Manganese

chromium – manganese – iron Mn Tc       Full table
General
Name, Symbol, Number	manganese, Mn, 25
Chemical series	transition metals
Group, Period, Block	7 , 4, d
Density, Hardness	7470 kg/m3, 6.0
Appearance	silvery metallic Missing image Mn,25.jpg
Atomic properties
Atomic weight	54.938049 amu
Atomic radius (calc.)	140 (161) pm
Covalent radius	139 pm
van der Waals radius	n/a pm
Electron configuration	[Ar]3d54s2
e- 's per energy level	2, 8,13,2
Oxidation states (Oxide)	7,6,4,2,3 (strong acid)
Crystal structure	cubic body centered
Physical properties
State of matter	solid (usually nonmagnetic)
Melting point	1517 K (2271 ?F)
Boiling point	2235 K (3564 ?F)
Molar volume	7.35 ×10-6 m3/mol
Heat of vaporization	226 kJ/mol
Heat of fusion	12.05 kJ/mol
Vapor pressure	121 Pa at 1517 K
Velocity of sound	5150 m/s at 293.15 K
Miscellaneous
Electronegativity	1.55 (Pauling scale)
Specific heat capacity	480 J/(kg*K)
Electrical conductivity	0.695 106/(m?ohm)
Thermal conductivity	7.82 W/(m*K)
1st ionization potential	717.3 kJ/mol
2nd ionization potential	1509 kJ/mol
3rd ionization potential	3248 kJ/mol
4th ionization potential	4940 kJ/mol
5th ionization potential	6990 kJ/mol
6th ionization potential	9220 kJ/mol
7th ionization potential	11500 kJ/mol
Most stable isotopes
iso NA half-life DM DE MeV DP 52Mn {syn.} 5.591 d ε 4.712 52Cr 53Mn {syn.} 3.74 million years ε 0.597 53Cr 54Mn {syn.} 312.3 d ε β- 1.377 0.697 54Cr 54Fe 55Mn 100% Mn is stable with 30 neutrons
SI units & STP are used except where noted.

Manganese is a chemical element in the periodic table that has the symbol Mn and atomic number 25.

Contents

1 Notable characteristics 2 Applications 3 History 4 Biological role 5 Occurrence 6 Compounds 7 Isotopes 8 Precautions 9 See also 10 References

Notable characteristics

Manganese is a gray-white metal, resembling iron. It is a hard metal and is very brittle, fusible with difficulty, but easily oxidized. Manganese metal is ferromagnetic only after special treatment.

The most common oxidation states of manganese are +2, +3, +4, +6 and +7, though oxidation states from +1 to +7 are observed. Mn²⁺ often competes with Mg²⁺ in biological systems, and manganese compounds where manganese is in oxidation state +7 are powerful oxidizing agents.

Applications

Manganese is essential to iron and steel production by virtue of its sulfur-fixing, deoxidizing, and alloying properties. Steelmaking, including its ironmaking component, has accounted for most manganese demand, presently in the range of 85% to 90% of the total demand. Among a variety of other uses, manganese is a key component of low-cost stainless steel formulations and certain widely used aluminium alloys. Manganese(IV) oxide (manganese dioxide) is used in the original type of dry cell battery. Manganese dioxide is also used as a catalyst. Manganese is used to decolorize glass (removing the greenish tinge that presence of iron produces) and, in higher concentration, make violet-colored glass. Manganese oxide is a brown pigment that can be used to make paint and is a component of natural umber. Potassium permanganate is a potent oxidizer and used in chemistry and in medicine as disinfectant agent.

The overall level and nature of manganese use in the United States is expected to remain about the same in the near term. No practical technologies exist for replacing manganese with other materials or for using domestic deposits or other accumulations to reduce the complete dependence of the United States on other countries for manganese ore.

Substitutes: Manganese has no satisfactory substitute in its major applications.

History

Manganese was in use in prehistoric times. Paints that were pigmented with manganese dioxide can be traced back 17,000 years. The Egyptians and Romans used manganese compounds in glass-making, to either remove color from glass or add color to it. Manganese can be found in the iron ores used by the Spartans. Some speculate that the exceptional hardness of Spartan steels derives from the inadvertent production of an iron-manganese alloy.

