Question

why ionization enthalpy of nitrogen is more than of oxygen

Answer 1

Ionization enthalpy of nitrogen is more than of oxygen because:

• The energy required to remove an electron from the outer shell of an atom or energy required to convert an atom into an ion by removing its electron is known as its ionization enthalpy.
• Nitrogen has an atomic number of 15 and has 3 electrons in 2p orbital. The maximum electrons that can be accommodated in the 2p orbital is 6. It means nitrogen has additional stability due to a half-filled 2p orbital.
• Oxygen having atomic number 16 has 4 electrons in a 2p orbital. This 1 electron can be removed easily from the 2p orbital as it is less stable because it is not being removed from a half-filled orbital.
• More energy is required to remove electrons in the case of nitrogen due to extra stability and hence its ionization enthalpy is greater.

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Answer 2

Answer:

Ionization energy can be thought of as the energy needed to extract an electron from the valence shell of an atom. Nitrogen is understood to have a half-filled p-orbital and exists quite stable.

Explanation:

Ionization energy is the minimum energy needed to release the most loosely held electron from one mole of gaseous atoms to create one mole of gaseous ions each with a charge of +1.

Ionization energy can be thought of as the energy needed to extract an electron from the valence shell of an atom. Nitrogen is understood to have a half-filled p-orbital and exists quite stable. Thus, the amount of energy needed to remove an electron from the valence shell of nitrogen will be much more increased than the energy needed to remove an electron from the valence shell of oxygen. Accordingly, the ionization of nitrogen will be higher than that of oxygen.

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