I sort of get what you're trying to say, but it's not true. The second electron you're removing is not in another level, it's the second electron of level 3. Same level as the first one you removed. And same level as the second electron of Al.JessicaHelena said:
Aluminum (Al) has a higher 2nd ionisation energy because it has a stable electron configuration with a full outer shell of electrons. This makes it more difficult to remove an electron from Al compared to other elements that have a partially filled outer shell.
The atomic structure of Al has 13 protons and 13 electrons. The first ionization energy involves removing an electron from the outermost shell, leaving Al with a stable configuration of 12 electrons. However, the second ionization energy requires removing an electron from the now stable inner shell, which requires more energy.
Yes, the atomic radius of Al does have an impact on its 2nd ionisation energy. As the atomic radius decreases, the outermost electrons are held more tightly by the nucleus, making it harder to remove an electron and increasing the ionization energy.
The shielding effect refers to the inner electrons in an atom blocking the attraction between the nucleus and outer electrons. In Al, the 2nd ionization energy involves removing an electron from the stable inner shell, which is more shielded from the nucleus compared to the outer shell. This makes it more difficult to remove an electron and results in a higher 2nd ionization energy.
Yes, the 2nd ionisation energy of Al is always higher than the 1st ionisation energy. This is because the first ionization energy involves removing an electron from the outermost shell, which is less stable compared to the inner shell. The second ionization energy involves removing an electron from the now stable inner shell, requiring more energy.
