Ion

"Cation and Anion" redirects here. For the particle physics/quantum computing concept, see Anyon. For other uses, see Ion (disambiguation). Hydrogen atom (center) contains a single proton and a single electron. Removal of the electron gives a cation (left), whereas addition of an electron gives an anion (right). The hydrogen anion, with its loosely held two-electron cloud, has a larger radius than the neutral atom, which in turn is much larger than the bare proton of the cation. Hydrogen forms the only cation that has no electrons, but even cations that (unlike hydrogen) still retain one or more electrons, are still smaller than the neutral atoms or molecules from which they are derived. An ion is an atom or molecule in which the total number of electrons is not equal to the total number of protons, giving it a net positive or negative electrical charge. The name was given by physicist Michael Faraday for the substances that allow a current to pass ("go") between electrodes in a solution, when an electric field is applied. It is from Greek ιον, meaning "going." The word ion also is responsible for electrical current being symbolized by the letter i in chemistry and physics. An anion (pronounced /ˈæn.aɪ.ən/ AN-eye-ən), from the Greek word ἄνω (ánō), meaning "up", is an ion with more electrons than protons, giving it a net negative charge (since electrons are negatively charged and protons are positively charged). Conversely, a cation (pronounced /ˈkæt.aɪ.ən/ KAT-eye-ən), from the Greek word κατά (katá), meaning "down", is an ion with fewer electrons than protons, giving it a positive charge. Since the charge on a proton is equal in magnitude to the charge on an electron, the net charge on an ion is equal to the number of protons in the ion minus the number of electrons. An ion consisting of a single atom is an atomic or monatomic ion; if it consists of two or more atoms, it is a molecular or polyatomic ion. Contents 1 General 1.1 History and Discovery 1.2 Characteristics 1.3 Natural Occurrences 1.3.1 Astronomical 1.3.2 Terrestrial 1.3.3 Biological 1.4 Related Technology 1.5 Portrayal in Literature and Media 2 Chemistry 2.1 Notation 2.1.1 Denoting the charged state 2.1.2 Sub-classes 2.2 Formation 2.2.1 Formation of monatomic ions 2.2.2 Formation of polyatomic and molecular ions 2.2.3 Ionization potential 2.3 Ionic bonding 2.4 Chemical Applications 2.4.1 Mass Spectroscopy 2.4.2 Catalysis 2.4.2.1 Transition Metal Ions Catalysis 2.4.2.2 Templated Synthesis of Organic Compounds 2.5 Common ions 3 See also 4 References // General This section requires expansion. History and Discovery Etymologically the word ion is the Greek ιον (going), the present participle of ιεναι, ienai, "to go." This term was introduced by English physicist and chemist Michael Faraday in 1834 for the (then unknown) species that goes from one electrode to the other through an aqueous medium.12 Faraday did not know the nature of these species, but he knew that since metals disolved into and entered solution at one electrode, and new metal came forth from solution at the other electrode, that some kind of substance moved through the solution in a current, conveying matter from one place to the other. Faraday also introduced the words anion and cation. In Faraday's nomenclature, cations were named because they were attracted to the cathode in a galvanic device and anions were named due to their attraction to the cathode. (For the origin of these names in turn, see the accompanying linked articles). Characteristics Ions in their gas-like state are highly reactive, and not present in large amounts in the daily environment of Earth (their major occurance is is flames, lightning and electrical sparks, and other plasmas). These gas-like ions rapidly interact with ions of opposite charge to give neutral molecules or ionic salts. Ions are also produced in the liquid or solid state whatn salts interact with solvents (for example, water) to produce "solvated ions," which are more stable, for reasons involving a combination of energy and entropy changes as the ions move away from each other to interact with the liquid. These stabilized species are more commonly found in the environment at low temperatures. A common example is the ions present in seawater, which are derived from the disolved salts there. All ions are charged, which means that like all charged objects they are: attracted to opposite electric charges (positive to negative, and vice versa), repelled by like charges, and when moving, travel in trajectories that are deflected by a magnetic field. Electrons (due to their smaller mass and thus larger space-filling properties as matter waves determine the size of atoms and molecules that possess any electrons at all. Thus, anions (negatively charged ions) are larger than the parent molecule or atom, as the excess electron(s) repell each other, and add to the physical size of the ion, because its size is determined by its electron cloud. Conversely, cations are generally smaller than the corresponding parent atom or molecule, for the same reason. One particular cation (that of hydrogen) contains no electrons, and thus is very much smaller than the parent hydrogen atom. Natural Occurrences Ions are ubiquitous in nature and are responsible for diverse phenomena from the luminescence of the Sun, and the existence of ionosphere on Earth. Atoms in their ionic state may have a different color from neutral atoms, and thus light absorption by metal ions gives the color of gemstones. In both inorganic and organic chemistry (including biochemistry), the interaction of water and ions is extremely important (an example is the energy that drives breakdown of ATP. The following sections describe contexts in which ions feature prominently and are arranged in decreasing physical length-scale, from the astronomical to the microscopic. Astronomical The remnant of "Tycho's Supernova", a huge ball of expanding plasma. The outer shell shown in blue is X-ray emission by high-speed electrons. 