In the 17th century, the German chemist Johann Glauber (although some people believe that it was discovered by Ignites Kaim in 1770) first produced permanganate, a useful laboratory reagent. By the mid 18th century, manganese dioxide was in use in the manufacture of chlorine. The Swedish chemist Scheele was the first to recognize that manganese was an element, and his colleague, Johan Gottlieb Gahn, isolated the pure element in 1774 by reduction of the dioxide with carbon. Around the beginning of the 19th century, scientists began exploring the use of manganese in steelmaking, with patents being granted for its use at the time. In 1816, it was noted that adding manganese to iron made it harder, without making it any more brittle. In 1837, British academic Couper noted an association between heavy exposure to manganese in mines with a form of Parkinson's Disease.

Biological role

Manganese is an essential trace nutrient in all forms of life.

The classes of enzymes that have manganese cofactors are very broad and include such classes as oxidoreductases, transferases, hydrolases, lyases, isomerases, ligases, lectins, and integrins. The best known manganese-containing polypeptides may be arginase, Mn-containing superoxide dismutase, and the diphtheria toxin.

Occurrence

Manganese occurs principally as pyrolusite (MnO₂), and to a lesser extent as rhodochrosite (MnCO₃). Land-based resources are large but irregularly distributed; those of the United States are very low grade and have potentially high extraction costs. South Africa and Ukraine account for more than 80% of the world's identified resources; South Africa accounts for more than 80% of the total exclusive of China and Ukraine.

US Import Sources (1998-2001): Manganese ore: Gabon, 70%; South Africa, 10%; Australia, 9%; Mexico, 5%; and other, 6%. Ferromanganese: South Africa, 47%; France, 22%; Mexico, 8%; Australia, 8%; and other, 15%. Manganese contained in all manganese imports: South Africa, 31%; Gabon, 21%; Australia, 13%; Mexico, 8%; and other, 27%.

Manganese is mined in Burkina Faso.

Vast quantities of manganese exist in manganese nodules on the ocean floor. Attempts to find economically viable methods of harvesting manganese nodules were abandoned in the 1970s.

Compounds

Potassium permanganate, also called Condy's crystals, is a commonly used laboratory reagent because of its oxidizing properties and finds use as a topical medicine (for example, in the treatment of fish diseases).

Manganese(IV) oxide (manganese dioxide) is used in dry cells, and can be used to decolorize glass that is polluted by trace amounts of iron. Manganese compounds can color glass an amethyst color, and are responsible for the color of true amethyst. Manganese dioxide is also used in the manufacture of oxygen and chlorine, and in drying black paints.

The most stable oxidation state for manganese is +2, and many manganese(II) compounds are known, such as manganese(II) sulfate (MnSO₄) and manganese(II) chloride (MnCl₂). This oxidation state is also seen in the mineral rhodochrosite, (manganese(II) carbonate). The +3 oxidation state is also known, in compounds such as manganese(III) acetate, but these are quite powerful oxidising agents.

Isotopes

Naturally occurring manganese is composed of 1 stable isotope; 55-Mn. 18 radioisotopes have been characterized with the most stable being 53-Mn with a half-life of 3.7 million years, 54-Mn with a half-life of 312.3 days, and 52-Mn with a half-life of 5.591 days. All of the remaining radioactive isotopes have half lives that are less than 3 hours and the majority of these have half lives that are less than 1 minute. This element also has 3 meta states.

Manganese is part of the iron group of elements which are thought to be synthesized in large stars shortly before supernova explosion. Manganese-53 decays to ⁵³Cr with a half-life of 3.7 million years. Because of its relatively short half-life, ⁵³Mn is an extinct radionuclide. Manganese isotopic contents are typically combined with chromium isotopic contents and have found application in isotope geology. 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 indicate an initial ⁵³Mn/⁵⁵Mn ratio that suggests Mn-Cr isotopic systematics 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.

The isotopes of manganese range in atomic weight from 46 amu (46-Mn) to 65 amu (65-Mn). The primary decay mode before the most abundant stable isotope, 55-Mn, is electron capture and the primary mode after is beta decay.

Precautions

Manganese in excess is toxic. Exposure to manganese dusts and fumes should not exceed the ceiling value of 5 mg/m³ for even short periods because of its toxicity level.

Acidic permanganate solutions will oxidize any organic material they come into contact with. The oxidation process can generate enough heat to ignite some organic substances.

A form of Parkinson's Disease-type neurodegeneration called "manganism" has been linked to manganese exposure since the early 19th Century. Allegations of inhalation-induced manganism have been made regarding the welding industry. Listed on the Hazardous Substance List, manganese is regulated by OSHA due to its high level of toxicity.

See also

• Potassium permanganate
• Magnet
• Chemical element
• Periodic Table

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References

• Los Alamos National Laboratory – Manganese (http://periodic.lanl.gov/elements/25.html)