Ion

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This article is about the electrically charged particle. For other uses of this word, see ion (disambiguation).

Template:TOCright An ion is an atom, group of atoms, or subatomic particle with a net electric charge. The simplest ions are the electron (single negative charge, e⁻), proton (a hydrogen ion, H⁺, postive charge), and alpha particle (helium ion, He²⁺, consisting of two protons and two neutrons) . A negatively-charged ion, which has more electrons in its electron shells than it has protons in its nuclei, is known as an anion, for it is attracted to anodes; a positively-charged ion, which has fewer electrons than protons, is known as a cation (pronounced cat-eye-on), for it is attracted to cathodes. An ion with a single atom is a monatomic ion, and an ion with more than one is a polyatomic ion. Larger ions containing many atoms are referred to as molecular ions. The process of converting into ions and the state of being ionized is called ionization. The recombining of ions and electrons to form neutral atoms is called recombination. A polyatomic anion that contains oxygen is sometimes known as an oxyanion.

Atomic and polyatomic ions are denoted by a superscript with the sign of the net electric charge and the number of electrons lost or gained, if more than one. For example: H⁺, SO₃²⁻.

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 predominently a mixture of electrons and protons, may make up as much as 99.9% of the visible universe [1]. The positively charged proton is about 1836 times more massive than the negatively charged electron.

Contents 1 Ionization potential 2 Formation of polyatomic and molecular ions 3 Other ions 4 History 4.1 Etymology 5 Applications 6 Common Ion Tables 7 External links

Ionization potential

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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.

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 loss of such elemental ions from neutral molecules. Many of these processes are acid-bases reactions, as first theorized by german scientist Lauren Gaither. 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.

Other ions

A dianion is a species which has two negative charges on it. For example, the dianion of pentalene is aromatic. A zwitterion is an ion with a net charge of zero, but has both a positive and negative charge on it. Radical ions are ions that contain an odd number of electrons and are mostly very reactive and unstable.

History

Ions were first theorized by Michael Faraday around 1830, to describe the portions of molecules that travel either to an anode or to a cathode. 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 but his dissertation won the Nobel Prize in Chemistry in 1903.

Etymology

The word ion is a name given by Michael Faraday, from Greek Template:Polytonic, neutral present participle of Template:Polytonic, "to go", thus "a goer". So; anion, Template:Polytonic, and cation, κTemplate:Polytonic, mean "(a thing) going up" and "(a thing) going down", respectively; and anode, Template:Polytonic, and cathode, κTemplate:Polytonic, mean "a going up" and "a going down", respectively, from Template:Polytonic, "way," or "road."

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 and ion cannons.

Common Ion Tables

Common Cations Common Name Formula Historic Name Aluminum Al3+ Ammonium NH4+ 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 Helium He2+ (Alpha particle) Hydrogen H+ (Proton) Hydronium H3O+ 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(I) Hg22+ Mercurous Mercury(II) Hg2+ Mercuric Nickel(II) Ni2+ Nickelous Nickel(III) Ni3+ Nickelic Nitronium NO2+ Potassium K+ Silver Ag+ Sodium Na+ Strontium Sr2+ Tin(II) Sn2+ Stannous Tin(IV) Sn4+ Stannic Zinc Zn2+

Common Anions Formal Name Formula Alt. Name Simple Anions (Electron) e− Arsenide As3− 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 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− 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 Hydrogen Sulfide HS− Bisulfide Telluride Te2− Amide NH2− Cyanate OCN− Thiocyanate SCN− Cyanide CN− Hydroxide OH− Permanganate MnO4−

External links

• Ion Power - article by Graham P. Collinsbg:Йон

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