Как пишется марганец в таблице менделеева

Not to be confused with Magnesium (Mg).

Manganese, ₂₅Mn

Pure manganese cube and oxidized manganese chips
Manganese
Pronunciation	​(MANG-gə-neez)
Appearance	silvery metallic
Standard atomic weight Ar°(Mn)	54.938043±0.000002 54.938±0.001 (abridged)[1]
Manganese in the periodic table
Hydrogen Helium Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson – ↑ Mn ↓ Tc chromium ← manganese → iron
Atomic number (Z)	25
Group	group 7
Period	period 4
Block	d-block
Electron configuration	[Ar] 3d5 4s2
Electrons per shell	2, 8, 13, 2
Physical properties
Phase at STP	solid
Melting point	1519 K ​(1246 °C, ​2275 °F)
Boiling point	2334 K ​(2061 °C, ​3742 °F)
Density (near r.t.)	7.21 g/cm3
when liquid (at m.p.)	5.95 g/cm3
Heat of fusion	12.91 kJ/mol
Heat of vaporization	221 kJ/mol
Molar heat capacity	26.32 J/(mol·K)
Vapor pressure P (Pa) 1 10 100 1 k 10 k 100 k at T (K) 1228 1347 1493 1691 1955 2333
Atomic properties
Oxidation states	−3, −2, −1, 0, +1, +2, +3, +4, +5, +6, +7 (depending on the oxidation state, an acidic, basic, or amphoteric oxide)
Electronegativity	Pauling scale: 1.55
Ionization energies	1st: 717.3 kJ/mol 2nd: 1509.0 kJ/mol 3rd: 3248 kJ/mol (more)
Atomic radius	empirical: 127 pm
Covalent radius	Low spin: 139±5 pm High spin: 161±8 pm
Spectral lines of manganese
Other properties
Natural occurrence	primordial
Crystal structure	​body-centered cubic (bcc)
Speed of sound thin rod	5150 m/s (at 20 °C)
Thermal expansion	21.7 µm/(m⋅K) (at 25 °C)
Thermal conductivity	7.81 W/(m⋅K)
Electrical resistivity	1.44 µΩ⋅m (at 20 °C)
Magnetic ordering	paramagnetic
Molar magnetic susceptibility	(α) +529.0×10−6 cm3/mol (293 K)[2]
Young’s modulus	198 GPa
Bulk modulus	120 GPa
Mohs hardness	6.0
Brinell hardness	196 MPa
CAS Number	7439-96-5
History
Discovery	Carl Wilhelm Scheele (1774)
First isolation	Johann Gottlieb Gahn (1774)
Main isotopes of manganese v e
Iso­tope Decay abun­dance half-life (t1/2) mode pro­duct 52Mn syn 5.6 d ε 52Cr β+ 52Cr γ – 53Mn trace 3.74×106 y ε 53Cr 54Mn syn 312 d ε 54Cr γ – 55Mn 100% stable
Category: Manganese view talk edit | references

Manganese is a chemical element with the symbol Mn and atomic number 25. It is a hard, brittle, silvery metal, often found in minerals in combination with iron. Manganese is a transition metal with a multifaceted array of industrial alloy uses, particularly in stainless steels. It improves strength, workability, and resistance to wear. Manganese oxide is used as an oxidising agent; as a rubber additive; and in glass making, fertilisers, and ceramics. Manganese sulfate can be used as a fungicide.

Manganese is also an essential human dietary element, important in macronutrient metabolism, bone formation, and free radical defense systems. It is a critical component in dozens of proteins and enzymes.^[3] It is found mostly in the bones, but also the liver, kidneys, and brain.^[4] In the human brain, the manganese is bound to manganese metalloproteins, most notably glutamine synthetase in astrocytes.

Manganese was first isolated in 1774. It is familiar in the laboratory in the form of the deep violet salt potassium permanganate. It occurs at the active sites in some enzymes.^[5] Of particular interest is the use of a Mn-O cluster, the oxygen-evolving complex, in the production of oxygen by plants.

Characteristics[edit]

Physical properties[edit]

Manganese is a silvery-gray metal that resembles iron. It is hard and very brittle, difficult to fuse, but easy to oxidize.^[6] Manganese metal and its common ions are paramagnetic.^[7] Manganese tarnishes slowly in air and oxidizes («rusts») like iron in water containing dissolved oxygen.

Isotopes[edit]

Naturally occurring manganese is composed of one stable isotope, ⁵⁵Mn. Several radioisotopes have been isolated and described, ranging in atomic weight from 44 u (⁴⁴Mn) to 69 u (⁶⁹Mn). The most stable are ⁵³Mn with a half-life of 3.7 million years, ⁵⁴Mn with a half-life of 312.2 days, and ⁵²Mn with a half-life of 5.591 days. All of the remaining radioactive isotopes have half-lives of less than three hours, and the majority of less than one minute. The primary decay mode in isotopes lighter than the most abundant stable isotope, ⁵⁵Mn, is electron capture and the primary mode in heavier isotopes is beta decay.^[8] Manganese also has three meta states.^[8]

Manganese is part of the iron group of elements, which are thought to be synthesized in large stars shortly before the supernova explosion.^{[9] 53}Mn decays to ⁵³Cr with a half-life of 3.7 million years. Because of its relatively short half-life, ⁵³Mn is relatively rare, produced by cosmic rays impact on iron.^[10] Manganese isotopic contents are typically combined with chromium isotopic contents and have found application in isotope geology and radiometric dating. Mn–Cr isotopic ratios reinforce the evidence from ²⁶Al and ¹⁰⁷Pd for the early history of the Solar System. Variations in ⁵³Cr/⁵²Cr and Mn/Cr ratios from several meteorites suggest an initial ⁵³Mn/⁵⁵Mn ratio, which indicate that Mn–Cr isotopic composition must result from in situ decay of ⁵³Mn in differentiated planetary bodies. Hence, ⁵³Mn provides additional evidence for nucleosynthetic processes immediately before coalescence of the Solar System.

Chemical compounds[edit]

Common oxidation states of manganese are +2, +3, +4, +6, and +7, although all oxidation states from −3 to +7 have been observed. Manganese in oxidation state +7 is represented by salts of the intensely purple permanganate anion MnO₄⁻. Potassium permanganate is a commonly used laboratory reagent because of its oxidizing properties; it is used as a topical medicine (for example, in the treatment of fish diseases). Solutions of potassium permanganate were among the first stains and fixatives to be used in the preparation of biological cells and tissues for electron microscopy.^[12]

Aside from various permanganate salts, Mn(VII) is represented by the unstable, volatile derivative Mn₂O₇. Oxyhalides (MnO₃F and MnO₃Cl) are powerful oxidizing agents.^[6] The most prominent example of Mn in the +6 oxidation state is the green anion manganate, [MnO₄]^2-. Manganate salts are intermediates in the extraction of manganese from its ores. Compounds with oxidation states +5 are somewhat elusive, one example is the blue anion hypomanganate [MnO₄]^3-.

Compounds with Mn in oxidation state +5 are rarely encountered and often found associated with an oxide (O^2-) or nitride (N^3-) ligand.^[13][14]

Mn(IV) is somewhat enigmatic because it is common in nature but far rarer in synthetic chemistry. The most common Mn ore, pyrolusite, is MnO₂. It is the dark brown pigment of many cave drawings but is also a common ingredient in dry cell batteries. Complexes of Mn(IV) are well known, but they require elaborate ligands. Mn(IV)-OH complexes are an intermediate in some enzymes, including the oxygen evolving center (OEC) in plants.^[15]

Simple derivatives Mn⁺³ are rarely encountered but can be stabilized by suitably basic ligands. Manganese(III) acetate is an oxidant useful in organic synthesis. Solid compounds of manganese(III) are characterized by its strong purple-red color and a preference for distorted octahedral coordination resulting from the Jahn-Teller effect.

A particularly common oxidation state for manganese in aqueous solution is +2, which has a pale pink color. Many manganese(II) compounds are known, such as the aquo complexes derived from manganese(II) sulfate (MnSO₄) and manganese(II) chloride (MnCl₂). This oxidation state is also seen in the mineral rhodochrosite (manganese(II) carbonate). Manganese(II) commonly exists with a high spin, S = 5/2 ground state because of the high pairing energy for manganese(II). There are no spin-allowed d–d transitions in manganese(II), which explain its faint color.^[16]

Oxidation states of manganese[17]
0	Mn 2(CO) 10
+1	MnC 5H 4CH 3(CO) 3
+2	MnCl 2, MnCO 3, MnO
+3	MnF 3, Mn(OAc) 3, Mn 2O 3
+4	MnO 2
+5	K 3MnO 4
+6	K 2MnO 4
+7	KMnO 4, Mn 2O 7
Common oxidation states are in bold.

Organomanganese compounds[edit]

Manganese forms a large variety of organometallic derivatives, i.e., compounds with Mn-C bonds. The organometallic derivatives include numerous examples of Mn in its lower oxidation states, i.e. Mn(-III) up through Mn(I). This area of organometallic chemistry is attractive because Mn is inexpensive and of relatively low toxicity.

Of greatest commercial interest is «MMT», methylcyclopentadienyl manganese tricarbonyl, which is used as an anti-knock compound added to gasoline (petrol) in some countries. It features Mn(I). Consistent with other aspects of Mn(II) chemistry, manganocene (Mn(C₅H₅)₂) is high-spin. In contrast, its neighboring metal iron forms an air-stable, low-spin derivative in the form of ferrocene (Fe(C₅H₅)₂). When conducted under an atmosphere of carbon monoxide, reduction of Mn(II) salts gives dimanganese decacarbonyl Mn₂(CO)₁₀, an orange and volatile solid. The air-stability of this Mn(0) compound (and its many derivatives) reflects the powerful electron-acceptor properties of carbon monoxide. Many alkene complexes and alkyne complexes are derived from Mn₂(CO)₁₀.

In Mn(CH₃)₂(dmpe)₂, Mn(II) is low spin, which contrasts with the high spin character of its precursor, MnBr₂(dmpe)₂ (dmpe = (CH₃)₂PCH₂CH₂P(CH₃)₂).^[18] Polyalkyl and polyaryl derivatives of manganese often exist in higher oxidation states, reflecting the electron-releasing properties of alkyl and aryl ligands. One example is [Mn(CH₃)₆]^2-.

History[edit]

The origin of the name manganese is complex. In ancient times, two black minerals were identified from the regions of the Magnetes (either Magnesia, located within modern Greece, or Magnesia ad Sipylum, located within modern Turkey).^[19]
They were both called magnes from their place of origin, but were considered to differ in sex. The male magnes attracted iron, and was the iron ore now known as lodestone or magnetite, and which probably gave us the term magnet. The female magnes ore did not attract iron, but was used to decolorize glass. This female magnes was later called magnesia, known now in modern times as pyrolusite or manganese dioxide.^{[citation needed]} Neither this mineral nor elemental manganese is magnetic. In the 16th century, manganese dioxide was called manganesum (note the two Ns instead of one) by glassmakers, possibly as a corruption and concatenation of two words, since alchemists and glassmakers eventually had to differentiate a magnesia nigra (the black ore) from magnesia alba (a white ore, also from Magnesia, also useful in glassmaking). Michele Mercati called magnesia nigra manganesa, and finally the metal isolated from it became known as manganese (German: Mangan). The name magnesia eventually was then used to refer only to the white magnesia alba (magnesium oxide), which provided the name magnesium for the free element when it was isolated much later.^[20]

Manganese dioxide, which is abundant in nature, has long been used as a pigment. The cave paintings in Gargas that are 30,000 to 24,000 years old are made from the mineral form of MnO₂ pigments.^[22]

Manganese compounds were used by Egyptian and Roman glassmakers, either to add to, or remove, color from glass.^[23] Use as «glassmakers soap» continued through the Middle Ages until modern times and is evident in 14th-century glass from Venice.^[24]

Because it was used in glassmaking, manganese dioxide was available for experiments by alchemists, the first chemists. Ignatius Gottfried Kaim (1770) and Johann Glauber (17th century) discovered that manganese dioxide could be converted to permanganate, a useful laboratory reagent.^[25] By the mid-18th century, the Swedish chemist Carl Wilhelm Scheele used manganese dioxide to produce chlorine. First, hydrochloric acid, or a mixture of dilute sulfuric acid and sodium chloride was made to react with manganese dioxide, and later hydrochloric acid from the Leblanc process was used and the manganese dioxide was recycled by the Weldon process. The production of chlorine and hypochlorite bleaching agents was a large consumer of manganese ores.

