Ion

For other uses, see the electrically charged particle.

An electrostatic potential map of the nitrate ion (NO₃⁻). Areas coloured red are lower in energy than areas colored yellow

An ion is an atom or molecule which has lost or gained one or more valence electrons, giving it a positive or negative electrical charge.

A negatively charged ion, which has more electrons in its electron shells than it has protons in its nuclei, is known as an anion (ana: Greek 'up') (Template:PronEng; an-eye-on). Conversely, a positively-charged ion, which has fewer electrons than protons, is known as a cation (kata: Greek 'down') (Template:PronEng; cat-eye-on).

An ion consisting of a single atom is called a monatomic ion, but if it consists of two or more atoms, it is a polyatomic ion. Polyatomic ions containing oxygen, such as carbonate and sulfate, are called oxyanions.

Ions are denoted in the same way as electrically neutral atoms and molecules except for the presence of a superscript indicating the sign of the net electric charge and the number of electrons lost or gained, if more than one. For example: H⁺ and SO₄²⁻.

Formation

Formation of polyatomic and molecular ions

Polyatomic and molecular ions are often formed by the combination of elemental ions such as H⁺ with neutral molecules or by the gain of such elemental ions from neutral molecules. A simple example of this is the ammonium ion NH₄⁺ which can be formed by ammonia NH₃ accepting a proton, H⁺. Ammonia and ammonium have the same number of electrons in essentially the same electronic configuration but differ in protons. The charge has been added by the addition of a proton (H⁺) not the addition or removal of electrons. The distinction between this and the removal of an electron from the whole molecule is important in large systems because it usually results in much more stable ions with complete electron shells. For example NH₃·⁺ is not stable because of an incomplete valence shell around nitrogen and is in fact a radical ion.

Ionization potential

Main article: Ionization potential

The energy required to detach an electron in its lowest energy state from an atom or molecule of a gas with less net electric charge is called the ionization potential, or ionization energy. The nth ionization energy of an atom is the energy required to detach its nth electron after the first n − 1 electrons have already been detached.

Each successive ionization energy is markedly greater than the last. Particularly great increases occur after any given block of atomic orbitals is exhausted of electrons. For this reason, ions tend to form in ways that leave them with full orbital blocks. For example, sodium has one valence electron, in its outermost shell, so in ionized form it is commonly found with one lost electron, as Na⁺. On the other side of the periodic table, chlorine has seven valence electrons, so in ionized form it is commonly found with one gained electron, as Cl⁻. Francium has the lowest ionization energy of all the elements and fluorine has the greatest. The ionization energy of metals is generally much lower than the ionization energy of nonmetals, which is why metals will generally lose electrons to form positively-charged ions while nonmetals will generally gain electrons to form negatively-charged ions.

A neutral atom contains an equal number of Z protons in the nucleus and Z electrons in the electron shell. The electrons' negative charges thus exactly cancel the protons' positive charges. In the simple view of the Free electron model, a passing electron is therefore not attracted to a neutral atom and cannot bind to it. In reality, however, the atomic electrons form a cloud into which the additional electron penetrates, thus being exposed to a net positive charge part of the time. Furthermore, the additional charge displaces the original electrons and all of the Z + 1 electrons rearrange into a new configuration.

Ions

• Anions are negatively charged ions, formed when an atom gains electrons in a reaction. Anions are negatively charged because there are more electrons associated with them than there are protons in their nuclei.

• Cations are positively charged ions, formed when an atom loses electrons in a reaction, forming an 'electron hole'. Cations are the opposite of anions, since cations have fewer electrons than protons.

• Radical ions: radical ions are ions that contain an odd number of electrons and are mostly very reactive and unstable.

Plasma

Main article: Plasma (physics)

A collection of non-aqueous gas-like ions, or even a gas containing a proportion of charged particles, is called a plasma, often called the fourth state of matter because its properties are quite different from solids, liquids, and gases. Astrophysical plasmas containing predominantly a mixture of electrons and protons, may make up as much as 99.9% of visible matter in the universe.

