Manganese

25

chromium ← manganese → iron


-
↑
Mn
↓
Tc




periodic table




General


Name, Symbol, Number

manganese, Mn, 25


Chemical series
transition metals


Group, Period, Block

7, 4, d


Appearance
silvery metallic 



Atomic mass
54.938045(5) g/mol


Electron configuration
[Ar] 3d5 4s2


Electrons per shell
2, 8, 13, 2


Physical properties


Phase
solid


Density (near r.t.)
7.21 g/cm³


Liquid density at m.p.
5.95 g/cm³


Melting point
1519 K
(1246 °C, 2275 °F)


Boiling point
2334 K
(2061 °C, 3742 °F)


Heat of fusion
12.91 kJ/mol


Heat of vaporization
221 kJ/mol


Heat capacity
(25 °C) 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


Crystal structure
cubic body centered


Oxidation states
7, 6, 4, 2, 3
(strongly acidic oxide)


Electronegativity
1.55 (Pauling scale)


Ionization energies
(more)

1st: 717.3 kJ/mol


2nd: 1509.0 kJ/mol


3rd: 3248 kJ/mol


Atomic radius
140 pm


Atomic radius (calc.)
161 pm


Covalent radius
139 pm


Miscellaneous


Magnetic ordering
nonmagnetic


Electrical resistivity
(20 °C) 1.44 µΩ·m


Thermal conductivity
(300 K) 7.81 W/(m·K)


Thermal expansion
(25 °C) 21.7 µm/(m·K)


Speed of sound (thin rod)
(20 °C) 5150 m/s


Speed of sound (thin rod)
(r.t.) 198 m/s


Bulk modulus
120 GPa


Mohs hardness
6.0


Brinell hardness
196 MPa


CAS registry number
7439-96-5


Notable isotopes




Main article: Isotopes of manganese


iso

NA

half-life

DM

DE (MeV)

DP


52Mn

syn

5.591 d

ε

-

52Cr


β+

0.575

52Cr


γ

0.7, 0.9, 1.4

-


53Mn

syn

3.74 ×106 y

ε

-

53Cr


54Mn

syn

312.3 d

ε

-

54Cr


γ

0.834

-


55Mn

100%

Mn is stable with 30 neutrons


Manganese (chemical symbol Mn, atomic number 25) is a gray-white metal that combines with other elements in various proportions. In nature, it occurs mainly in the form of a black-brown oxide (MnO2), which was used as a paint pigment as far back as 17,000 years ago. Manganese is part of the iron group of elements that are thought to be synthesized in large stars shortly before supernova explosion.

Contents

1 Occurrence
2 History
3 Notable characteristics

3.1 Isotopes


4 Applications
5 Biological role
6 Compounds
7 Precautions
8 See also
9 Notes
10 References
11 External links
12 Credits



The greatest demand for manganese is for the production of iron and steel. In addition, it is a key component of low-cost stainless steel and certain aluminum alloys. At low concentrations, it is used to decolorize glass, while at higher concentrations, it is used to make violet-colored glass. Manganese dioxide, besides being a useful pigment, is a catalyst and a component of certain dry cell batteries. Potassium permanganate is a potent oxidizer and disinfectant. Manganese (in the form of manganese ions) is an essential trace nutrient in all known forms of life. On the other hand, excess manganese is toxic.

Occurrence
 Manganese ore
Manganese occurs principally as the mineral pyrolusite (manganese(IV) oxide, MnO2), and to a lesser extent as rhodochrosite (manganese(II) carbonate, 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 percent of the world's identified resources. In addition, manganese is mined in Burkina Faso and Gabon. Vast quantities of manganese exist in manganese nodules on the ocean floor, but attempts to find economically viable methods of harvesting manganese nodules were abandoned in the 1970s.
U.S. import sources (1998-2001):

Manganese ore: Gabon, 70 percent; South Africa, ten percent; Australia, nine percent; Mexico, five percent; and other, six percent.
Ferromanganese: South Africa, 47 percent; France, 22 percent; Mexico, eight percent; Australia, eight percent; and other, 15 percent.
Manganese contained in all manganese imports: South Africa, 31 percent; Gabon, 21 percent; Australia, 13 percent; Mexico, eight percent; and other, 27 percent.
History
Manganese (from the Latin word magnes, meaning "magnet") was in use in prehistoric times, in the form of its compounds. Paints that were pigmented with manganese dioxide (manganese(IV) oxide) 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 seventeenth century, German chemist Johann Glauber first produced permanganate, a useful laboratory reagent. (Some, however, believe that it was discovered by Ignites Kaim in 1770). By the mid-eighteenth century, manganese dioxide was in use in the manufacture of chlorine. Swedish chemist Carl Wilhelm 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 nineteenth century, scientists began exploring the use of manganese in steelmaking, and patents were 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 James Couper noted an association between heavy exposure to manganese in mines with a form of Parkinson's disease. In 1912, patents were issued in the United States for methods of using manganese for "Parkerizing" (electrochemical conversion coating of) firearms to protect them from rust and corrosion.