Scheele and others were aware that pyrolusite (mineral form of manganese dioxide) contained a new element. Johan Gottlieb Gahn was the first to isolate an impure sample of manganese metal in 1774, which he did by reducing the dioxide with carbon.

The manganese content of some iron ores used in Greece led to speculations that steel produced from that ore contains additional manganese, making the Spartan steel exceptionally hard.^[26] Around the beginning of the 19th century, manganese was used in steelmaking and several patents were granted. In 1816, it was documented that iron alloyed with manganese was harder but not more brittle. In 1837, British academic James Couper noted an association between miners’ heavy exposure to manganese and a form of Parkinson’s disease.^[27] In 1912, United States patents were granted for protecting firearms against rust and corrosion with manganese phosphate electrochemical conversion coatings, and the process has seen widespread use ever since.^[28]

The invention of the Leclanché cell in 1866 and the subsequent improvement of batteries containing manganese dioxide as cathodic depolarizer increased the demand for manganese dioxide. Until the development of batteries with nickel-cadmium and lithium, most batteries contained manganese. The zinc–carbon battery and the alkaline battery normally use industrially produced manganese dioxide because naturally occurring manganese dioxide contains impurities. In the 20th century, manganese dioxide was widely used as the cathodic for commercial disposable dry batteries of both the standard (zinc–carbon) and alkaline types.^[29]

Occurrence[edit]

Manganese comprises about 1000 ppm (0.1%) of the Earth’s crust, the 12th most abundant of the crust’s elements.^[4] Soil contains 7–9000 ppm of manganese with an average of 440 ppm.^[4] The atmosphere contains 0.01 μg/m³.^[4] Manganese occurs principally as pyrolusite (MnO₂), braunite (Mn²⁺Mn³⁺₆)SiO₁₂),^[30] psilomelane (Ba,H₂O)₂Mn₅O₁₀, and to a lesser extent as rhodochrosite (MnCO₃).

Manganese ore	Psilomelane (manganese ore)	Spiegeleisen is an iron alloy with a manganese content of approximately 15%	Manganese oxide dendrites on limestone from Solnhofen, Germany – a kind of pseudofossil. Scale is in mm	Mineral rhodochrosite (manganese(II) carbonate)

The most important manganese ore is pyrolusite (MnO₂). Other economically important manganese ores usually show a close spatial relation to the iron ores, such as sphalerite.^[6][32] Land-based resources are large but irregularly distributed. About 80% of the known world manganese resources are in South Africa; other important manganese deposits are in Ukraine, Australia, India, China, Gabon and Brazil.^[31] According to 1978 estimate, the ocean floor has 500 billion tons of manganese nodules.^[33] Attempts to find economically viable methods of harvesting manganese nodules were abandoned in the 1970s.^[34]

In South Africa, most identified deposits are located near Hotazel in the Northern Cape Province, with a 2011 estimate of 15 billion tons. In 2011 South Africa produced 3.4 million tons, topping all other nations.^[35]

Manganese is mainly mined in South Africa, Australia, China, Gabon, Brazil, India, Kazakhstan, Ghana, Ukraine and Malaysia.^[36]

Production[edit]

For the production of ferromanganese, the manganese ore is mixed with iron ore and carbon, and then reduced either in a blast furnace or in an electric arc furnace.^[37] The resulting ferromanganese has a manganese content of 30 to 80%.^[6] Pure manganese used for the production of iron-free alloys is produced by leaching manganese ore with sulfuric acid and a subsequent electrowinning process.^[38]

A more progressive extraction process involves directly reducing (a low grade) manganese ore by heap leaching. This is done by percolating natural gas through the bottom of the heap; the natural gas provides the heat (needs to be at least 850 °C) and the reducing agent (carbon monoxide). This reduces all of the manganese ore to manganese oxide (MnO), which is a leachable form. The ore then travels through a grinding circuit to reduce the particle size of the ore to between 150 and 250 μm, increasing the surface area to aid leaching. The ore is then added to a leach tank of sulfuric acid and ferrous iron (Fe²⁺) in a 1.6:1 ratio. The iron reacts with the manganese dioxide (MnO₂) to form iron hydroxide (FeO(OH)) and elemental manganese (Mn):

This process yields approximately 92% recovery of the manganese. For further purification, the manganese can then be sent to an electrowinning facility.^[39]

In 1972 the CIA’s Project Azorian, through billionaire Howard Hughes, commissioned the ship Hughes Glomar Explorer with the cover story of harvesting manganese nodules from the sea floor.^[40] That triggered a rush of activity to collect manganese nodules, which was not actually practical. The real mission of Hughes Glomar Explorer was to raise a sunken Soviet submarine, the K-129, with the goal of retrieving Soviet code books.^[41]

An abundant resource of manganese in the form of Mn nodules found on the ocean floor.^[42][43] These nodules, which are composed of 29% manganese,^[44] are located along the ocean floor and the potential impact of mining these nodules is being researched. Physical, chemical, and biological environmental impacts can occur due to this nodule mining disturbing the seafloor and causing sediment plumes to form. This suspension includes metals and inorganic nutrients, which can lead to contamination of the near-bottom waters from dissolved toxic compounds. Mn nodules are also the grazing grounds, living space, and protection for endo- and epifaunal systems. When theses nodules are removed, these systems are directly affected. Overall, this can cause species to leave the area or completely die off.^[45] Prior to the commencement of the mining itself, research is being conducted by United Nations affiliated bodies and state-sponsored companies in an attempt to fully understand environmental impacts in the hopes of mitigating these impacts.^[46]

Oceanic environment[edit]

Many trace elements in the ocean come from metal-rich hydrothermal particles from hydrothermal vents.^[47] Dissolved manganese (dMn) is found throughout the world’s oceans, 90% of which originates from hydrothermal vents.^[48] Particulate Mn develops in buoyant plumes over an active vent source, while the dMn behaves conservatively.^[47] Mn concentrations vary between the water columns of the ocean. At the surface, dMn is elevated due to input from external sources such as rivers, dust, and shelf sediments. Coastal sediments normally have lower Mn concentrations, but can increase due to anthropogenic discharges from industries such as mining and steel manufacturing, which enter the ocean from river inputs. Surface dMn concentrations can also be elevated biologically through photosynthesis and physically from coastal upwelling and wind-driven surface currents. Internal cycling such as photo-reduction from UV radiation can also elevate levels by speeding up the dissolution of Mn-oxides and oxidative scavenging, preventing Mn from sinking to deeper waters.^[49] Elevated levels at mid-depths can occur near mid-ocean ridges and hydrothermal vents. The hydrothermal vents release dMn enriched fluid into the water. The dMn can then travel up to 4,000 km due to the microbial capsules present, preventing exchange with particles, lowing the sinking rates. Dissolved Mn concentrations are even higher when oxygen levels are low. Overall, dMn concentrations are normally higher in coastal regions and decrease when moving offshore.^[49]

Soils[edit]

Manganese occurs in soils in three oxidation states: the divalent cation, Mn²⁺ and as brownish-black oxides and hydroxides containing Mn (III,IV), such as MnOOH and MnO₂. Soil pH and oxidation-reduction conditions affect which of these three forms of Mn is dominant in a given soil. At pH values less than 6 or under anaerobic conditions, Mn(II) dominates, while under more alkaline and aerobic conditions, Mn(III,IV) oxides and hydroxides predominate. These effects of soil acidity and aeration state on the form of Mn can be modified or controlled by microbial activity. Microbial respiration can cause both the oxidation of Mn²⁺ to the oxides, and it can cause reduction of the oxides to the divalent cation.^[50]

The Mn(III,IV) oxides exist as brownish-black stains and small nodules on sand, silt, and clay particles. These surface coatings on other soil particles have high surface area and carry negative charge. The charged sites can adsorb and retain various cations, especially heavy metals (e.g., Cr³⁺, Cu²⁺, Zn²⁺, and Pb²⁺). In addition, the oxides can adsorb organic acids and other compounds. The adsorption of the metals and organic compounds can then cause them to be oxidized while the Mn(III,IV) oxides are reduced to Mn²⁺ (e.g., Cr³⁺ to Cr(VI) and colorless hydroquinone to tea-colored quinone polymers).^[51]

Applications[edit]

Manganese has no satisfactory substitute in its major applications in metallurgy.^[31] In minor applications (e.g., manganese phosphating), zinc and sometimes vanadium are viable substitutes.

Steel[edit]

Manganese is essential to iron and steel production by virtue of its sulfur-fixing, deoxidizing, and alloying properties, as first recognized by the British metallurgist Robert Forester Mushet (1811–1891) who, in 1856, introduced the element, in the form of Spiegeleisen, into steel for the specific purpose of removing excess dissolved oxygen, sulfur, and phosphorus in order to improve its malleability. Steelmaking,^[52] including its ironmaking component, has accounted for most manganese demand, presently in the range of 85% to 90% of the total demand.^[38] Manganese is a key component of low-cost stainless steel.^[53][54] Often ferromanganese (usually about 80% manganese) is the intermediate in modern processes.

Small amounts of manganese improve the workability of steel at high temperatures by forming a high-melting sulfide and preventing the formation of a liquid iron sulfide at the grain boundaries. If the manganese content reaches 4%, the embrittlement of the steel becomes a dominant feature. The embrittlement decreases at higher manganese concentrations and reaches an acceptable level at 8%. Steel containing 8 to 15% of manganese has a high tensile strength of up to 863 MPa.^[55][56] Steel with 12% manganese was discovered in 1882 by Robert Hadfield and is still known as Hadfield steel (mangalloy). It was used for British military steel helmets and later by the U.S. military.^[57]

Aluminium alloys[edit]

Manganese is used in production of alloys with aluminium. Aluminium with roughly 1.5% manganese has increased resistance to corrosion through grains that absorb impurities which would lead to galvanic corrosion.^[58] The corrosion-resistant aluminium alloys 3004 and 3104 (0.8 to 1.5% manganese) are used for most beverage cans.^[59] Before 2000, more than 1.6 million tonnes of those alloys were used; at 1% manganese, this consumed 16,000 tonnes of manganese.^{[failed verification][59]}

Batteries[edit]

Manganese(IV) oxide was used in the original type of dry cell battery as an electron acceptor from zinc, and is the blackish material in carbon–zinc type flashlight cells. The manganese dioxide is reduced to the manganese oxide-hydroxide MnO(OH) during discharging, preventing the formation of hydrogen at the anode of the battery.^[60]

MnO₂ + H₂O + e⁻ → MnO(OH) + OH⁻

The same material also functions in newer alkaline batteries (usually battery cells), which use the same basic reaction, but a different electrolyte mixture. In 2002, more than 230,000 tons of manganese dioxide was used for this purpose.^[29][60]

Resistors[edit]

Copper alloys of manganese, such as Manganin, are commonly found in metal element shunt resistors used for measuring relatively large amounts of current. These alloys have very low temperature coefficient of resistance and are resistant to sulfur. This makes the alloys particularly useful in harsh automotive and industrial environments.^[61]

Niche[edit]

Methylcyclopentadienyl manganese tricarbonyl is an additive in some unleaded gasoline to boost octane rating and reduce engine knocking.

Manganese(IV) oxide (manganese dioxide, MnO₂) is used as a reagent in organic chemistry for the oxidation of benzylic alcohols (where the hydroxyl group is adjacent to an aromatic ring). Manganese dioxide has been used since antiquity to oxidize and neutralize the greenish tinge in glass from trace amounts of iron contamination.^[24] MnO₂ is also used in the manufacture of oxygen and chlorine and in drying black paints. In some preparations, it is a brown pigment for paint and is a constituent of natural umber.

