Anion
- This article is about the electrically charged molecule. For other uses of this word, see ion (disambiguation).
An ion is an atom or group of atoms with a net electric charge. A negatively charged ion, which has gained one or more electrons, is known as an anion, for it is attracted to anodes, and a positively charged ion, which has lost one or more electrons, is known as a cation (pronounced cat eye on), for it is attracted to cathodes.
Scientific fields
In chemistry, an ion is an electrically charged molecule or atom that has gained or lost electrons from its normal complement in a process known as ionization.
In physics, completely ionized atomic nuclei, such as those in alpha radiation, are more commonly called charged particles. Ionization is usually performed by the application of high energy to atoms, in the form of electrical voltage or by high-energy radiation. An ionized gas is called plasma.
History
Ions were first theorized by Michael Faraday around 1830, to describe the portions of molecules that travel either to an anion or to a cation. However, the mechanism by which this was achieved was not described until 1884 by Svante August Arrhenius in his doctoral dissertation to the University of Uppsala. His theory was initially not accepted (he got his degree with a minimum passing grade) but he won the Nobel Prize in Chemistry in 1903 for the same dissertation.
Analysis
For single atoms in a vacuum, there are physical constants associated with the process of ionization. The energy needed to remove electrons from an atom is called the ionization energy, or ionization potential. These terms are also used to describe ionization of molecules and solids, but the values are not constant because ionization can be affected by the local chemistry, geometry, and temperature.
Ionization energies decrease down a group of the Periodic Table, and increase left-to-right across a period. These trends are exact opposite of the atomic radius periodic trends. Electrons in smaller atoms are attracted more strongly to the nucleus, therefore the ionization energy is greater. In larger atoms, the electrons are not held as strongly so the required ionization energy is lesser.
| Element |
First |
Second |
Third |
Fourth |
Fifth |
Sixth |
Seventh |
| Na |
496 |
4,560 |
| Mg |
738 |
1,450 |
7,730 |
| Al |
577 |
1,816 |
2,744 |
11,600 |
| Si |
786 |
1,577 |
3,228 |
4,354 |
16,100 |
| P |
1,060 |
1,890 |
2,905 |
4,950 |
6,270 |
21,200 |
| S |
999 |
2,260 |
3,375 |
4,565 |
6,950 |
8,490 |
11,000 |
| Cl |
1,256 |
2,295 |
3,850 |
5,160 |
6,560 |
9,360 |
11,000 |
| Ar |
1,520 |
2,665 |
3,945 |
5,770 |
7,230 |
8,780 |
12,000 |
| Successive Ionization Energies in kJ/mol |
The first ionization energy is the energy required to remove one electron, the second to remove two electrons, and so on. The successive ionization energies are always greater than the previous, and a certain nth ionization energy will be significantly larger than the rest. For this reason, ions tend to form in certain ways. For example, sodium is found as Na+, but not usually Na2+ due to the large amount of ionization energy required. Likewise, magnesium is found as Mg2+, but not Mg3+ and aluminum may exist as an Al3+ cation.
Etymology
The word "ion" is from Greek ion, present participle of ienai "go", thus "a goer". "Anion" and "cation" mean "up-goer" and "down-goer", and "anode" and "cathode" are "way up" and "way down" (hodos = road, way).
