Ionization

Ionization: 

Ionization Ionization- when an atom gains or loses electrons in order to achieve the ideal state of 8 valence electrons. Valence electrons- the electrons in the outermost shell, available to be lost or gained in a chemical bond.

Valence Electrons: 

Valence Electrons The amount of valence electrons an atom has corresponds to its group in the periodic table. As you move left to right, the number of valence electrons increases, ending with the ideal number of 8. The noble gases (group 18) do not form bonds because they naturally have the stable configuration of eight.

Ionization Charge: 

Ionization Charge Ionization charge is directly linked to number of valence electrons, because the number of electrons an atom will have to lose or gain determines what its charge will be. For example, Group 1 elements will need to lose one valence electron. This will result in an uneven ratio of protons to electrons, and a charge of +1. Similarly, Group 17 elements will need to gain 1 electron, resulting in a charge of -1.

Cations: 

Cations The atoms that lose electrons and have a resulting positive charge are called cations. Groups 1, 2, and 13 will ionize as cations. Beryllium (Be), for example, must lose two electrons. Therefore, Beryllium ions will have a charge of +2.

Anions: 

Anions Anions are the negative counterpart to cations. Instead of losing electrons, they have gained them, thus having a negative charge. Tellurium has 6 valence electrons, and will gain two when it ionizes. Its ionization charge will then be -2.