14. Which of the following species would be expected to have the lowest ionization energy? 1 pointF-NeO2-Mg2+Na+

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. The trend of ionization energy in the periodic table is that it generally increases as you move from left to right across a period and decreases as you move down a group.

1. F- (Fluoride) - This is a negative ion (anion) which means it has gained an extra electron. Anions are usually larger and require less energy to remove an electron, so they have lower ionization energies.

2. Ne (Neon) - This is a noble gas with a full electron shell. Noble gases have the highest ionization energies because they have stable electron configurations and it requires a lot of energy to remove an electron.

3. O2- (Oxide) - This is another anion, so it will also have a lower ionization energy. However, oxygen is higher up on the periodic table than fluorine, so it will have a slightly higher ionization energy than F-.

4. Mg2+ (Magnesium) - This is a positive ion (cation) which means it has lost electrons. Cations are usually smaller and require more energy to remove an electron, so they have higher ionization energies.

5. Na+ (Sodium) - This is another cation, so it will also have a higher ionization energy. However, sodium is lower on the periodic table than magnesium, so it will have a slightly lower ionization energy than Mg2+.

So, based on these trends, F- would be expected to have the lowest ionization energy.