Which of the following electron configurations indicates an atom with the highest ionization energy?
2,8,7
2,8,8,1
2,8,8,2
2,8,8,7
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as we know ionization energy is the energy required to remove the valence electron from an atom.the farther an electron to the nucleus the lower the ionization energy because the electrostatic force of attraction the nucleus has for the electron is small,however the nearer the electron the higher the energy because the nucleus is exerting greater force.hence option B,C&D have four shells where as A has three only thus it more closer to the nucleus therefore the energy required to remove the electron will be high
The correct answer is A the farther electron is to the nucleus the lower its ionisation energy and vice versa and A has three shells unlike others with four shells so so A has the shell closest to the nucleus so it has the highest ionisation energy another reason is that metals have low ionisation energy and if check option A is chlorine which is a non metal an halogen this answer is not totally true but its a confirmation of the first one. 
The atom with the highest ionization energy is the one that is most stable, and a full electron shell contributes to this stability.
Option **C. 2,8,8,2** represents an atom with a completely filled outer shell (noble gas configuration), which makes it the most stable among the given options. Therefore, it would require the highest amount of energy to remove an electron, i.e., it has the highest ionization energy. So, the correct answer is **C**.
