Which of the following configurations has the highest ionization energy?

1 s^{2} 2 s^{2} 2 p^{1}

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1 s^{2} 2 s^{2} 2 p^{3}

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1 s^{2} 2 s^{2} 2 p^{2}

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1 s^{2} 2 s^{2} 2 p^{4}

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Solution

The correct option is C $1 s^{2} 2 s^{2} 2 p^{3}$
The electron will move from a lower stationary state to a higher stationary state when the required amount of energy is absorbed by the electron or energy is emitted when the electron moves from a higher stationary state to lower stationary state. The energy change does not continuously take place.

Hence, the correct option is $B$

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Which of the following configurations represent atoms of the elements having the highest second ionization energy?

Which of the following configurations represents an atom of the group having the highest second ionization energy?

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