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Which of the following order is correct for the first ionization energies of their elements?
- a)B < Be < O < N
- b)B < Be < N < O
- c)Be < B < N < O
- d)B < O < Be < N
Correct answer is option 'A'. Can you explain this answer?
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Which of the following order is correct for the first ionization energ...
Boron, B is smaller than beryllium, Be atom. Hence we expect increase in ionization energy from Be to B.
However, Be atom has greater ionization energy than B atom. The reason is - in case of Beryllium, the last electron is in the s-orbital and in Boron, the last electron is in the p-orbital. We know that removal of electron from s-orbital requires more energy than the electron from p-orbital.
2s22p3 configuration is more stable than 2s22p4 due to half filled p-sublevel. The electrons in the p-orbital in N atom experience less repulsion, thus more stable and more ionization energy. Whereas in case of O atom the 4th p-electron atom can be removed more easily as it experiences more repulsion from the electrons in the p-orbitals already present. Hence nitrogen, Oxygen atom has less ionization energy than Nitrogen atom.
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Which of the following order is correct for the first ionization energ...
The question is incomplete as it does not provide the full list of elements to be compared. Please provide the complete list of elements for a proper comparison.
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Which of the following order is correct for the first ionization energies of their elements?a)B < Be < O < Nb)B < Be < N < Oc)Be < B < N < Od)B < O < Be < NCorrect answer is option 'A'. Can you explain this answer?
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