Applications

Ions are essential to life. Sodium, potassium, calcium and other ions play an important role in the cells of living organisms, particularly in cell membranes. They have many practical, everyday applications in items such as smoke detectors, and are also finding use in unconventional technologies such as ion engines. Inorganic dissolved ions are a component of total dissolved solids, an indicator of water quality in the world. High levels of atmospheric anions can produce a relaxation effect in animals by decreasing activity in neural and muscular tissue. This atmospheric effect has been reported to reduce anxiety and manic symptoms .

Negative 'Ions' and Air Ionisers

Many manufacturers sell devices that release 'negative ions' into the air, claiming that a higher concentration of negative ions will make a room feel less 'stuffy'. Some also claim health benefits such as relieving asthma and depression.

The 'ions' referred to are in fact charged oxygen or nitrogen molecules surrounded by a cluster of water molecules, rather than ions. Scientific studies have shown no particular benefit from a greater concentration of negative ions. <- Whoever the hell write this should also consider reading this http://www.peakpureair.com/negative_ions.htm

Negative air ionization can reduce the concentration of bioaerosols and dust particles in the air by causing them to bond, forming larger particles and thus falling out of the air. This may help reduce infection due to airborne contamination. Ionization was shown to reduce transmission of the Newcastle Disease Virus in an experiment with chickens.

Common ions

Common Cations Common Name Formula Historic Name Simple Cations Aluminium Al3+ Barium Ba2+ Beryllium Be2+ Caesium Cs+ Calcium Ca2+ Chromium(II) Cr2+ Chromous Chromium(III) Cr3+ Chromic Chromium(VI) Cr6+ Chromyl Cobalt(II) Co2+ Cobaltous Cobalt(III) Co3+ Cobaltic Copper(I) Cu+ Cuprous Copper(II) Cu2+ Cupric Copper(III) Cu3+ Gallium Ga3+ Helium He2+ (Alpha particle) Hydrogen H+ (Proton) Iron(II) Fe2+ Ferrous Iron(III) Fe3+ Ferric Lead(II) Pb2+ Plumbous Lead(IV) Pb4+ Plumbic Lithium Li+ Magnesium Mg2+ Manganese(II) Mn2+ Manganous Manganese(III) Mn3+ Manganic Manganese(IV) Mn4+ Manganyl Manganese(VII) Mn7+ Mercury(II) Hg2+ Mercuric Nickel(II) Ni2+ Nickelous Nickel(III) Ni3+ Nickelic Potassium K+ Silver Ag+ Sodium Na+ Strontium Sr2+ Tin(II) Sn2+ Stannous Tin(IV) Sn4+ Stannic Zinc Zn2+ Polyatomic Cations Ammonium NH4+ Hydronium H3O+ Nitronium NO2+ Uranyl UO22+ Mercury(I) Hg22+ Mercurous

Common Anions Formal Name Formula Alt. Name Simple Anions Arsenide As3− Azide N3− Bromide Br− Chloride Cl− Fluoride F− Hydride H− Iodide I− Nitride N3− Oxide O2− Phosphide P3− Sulfide S2− Peroxide O22− Oxoanions Arsenate AsO43− Arsenite AsO33− Borate BO33− Bromate BrO3− Hypobromite BrO− Carbonate CO32− Hydrogen carbonate HCO3− Bicarbonate Hydroxide OH− Chlorate ClO3− Perchlorate ClO4− Chlorite ClO2− Hypochlorite ClO− Chromate CrO42− Dichromate Cr2O72− Iodate IO3− Nitrate NO3− Nitrite NO2− Phosphate PO43− Hydrogen phosphate HPO42− Dihydrogen phosphate H2PO4− Permanganate MnO4− Phosphite PO33− Sulfate SO42− Thiosulfate S2O32− Hydrogen sulfate HSO4− Bisulfate Sulfite SO32− Hydrogen sulfite HSO3− Bisulfite Anions from Organic Acids Acetate C2H3O2− Formate HCO2− Oxalate C2O42− Hydrogen oxalate HC2O4− Bioxalate Other Anions hydrosulfide HS− Bisulfide Telluride Te2− Amide NH2− Cyanate OCN− Thiocyanate SCN− Cyanide CN−

External links

• Department of Education, Newfoundland and Labrador-Canada "Template:PDFlink". A Periodic table reporting ionic charges for every chemical element.