Tetravalent manganese is used as an activator in red-emitting phosphors. While many compounds are known which show luminescence,^[62] the majority are not used in commercial application due to low efficiency or deep red emission.^[63][64] However, several Mn⁴⁺ activated fluorides were reported as potential red-emitting phosphors for warm-white LEDs.^[65][66] But to this day, only K₂SiF₆:Mn⁴⁺ is commercially available for use in warm-white LEDs.^[67]

The metal is occasionally used in coins; until 2000, the only United States coin to use manganese was the «wartime» nickel from 1942 to 1945.^[68] An alloy of 75% copper and 25% nickel was traditionally used for the production of nickel coins. However, because of shortage of nickel metal during the war, it was substituted by more available silver and manganese, thus resulting in an alloy of 56% copper, 35% silver and 9% manganese. Since 2000, dollar coins, for example the Sacagawea dollar and the Presidential $1 coins, are made from a brass containing 7% of manganese with a pure copper core.^[69] In both cases of nickel and dollar, the use of manganese in the coin was to duplicate the electromagnetic properties of a previous identically sized and valued coin in the mechanisms of vending machines. In the case of the later U.S. dollar coins, the manganese alloy was intended to duplicate the properties of the copper/nickel alloy used in the previous Susan B. Anthony dollar.

Manganese compounds have been used as pigments and for the coloring of ceramics and glass. The brown color of ceramic is sometimes the result of manganese compounds.^[70] In the glass industry, manganese compounds are used for two effects. Manganese(III) reacts with iron(II) to reduce strong green color in glass by forming less-colored iron(III) and slightly pink manganese(II), compensating for the residual color of the iron(III).^[24] Larger quantities of manganese are used to produce pink colored glass. In 2009, Professor Mas Subramanian and associates at Oregon State University discovered that manganese can be combined with yttrium and indium to form an intensely blue, non-toxic, inert, fade-resistant pigment, YInMn blue, the first new blue pigment discovered in 200 years.

Biological role[edit]

Biochemistry[edit]

The classes of enzymes that have manganese cofactors include oxidoreductases, transferases, hydrolases, lyases, isomerases and ligases. Other enzymes containing manganese are arginase and Mn-containing superoxide dismutase (Mn-SOD). Also the enzyme class of reverse transcriptases of many retroviruses (though not lentiviruses such as HIV) contains manganese. Manganese-containing polypeptides are the diphtheria toxin, lectins and integrins.^[71]

Biological role in humans[edit]

Manganese is an essential human dietary element. It is present as a coenzyme in several biological processes, which include macronutrient metabolism, bone formation, and free radical defense systems. It is a critical component in dozens of proteins and enzymes.^[3] The human body contains about 12 mg of manganese, mostly in the bones. The soft tissue remainder is concentrated in the liver and kidneys.^[4] In the human brain, the manganese is bound to manganese metalloproteins, most notably glutamine synthetase in astrocytes.^[72]

Nutrition[edit]

The U.S. Institute of Medicine (IOM) updated Estimated Average Requirements (EARs) and Recommended Dietary Allowances (RDAs) for minerals in 2001. For manganese there was not sufficient information to set EARs and RDAs, so needs are described as estimates for Adequate Intakes (AIs). As for safety, the IOM sets Tolerable upper intake levels (ULs) for vitamins and minerals when evidence is sufficient. In the case of manganese the adult UL is set at 11 mg/day. Collectively the EARs, RDAs, AIs and ULs are referred to as Dietary Reference Intakes (DRIs).^[73] Manganese deficiency is rare.^[74]

The European Food Safety Authority (EFSA) refers to the collective set of information as Dietary Reference Values, with Population Reference Intake (PRI) instead of RDA, and Average Requirement instead of EAR. AI and UL defined the same as in United States. For people ages 15 and older the AI is set at 3.0 mg/day. AIs for pregnancy and lactation is 3.0 mg/day. For children ages 1–14 years the AIs increase with age from 0.5 to 2.0 mg/day. The adult AIs are higher than the U.S. RDAs.^[75] The EFSA reviewed the same safety question and decided that there was insufficient information to set a UL.^[76]

For U.S. food and dietary supplement labeling purposes the amount in a serving is expressed as a percent of Daily Value (%DV). For manganese labeling purposes 100% of the Daily Value was 2.0 mg, but as of 27 May 2016 it was revised to 2.3 mg to bring it into agreement with the RDA.^[77][78] A table of the old and new adult daily values is provided at Reference Daily Intake.

Excessive exposure or intake may lead to a condition known as manganism, a neurodegenerative disorder that causes dopaminergic neuronal death and symptoms similar to Parkinson’s disease.^[4][79]

Deficiency[edit]

Manganese deficiency in humans, which is rare, results in a number of medical problems. A deficiency of manganese causes skeletal deformation in animals and inhibits the production of collagen in wound healing.^{[citation needed]}

Toxicity in marine life[edit]

Many enzymatic systems need Mn to function, but in high levels, Mn can become toxic. One environmental reason Mn levels can increase in seawater is when hypoxic periods occur.^[80] Since 1990 there have been reports of Mn accumulation in marine organisms including fish, crustaceans, mollusks, and echinoderms. Specific tissues are targets in different species, including the gills, brain, blood, kidney, and liver/hepatopancreas. Physiological effects have been reported in these species. Mn can affect the renewal of immunocytes and their functionality, such as phagocytosis and activation of pro-phenoloxidase, suppressing the organisms’ immune systems. This causes the organisms to be more susceptible to infections. As climate change occurs, pathogen distributions increase, and in order for organisms to survive and defend themselves against these pathogens, they need a healthy, strong immune system. If their systems are compromised from high Mn levels, they will not be able to fight off these pathogens and die.^[48]

Biological role in bacteria[edit]

Mn-SOD is the type of SOD present in eukaryotic mitochondria, and also in most bacteria (this fact is in keeping with the bacterial-origin theory of mitochondria). The Mn-SOD enzyme is probably one of the most ancient, for nearly all organisms living in the presence of oxygen use it to deal with the toxic effects of superoxide (O⁻
₂), formed from the 1-electron reduction of dioxygen. The exceptions, which are all bacteria, include Lactobacillus plantarum and related lactobacilli, which use a different nonenzymatic mechanism with manganese (Mn²⁺) ions complexed with polyphosphate, suggesting a path of evolution for this function in aerobic life.

Biological role in plants[edit]

Manganese is also important in photosynthetic oxygen evolution in chloroplasts in plants. The oxygen-evolving complex (OEC) is a part of photosystem II contained in the thylakoid membranes of chloroplasts; it is responsible for the terminal photooxidation of water during the light reactions of photosynthesis, and has a metalloenzyme core containing four atoms of manganese.^[81][82] To fulfill this requirement, most broad-spectrum plant fertilizers contain manganese.

Precautions[edit]

Manganese

Hazards
GHS labelling:
Hazard statements	H401
Precautionary statements	P273, P501[83]
NFPA 704 (fire diamond)	0 0 0

Manganese compounds are less toxic than those of other widespread metals, such as nickel and copper.^[84] However, exposure to manganese dusts and fumes should not exceed the ceiling value of 5 mg/m³ even for short periods because of its toxicity level.^[85] Manganese poisoning has been linked to impaired motor skills and cognitive disorders.^[86]

Permanganate exhibits a higher toxicity than manganese(II) compounds. The fatal dose is about 10 g, and several fatal intoxications have occurred. The strong oxidative effect leads to necrosis of the mucous membrane. For example, the esophagus is affected if the permanganate is swallowed. Only a limited amount is absorbed by the intestines, but this small amount shows severe effects on the kidneys and on the liver.^[87][88]

Manganese exposure in United States is regulated by the Occupational Safety and Health Administration (OSHA).^[89] People can be exposed to manganese in the workplace by breathing it in or swallowing it. OSHA has set the legal limit (permissible exposure limit) for manganese exposure in the workplace as 5 mg/m³ over an 8-hour workday. The National Institute for Occupational Safety and Health (NIOSH) has set a recommended exposure limit (REL) of 1 mg/m³ over an 8-hour workday and a short term limit of 3 mg/m³. At levels of 500 mg/m³, manganese is immediately dangerous to life and health.^[90]

Generally, exposure to ambient Mn air concentrations in excess of 5 μg Mn/m3 can lead to Mn-induced symptoms. Increased ferroportin protein expression in human embryonic kidney (HEK293) cells is associated with decreased intracellular Mn concentration and attenuated cytotoxicity, characterized by the reversal of Mn-reduced glutamate uptake and diminished lactate dehydrogenase leakage.^[91]

Environmental health concerns[edit]

In drinking water[edit]

Waterborne manganese has a greater bioavailability than dietary manganese. According to results from a 2010 study,^[92] higher levels of exposure to manganese in drinking water are associated with increased intellectual impairment and reduced intelligence quotients in school-age children. It is hypothesized that long-term exposure due to inhaling the naturally occurring manganese in shower water puts up to 8.7 million Americans at risk.^[93] However, data indicates that the human body can recover from certain adverse effects of overexposure to manganese if the exposure is stopped and the body can clear the excess.^[94]

In gasoline[edit]

Methylcyclopentadienyl manganese tricarbonyl (MMT) is a gasoline additive used to replace lead compounds for unleaded gasolines to improve the octane rating of low octane petroleum distillates. It reduces engine knock agent through the action of the carbonyl groups. Fuels containing manganese tend to form manganese carbides, which damage exhaust valves. Compared to 1953, levels of manganese in air have dropped.^[95]

In tobacco smoke[edit]

The tobacco plant readily absorbs and accumulates heavy metals such as manganese from the surrounding soil into its leaves. These are subsequently inhaled during tobacco smoking.^[96] While manganese is a constituent of tobacco smoke,^[97] studies have largely concluded that concentrations are not hazardous for human health.^[98]

Role in neurological disorders[edit]

Manganism[edit]

Manganese overexposure is most frequently associated with manganism, a rare neurological disorder associated with excessive manganese ingestion or inhalation. Historically, persons employed in the production or processing of manganese alloys^[99][100] have been at risk for developing manganism; however, current health and safety regulations protect workers in developed nations.^[89] The disorder was first described in 1837 by British academic John Couper, who studied two patients who were m.^[27]

Manganism is a biphasic disorder. In its early stages, an intoxicated person may experience depression, mood swings, compulsive behaviors, and psychosis. Early neurological symptoms give way to late-stage manganism, which resembles Parkinson’s disease. Symptoms include weakness, monotone and slowed speech, an expressionless face, tremor, forward-leaning gait, inability to walk backwards without falling, rigidity, and general problems with dexterity, gait and balance.^[27][101] Unlike Parkinson’s disease, manganism is not associated with loss of the sense of smell and patients are typically unresponsive to treatment with L-DOPA.^[102] Symptoms of late-stage manganism become more severe over time even if the source of exposure is removed and brain manganese levels return to normal.^[101]

Chronic manganese exposure has been shown to produce a parkinsonism-like illness characterized by movement abnormalities.^[103] This condition is not responsive to typical therapies used in the treatment of PD, suggesting an alternative pathway than the typical dopaminergic loss within the substantia nigra.^[103] Manganese may accumulate in the basal ganglia, leading to the abnormal movements.^[104] A mutation of the SLC30A10 gene, a manganese efflux transporter necessary for decreasing intracellular Mn, has been linked with the development of this Parkinsonism-like disease.^[105] The Lewy bodies typical to PD are not seen in Mn-induced parkinsonism.^[104]

Animal experiments have given the opportunity to examine the consequences of manganese overexposure under controlled conditions. In (non-aggressive) rats, manganese induces mouse-killing behavior.^[106]

Childhood developmental disorders[edit]

Several recent studies attempt to examine the effects of chronic low-dose manganese overexposure on child development. The earliest study was conducted in the Chinese province of Shanxi. Drinking water there had been contaminated through improper sewage irrigation and contained 240–350 μg Mn/L. Although Mn concentrations at or below 300 μg Mn/L were considered safe at the time of the study by the US EPA and 400 μg Mn/L by the World Health Organization, the 92 children sampled (between 11 and 13 years of age) from this province displayed lower performance on tests of manual dexterity and rapidity, short-term memory, and visual identification, compared to children from an uncontaminated area. More recently, a study of 10-year-old children in Bangladesh showed a relationship between Mn concentration in well water and diminished IQ scores. A third study conducted in Quebec examined school children between the ages of 6 and 15 living in homes that received water from a well containing 610 μg Mn/L; controls lived in homes that received water from a 160 μg Mn/L well. Children in the experimental group showed increased hyperactive and oppositional behavior.^[92]

The current maximum safe concentration under EPA rules is 50 μg Mn/L.^[107]

Neurodegenerative diseases[edit]

A protein called DMT1 is the major transporter in manganese absorption from the intestine, and may be the major transporter of manganese across the blood–brain barrier. DMT1 also transports inhaled manganese across the nasal epithelium. The proposed mechanism for manganese toxicity is that dysregulation leads to oxidative stress, mitochondrial dysfunction, glutamate-mediated excitotoxicity, and aggregation of proteins.^[108]

See also[edit]

• Manganese exporter, membrane transport protein
• List of countries by manganese production
• Parkerizing

References[edit]

External links[edit]

• National Pollutant Inventory – Manganese and compounds Fact Sheet
• International Manganese Institute
• NIOSH Manganese Topic Page
• Manganese at The Periodic Table of Videos (University of Nottingham)
• All about Manganese Dendrites

Not to be confused with Magnesium (Mg).

