explain by the first i.e of magnesium is more than that of aluminium
Answers
Before knowing this answer you have to know few things that is ionization energy and orbital configurations. Let see what are those.
Ionization energy or we will call it as ionozation potential means the amount of energy required to remove an elctron from the outet most orbital. Now let's see how ionization potential varies from magnesium and alluminum. Lets write the orbital configuration for magnesium and alluminum not violating the hunds rule, aufbau principle and moeller diagram Before going to write the orbital configurations be through with the rules.
The atomic number of magnesium is 12.So the orbital configuration is as follows.
1s2 2s2 2p6 3s2.This is the configuration of magnesium or the arrangement of electrons in the shells. See there are no free electrons in the above configuration indeed all are bonded. So if u want to remove an electrom from the outermost shell you must have to remove the electron from 3s orbital (why 3s orbital particularly?)see the alignment of moeller chart then you can get the perfect picture of that. So the energy reauired to remove an elctron from the bonded position is not an easy task so it needs a lot of energy. And the energy would be in terms of eV or in joules.
Consider in the case of Alluminum the atomic number is 13 then write the orbital configuration of that it is as follows.
Al-1s2 2s2 2p6 3s2 3p1.see the difference between the configuration of magnesium and alluminum, here in case of alluminum we found one single electron which is not bonded is in the outermost shell, so it is easy to remove an elctron of such kind and the energy required is even less compared to thr above. So because of the above reason the ionization energy of magnesium is more than the ionization energy of alluminum.
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