The difference between the first and second ionization energies for magnesium is approximately 700 kJ/mol.  The difference between the second and third ionization energies will likely be:A.higher because the first and second ionization energies remove electrons from the p orbitals whereas the third removes an electron from an s orbital.B.higher because the first and second ionization energies remove valence electrons whereas the third removes a core electron.C.lower because the first and second ionization energies remove spin-paired electrons whereas the third removes an electron that is not spin-paired.D.lower because the first and second ionization energies remove electrons from the n = 2 subshell whereas the third removes an electron from the n = 3 subshell.

The difference between the second and third ionization energies will likely be higher because the first and second ionization energies remove valence electrons whereas the third removes a core electron.

Here's why:

Ionization energy is the energy required to remove an electron from an atom or ion. The first ionization energy of magnesium is the energy needed to remove the first, most loosely held electron. The second ionization energy is the energy needed to remove the next electron, and so on.

In the case of magnesium, the first two electrons are in the 3s orbital, which are the valence electrons. These are relatively easy to remove because they are further from the nucleus and less tightly held.

However, the third electron is a core electron, from the 2p orbital. Core electrons are closer to the nucleus and more tightly held, so it requires more energy to remove them. Therefore, the third ionization energy is significantly higher than the second.

So, the correct answer is B. "Higher because the first and second ionization energies remove valence electrons whereas the third removes a core electron."