Manganese, ₂₅Mn

Pure manganese cube and oxidized manganese chips
Manganese
Pronunciation	​(MANG-gə-neez)
Appearance	silvery metallic
Standard atomic weight Ar°(Mn)	54.938043±0.000002 54.938±0.001 (abridged)[1]
Manganese in the periodic table
Hydrogen Helium Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson – ↑ Mn ↓ Tc chromium ← manganese → iron
Atomic number (Z)	25
Group	group 7
Period	period 4
Block	d-block
Electron configuration	[Ar] 3d5 4s2
Electrons per shell	2, 8, 13, 2
Physical properties
Phase at STP	solid
Melting point	1519 K ​(1246 °C, ​2275 °F)
Boiling point	2334 K ​(2061 °C, ​3742 °F)
Density (near r.t.)	7.21 g/cm3
when liquid (at m.p.)	5.95 g/cm3
Heat of fusion	12.91 kJ/mol
Heat of vaporization	221 kJ/mol
Molar heat capacity	26.32 J/(mol·K)
Vapor pressure P (Pa) 1 10 100 1 k 10 k 100 k at T (K) 1228 1347 1493 1691 1955 2333
Atomic properties
Oxidation states	−3, −2, −1, 0, +1, +2, +3, +4, +5, +6, +7 (depending on the oxidation state, an acidic, basic, or amphoteric oxide)
Electronegativity	Pauling scale: 1.55
Ionization energies	1st: 717.3 kJ/mol 2nd: 1509.0 kJ/mol 3rd: 3248 kJ/mol (more)
Atomic radius	empirical: 127 pm
Covalent radius	Low spin: 139±5 pm High spin: 161±8 pm
Spectral lines of manganese
Other properties
Natural occurrence	primordial
Crystal structure	​body-centered cubic (bcc)
Speed of sound thin rod	5150 m/s (at 20 °C)
Thermal expansion	21.7 µm/(m⋅K) (at 25 °C)
Thermal conductivity	7.81 W/(m⋅K)
Electrical resistivity	1.44 µΩ⋅m (at 20 °C)
Magnetic ordering	paramagnetic
Molar magnetic susceptibility	(α) +529.0×10−6 cm3/mol (293 K)[2]
Young’s modulus	198 GPa
Bulk modulus	120 GPa
Mohs hardness	6.0
Brinell hardness	196 MPa
CAS Number	7439-96-5
History
Discovery	Carl Wilhelm Scheele (1774)
First isolation	Johann Gottlieb Gahn (1774)
Main isotopes of manganese v e
Iso­tope Decay abun­dance half-life (t1/2) mode pro­duct 52Mn syn 5.6 d ε 52Cr β+ 52Cr γ – 53Mn trace 3.74×106 y ε 53Cr 54Mn syn 312 d ε 54Cr γ – 55Mn 100% stable
Category: Manganese view talk edit | references

Manganese is a chemical element with the symbol Mn and atomic number 25. It is a hard, brittle, silvery metal, often found in minerals in combination with iron. Manganese is a transition metal with a multifaceted array of industrial alloy uses, particularly in stainless steels. It improves strength, workability, and resistance to wear. Manganese oxide is used as an oxidising agent; as a rubber additive; and in glass making, fertilisers, and ceramics. Manganese sulfate can be used as a fungicide.

Manganese is also an essential human dietary element, important in macronutrient metabolism, bone formation, and free radical defense systems. It is a critical component in dozens of proteins and enzymes.^[3] It is found mostly in the bones, but also the liver, kidneys, and brain.^[4] In the human brain, the manganese is bound to manganese metalloproteins, most notably glutamine synthetase in astrocytes.

Manganese was first isolated in 1774. It is familiar in the laboratory in the form of the deep violet salt potassium permanganate. It occurs at the active sites in some enzymes.^[5] Of particular interest is the use of a Mn-O cluster, the oxygen-evolving complex, in the production of oxygen by plants.

Characteristics[edit]

Physical properties[edit]

Manganese is a silvery-gray metal that resembles iron. It is hard and very brittle, difficult to fuse, but easy to oxidize.^[6] Manganese metal and its common ions are paramagnetic.^[7] Manganese tarnishes slowly in air and oxidizes («rusts») like iron in water containing dissolved oxygen.

Isotopes[edit]

Naturally occurring manganese is composed of one stable isotope, ⁵⁵Mn. Several radioisotopes have been isolated and described, ranging in atomic weight from 44 u (⁴⁴Mn) to 69 u (⁶⁹Mn). The most stable are ⁵³Mn with a half-life of 3.7 million years, ⁵⁴Mn with a half-life of 312.2 days, and ⁵²Mn with a half-life of 5.591 days. All of the remaining radioactive isotopes have half-lives of less than three hours, and the majority of less than one minute. The primary decay mode in isotopes lighter than the most abundant stable isotope, ⁵⁵Mn, is electron capture and the primary mode in heavier isotopes is beta decay.^[8] Manganese also has three meta states.^[8]

Manganese is part of the iron group of elements, which are thought to be synthesized in large stars shortly before the supernova explosion.^{[9] 53}Mn decays to ⁵³Cr with a half-life of 3.7 million years. Because of its relatively short half-life, ⁵³Mn is relatively rare, produced by cosmic rays impact on iron.^[10] Manganese isotopic contents are typically combined with chromium isotopic contents and have found application in isotope geology and radiometric dating. Mn–Cr isotopic ratios reinforce the evidence from ²⁶Al and ¹⁰⁷Pd for the early history of the Solar System. Variations in ⁵³Cr/⁵²Cr and Mn/Cr ratios from several meteorites suggest an initial ⁵³Mn/⁵⁵Mn ratio, which indicate that Mn–Cr isotopic composition must result from in situ decay of ⁵³Mn in differentiated planetary bodies. Hence, ⁵³Mn provides additional evidence for nucleosynthetic processes immediately before coalescence of the Solar System.

Chemical compounds[edit]

Common oxidation states of manganese are +2, +3, +4, +6, and +7, although all oxidation states from −3 to +7 have been observed. Manganese in oxidation state +7 is represented by salts of the intensely purple permanganate anion MnO₄⁻. Potassium permanganate is a commonly used laboratory reagent because of its oxidizing properties; it is used as a topical medicine (for example, in the treatment of fish diseases). Solutions of potassium permanganate were among the first stains and fixatives to be used in the preparation of biological cells and tissues for electron microscopy.^[12]

Aside from various permanganate salts, Mn(VII) is represented by the unstable, volatile derivative Mn₂O₇. Oxyhalides (MnO₃F and MnO₃Cl) are powerful oxidizing agents.^[6] The most prominent example of Mn in the +6 oxidation state is the green anion manganate, [MnO₄]^2-. Manganate salts are intermediates in the extraction of manganese from its ores. Compounds with oxidation states +5 are somewhat elusive, one example is the blue anion hypomanganate [MnO₄]^3-.

Compounds with Mn in oxidation state +5 are rarely encountered and often found associated with an oxide (O^2-) or nitride (N^3-) ligand.^[13][14]

Mn(IV) is somewhat enigmatic because it is common in nature but far rarer in synthetic chemistry. The most common Mn ore, pyrolusite, is MnO₂. It is the dark brown pigment of many cave drawings but is also a common ingredient in dry cell batteries. Complexes of Mn(IV) are well known, but they require elaborate ligands. Mn(IV)-OH complexes are an intermediate in some enzymes, including the oxygen evolving center (OEC) in plants.^[15]

Simple derivatives Mn⁺³ are rarely encountered but can be stabilized by suitably basic ligands. Manganese(III) acetate is an oxidant useful in organic synthesis. Solid compounds of manganese(III) are characterized by its strong purple-red color and a preference for distorted octahedral coordination resulting from the Jahn-Teller effect.

A particularly common oxidation state for manganese in aqueous solution is +2, which has a pale pink color. Many manganese(II) compounds are known, such as the aquo complexes derived from manganese(II) sulfate (MnSO₄) and manganese(II) chloride (MnCl₂). This oxidation state is also seen in the mineral rhodochrosite (manganese(II) carbonate). Manganese(II) commonly exists with a high spin, S = 5/2 ground state because of the high pairing energy for manganese(II). There are no spin-allowed d–d transitions in manganese(II), which explain its faint color.^[16]

Oxidation states of manganese[17]
0	Mn 2(CO) 10
+1	MnC 5H 4CH 3(CO) 3
+2	MnCl 2, MnCO 3, MnO
+3	MnF 3, Mn(OAc) 3, Mn 2O 3
+4	MnO 2
+5	K 3MnO 4
+6	K 2MnO 4
+7	KMnO 4, Mn 2O 7
Common oxidation states are in bold.

Organomanganese compounds[edit]

Manganese forms a large variety of organometallic derivatives, i.e., compounds with Mn-C bonds. The organometallic derivatives include numerous examples of Mn in its lower oxidation states, i.e. Mn(-III) up through Mn(I). This area of organometallic chemistry is attractive because Mn is inexpensive and of relatively low toxicity.

Of greatest commercial interest is «MMT», methylcyclopentadienyl manganese tricarbonyl, which is used as an anti-knock compound added to gasoline (petrol) in some countries. It features Mn(I). Consistent with other aspects of Mn(II) chemistry, manganocene (Mn(C₅H₅)₂) is high-spin. In contrast, its neighboring metal iron forms an air-stable, low-spin derivative in the form of ferrocene (Fe(C₅H₅)₂). When conducted under an atmosphere of carbon monoxide, reduction of Mn(II) salts gives dimanganese decacarbonyl Mn₂(CO)₁₀, an orange and volatile solid. The air-stability of this Mn(0) compound (and its many derivatives) reflects the powerful electron-acceptor properties of carbon monoxide. Many alkene complexes and alkyne complexes are derived from Mn₂(CO)₁₀.

In Mn(CH₃)₂(dmpe)₂, Mn(II) is low spin, which contrasts with the high spin character of its precursor, MnBr₂(dmpe)₂ (dmpe = (CH₃)₂PCH₂CH₂P(CH₃)₂).^[18] Polyalkyl and polyaryl derivatives of manganese often exist in higher oxidation states, reflecting the electron-releasing properties of alkyl and aryl ligands. One example is [Mn(CH₃)₆]^2-.

