What is the differences between first and second ionization energy?

Answer 1

The first ionization energy is the energy that is required in order to remove the first electron from an atom in the GAS phase, the second ionization energy is the energy required to remove the second electron from an atom in the GAS phase. Ionization energy will generally increase for every electron that is removed and increases from left to right in the Periodic Table and moving up the periods.

Answer 2

First ionization energy is the energy required to remove one electron from an atom; second ionization is the energy required to remove another. Every element has a different set of ionization energies, and it's based upon the attraction between the positively charged nucleus and the negatively charged electron cloud, with electrons in different positions relative to the nucleus. Elements with relatively low first ionization energies and much higher second ionization energies are most likely in group 1. Members of this group only need to lose one electron to react successfully, so nature makes it very difficult for them to lose another.

Answer 3

The first ionization energy is the energy required to remove the outermost electron from a neutral atom, while the second ionization energy is the energy required to remove a second electron from the atom after the first electron has already been removed. Second ionization energy is typically higher than the first ionization energy due to the increased difficulty in removing electrons from a positively charged ion.