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The ionisation energy of N is more than that of O. As nitrogen has a half filled orbital any oxygen is unstable when comparing with nitrogen . Hence oxygen undergoes ionisation at a comparatively lower energy

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In nitrogen atom, three 2p electrons are located in diff. atomic orbitals (Hund's rule). But in oxygen atom, there are four 2 electrons, so 2 of them are located in the same atomic orbital resulting in an increased e-e repulsion. So, it is easier to remove the electron from oxygen than from nitrogen.

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Oxygen undergoes ionization with lower energy and oxygen becomes stable by losing one electron. In other words, oxygen becomes easier to be ionized.

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Oxygen is more unstable than nitrogen so its easier for oxygen to ionise. Thus oxygen requires less ionisation enthalpy than nitrogen. Nitrogen has 3 electrons in its 2p shell thus its more stable. Since its more stable it requires more ionisation enthalpy. Hence the excepption in the trend is formed.

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Due to penetration of s orbital to the nucleus. Electrons in nitrogen, the electrons occupy the 1s,2s and 2p orbitals. Whereas it is 1s and 2s orbitals for oxygen. Hence the orbitals of oxygen are penetrated more than those of nitrogen. This causes nitrogen to lose electrons easily and hence have higher ionization enthalpy.

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N=1s^2 2s^2 2p^3
O=1s^2 2s^2 2p^4
as nitrogen has a half filled configuration but oxygen doesn't and we know that half filled p orbital is more stable.Hence  NITROGEN HAS A HIGHER IONIZATION THAN O2

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In the nitrogen atom, the 2p orbital is already half filled. It is more stable as compared to an oxygen atom. Hence oxygen atom loses an electron with lower energy as compared to a nitrogen atom.Oxygen has to lose an e- to gain half filled 2p orbit. Nitrogen has to use more energy to lose an e.

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Oxygen is less stable than Nitrogen, so oxygen can go ionization at lower energy. So, this is y nitrogen has a higher ionization energy than oxygen . This is because oxygen can lose one electron so it can attain a half-filled stable oribital.

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Oxygen is unstable compared to nitrogen. It is much easier for oxygen to ionize. oxygen requires less energy for ionization. Also nitrogen is half filled, which according to hunds rule makes it more stable

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oxygen is more stable than nitrogen.oxygen is way more easier to get ionised.oxygen requires less ionization enthalpy than nitrogen.nitrogen has 3 electrons in its 2p orbitals therefore its more stable.

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Nitrogen is having higher ionization than oxygen because due to higher inter- electronic repulsion removing an electron from an oxygen atom requires less energy.also the oxygen by removing one electron is attaining half filled stability whereas nitrogen consumes more energy because of removing electron from half filled stable atom

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Nitrogen has a half filled orbital. ... On the other hand, since Oxygen is already unstable relative to Nitrogen, by losing one electron it attains a stable half filled orbital.

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oxygen is very unstable compared to nitrogen. so oxygen ionizes at lower energy.

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#more energy to remove an electron from a very stable element like nitrogen
#Nitrogen has higher ionization than oxygen

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Nitrogen has a half filled orbital. On the other hand, since Oxygen is already unstable relative to Nitrogen, by losing one electron it attains a stable half filled orbital. So oxygen undergoes ionization at a relatively lower energy. This is why nitrogen has a higher ionization energy than oxygen.

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Nitrogen is more stable than oxygen due to its half filled orbital. More energy is required to remove an electron from a stable atom . Hence, more ionization enthalpy is needed for nitrogen than oxygen .

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As oxygen is more unstable than nitrogen so it ionizes easily by losing 1 electon.

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nitrogen is stable and oxygen is unstable. And the ionization of nitrogen is more than that of oxygen.

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Oxygen is stabilised through Nitrogen while losing one electron while it is only a half filled orbital. Therefore to gain electron it doesn’t require much energy making Nitrogen having higher concentration of ionised energy

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oxygen is unstable more than nitrogen , so by loosing one electron it gets stable . so oxygen gets ionized with lesser energy, so nitrogen has higher energy

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oxygen is unstable releative to nitrogen by losing one electron it attains a stable half filled orbital.

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because nitogen has less ionization enthalpy than oxygen because it has half filled orbit  and not stable

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because oxygen is not stable and nitrogen having higher ionization so nitrogen is more stable than oxygen..

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o2 is less stable than n2  so o2 can be ionized at low energy so that is y n2 has higher ionization energy than o2

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Nitrogen has a half filled orbital. On the other hand, since Oxygen is already unstable relative to Nitrogen, by losing one electron it attains a stable half filled orbital. So oxygen undergoes ionization at a relatively lower energy. This is why nitrogen has a higher ionization energy than oxygen.

Read more on:https://www.toppr.com/ask/question/ionization-enthalpy-of-nitrogen-is-more-than-oxygen-because-of/

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Nitrogen has a half filled orbital. On the other hand, since Oxygen is already unstable relative to Nitrogen, by losing one electron it attains a stable half filled orbital. So oxygen undergoes ionization at a relatively lower energy. This is why nitrogen has a higher ionization energy than oxygen.

Read more on:https://www.toppr.com/ask/question/ionization-enthalpy-of-nitrogen-is-more-than-oxygen-because-of/

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O2 is already unstable related to nitrogen as we know that N2 is a half filled orbital, this is why we can say that N2 is having a higher ionization enthalphy.