History[edit]

The origin of the name manganese is complex. In ancient times, two black minerals were identified from the regions of the Magnetes (either Magnesia, located within modern Greece, or Magnesia ad Sipylum, located within modern Turkey).^[19]
They were both called magnes from their place of origin, but were considered to differ in sex. The male magnes attracted iron, and was the iron ore now known as lodestone or magnetite, and which probably gave us the term magnet. The female magnes ore did not attract iron, but was used to decolorize glass. This female magnes was later called magnesia, known now in modern times as pyrolusite or manganese dioxide.^{[citation needed]} Neither this mineral nor elemental manganese is magnetic. In the 16th century, manganese dioxide was called manganesum (note the two Ns instead of one) by glassmakers, possibly as a corruption and concatenation of two words, since alchemists and glassmakers eventually had to differentiate a magnesia nigra (the black ore) from magnesia alba (a white ore, also from Magnesia, also useful in glassmaking). Michele Mercati called magnesia nigra manganesa, and finally the metal isolated from it became known as manganese (German: Mangan). The name magnesia eventually was then used to refer only to the white magnesia alba (magnesium oxide), which provided the name magnesium for the free element when it was isolated much later.^[20]

Manganese dioxide, which is abundant in nature, has long been used as a pigment. The cave paintings in Gargas that are 30,000 to 24,000 years old are made from the mineral form of MnO₂ pigments.^[22]

Manganese compounds were used by Egyptian and Roman glassmakers, either to add to, or remove, color from glass.^[23] Use as «glassmakers soap» continued through the Middle Ages until modern times and is evident in 14th-century glass from Venice.^[24]

Because it was used in glassmaking, manganese dioxide was available for experiments by alchemists, the first chemists. Ignatius Gottfried Kaim (1770) and Johann Glauber (17th century) discovered that manganese dioxide could be converted to permanganate, a useful laboratory reagent.^[25] By the mid-18th century, the Swedish chemist Carl Wilhelm Scheele used manganese dioxide to produce chlorine. First, hydrochloric acid, or a mixture of dilute sulfuric acid and sodium chloride was made to react with manganese dioxide, and later hydrochloric acid from the Leblanc process was used and the manganese dioxide was recycled by the Weldon process. The production of chlorine and hypochlorite bleaching agents was a large consumer of manganese ores.

Scheele and others were aware that pyrolusite (mineral form of manganese dioxide) contained a new element. Johan Gottlieb Gahn was the first to isolate an impure sample of manganese metal in 1774, which he did by reducing the dioxide with carbon.

The manganese content of some iron ores used in Greece led to speculations that steel produced from that ore contains additional manganese, making the Spartan steel exceptionally hard.^[26] Around the beginning of the 19th century, manganese was used in steelmaking and several patents were granted. In 1816, it was documented that iron alloyed with manganese was harder but not more brittle. In 1837, British academic James Couper noted an association between miners’ heavy exposure to manganese and a form of Parkinson’s disease.^[27] In 1912, United States patents were granted for protecting firearms against rust and corrosion with manganese phosphate electrochemical conversion coatings, and the process has seen widespread use ever since.^[28]

The invention of the Leclanché cell in 1866 and the subsequent improvement of batteries containing manganese dioxide as cathodic depolarizer increased the demand for manganese dioxide. Until the development of batteries with nickel-cadmium and lithium, most batteries contained manganese. The zinc–carbon battery and the alkaline battery normally use industrially produced manganese dioxide because naturally occurring manganese dioxide contains impurities. In the 20th century, manganese dioxide was widely used as the cathodic for commercial disposable dry batteries of both the standard (zinc–carbon) and alkaline types.^[29]

Occurrence[edit]

Manganese comprises about 1000 ppm (0.1%) of the Earth’s crust, the 12th most abundant of the crust’s elements.^[4] Soil contains 7–9000 ppm of manganese with an average of 440 ppm.^[4] The atmosphere contains 0.01 μg/m³.^[4] Manganese occurs principally as pyrolusite (MnO₂), braunite (Mn²⁺Mn³⁺₆)SiO₁₂),^[30] psilomelane (Ba,H₂O)₂Mn₅O₁₀, and to a lesser extent as rhodochrosite (MnCO₃).

Manganese ore	Psilomelane (manganese ore)	Spiegeleisen is an iron alloy with a manganese content of approximately 15%	Manganese oxide dendrites on limestone from Solnhofen, Germany – a kind of pseudofossil. Scale is in mm	Mineral rhodochrosite (manganese(II) carbonate)

The most important manganese ore is pyrolusite (MnO₂). Other economically important manganese ores usually show a close spatial relation to the iron ores, such as sphalerite.^[6][32] Land-based resources are large but irregularly distributed. About 80% of the known world manganese resources are in South Africa; other important manganese deposits are in Ukraine, Australia, India, China, Gabon and Brazil.^[31] According to 1978 estimate, the ocean floor has 500 billion tons of manganese nodules.^[33] Attempts to find economically viable methods of harvesting manganese nodules were abandoned in the 1970s.^[34]

In South Africa, most identified deposits are located near Hotazel in the Northern Cape Province, with a 2011 estimate of 15 billion tons. In 2011 South Africa produced 3.4 million tons, topping all other nations.^[35]

Manganese is mainly mined in South Africa, Australia, China, Gabon, Brazil, India, Kazakhstan, Ghana, Ukraine and Malaysia.^[36]

Production[edit]

For the production of ferromanganese, the manganese ore is mixed with iron ore and carbon, and then reduced either in a blast furnace or in an electric arc furnace.^[37] The resulting ferromanganese has a manganese content of 30 to 80%.^[6] Pure manganese used for the production of iron-free alloys is produced by leaching manganese ore with sulfuric acid and a subsequent electrowinning process.^[38]

A more progressive extraction process involves directly reducing (a low grade) manganese ore by heap leaching. This is done by percolating natural gas through the bottom of the heap; the natural gas provides the heat (needs to be at least 850 °C) and the reducing agent (carbon monoxide). This reduces all of the manganese ore to manganese oxide (MnO), which is a leachable form. The ore then travels through a grinding circuit to reduce the particle size of the ore to between 150 and 250 μm, increasing the surface area to aid leaching. The ore is then added to a leach tank of sulfuric acid and ferrous iron (Fe²⁺) in a 1.6:1 ratio. The iron reacts with the manganese dioxide (MnO₂) to form iron hydroxide (FeO(OH)) and elemental manganese (Mn):

This process yields approximately 92% recovery of the manganese. For further purification, the manganese can then be sent to an electrowinning facility.^[39]

In 1972 the CIA’s Project Azorian, through billionaire Howard Hughes, commissioned the ship Hughes Glomar Explorer with the cover story of harvesting manganese nodules from the sea floor.^[40] That triggered a rush of activity to collect manganese nodules, which was not actually practical. The real mission of Hughes Glomar Explorer was to raise a sunken Soviet submarine, the K-129, with the goal of retrieving Soviet code books.^[41]

An abundant resource of manganese in the form of Mn nodules found on the ocean floor.^[42][43] These nodules, which are composed of 29% manganese,^[44] are located along the ocean floor and the potential impact of mining these nodules is being researched. Physical, chemical, and biological environmental impacts can occur due to this nodule mining disturbing the seafloor and causing sediment plumes to form. This suspension includes metals and inorganic nutrients, which can lead to contamination of the near-bottom waters from dissolved toxic compounds. Mn nodules are also the grazing grounds, living space, and protection for endo- and epifaunal systems. When theses nodules are removed, these systems are directly affected. Overall, this can cause species to leave the area or completely die off.^[45] Prior to the commencement of the mining itself, research is being conducted by United Nations affiliated bodies and state-sponsored companies in an attempt to fully understand environmental impacts in the hopes of mitigating these impacts.^[46]

Oceanic environment[edit]

Many trace elements in the ocean come from metal-rich hydrothermal particles from hydrothermal vents.^[47] Dissolved manganese (dMn) is found throughout the world’s oceans, 90% of which originates from hydrothermal vents.^[48] Particulate Mn develops in buoyant plumes over an active vent source, while the dMn behaves conservatively.^[47] Mn concentrations vary between the water columns of the ocean. At the surface, dMn is elevated due to input from external sources such as rivers, dust, and shelf sediments. Coastal sediments normally have lower Mn concentrations, but can increase due to anthropogenic discharges from industries such as mining and steel manufacturing, which enter the ocean from river inputs. Surface dMn concentrations can also be elevated biologically through photosynthesis and physically from coastal upwelling and wind-driven surface currents. Internal cycling such as photo-reduction from UV radiation can also elevate levels by speeding up the dissolution of Mn-oxides and oxidative scavenging, preventing Mn from sinking to deeper waters.^[49] Elevated levels at mid-depths can occur near mid-ocean ridges and hydrothermal vents. The hydrothermal vents release dMn enriched fluid into the water. The dMn can then travel up to 4,000 km due to the microbial capsules present, preventing exchange with particles, lowing the sinking rates. Dissolved Mn concentrations are even higher when oxygen levels are low. Overall, dMn concentrations are normally higher in coastal regions and decrease when moving offshore.^[49]

Soils[edit]

Manganese occurs in soils in three oxidation states: the divalent cation, Mn²⁺ and as brownish-black oxides and hydroxides containing Mn (III,IV), such as MnOOH and MnO₂. Soil pH and oxidation-reduction conditions affect which of these three forms of Mn is dominant in a given soil. At pH values less than 6 or under anaerobic conditions, Mn(II) dominates, while under more alkaline and aerobic conditions, Mn(III,IV) oxides and hydroxides predominate. These effects of soil acidity and aeration state on the form of Mn can be modified or controlled by microbial activity. Microbial respiration can cause both the oxidation of Mn²⁺ to the oxides, and it can cause reduction of the oxides to the divalent cation.^[50]

The Mn(III,IV) oxides exist as brownish-black stains and small nodules on sand, silt, and clay particles. These surface coatings on other soil particles have high surface area and carry negative charge. The charged sites can adsorb and retain various cations, especially heavy metals (e.g., Cr³⁺, Cu²⁺, Zn²⁺, and Pb²⁺). In addition, the oxides can adsorb organic acids and other compounds. The adsorption of the metals and organic compounds can then cause them to be oxidized while the Mn(III,IV) oxides are reduced to Mn²⁺ (e.g., Cr³⁺ to Cr(VI) and colorless hydroquinone to tea-colored quinone polymers).^[51]

Applications[edit]

Manganese has no satisfactory substitute in its major applications in metallurgy.^[31] In minor applications (e.g., manganese phosphating), zinc and sometimes vanadium are viable substitutes.

Steel[edit]

Manganese is essential to iron and steel production by virtue of its sulfur-fixing, deoxidizing, and alloying properties, as first recognized by the British metallurgist Robert Forester Mushet (1811–1891) who, in 1856, introduced the element, in the form of Spiegeleisen, into steel for the specific purpose of removing excess dissolved oxygen, sulfur, and phosphorus in order to improve its malleability. Steelmaking,^[52] including its ironmaking component, has accounted for most manganese demand, presently in the range of 85% to 90% of the total demand.^[38] Manganese is a key component of low-cost stainless steel.^[53][54] Often ferromanganese (usually about 80% manganese) is the intermediate in modern processes.

Small amounts of manganese improve the workability of steel at high temperatures by forming a high-melting sulfide and preventing the formation of a liquid iron sulfide at the grain boundaries. If the manganese content reaches 4%, the embrittlement of the steel becomes a dominant feature. The embrittlement decreases at higher manganese concentrations and reaches an acceptable level at 8%. Steel containing 8 to 15% of manganese has a high tensile strength of up to 863 MPa.^[55][56] Steel with 12% manganese was discovered in 1882 by Robert Hadfield and is still known as Hadfield steel (mangalloy). It was used for British military steel helmets and later by the U.S. military.^[57]

Aluminium alloys[edit]

Manganese is used in production of alloys with aluminium. Aluminium with roughly 1.5% manganese has increased resistance to corrosion through grains that absorb impurities which would lead to galvanic corrosion.^[58] The corrosion-resistant aluminium alloys 3004 and 3104 (0.8 to 1.5% manganese) are used for most beverage cans.^[59] Before 2000, more than 1.6 million tonnes of those alloys were used; at 1% manganese, this consumed 16,000 tonnes of manganese.^{[failed verification][59]}

Batteries[edit]

Manganese(IV) oxide was used in the original type of dry cell battery as an electron acceptor from zinc, and is the blackish material in carbon–zinc type flashlight cells. The manganese dioxide is reduced to the manganese oxide-hydroxide MnO(OH) during discharging, preventing the formation of hydrogen at the anode of the battery.^[60]

MnO₂ + H₂O + e⁻ → MnO(OH) + OH⁻

The same material also functions in newer alkaline batteries (usually battery cells), which use the same basic reaction, but a different electrolyte mixture. In 2002, more than 230,000 tons of manganese dioxide was used for this purpose.^[29][60]

Resistors[edit]

Copper alloys of manganese, such as Manganin, are commonly found in metal element shunt resistors used for measuring relatively large amounts of current. These alloys have very low temperature coefficient of resistance and are resistant to sulfur. This makes the alloys particularly useful in harsh automotive and industrial environments.^[61]

Niche[edit]

Methylcyclopentadienyl manganese tricarbonyl is an additive in some unleaded gasoline to boost octane rating and reduce engine knocking.

