Less amount of energy is required to remove ' $s$ ' electron than ' $p$ ' electron.

True

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False

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Solution

The correct option is B False
For a given shell/ principal quantum number $n$ , the $s$ -orbital is closer to the nucleus and its electrons have a high attraction towards the nuclear charge that held them tightly to the nucleus. Whereas $p$ orbital is relatively diffuse and experience lesser penetration/ attraction to the nucleus. Therefore, the effective nuclear force of attraction is lower with an electron in $p$ orbital as compared to that in $s$ orbital electrons. Thus, a higher amount of energy is required to remove an electron from $s$ orbital than from $p$ orbital. Option $B$ is correct.

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Less amount of energy is required to remove 's' electron than 'p' electron.

Less amount of energy is required to remove ' $s$ ' electron than ' $p$ ' electron.