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. >99.9% of visible matter in the Universe may be in the form of plasmas.3 These include our Sun and other stars, the space between planets, as well as the space in between stars. Plasmas are often called the fourth state of matter because its properties are substantially different from solids, liquids, and gases. Astrophysical plasmas containing predominantly a mixture of electrons and protons (ionized hydrogen). Terrestrial ionosphere, salinity and ionic composition of water Biological ion gradient across membrane, co-factors and catalysis Related Technology Ions can be non-chemically prepared using various ion sources, usually involving high voltage or temperature. These are used in a multitude of devices such as mass spectrometers, optical emission spectrometers, particle accelerators, ion implanters and ion engines. As reactive charged particles, they are also used in air purification by disrupting microbes, and in household items such as smoke detectors. As signaling and metabolism in organisms are controlled by a precise ionic gradient across membranes, the disruption of this gradient contributes to cell death. This is a common mechanism exploited by natural and artificial biocides, including the ion channels gramicidin and amphotericin (a fungicide). Inorganic dissolved ions are a component of total dissolved solids, an indicator of water quality in the world. Portrayal in Literature and Media Chemistry Notation Denoting the charged state Equivalent notations for an iron atom (Fe) that lost two electrons. When writing the chemical formula for an ion, its net charge is written in superscript immediately after the chemical structure for the molecule/atom. The net charge is written with the magnitude before the sign; that is, a doubly charged cation is indicated as 2+ instead of +2. Conventionally the magnitude of the charge is omitted for singly charged molecules/atoms; for example, the sodium cation is indicated as Na+ and not Na1+. An alternative (and acceptable) way of showing a molecule/atom with multiple charges is by drawing out the signs multiple times; this is often seen with transition metals. Chemists sometimes circle the sign; this is merely ornamental and does not alter the chemical meaning. All three representations of Fe2+ shown in the figure are thus equivalent. Mixed Roman numerals and charge notations for the uranyl ion. The oxidation state of the metal is shown as superscripted Roman numerals, whereas the charge of the entire complex is shown by the angle symbol together with the magnitude and sign of the net charge. Monatomic ions are sometimes also denoted with Roman numerals; for example, the Fe2+ example seen above is occasionally referred to as Fe(II) or FeII. The Roman numeral designates the formal oxidation state of an element, whereas the superscripted numerals denotes the net charge. The two notations are therefore exchangeable for monatomic ions, but the Roman numerals cannot be applied to polyatomic ions. It is however possible to mix the notations for the individual metal center with a polyatomic complex, as shown by the uranyl ion example. Sub-classes If an ion contains unpaired electrons, it is called a radical ion. Just like uncharged radicals, radical ions are very reactive. Polyatomic ions containing oxygen, such as carbonate and sulfate, are called oxyanions. Molecular ions that contain at least one carbon to hydrogen bond are called organic ions. If the charge in an organic ion is formally centered on a carbon, it is termed a carbocation (if positively charged) or carboanion (if negatively charged). Formation Formation of monatomic ions Monatomic ions are formed by the addition of electrons to the valence shell of the atom, which is the outer-most electron shell in an atom, or the losing of electrons from this shell. The inner shells of an atom are filled with electrons that are tightly bound to the positively charged atomic nucleus, and so do not participate in this kind of chemical interaction. The process of gaining or losing electrons from a neutral atom or molecule is called ionization. Atoms can be ionized by bombardment with radiation, but the more usual process of ionization encountered in chemistry is the transfer of electrons between atoms or molecules. This transfer is usually driven by the attaining of stable ("closed shell") electronic configurations. Atoms will gain or lose electrons depending on which action takes the least energy. For example, a sodium atom, Na, has a single electron in its valence shell, surrounding 2 stable, filled inner shells of 2 and 8 electrons. Since these filled shells are very stable, a sodium atom tends to lose its extra electron and attain this stable configuration, becoming a sodium cation in the process Na → Na+ + e− On the other hand, a chlorine atom, Cl, has 7 electrons in its valence shell, which is one short of the stable, filled shell with 8 electrons. Thus, a chlorine atom tends to gain an extra electron and attain a stable 8-electron configuration, becoming a chloride anion in the process: Cl + e− → Cl− This driving force is what causes sodium and chlorine to undergo a chemical reaction, where the "extra" electron is transferred from sodium to chlorine, forming sodium cations and chloride anions. Being oppositely charged, these cations and anions form ionic