Chromium

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Vanadium - Chromium - Manganese Cr Mo       Full table
General
Name, Symbol, Number	Chromium, Cr, 24
Chemical series	Transition metals
Group, Period, Block	6 , 4 , d
Density, Hardness	7140 kg/m3, 8.5
Appearance	silvery metallic
Atomic Properties
Atomic weight	51.9961 amu
Atomic radius (calc.)	140 (166) pm
Covalent radius	127 pm
van der Waals radius	n/a pm
Electron configuration	[Ar]3d54s1
e- 's per energy level	2, 8, 13, 1
Oxidation states (Oxide)	6,3,2 (strong acid)
Crystal structure	Cubic, body centered
Physical Properties
State of matter	solid (__)
Melting point	2130 K (3375 °F)
Boiling point	2945 K (4842 °F)
Molar volume	7.23 ×10-3 m3/mol
Heat of vaporization	344.3 kJ/mol
Heat of fusion	16.9 kJ/mol
Vapor pressure	990 Pa at 2130 K
Velocity of sound	5940 m/s at 293.15 K
Miscellaneous
Electronegativity	1.66 (Pauling scale)
Specific heat capacity	450 J/(kg*K)
Electrical conductivity	7.74 106/m ohm
Thermal conductivity	93.7 W/(m*K)
1st ionization potential	652.9 kJ/mol
2nd ionization potential	1590.6 kJ/mol
3rd ionization potential	2987 kJ/mol
4th ionization potential	4743 kJ/mol
5th ionization potential	6702 kJ/mol
6th ionization potential	8744.9 kJ/mol
Most Stable Isotopes
iso NA half-life DM DE MeV DP 50Cr {syn.} > 1.8E17 years e capture ??? 50Ti 51Cr {syn.} 27.7025 days e capture 0.753 51V 52Cr 83.789% Cr is stable with 28 neutrons 53Cr 9.501% Cr is stable with 29 neutrons 54Cr 2.365% Cr is stable with 30 neutrons
SI units & STP are used except where noted.

Chromium is a chemical element in the periodic table that has the symbol Cr and atomic number 24.

Table of contents 1 Notable Characteristics 2 Applications 3 History 4 Biological Role 5 Occurrence 6 Compounds 7 Isotopes 8 Precautions 9 External Links

Notable Characteristics Chromium is a steel-gray, lustrous, hard metal that takes a high polish, is fusible with difficulty, and is resistant to corrosion and tarnishing.

The most common oxidation states of chromium are +2, +3, and +6, with +3 being the most stable. +4 and +5 are relatively rare. Chromium compounds of oxidation state 6 are powerful oxidants. Applications Uses of chromium:

• In metallurgy, to impart corrosion resistance and a shiny finish:
  • as an alloy constituent, e.g. in stainless steel,
  • in chrome plating[?],
  • in anodized aluminum[?].
• As a catalyst.
• Chromite is used to make molds for the firing of bricks.
• Chromium salts color glass an emerald green.
• The chromates and oxides are used in dyes and paints.
• Potassium dichromate is a chemical reagent, used in cleaning laboratory glassware and as a titrating agent. It is also used as a mordant (i.e. a fixing agent) for dyes in fabric.

History In 1761, Johann Gottlob Lehmann found an orange-red mineral in the Ural Mountains which he named Siberian red lead. Though misidentified as a lead compound with selenium and iron components, the material was in fact a lead chromate (PbCrO₄).

In 1770, Peter Simon Pallas visited the same site as Lehmann and found a red "lead" mineral that had very useful properties as a pigment in paints. The use of Siberian red lead as a paint pigment developed rapidly. A bright yellow made from crocoite became a very fashionable color.

In 1797, Nicolas-Louis Vauquelin received samples of crocoite ore. He was able to produce chromium oxide (CrO₃) by mixing crocoite with hydrochloric acid. In 1798, Vauquelin discovered that he could isolate metallic chromium by heating the oxide in a charcoal oven. He was also able to detect traces of chromium in precious gems, such as ruby, or emerald.

