Answer to Question #47903 in Atomic and Nuclear Physics for tinu

Question

to find the ionisation energy of atoms in a period,if we move from left to right to the periodic table,the ionisation energy generally increases.because with the increase of atomic number,there is an increase of nuclear charge and so the nucleus of an atom has more attaraction to the electron and thus the ionisation energy increases.i know ionisation energy of Be is greater than B.i know the reason too.for this case Be has stable 2s2 thats why.i found another reason.the last electron of Be is removed from s orbital and the last electron of B from p orbital.and s is closer to the nucleus than p orbital.so to remove electron from s orbital is harder than to remove from p orbital as the attraction of the nucleus and s orbital is more than p.now my question is why in a period to find ionisation energy we dont say that with the increase of atomic number the last electron is in s,p,d.and s is too close to nucleus and the others are not closer like s orbital.why not the left sided atoms have more ionisation energy