Notable characteristics
 Manganese
In chemistry, manganese is considered a transition metal. It is placed in period four and group seven (former group 7B) of the periodic table. In period four, it lies between chromium (Cr) and iron (Fe), and in group seven, it is positioned above technetium (Tc) and rhenium (Re). Manganese is very brittle, fusible with difficulty, but easily oxidized. After special treatment, manganese metal becomes ferromagnetic—that is, it acquires the "normal" form of magnetism that most people are familiar with.
Manganese combines with various other elements in different proportions. The oxidation states of manganese are known to range from +1 to +7, but the most common ones are +2, +3, +4, +6, and +7. Mn2+ often competes with Mg2+ in biological systems. Compounds in which manganese is in oxidation state +7 are powerful oxidizing agents.

Isotopes
The isotopes of manganese range in atomic weight from 46 atomic mass units (amu) (46Mn) to 65 amu (65Mn). Naturally occurring manganese consists of one stable isotope: 55Mn. In addition, 18 radioisotopes have been characterized, of which the most stable is 53Mn, with a half-life of 3.7 million years. The isotope 54Mn has a half-life of 312.3 days, and 52Mn has a half-life of 5.591 days. The remaining radioactive isotopes have half-lives under three hours, and most of these have half-lives less than one minute.
Manganese is part of the iron group of elements that are thought to be synthesized in large stars shortly before supernova explosion. Given that 53Mn decays to 53Cr, 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 isotopic ratios of other elements (26Al and 107Pd) for the early history of the solar system.

Applications
 Manganite, a manganese oxide
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 85–90 percent of the total demand. Among its other uses, manganese is a key component of low-cost stainless steel formulations and certain widely used aluminum alloys. It is also added to gasoline to reduce engine knock. At low concentrations, manganese is used to decolorize glass, as it removes the greenish tinge generated by the presence of iron; at higher concentrations, it is used to make violet-colored glass.
Manganese dioxide, a component of natural umber, is useful as a black-brown pigment in paint. It is also a catalyst and is used in the original type of dry cell battery. Potassium permanganate is a potent oxidizer used in chemical reactions; it is also used in medicine as a disinfectant. The technique known as manganese phosphating (or Parkerizing) is used to prevent the rusting and corrosion of steel. On rare occasions, manganese is used in coins. The only U.S. coins to use manganese were the "wartime" nickel (1942–1945) and the Sacagawea dollar (2000–present).
In 1912, patents were issued in the United States for methods of using manganese for "Parkerizing" (electrochemical conversion coating of) firearms to protect them from rust and corrosion, and these methods have been in widespread use ever since.
Manganese has no satisfactory substitute in its major applications. In minor applications, (such as manganese phosphating), zinc and sometimes vanadium are viable substitutes.

Biological role
Manganese (in the form of manganese ions) is an essential trace nutrient in all known forms of life. Many classes of enzymes have manganese cofactors. They include oxidoreductases, transferases, hydrolases, lyases, isomerases, ligases, lectins, and integrins. The best-known manganese-containing polypeptides (protein-like chains) may be arginase, Mn-containing superoxide dismutase, and the diphtheria toxin.

Compounds
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—these are quite powerful oxidizing agents.
Potassium permanganate (KMnO4), also called Condy's crystals, is an oxidizing agent and a commonly used laboratory reagent. It also finds use as a topical medicine, such as in the treatment of fish diseases.
Manganese(IV) oxide (manganese dioxide, MnO2) is used in dry cells, and can be used to decolorize glass that is polluted by trace amounts of iron. It is also used in the manufacture of oxygen and chlorine and in black paints. Manganese compounds can color glass an amethyst color, and are responsible for the color of true amethyst.

Precautions
Manganese in excess is toxic. Exposure to manganese dusts and fumes should not exceed the upper limit of five milligrams per cubic meter (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.
In 2005, a study suggested a possible link between manganese inhalation and central nervous system toxicity in rats.[1] It is hypothesized that long-term exposure to naturally occurring manganese in shower water puts up to 8.7 million Americans at risk.
A form of Parkinson's disease-type neurodegeneration called "manganism" has been linked to manganese exposure among miners and smelters since the early nineteenth century. Allegations of inhalation-induced manganism have been made regarding the welding industry. In the United States, manganese exposure in workplaces is regulated by the Occupational Safety and Health Administration (OSHA).[2]

See also
Chemical element
Magnetism
Periodic table
Transition metal
Notes

↑ Article Retrieved December 18, 2007.

↑ U.S. Department of Labor Retrieved December 18, 2007.


ReferencesISBN links support NWE through referral fees
Los Alamos National Laboratory – Manganese Retrieved December 18, 2007.
External links
All links retrieved November 5, 2022.

WebElements.com – Manganese
International Manganese Institute

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