During the 1800s chromium was primarily used as a component of paints but now the primary use (85%) is for metal alloys, with the remainder used in the chemical industry and refractory and foundry industries. Biological Role Trivalent chromium is an essential trace metal and is required for the proper metabolism of sugar in humans. Chromium deficiencies can affect the potency of insulin in regulating sugar balance. Unlike other essential trace metals, chromium has not been found in a metalloprotein with biological activity. Therefore, the functional basis for the chromium requirement in the diet remains unexplained.

Occurrence Chromium is mined as chromite (FeCr₂O₄) ore. Chromium is obtained commercially by heating the ore in the presence of aluminum or silicon. Roughly half the chromite ore in the world is produced in South Africa. Kazakhstan, India and Turkey are also substantial producers. Untapped chromite deposits are plentiful, but geographically concentrated in Kazakhstan and southern Africa. Approximately 15 million tons of marketable chromite ore were produced in 2000, and converted into approximately 4 million tons of ferro-chrome with an approximate market value of 2.5 billion US dollars.

Though native chromium deposits are rare, some native chromium metal has been discovered. The Udachnaya Mine in Russia produces samples of the native metal. This mine is a kimberlite pipe rich in diamonds, and the reducing environment so provided helped produce both elemental chromium and diamond. Compounds

Potassium dichromate is a powerful oxidizing agent and is the preferred compound for cleaning laboratory glassware of any possible organics. Chrome green is the green oxide of chromium, Cr₂O₃, used in enamel painting, and glass staining. Chrome yellow is a brilliant yellow pigment, PbCrO₄, used by painters.

Isotopes Naturally occurring chromium is composed of 3 stable isotopes; 52-Cr, 53-Cr, and 54-Cr with 52-Cr being the most abundant (83.789% natural abundance). 19 radioisotopes have been characterized with the most stable being 50-Cr with a half-life of (more than) 1.8E17 years, and 51-Cr with a half-life of 27.7025 days. All of the remaining radioactive isotopes have half-lifes that are less than 24 hours and the majority of these have half lifes that are less than 1 minute. This element also has 2 meta states.

Chromium-53 is the radiogenic decay product of ⁵³Mn. Chromium isotopic contents are typically combined with manganese isotopic contents and have found application in isotope geology[?]. Mn-Cr isotope 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 isotope systematics must result from in-situ decay of ⁵³Mn in differentiated planetary bodies. Hence ⁵³Cr provides additional evidence for nucleosynthetic processes immediately before coalescence of the solar system.

The isotopes of chromium range in atomic weight from 43 amu (43-Cr) to 67 amu (67-Cr). The primary decay mode before the most abundant stable isotope, 52-Cr, is electron capture and the primary mode after is beta. Precautions Chromium metal and chromium(III) compounds are not usually considered health hazards, but chromium (VI) compounds can be toxic if orally ingested. The lethal dose of poisonous chromium (VI) compounds is about one half teaspoon of material. At nonlethal doses, chromium(VI) is an established human carcinogen. Most chromium (VI) compounds are irritating to eyes, skin and mucous membranes. Chronic exposure to chromium (VI) compounds can cause permanent eye injury, unless properly treated.

The 1958 the World Heath Organization recommended a maximum allowable concentration of 0.05 mg/liter in drinking water for chromium (VI), based on health concerns. This recommendation has been reviewed a number of times and this value has not been revised in the meantime.

External Links

• WebElements.com - Chromium (http://www.webelements.com/webelements/elements/text/Cr/index)
• EnvironmentalChemistry.com - Chromium (http://environmentalchemistry.com/yogi/periodic/Cr)
• International Chromium Development Association (http://www.chromium-asoc.com/)
• It's Elemental - The Element Chromium (http://education.jlab.org/itselemental/ele024)
• Native Chromium (http://mineral.galleries.com/minerals/elements/chromium/chromium.htm)
• The Merck Manual - Mineral Deficiency and Toxicity (http://www.merck.com/pubs/mmanual/section1/chapter4/4f.htm)