Manganese(IV) oxide (manganese dioxide, MnO₂) is used as a reagent in organic chemistry for the oxidation of benzylic alcohols (where the hydroxyl group is adjacent to an aromatic ring). Manganese dioxide has been used since antiquity to oxidize and neutralize the greenish tinge in glass from trace amounts of iron contamination.^[24] MnO₂ is also used in the manufacture of oxygen and chlorine and in drying black paints. In some preparations, it is a brown pigment for paint and is a constituent of natural umber.

Tetravalent manganese is used as an activator in red-emitting phosphors. While many compounds are known which show luminescence,^[62] the majority are not used in commercial application due to low efficiency or deep red emission.^[63][64] However, several Mn⁴⁺ activated fluorides were reported as potential red-emitting phosphors for warm-white LEDs.^[65][66] But to this day, only K₂SiF₆:Mn⁴⁺ is commercially available for use in warm-white LEDs.^[67]

The metal is occasionally used in coins; until 2000, the only United States coin to use manganese was the «wartime» nickel from 1942 to 1945.^[68] An alloy of 75% copper and 25% nickel was traditionally used for the production of nickel coins. However, because of shortage of nickel metal during the war, it was substituted by more available silver and manganese, thus resulting in an alloy of 56% copper, 35% silver and 9% manganese. Since 2000, dollar coins, for example the Sacagawea dollar and the Presidential $1 coins, are made from a brass containing 7% of manganese with a pure copper core.^[69] In both cases of nickel and dollar, the use of manganese in the coin was to duplicate the electromagnetic properties of a previous identically sized and valued coin in the mechanisms of vending machines. In the case of the later U.S. dollar coins, the manganese alloy was intended to duplicate the properties of the copper/nickel alloy used in the previous Susan B. Anthony dollar.

Manganese compounds have been used as pigments and for the coloring of ceramics and glass. The brown color of ceramic is sometimes the result of manganese compounds.^[70] In the glass industry, manganese compounds are used for two effects. Manganese(III) reacts with iron(II) to reduce strong green color in glass by forming less-colored iron(III) and slightly pink manganese(II), compensating for the residual color of the iron(III).^[24] Larger quantities of manganese are used to produce pink colored glass. In 2009, Professor Mas Subramanian and associates at Oregon State University discovered that manganese can be combined with yttrium and indium to form an intensely blue, non-toxic, inert, fade-resistant pigment, YInMn blue, the first new blue pigment discovered in 200 years.

Biological role[edit]

Biochemistry[edit]

The classes of enzymes that have manganese cofactors include oxidoreductases, transferases, hydrolases, lyases, isomerases and ligases. Other enzymes containing manganese are arginase and Mn-containing superoxide dismutase (Mn-SOD). Also the enzyme class of reverse transcriptases of many retroviruses (though not lentiviruses such as HIV) contains manganese. Manganese-containing polypeptides are the diphtheria toxin, lectins and integrins.^[71]

Biological role in humans[edit]

Manganese is an essential human dietary element. It is present as a coenzyme in several biological processes, which include macronutrient metabolism, bone formation, and free radical defense systems. It is a critical component in dozens of proteins and enzymes.^[3] The human body contains about 12 mg of manganese, mostly in the bones. The soft tissue remainder is concentrated in the liver and kidneys.^[4] In the human brain, the manganese is bound to manganese metalloproteins, most notably glutamine synthetase in astrocytes.^[72]

Nutrition[edit]

The U.S. Institute of Medicine (IOM) updated Estimated Average Requirements (EARs) and Recommended Dietary Allowances (RDAs) for minerals in 2001. For manganese there was not sufficient information to set EARs and RDAs, so needs are described as estimates for Adequate Intakes (AIs). As for safety, the IOM sets Tolerable upper intake levels (ULs) for vitamins and minerals when evidence is sufficient. In the case of manganese the adult UL is set at 11 mg/day. Collectively the EARs, RDAs, AIs and ULs are referred to as Dietary Reference Intakes (DRIs).^[73] Manganese deficiency is rare.^[74]

The European Food Safety Authority (EFSA) refers to the collective set of information as Dietary Reference Values, with Population Reference Intake (PRI) instead of RDA, and Average Requirement instead of EAR. AI and UL defined the same as in United States. For people ages 15 and older the AI is set at 3.0 mg/day. AIs for pregnancy and lactation is 3.0 mg/day. For children ages 1–14 years the AIs increase with age from 0.5 to 2.0 mg/day. The adult AIs are higher than the U.S. RDAs.^[75] The EFSA reviewed the same safety question and decided that there was insufficient information to set a UL.^[76]

For U.S. food and dietary supplement labeling purposes the amount in a serving is expressed as a percent of Daily Value (%DV). For manganese labeling purposes 100% of the Daily Value was 2.0 mg, but as of 27 May 2016 it was revised to 2.3 mg to bring it into agreement with the RDA.^[77][78] A table of the old and new adult daily values is provided at Reference Daily Intake.

Excessive exposure or intake may lead to a condition known as manganism, a neurodegenerative disorder that causes dopaminergic neuronal death and symptoms similar to Parkinson’s disease.^[4][79]

Deficiency[edit]

Manganese deficiency in humans, which is rare, results in a number of medical problems. A deficiency of manganese causes skeletal deformation in animals and inhibits the production of collagen in wound healing.^{[citation needed]}

Toxicity in marine life[edit]

Many enzymatic systems need Mn to function, but in high levels, Mn can become toxic. One environmental reason Mn levels can increase in seawater is when hypoxic periods occur.^[80] Since 1990 there have been reports of Mn accumulation in marine organisms including fish, crustaceans, mollusks, and echinoderms. Specific tissues are targets in different species, including the gills, brain, blood, kidney, and liver/hepatopancreas. Physiological effects have been reported in these species. Mn can affect the renewal of immunocytes and their functionality, such as phagocytosis and activation of pro-phenoloxidase, suppressing the organisms’ immune systems. This causes the organisms to be more susceptible to infections. As climate change occurs, pathogen distributions increase, and in order for organisms to survive and defend themselves against these pathogens, they need a healthy, strong immune system. If their systems are compromised from high Mn levels, they will not be able to fight off these pathogens and die.^[48]

Biological role in bacteria[edit]

Mn-SOD is the type of SOD present in eukaryotic mitochondria, and also in most bacteria (this fact is in keeping with the bacterial-origin theory of mitochondria). The Mn-SOD enzyme is probably one of the most ancient, for nearly all organisms living in the presence of oxygen use it to deal with the toxic effects of superoxide (O⁻
₂), formed from the 1-electron reduction of dioxygen. The exceptions, which are all bacteria, include Lactobacillus plantarum and related lactobacilli, which use a different nonenzymatic mechanism with manganese (Mn²⁺) ions complexed with polyphosphate, suggesting a path of evolution for this function in aerobic life.

Biological role in plants[edit]

Manganese is also important in photosynthetic oxygen evolution in chloroplasts in plants. The oxygen-evolving complex (OEC) is a part of photosystem II contained in the thylakoid membranes of chloroplasts; it is responsible for the terminal photooxidation of water during the light reactions of photosynthesis, and has a metalloenzyme core containing four atoms of manganese.^[81][82] To fulfill this requirement, most broad-spectrum plant fertilizers contain manganese.

Precautions[edit]

Manganese

Hazards
GHS labelling:
Hazard statements	H401
Precautionary statements	P273, P501[83]
NFPA 704 (fire diamond)	0 0 0

Manganese compounds are less toxic than those of other widespread metals, such as nickel and copper.^[84] However, exposure to manganese dusts and fumes should not exceed the ceiling value of 5 mg/m³ even for short periods because of its toxicity level.^[85] Manganese poisoning has been linked to impaired motor skills and cognitive disorders.^[86]

Permanganate exhibits a higher toxicity than manganese(II) compounds. The fatal dose is about 10 g, and several fatal intoxications have occurred. The strong oxidative effect leads to necrosis of the mucous membrane. For example, the esophagus is affected if the permanganate is swallowed. Only a limited amount is absorbed by the intestines, but this small amount shows severe effects on the kidneys and on the liver.^[87][88]

Manganese exposure in United States is regulated by the Occupational Safety and Health Administration (OSHA).^[89] People can be exposed to manganese in the workplace by breathing it in or swallowing it. OSHA has set the legal limit (permissible exposure limit) for manganese exposure in the workplace as 5 mg/m³ over an 8-hour workday. The National Institute for Occupational Safety and Health (NIOSH) has set a recommended exposure limit (REL) of 1 mg/m³ over an 8-hour workday and a short term limit of 3 mg/m³. At levels of 500 mg/m³, manganese is immediately dangerous to life and health.^[90]

Generally, exposure to ambient Mn air concentrations in excess of 5 μg Mn/m3 can lead to Mn-induced symptoms. Increased ferroportin protein expression in human embryonic kidney (HEK293) cells is associated with decreased intracellular Mn concentration and attenuated cytotoxicity, characterized by the reversal of Mn-reduced glutamate uptake and diminished lactate dehydrogenase leakage.^[91]

Environmental health concerns[edit]

In drinking water[edit]

Waterborne manganese has a greater bioavailability than dietary manganese. According to results from a 2010 study,^[92] higher levels of exposure to manganese in drinking water are associated with increased intellectual impairment and reduced intelligence quotients in school-age children. It is hypothesized that long-term exposure due to inhaling the naturally occurring manganese in shower water puts up to 8.7 million Americans at risk.^[93] However, data indicates that the human body can recover from certain adverse effects of overexposure to manganese if the exposure is stopped and the body can clear the excess.^[94]

In gasoline[edit]

Methylcyclopentadienyl manganese tricarbonyl (MMT) is a gasoline additive used to replace lead compounds for unleaded gasolines to improve the octane rating of low octane petroleum distillates. It reduces engine knock agent through the action of the carbonyl groups. Fuels containing manganese tend to form manganese carbides, which damage exhaust valves. Compared to 1953, levels of manganese in air have dropped.^[95]

In tobacco smoke[edit]

The tobacco plant readily absorbs and accumulates heavy metals such as manganese from the surrounding soil into its leaves. These are subsequently inhaled during tobacco smoking.^[96] While manganese is a constituent of tobacco smoke,^[97] studies have largely concluded that concentrations are not hazardous for human health.^[98]

Role in neurological disorders[edit]

Manganism[edit]

Manganese overexposure is most frequently associated with manganism, a rare neurological disorder associated with excessive manganese ingestion or inhalation. Historically, persons employed in the production or processing of manganese alloys^[99][100] have been at risk for developing manganism; however, current health and safety regulations protect workers in developed nations.^[89] The disorder was first described in 1837 by British academic John Couper, who studied two patients who were m.^[27]

Manganism is a biphasic disorder. In its early stages, an intoxicated person may experience depression, mood swings, compulsive behaviors, and psychosis. Early neurological symptoms give way to late-stage manganism, which resembles Parkinson’s disease. Symptoms include weakness, monotone and slowed speech, an expressionless face, tremor, forward-leaning gait, inability to walk backwards without falling, rigidity, and general problems with dexterity, gait and balance.^[27][101] Unlike Parkinson’s disease, manganism is not associated with loss of the sense of smell and patients are typically unresponsive to treatment with L-DOPA.^[102] Symptoms of late-stage manganism become more severe over time even if the source of exposure is removed and brain manganese levels return to normal.^[101]

