Why is Nitrogen has higher Ionisation Energy than Oxygen?

Question

I am studying A Level Chemistry and my teacher asked a question.
What is ionisation energy?
I know it is, the energy needed to remove electrons.
Which element Nitrogen or Oxygen has higher first ionisation energy? Why?
It's Nitrogen right? But why?

Please also include what factors effect ionisation energy and please explain it too..

Thank You VERY MUCH!!! Wie Viele Danke...!!

Answer 1

Ionisation energy is the minimum energy needed to remove a mole of electrons from a mole of gaseous atoms.

O has a lower 1st IE than N because O is 1s2 2s2 2p4 and N is 1s2 2s2 2p3. The 4th electron in the O atom's outer level has to pair up with one of the others, and this introduces repulsions, which makes it easier to remove.

The relevant factors are nuclear charge, atomic radius and screening by inner electrons.

Answer 2

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RE:
Why is Nitrogen has higher Ionisation Energy than Oxygen?
I am studying A Level Chemistry and my teacher asked a question.
What is ionisation energy?
I know it is, the energy needed to remove electrons.
Which element Nitrogen or Oxygen has higher first ionisation energy? Why?
It's Nitrogen right? But why?

Please also include what factors...

Answer 3

Ionization Energy Of Nitrogen

Answer 4

Nitrogen 1st ionisation energy = 1400 kJ/mol
Nitrogen Electronic configuration = 1s2. 2s2, 2p3
Oxigen 1st ionisation energy = 1310 kJ/mol
Oxigen electronic configuration
1s2, 2s2,2p4 ( 2p(x)2, 2p (y)1 , 2p(z)1

The difference is that in oxigen the electron being removed is one of the 2p(x)2 pair.
The repulsion between the two electrons in the same orbital means that the electron is easier to remove then it would otherwise be.

Answer 5

he ionization potential, ionization energy or EI of an atom or molecule is the energy required to remove one mole of electrons from one mole of isolated gaseous atoms or ions. More generally, the nth ionization energy is the energy required to strip it of an nth mole of electrons after the first n − 1 mole of electrons have already been removed. It is considered in physical chemistry as a measure of the "reluctance" of an atom or ion to surrender an electron, or the "strength" by which the electron is bounded; the greater the ionization energy, the more difficult it is to remove an electron. The ionization potential is an indicator of the reactivity of an element. Elements with low ionization energy tend to be reducing agents and to form salts.



As the p orbital is more stable when its completely filled or half filled and in Nitrogen its half filled so p orbital in Nitrogen is more stable than in Oxygen so the ionization energy becomes high in Nitrogen than Oxygen.