Final answer:
To determine which element has a higher second ionization energy, consider the atomic radius, first ionization energy, nuclear charge, and electron affinity. Generally, a smaller atomic radius and higher nuclear charge indicate a higher second ionization energy. High first ionization energy and electron affinity often correlate with high second ionization energies.
Step-by-step explanation:
To determine which element has a higher second ionization energy, we need to look at various factors, including the atomic radius, electron affinity, nuclear charge, and the first ionization energy. The second ionization energy is the energy required to remove a second electron from an atom. In general, as the atomic radius decreases, the ionization energy increases because electrons are closer to the nucleus and more strongly attracted by the nucleus. A smaller atomic radius usually means a higher second ionization energy.
First ionization energy is also a key indicator; elements with high first ionization energies tend to have high second ionization energies as well, because they have a strong hold on their electrons. The nuclear charge, which is the total charge of the nucleus due to its protons, also affects ionization energy: the greater the nuclear charge, the higher the ionization energy, as there is a stronger attraction for the electrons. Electron affinity refers to the amount of energy released when an atom acquires an electron. High electron affinity (a large negative value) correlates with high ionization energy, especially for second and subsequent electrons, because such atoms strongly attract electrons to begin with, making it more difficult to remove them.