Chronic manganese exposure has been shown to produce a parkinsonism-like illness characterized by movement abnormalities.^[103] This condition is not responsive to typical therapies used in the treatment of PD, suggesting an alternative pathway than the typical dopaminergic loss within the substantia nigra.^[103] Manganese may accumulate in the basal ganglia, leading to the abnormal movements.^[104] A mutation of the SLC30A10 gene, a manganese efflux transporter necessary for decreasing intracellular Mn, has been linked with the development of this Parkinsonism-like disease.^[105] The Lewy bodies typical to PD are not seen in Mn-induced parkinsonism.^[104]

Animal experiments have given the opportunity to examine the consequences of manganese overexposure under controlled conditions. In (non-aggressive) rats, manganese induces mouse-killing behavior.^[106]

Childhood developmental disorders[edit]

Several recent studies attempt to examine the effects of chronic low-dose manganese overexposure on child development. The earliest study was conducted in the Chinese province of Shanxi. Drinking water there had been contaminated through improper sewage irrigation and contained 240–350 μg Mn/L. Although Mn concentrations at or below 300 μg Mn/L were considered safe at the time of the study by the US EPA and 400 μg Mn/L by the World Health Organization, the 92 children sampled (between 11 and 13 years of age) from this province displayed lower performance on tests of manual dexterity and rapidity, short-term memory, and visual identification, compared to children from an uncontaminated area. More recently, a study of 10-year-old children in Bangladesh showed a relationship between Mn concentration in well water and diminished IQ scores. A third study conducted in Quebec examined school children between the ages of 6 and 15 living in homes that received water from a well containing 610 μg Mn/L; controls lived in homes that received water from a 160 μg Mn/L well. Children in the experimental group showed increased hyperactive and oppositional behavior.^[92]

The current maximum safe concentration under EPA rules is 50 μg Mn/L.^[107]

Neurodegenerative diseases[edit]

A protein called DMT1 is the major transporter in manganese absorption from the intestine, and may be the major transporter of manganese across the blood–brain barrier. DMT1 also transports inhaled manganese across the nasal epithelium. The proposed mechanism for manganese toxicity is that dysregulation leads to oxidative stress, mitochondrial dysfunction, glutamate-mediated excitotoxicity, and aggregation of proteins.^[108]

See also[edit]

• Manganese exporter, membrane transport protein
• List of countries by manganese production
• Parkerizing

References[edit]

External links[edit]

• National Pollutant Inventory – Manganese and compounds Fact Sheet
• International Manganese Institute
• NIOSH Manganese Topic Page
• Manganese at The Periodic Table of Videos (University of Nottingham)
• All about Manganese Dendrites

Энергия ионизации

Чем ближе электрон к центру атома — тем больше энергии необходимо, что бы его оторвать.
Энергия, затрачиваемая на отрыв электрона от атома называется энергией ионизации и обозначается E_o.
Если не указано иное, то энергия ионизации — это энергия отрыва первого электрона, также существуют энергии
ионизации для каждого последующего электрона.

Энергия ионизации Mn:
E_o = 717 кДж/моль

— Что такое ион читайте в статье.

---

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25 Хром ← Марганец → Железо 25Mn
Внешний вид простого вещества
Твёрдый, хрупкий металл светло-серого цвета
Свойства атома
Имя, символ, номер	Марганец / Manganum (Mn), 25
Атомная масса (молярная масса)	54,93805 а. е. м. (г/моль)
Электронная конфигурация	[Ar] 3d5 4s2
Радиус атома	135 пм
Химические свойства
Ковалентный радиус	117 пм
Радиус иона	(+7e) 46 (+2e) 80 пм
Электроотрицательность	1,55 (шкала Полинга)
Электродный потенциал	-1,180 В
Степени окисления	7, 6, 5, 4, 3, 2, 0, −1
Энергия ионизации (первый электрон)	716,8 (7,43) кДж/моль (эВ)
Термодинамические свойства простого вещества
Плотность (при н. у.)	7,21 г/см³
Температура плавления	1 517 K
Температура кипения	2 235 K
Теплота плавления	(13,4) кДж/моль
Теплота испарения	221 кДж/моль
Молярная теплоёмкость	26,3[1] Дж/(K·моль)
Молярный объём	7,39 см³/моль
Кристаллическая решётка простого вещества
Структура решётки	кубическая
Параметры решётки	8,890 Å
Температура Дебая	400 K
Прочие характеристики
Теплопроводность	(300 K) (7,8) Вт/(м·К)

Ма́рганец — элемент побочной подгруппы седьмой группы четвёртого периода периодической системы химических элементов Д. И. Менделеева, с атомным номером 25. Обозначается символом Mn (лат. Manganum, ма́нганум, в составе формул по-русски читается как марганец, например, KMnO₄ — калий марганец о четыре; но нередко читают и как манган). Простое вещество марганец (CAS-номер: 7439-96-5) — металл серебристо-белого цвета. Известны пять аллотропных модификаций марганца — четыре с кубической и одна с тетрагональной кристаллической решёткой^[1].

История открытия

Один из основных минералов марганца — пиролюзит — был известен в древности как чёрная магнезия и использовался при варке стекла для его осветления. Его считали разновидностью магнитного железняка, а тот факт, что он не притягивается магнитом, Плиний Старший объяснил женским полом черной магнезии, к которому магнит «равнодушен». В 1774 г. шведский химик К. Шееле показал, что в руде содержится неизвестный металл. Он послал образцы руды своему другу химику Ю. Гану, который, нагревая в печке пиролюзит с углем, получил металлический марганец. В начале XIX века для него было принято название «манганум» (от немецкого Manganerz — марганцевая руда).

Распространённость в природе

Марганец — 14-й элемент по распространённости на Земле, а после железа — второй тяжёлый металл, содержащийся в земной коре (0,03 % от общего числа атомов земной коры). Весовое количество марганца увеличивается от кислых (600 г/т) к основным породам (2,2 кг/т). Сопутствует железу во многих его рудах, однако встречаются и самостоятельные месторождения марганца. В чиатурском месторождении (район Кутаиси) сосредоточено до 40 % марганцевых руд. Марганец, рассеянный в горных породах вымывается водой и уносится в Мировой океан. При этом его содержание в морской воде незначительно (10⁻⁷—10⁻⁶%), а в глубоких местах океана его концентрация возрастает до 0,3 % вследствие окисления растворённым в воде кислородом с образованием нерастворимого в воде оксида марганца, который в гидратированной форме (MnO₂·xH₂O) и опускается в нижние слои океана, формируя так называемые железо-марганцевые конкреции на дне, в которых количество марганца может достигать 45 % (также в них имеются примеси меди, никеля, кобальта). Такие конкреции могут стать в будущем источником марганца для промышленности.

В России является остродефицитным сырьём, известны месторождения: «Усинское» в Кемеровской области, «Полуночное» в Свердловской, «Порожинское» в Красноярском крае, «Южно-Хинганское» в Еврейской автономной области, «Рогачёво-Тайнинская» площадь и «Северо-Тайнинское» поле на Новой Земле.

Минералы марганца

• пиролюзит MnO₂·xH₂O, самый распространённый минерал (содержит 63,2 % марганца);
• манганит (бурая марганцевая руда) MnO(OH) (62,5 % марганца);
• браунит 3Mn₂O₃·MnSiO₃ (69,5 % марганца);
• гаусманит (Mn^IIMn₂^III)O₄
• родохрозит (марганцевый шпат, малиновый шпат) MnCO₃ (47,8 % марганца);
• псиломелан mMnO • MnO₂ • nH₂O (45-60 % марганца);
• пурпурит (Mn³⁺[PO₄]), 36,65 % марганца.

Получение

1. Алюминотермическим методом, восстанавливая оксид Mn₂O₃, образующийся при прокаливании пиролюзита:

   

   

2. Восстановлением железосодержащих оксидных руд марганца коксом. Этим способом в металлургии обычно получают ферромарганец (≅80 % Mn).
3. Чистый металлический марганец получают электролизом

Физические свойства

Некоторые свойства приведены в таблице. Другие свойства марганца:

• Работа выхода электрона: 4,1 эВ
• Коэффициент линейного температурного расширения: 0,000022 см/см/°C (при 0 °C)
• Электропроводность: 0,00695·10⁶ Ом⁻¹·см⁻¹
• Теплопроводность: 0,0782 Вт/см·K
• Энтальпия атомизации: 280,3 кДж/моль при 25 °C
• Энтальпия плавления: 14,64 кДж/моль
• Энтальпия испарения: 219,7 кДж/моль
• Твёрдость
  • по шкале Бринелля: Мн/м²
  • по шкале Мооса: 4^[2]
• Давление паров: 121 Па при 1244 °C
• Молярный объём: 7,35 см³/моль

Химические свойства

Стандартные окислительно-восстановительные потенциалы по отношению к водородному электроду

Окисленная форма	Восстановленная форма	Среда	E0, В
Mn2+	Mn	H+	−1,186
Mn3+	Mn2+	H+	+1,51
MnO2	Mn3+	H+	+0,95
MnO2	Mn2+	H+	+1,23
MnO2	Mn(OH)2	OH−	−0,05
MnO42−	MnO2	H+	+2,26
MnO42−	MnO2	OH−	+0,62
MnO4−	MnO42−	OH−	+0,56
MnO4−	H2MnO4	H+	+1,22
MnO4−	MnO2	H+	+1,69
MnO4−	MnO2	OH−	+0,60
MnO4−	Mn2+	H+	+1,51

Характерные степени окисления марганца: +2, +3, +4, +6, +7 (+1, +5 мало характерны).

При окислении на воздухе пассивируется. Порошкообразный марганец сгорает в кислороде (Mn + O₂ → MnO₂). Марганец при нагревании разлагает воду, вытесняя водород (Mn + 2H₂O →(t) Mn(OH)₂ + H₂↑), образующийся гидроксид марганца замедляет реакцию.

Марганец поглощает водород, с повышением температуры его растворимость в марганце увеличивается. При температуре выше 1200 °C взаимодействует с азотом, образуя различные по составу нитриды.

Углерод реагирует с расплавленным марганцем, образуя карбиды Mn₃C и другие. Образует также силициды, бориды, фосфиды.

C соляной и серной кислотами реагирует по уравнению:

С концентрированной серной кислотой реакция идёт по уравнению:

С разбавленой азотной кислотой реакция идёт по уравнению:

В щелочном растворе марганец устойчив.

Марганец образует следующие оксиды: MnO, Mn₂O₃, MnO₂, MnO₃ (не выделен в свободном состоянии) и марганцевый ангидрид Mn₂O₇.

Mn₂O₇ в обычных условиях жидкое маслянистое вещество тёмно-зелёного цвета, очень неустойчивое; в смеси с концентрированной серной кислотой воспламеняет органические вещества. При 90 °C Mn₂O₇ разлагается со взрывом. Наиболее устойчивы оксиды Mn₂O₃ и MnO₂, а также комбинированный оксид Mn₃O₄ (2MnO·MnO₂, или соль Mn₂MnO₄).

При сплавлении оксида марганца (IV) (пиролюзит) со щелочами в присутствии кислорода образуются манганаты:

Раствор манганата имеет тёмно-зелёный цвет. При подкислении протекает реакция:

Раствор окрашивается в малиновый цвет из-за появления аниона MnO₄⁻, и из него выпадает коричневый осадок оксида-гидроксида марганца (IV).

Марганцевая кислота очень сильная, но неустойчивая, её невозможно сконцентрировать более, чем до 20 %. Сама кислота и её соли (перманганаты) — сильные окислители. Например, перманганат калия в зависимости от pH раствора окисляет различные вещества, восстанавливаясь до соединений марганца разной степени окисления. В кислой среде — до соединений марганца (II), в нейтральной — до соединений марганца (IV), в сильно щелочной — до соединений марганца (VI).

При прокаливании перманганаты разлагаются с выделением кислорода (один из лабораторных способов получения чистого кислорода). Реакция идёт по уравнению (на примере перманганата калия):

Под действием сильных окислителей ион Mn²⁺ переходит в ион MnO₄⁻:

Эта реакция используется для качественного определения Mn²⁺ (см. в разделе «Определение методами химического анализа»).

При подщелачивании растворов солей Mn (II) из них выпадает осадок гидроксида марганца (II), быстро буреющий на воздухе в результате окисления. Подробное описание реакции см. в разделе «Определение методами химического анализа».

