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Examples of Ionization

The term “ionization” refers to the use of heat, electricity, chemicals, discharge or radiation in order to transform atoms that are neutral to atoms with either a positive or negative electric charge.

Ionization: Changing Atoms Into Charged Ions

There are lots of different examples of ionization because there are lots of situations where atoms are transformed.
Some examples that you may be familiar with include:

  • When sodium and chlorine combine to make salt, the sodium atom gives up an electron resulting in a positive charge while chlorine gets the electron and becomes negatively charged as a result.
  • When previously neutral hydrogen chloride gas and water combine they make hydronium ions that are positively charged and chloride ions that are negatively charged.
  • When metallic zinc is exposed to acid it loses electrons and therefore becomes positively charged.

In each of these different situations, the charge of the atoms change as a result of the exposure to other elements or the combination with other elements.

Creation of Ionic Bonds and Ionization

The same process of ionization, the change in charge, as described above can happen when any of the following ionic bonds are created:

  • Lithium Fluoride
  • Lithium Chloride
  • Lithium Bromide
  • Lithium Iodide
  • Sodium Fluoride
  • Sodium Chloride
  • Sodium Bromide
  • Sodium Iodide
  • Potassium Fluoride
  • Potassium Chloride
  • Potassium Bromide
  • Potassium Iodide
  • Cesium Fluoride
  • Cesium Chloride
  • Cesium Bromide
  • Cesium Iodide
  • Beryllium Oxide
  • Beryllium Sulfide
  • Beryllium Selenide
  • Magnesium Oxide
  • Magnesium Sulfide
  • Magnesium Selenide
  • Calcium Oxide
  • Calcium Sulfide
  • Calcium Selenide
  • Barium Oxide
  • Barium Sulfide
  • Barium Selenide
  • Copper(I) Fluoride
  • Copper(I) Chloride
  • Copper(I) Bromide
  • Copper(I) Iodide
  • Copper(II) Oxide
  • Copper(II) Sulfide
  • Copper(II) Selenide
  • Iron(II) Oxide
  • Iron(II) Sulfide
  • Iron(II) Selenide
  • Cobalt(II) Oxide
  • Cobalt(II) Sulfide
  • Cobalt(II) Selenide
  • Nickel(II) Oxide
  • Nickel(II) Sulfide
  • Nickel(II) Selenide
  • Lead(II) Oxide
  • Lead(II) Sulfide
  • Lead(II) Selenide
  • Tin(II) Oxide
  • Tin(II) Sulfide
  • Tin(II) Selenide
  • Lithium Oxide
  • Lithium Sulfide
  • Lithium Selenide
  • Sodium Oxide
  • Sodium Sulfide
  • Sodium Selenide
  • Potassium Oxide
  • Potassium Sulfide
  • Potassium Selenide
  • Cesium Oxide
  • Cesium Sulfide
  • Cesium Selenide
  • Beryllium Fluoride
  • Beryllium Chloride
  • Beryllium Bromide
  • Beryllium Iodide
  • Magnesium Fluoride
  • Magnesium Chloride
  • Magnesium Bromide
  • Magnesium Iodide
  • Calcium Fluoride
  • Calcium Chloride
  • Calcium Bromide
  • Calcium Iodide
  • Barium Fluoride
  • Barium Chloride
  • Barium Bromide
  • Barium Iodide
  • Iron(II) Fluoride
  • Iron(II) Chloride
  • Iron(II) Bromide
  • Iron(II) Iodide
  • Cobalt(II) Fluoride
  • Cobalt(II) Chloride
  • Cobalt(II) Bromide
  • Cobalt(II) Iodide
  • Nickel(II) Fluoride
  • Nickel(II) Chloride
  • Nickel(II) Bromide
  • Nickel(II) Iodide
  • Copper(II) Fluoride
  • Copper(II) Chloride
  • Copper(II) Bromide
  • Copper(II) Iodide
  • Tin(II) Fluoride
  • Tin(II) Chloride
  • Tin(II) Bromide
  • Tin(II) Iodide
  • Lead(II) Fluoride
  • Lead(II) Chloride
  • Lead(II) Bromide
  • Lead(II) Iodide
  • Iron(III) Fluoride
  • Iron(III) Chloride
  • Iron(III) Bromide
  • Iron(III) Iodide
  • Cobalt(III) Fluoride
  • Cobalt(III) Chloride
  • Cobalt(III) Bromide
  • Cobalt(III) Iodide
  • Nickel(III) Fluoride
  • Nickel(III) Chloride
  • Nickel(III) Bromide
  • Nickel(III) Iodide
  • Tin(IV) Fluoride
  • Tin(IV) Chloride
  • Tin(IV) Bromide
  • Tin(IV) Iodide
  • Lead(IV) Fluoride
  • Lead(IV) Chloride
  • Lead(IV) Bromide
  • Lead(IV) Iodide
  • Lithium Nitride
  • Lithium Phosphide
  • Sodium Nitride
  • Sodium Phosphide
  • Potassium Nitride
  • Potassoum Phosphide
  • Cesium Nitride
  • Cesium Phosphide
  • Hydrogen Acetate
  • Lithium Acetate
  • Lithium Hydrogen Carbonate

Understanding ionization is very important in studying science because ionization explains how the charge of atoms are changed and can help to explain how atoms are transformed. You can observe lots of different examples of ionization in a lab setting and you can see the results both in science and in compounds that you encounter in your life.

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