bonds and combine together to form sodium chloride, NaCl, more commonly known as rock salt. Na+ + Cl− → NaCl Formation of polyatomic and molecular ions An electrostatic potential map of the nitrate ion (NO− 3). The 3-dimensional shell represents a single arbitrary isopotential. Polyatomic and molecular ions are often formed by the gaining or losing of elemental ions such as H+ in neutral molecules. For example, when ammonia, NH3, accepts a proton, H+, it forms the ammonium ion, NH+ 4. Ammonia and ammonium have the same number of electrons in essentially the same electronic configuration, but ammonium has an extra proton that gives it a net positive charge. Ammonia can also lose an electron to gain a positive charge, forming the ion ·NH+ 3. However, this ion is unstable, because it has an incomplete valence shell around the nitrogen atom, making it a very reactive radical ion. Due to the instability of radical ions, polyatomic and molecular ions are usually formed by gaining or losing elemental ions such as H+, rather than gaining or losing electrons. This allows the molecule to preserve its stable electronic configuration while acquiring an electrical charge. 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−. Caesium has the lowest measured ionization energy of all the elements and helium has the greatest.4 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. Ionic bonding Main article: Ionic bond Ionic bonding is a kind of chemical bonding that arises from the mutual attraction of oppositely charged ions. Since ions of like charge repel each other, they do not usually exist on their own. Instead, many of them may form a crystal lattice, in which ions of opposite charge are bound to each other. The resulting compound is called an ionic compound, and is said to be held together by ionic bonding. In ionic compounds there arise characteristic distances between ion neighbors from which the spatial extension and the ionic radius of individual ions may be derived. The most common type of ionic bonding is seen in compounds of metals and nonmetals (except noble gases, which rarely form chemical compounds). Metals are characterized by having a small number of electrons in excess of a stable, closed-shell electronic configuration. As such, they have the tendency to lose these extra electrons in order to attain a stable configuration. This property is known as electropositivity. Non-metals, on the other hand, are characterized by having an electron configuration just a few electrons short of a stable configuration. As such, they have the tendency to gain more electrons in order to achieve a stable configuration. This tendency is known as electronegativity. When a highly electropositive metal is combined with a highly electronegative nonmetal, the extra electrons from the metal atoms are transferred to the electron-deficient nonmetal atoms. This reaction produces metal cations and nonmetal anions, which are attracted to each other to form a salt. Chemical Applications This section requires expansion. Gas-like ions and solvated ions both have tremendous impact on chemical analysis and synthesis. Mass Spectroscopy Catalysis Transition Metal Ions Catalysis Templated Synthesis of Organic Compounds Common ions Common Cations Common Name Formula Historic Name Simple Cations Aluminium Al3+ Calcium Ca2+ Copper(II) Cu2+ cupric Hydrogen H+ Iron(II) Fe2+ ferrous Iron(III) Fe3+ ferric Magnesium Mg2+ Mercury(II) Hg2+ mercuric Potassium K+ kalic Silver Ag+ Sodium Na+ natric Polyatomic Cations Ammonium NH+ 4 Oxonium H3O+ hydronium Mercury(I) Hg2+ 2 mercurous Common Anions Formal Name Formula Alt. Name Simple Anions Chloride Cl− Fluoride F− Oxide O2− Oxoanions Carbonate CO2− 3 Hydrogen carbonate HCO− 3 bicarbonate Hydroxide OH− Nitrate NO− 3 Phosphate PO3− 4 Sulfate SO2− 4 Anions from Organic Acids Acetate CH3COO− ethanoate Formate HCOO− methanoate Oxalate C2O2− 4 ethandioate Cyanide CN− See also Air ionizer Anode Cathode Ion beam Ion source Ionic radius Auroras References ^ BBC - Michael Faraday. UK: BBC. http://www.bbc.co.uk/history/historic_figures/faraday_michael.shtml.  ^ "Online etymology dictionary". http://www.etymonline.com/index.php?term=ion. Retrieved 2011-01-07.  ^ Plasma, Plasma, Everywhere Science@NASA Headline news, Space Science n° 158, September 7, 1999. ^ http://www.lenntech.com/Periodic-chart-elements/ionization-energy.htm Chemical elements listed by ionization energy This article needs additional citations for verification. Please help improve this article by adding reliable references. Unsourced material may be challenged and removed. (December 2007) v · d · eGalvanic cells Non-rechargeable: primary cells Alkaline battery · Aluminium battery · Bunsen cell · Chromic acid cell · Clark cell · Daniell cell · Dry cell · Grove cell · Leclanché cell · Lithium battery · Mercury battery · Nickel oxyhydroxide battery · Silver-oxide battery · Weston cell · Zamboni pile · Zinc–air battery · Zinc–carbon battery · Zinc–chloride battery Rechargeable: secondary cells Lead–acid battery · Lead-acid battery (gel) · Lithium air battery · Lithium-ion battery · Lithium-ion polymer battery · Lithium iron phosphate battery · Lithium sulfur battery · Lithium-titanate battery · Nickel-cadmium battery · Nickel hydrogen battery · Nickel-iron battery · Nickel-lithium battery · Nickel-metal hydride battery · Low self-discharge NiMH battery · Nickel-zinc battery · Rechargeable alkaline battery · Sodium-sulfur battery · Vanadium redox battery · Zinc-bromine battery Kinds of cells Battery · Concentration cell · Flow battery · Fuel cell · Trough battery · Voltaic pile Parts of cells Anode · Catalyst · Cathode · Electrolyte · Half cell · Ions · Salt bridge