What is Ionization Energy?
Ionization energy is the amount of energy that is required to remove an electron from an isolated atom, when this atom is in the gas phase. It also indicates how "tightly" the atom is holding onto its electrons. Any given atom can have more than one ionization energy as every electron can have its own ionization energy. The atoms with the largest ionization energies are the smaller electrons, due to the fact that their valence electrons are closer to the nucleus (center) of the electron, making them harder to remove. Atoms that have one "extra" electron than a full outer shell have very low ionization energies as an atom "wants" to have a full outer shell.
Typically, ionization energies increase left to right on the periodic table. There are a few reasons for this but one of them is that atoms have more and more "extra" electrons as you go left to right. This is especially important when dealing with noble gases, as noble gases have the highest ionization energies because they already have a full outer shell of electrons. These elements don’t "want" to react with other elements, so they hold onto their electrons very tightly.
Lets take three elements, Helium, Florine, and Lithium, as examples. They, along with almost all other elements, all follow the patterns of the periodic table. Helium has the highest ionization energy because it has a full outer shell so it wants to keep its electrons and it's electrons are close to the nucleus; Fluorine would have the second highest ionization energy because it wants to attract one more electron while keeping the electrons it has; and finally, Lithium would have the lowest ionization energy because it wants to get rid of its valence electron in order to have to a full outer shell.
Typically, ionization energies increase left to right on the periodic table. There are a few reasons for this but one of them is that atoms have more and more "extra" electrons as you go left to right. This is especially important when dealing with noble gases, as noble gases have the highest ionization energies because they already have a full outer shell of electrons. These elements don’t "want" to react with other elements, so they hold onto their electrons very tightly.
Lets take three elements, Helium, Florine, and Lithium, as examples. They, along with almost all other elements, all follow the patterns of the periodic table. Helium has the highest ionization energy because it has a full outer shell so it wants to keep its electrons and it's electrons are close to the nucleus; Fluorine would have the second highest ionization energy because it wants to attract one more electron while keeping the electrons it has; and finally, Lithium would have the lowest ionization energy because it wants to get rid of its valence electron in order to have to a full outer shell.