The first ionization potential in electron volts of nitrogen and oxygen atoms are respectively given by:a)14.6, 13.6b)13.6, 14.6c)13.6, 13.6d)14.6, 14.6The correct answer is option 'A'. Can you explain this answer?

Question

Answer

First Ionization Potential of Nitrogen and Oxygen Atoms

The first ionization potential is the minimum amount of energy required to remove one electron from an atom in its gaseous state. The ionization potential is measured in electron volts (eV). The first ionization potential of nitrogen and oxygen atoms are given below:

- Nitrogen: 14.6 eV
- Oxygen: 13.6 eV

Explanation

The correct answer is option 'A' which states that the first ionization potential of nitrogen is higher than that of oxygen. This means that it requires more energy to remove an electron from a nitrogen atom than from an oxygen atom.

The reason for this difference lies in the electronic configuration of these atoms. Nitrogen has an electronic configuration of 1s² 2s² 2p³, which means that it has five electrons in its outermost shell. Oxygen, on the other hand, has an electronic configuration of 1s² 2s² 2p⁴, which means that it has six electrons in its outermost shell.

The valence electrons in nitrogen are located in three different orbitals - 2s and two orbitals of 2p. The 2s electrons are closer to the nucleus and experience greater attraction than the 2p electrons. Therefore, the ionization potential of nitrogen is higher than that of oxygen.

Conclusion

In summary, the first ionization potential of nitrogen is 14.6 eV, while that of oxygen is 13.6 eV. The higher ionization potential of nitrogen is due to the electronic configuration of its valence electrons, which are located in orbitals that experience greater attraction to the nucleus.

Answer

From the electronic configuration of N and O:-

N:- [He]2s2 2p3

O:- [He]2s2 2p4

On the 1st ionisation of N, the stable p3 configuration is lost but in case of O the stable p3 config. is gained.

Thus the IE of O is lesser than that of N.

Answer

Because nitrigen has half filled p orbital. So more energy is required to remove electron from stable configuratiin.

Answer

Plz explain in detail me

Answer

The first ip value of N is greater than O because in N breaking of half filled 2p configuration is required which is very difficult and this does not occur for O

Answer

How to calculate numerical value of electronegativity of nitrogen and oxygen

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