Соли MnCl₃, Mn₂(SO₄)₃ неустойчивы. Гидроксиды Mn(OH)₂ и Mn(OH)₃ имеют основной характер, MnO(OH)₂ — амфотерный. Хлорид марганца (IV) MnCl₄ очень неустойчив, разлагается при нагревании, чем пользуются для получения хлора:

Применение в промышленности

Марганец в виде ферромарганца применяется для «раскисления» стали при её плавке, то есть для удаления из неё кислорода. Кроме того, он связывает серу, что также улучшает свойства сталей. Введение до 12-13 % Mn в сталь (так называемая Сталь Гадфильда), иногда в сочетании с другими легирующими металлами, сильно упрочняет сталь, делает её твердой и сопротивляющейся износу и ударам (эта сталь резко упрочняется и становится тверже при ударах). Такая сталь используется для изготовления шаровых мельниц, землеройных и камнедробильных машин, броневых элементов и т. д. В «зеркальный чугун» вводится до 20 % Mn.

Сплав 83 % Cu, 13 % Mn и 4 % Ni (манганин) обладает высоким электросопротивлением, мало изменяющимся с изменением температуры. Поэтому его применяют для изготовления реостатов и пр.

Марганец вводят в бронзы и латуни.

Значительное количество диоксида марганца потребляется при производстве марганцево-цинковых гальванических элементов, MnO₂ используется в таких элементах в качестве окислителя-деполяризатора.

Соединения марганца также широко используются как в тонком органическом синтезе (MnO₂ и KMnO₄ в качестве окислителей), так и промышленном органическом синтезе (компоненты катализаторов окисления углеводородов, например, в производстве терефталевой кислоты окислением p-ксилола, окисление парафинов в высшие жирные кислоты).

Цены на металлический марганец в слитках чистотой 95 % в 2006 году составили в среднем 2,5 долл/кг.

Арсенид марганца обладает гигантским магнитокалорическим эффектом, усиливающимся под давлением. Теллурид марганца перспективный термоэлектрический материал(термо-э.д.с 500 мкВ/К).

Определение методами химического анализа

Марганец принадлежит к пятой аналитической группе катионов.

Специфические реакции, используемые в аналитической химии для обнаружения катионов Mn²⁺ следующие:

1. Едкие щёлочи с солями марганца (II) дают белый осадок гидроксида марганца (II):

Осадок на воздухе меняет цвет на бурый из-за окисления кислородом воздуха.

Выполнение реакции. К двум каплям раствора соли марганца добавляют две капли раствора щёлочи. Наблюдают изменение цвета осадка.

2. Пероксид водорода в присутствии щёлочи окисляет соли марганца (II) до тёмно-бурого соединения марганца (IV):

Выполнение реакции. К двум каплям раствора соли марганца добавляют четыре капли раствора щёлочи и две капли раствора H₂O₂.

3. Диоксид свинца PbO₂ в присутствии концентрированной азотной кислоты при нагревании окисляет Mn²⁺ до MnO₄⁻ с образованием марганцевой кислоты малинового цвета:

Эта реакция дает отрицательный результат в присутствии восстановителей, например хлороводородной кислоты и её солей, так как они взаимодействуют с диоксидом свинца, а также с образовавшейся марганцевой кислотой. При больших количествах марганца эта реакция не удаётся, так как избыток ионов Mn²⁺ восстанавливает образующуюся марганцевую кислоту HMnO₄ до MnO(OH)₂, и вместо малиновой окраски появляется бурый осадок. Вместо диоксида свинца для окисления Mn²⁺ в MnO₄⁻ могут быть использованы другие окислители, например персульфат аммония (NH₄)₂S₂O₈ в присутствии катализатора — ионов Ag⁺ или висмутата натрия NaBiO₃:

Выполнение реакции. В пробирку вносят стеклянным шпателем немного PbO₂, а затем 5 капель концентрированной азотной кислоты HNO₃ и нагревают смесь на кипящей водяной бане. В нагретую смесь добавляют 1 каплю раствора сульфата марганца (II) MnSO₄ и снова нагревают 10—15 мин, встряхивая время от времени содержимое пробирки. Дают избытку диоксида свинца осесть и наблюдают малиновую окраску образовавшейся марганцевой кислоты.

При окислении висмутатом натрия реакцию проводят следующим образом. В пробирку помещают 1—2 капли раствора сульфата марганца (II) и 4 капли 6 н. HNO₃, добавляют несколько крупинок висмутата натрия и встряхивают. Наблюдают появление малиновой окраски раствора.

4. Сульфид аммония (NH₄)₂S осаждает из раствора солей марганца сульфид марганца (II), окрашенный в телесный цвет:

Осадок легко растворяется в разбавленных минеральных кислотах и даже в уксусной кислоте.

Выполнение реакции. В пробирку помещают 2 капли раствора соли марганца (II) и добавляют 2 капли раствора сульфида аммония.

Биологическая роль и содержание в живых организмах

Марганец содержится в организмах всех растений и животных, хотя его содержание обычно очень мало, порядка тысячных долей процента, он оказывает значительное влияние на жизнедеятельность, то есть является микроэлементом. Марганец оказывает влияние на рост, образование крови и функции половых желёз. Особо богаты марганцем листья свёклы — до 0,03 %, а также большие его количества содержатся в организмах рыжих муравьёв — до 0,05 %. Некоторые бактерии содержат до нескольких процентов марганца.

Избыточное накопление марганца в организме сказывается, в первую очередь, на функционировании центральной нервной системы. Это проявляется в утомляемости, сонливости, ухудшении функций памяти. Марганец является политропным ядом, поражающим также легкие, сердечно-сосудистую и гепатобиллиарную системы, вызывает аллергический и мутагенный эффект^{[источник не указан 372 дня]}.

Токсичность

Токсическая доза для человека составляет 40 мг марганца в день. Летальная доза для человека не определена.

При пероральном поступлении марганец относится к наименее ядовитым микроэлементам. Главными признаками отравления марганцем у животных являются угнетение роста, понижение аппетита, нарушение метаболизма железа и изменение функции мозга.

Сообщений о случаях отравления марганцем у людей, вызванных приемом пищи с высоким содержанием марганца, нет. В основном отравление людей наблюдается в случаях хронической ингаляции больших количеств марганца на производстве. Оно проявляется в виде тяжелых нарушений психики, включая гиперраздражительность, гипермоторику и галлюцинации — «марганцевое безумие». В дальнейшем развиваются изменения в экстрапирамидной системе, подобные болезни Паркинсона.

Чтобы развилась клиническая картина хронического отравления марганцем обычно требуется несколько лет. Она характеризуется достаточно медленным нарастанием патологических изменений в организме, вызываемый повышенным содержанием марганца в окружающей среде (в частности, распространение эндемического зоба, не связанного с дефицитом йода).

См. также

• Список стран по производству марганца
• Категория:Соединения марганца
• Отравление марганцем

Примечания

Ссылки

	Марганец на Викискладе?

• Марганец на Webelements
• Марганец в Популярной библиотеке химических элементов
• Марганец в месторождениях
• Марганец и его соединения

Соединения марганца

Арсенид димарганца (Mn2As) • Арсенид марганца (MnAs) • Ацетат марганца(II) (Mn(CH3COO)2) • Борид марганца (MnB) • Бромид марганца(II) (MnBr2) • Гексакарбонил марганца (Mn(CO)6) • Гидроксид марганца(II) (Mn(OH)2) • Гидроортофосфат марганца(II) (MnHPO4) • Декакарбонилдимарганец (Mn2(CO)10) • Диборид марганца (MnB2) • Дигидроортофосфат марганца(II) (Mn(H2PO4)2) • Динитрид пентамарганца (Mn5N2) • Динитрид тримарганца (Mn3N2) • Дисилицид марганца (MnSi2) • Дифосфид тримарганца (Mn3P2) • Иодид марганца(II) (MnI2) • Метагидроксид марганца (MnO(OH)) • Карбид тримарганца (Mn3C) • Карбиды марганца • Карбонат марганца(II) (MnCO3) • Манганат бария (BaMnO4) • Манганат калия (K2MnO4) • Манганат натрия (Na2MnO4) • Марганцовая кислота (HMnO4) • Метасиликат марганца(II) (MnSiO3) • Нитрат марганца(II) (Mn(NO3)2) • Нитрид димарганца (Mn2N) • Нитрид тетрамарганца (Mn4N) • Оксид марганца(II) (MnO) • Оксид марганца(II,III) (Mn3O4) • Оксид марганца(II,IV) (Mn5O8) • Оксид марганца(III) (Mn2O3) • Оксид марганца(IV) (MnO2) • Оксид марганца(VI) (MnO3) • Оксид марганца(VII) (Mn2O7) • Ортосиликат марганца(II) (Mn2SiO4) • Ортофосфат марганца(II) (Mn3(PO4)2) • Перманганат калия (KMnO4) • Перманганат лития (LiMnO4) • Перманганат натрия (NaMnO4) • Перманганат серебра (AgMnO4) • Пирофосфат марганца(II) (Mn2P2O7) • Силицид димарганца (Mn2Si) • Силицид марганца (MnSi) • Сульфат марганца(II) (MnSO4) • Сульфат марганца(III) (Mn2(SO4)3) • Сульфат марганца(IV) (Mn(SO4)2) • Сульфид марганца(II) (MnS) • Сульфид марганца(IV) (MnS2) • Тетраоксоманганат(V) натрия (Na3MnO4) • Тиоцианат марганца(II) (Mn(SCN)2) • Фосфид димарганца (Mn2P) • Фосфид марганца (MnP) • Фосфид тетрамарганца (Mn4P) • Фосфид тримарганца (Mn3P) • Фторид марганца(II) (MnF2) • Фторид марганца(III) (MnF3) • Фторид марганца(IV) (MnF4) • Хлорид марганца(II) (MnCl2) • Хлорид марганца(III) (MnCl3) Хлорид марганца(IV) (MnCl4)

Периодическая система химических элементов Д. И. Менделеева
	1	2															3	4	5	6	7	8	9	10	11	12	13	14	15	16	17	18
1	H		He
2	Li	Be		B	C	N	O	F	Ne
3	Na	Mg		Al	Si	P	S	Cl	Ar
4	K	Ca		Sc	Ti	V	Cr	Mn	Fe	Co	Ni	Cu	Zn	Ga	Ge	As	Se	Br	Kr
5	Rb	Sr		Y	Zr	Nb	Mo	Tc	Ru	Rh	Pd	Ag	Cd	In	Sn	Sb	Te	I	Xe
6	Cs	Ba	La	Ce	Pr	Nd	Pm	Sm	Eu	Gd	Tb	Dy	Ho	Er	Tm	Yb	Lu	Hf	Ta	W	Re	Os	Ir	Pt	Au	Hg	Tl	Pb	Bi	Po	At	Rn
7	Fr	Ra	Ac	Th	Pa	U	Np	Pu	Am	Cm	Bk	Cf	Es	Fm	Md	No	Lr	Rf	Db	Sg	Bh	Hs	Mt	Ds	Rg	Cn	Uut	Fl	Uup	Lv	Uus	Uuo
Щелочные металлы  Щёлочноземельные металлы  Лантаноиды Актиноиды Переходные металлы Другие металлы Металлоиды Другие неметаллы Галогены Инертные газы

Электрохимический ряд активности металлов
Eu, Sm, Li, Cs, Rb, K, Ra, Ba, Sr, Ca, Na, Ac, La, Ce, Pr, Nd, Pm, Gd, Tb, Mg, Y, Dy, Am, Ho, Er, Tm, Lu, Sc, Pu, Th, Np, U, Hf, Be, Al, Ti, Zr, Yb, Mn, V, Nb, Pa, Cr, Zn, Ga, Fe, Cd, In, Tl, Co, Ni, Te, Mo, Sn, Pb, H2, W, Sb, Bi, Ge, Re, Cu, Tc, Te, Rh, Po, Hg, Ag, Pd, Os, Ir, Pt, Au Элементы расположены в порядке возрастания стандартного электродного потенциала.