The energy required to remove an electron is always much, much greater if the atom is isoelectronic with a noble gas before the electron is removed.
The energy needed to remove an electron from a separate molecule or an atom is known as ionization energy. On the periodic table, from left to right across the period, the ionization energy increases from left to right.
An isoelectronic atom refers to two atoms containing a similar amount of electronic structure. As a result, they have the same number of valence electrons.
Now, we know that the noble gas is at the extreme right-hand side of the periodic table, thus they have the greatest ionization energy. Thus, the energy required to remove an electron will be much greater if the atom is isoelectronic with noble gas before the electron is removed.
Therefore, we can conclude that the energy required to remove an electron is always much, much greater if the atom is isoelectronic with a noble gas before the electron is removed.
Learn more about isoelectric atoms here:
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