CHEMISTRY : Metal Cation Identification

Information on MERCURY

1. General Information


2. Occurence Uses and Properties


3. History of the Metal


4. Compounds
5. Back to Main Metal List

Mercury is the only elemental metal that is liquid at ordinary temperatures (cesium melts at about 28.5 C [83 F], gallium at about 30 C [86 F], and rubidium at about 39 C [102 F]). Mercury is silvery white, slowly tarnishes in moist air, freezes into a soft solid like tin or lead at about -39 C (-38 F), and alloys with most metals (iron is a notable exception) to form amalgams. Mercury does not wet glass or cling to it, and this property, coupled with its uniform volume expansion throughout its liquid range, makes it useful in thermometers. Barometers and manometers utilize its high density and low vapour pressure. The good electrical conductivity of mercury makes it exceptionally useful in sealed electrical switches and relays. An electrical discharge through mercury vapour produces a bluish glow rich in ultraviolet light, a phenomenon exploited in ultraviolet, fluorescent, and high-pressure mercury-vapour lamps. Mercury's high thermal neutron-capture cross section (360 barns) and good thermal conductivity make it applicable as a shield and coolant in nuclear reactors. Much mercury is utilized in the preparation of pharmaceuticals, agricultural and industrial fungicides, as dental fillings, and in the electrolytic production of chlorine and caustic soda.

Mercury occurs in the Earth's crust on the average of about 0.08 gram (0.003 ounce) per ton of rock. The principal ore is the red sulfide, cinnabar. Native mercury occurs in isolated drops and occasionally in larger fluid masses, usually with cinnabar, near volcanoes or hot springs. The free metal has been found in Spain (Almadén); in Yugoslavia, at Mount Avala; in Slovenia, at Idrija; in Germany (Moschellandsberg); and in the United States (Terlingua, Texas, and New Almaden, Calif.). For mineralogical properties, see native element (table).

Extremely rare natural alloys of mercury have also been found: moschellandsbergite (with silver), potarite (with palladium), and gold amalgam. Mercury is extracted from cinnabar by roasting it in air, followed by condensation of the mercury vapour. Mercury is toxic. Poisoning may result from inhalation of the vapour, ingestion of soluble compounds, or absorption of mercury through the skin.

Natural mercury is a mixture of seven stable isotopes: 196Hg (0.15 percent), 198Hg (10.02 percent), 199Hg (16.84 percent), 200Hg (23.13 percent), 201Hg (13.22 percent), 202Hg (29.80 percent), and 204Hg (6.85 percent). As a wavelength standard and for other precise work, isotopically pure mercury consisting of only mercury-198 is prepared by neutron bombardment of natural gold, gold-197.

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History

Mercury was known in Egypt and also probably in the East as early as 1500 BC. The name mercury originated in 6th-century alchemy, in which the symbol of the planet was used to represent the metal; the chemical symbol Hg derives from the Latin hydrargyrum, "liquid silver." Although its toxicity was recognized at an early date, its main appliCATion was for medical purposes.

The chief commercial source of mercury is cinnabar, or mercury sulfide, which is mined in shaft or open-pit operations and refined by flotation. Over half the world supply of mercury comes from Spain and Italy. Most of the methods of extraction of mercury rely on the volatility of the metal and the fact that cinnabar is readily decomposed by air or by lime to yield the free metal. Because of the toxicity of mercury and the threat of rigid pollution control, attention is being directed toward safer methods of extracting mercury. These generally rely on the fact that cinnabar is readily soluble in solutions of sodium hypochlorite or sulfide, from which the mercury can be recovered by precipitation with zinc or aluminum or by electrolysis. (For treatment of the commercial production of mercury, see mercury processing .)

The compounds of mercury are either of +1 or +2 oxidation state. Mercury(II) or mercuric compounds predominate. Mercury does not combine with oxygen to produce mercury(II) oxide, HgO, at a useful rate until heated to the range of 300 to 350 C (572 to 662 F). At temperatures of about 400 C (752 F) and above, the reaction reverses with the compound decomposing into its elements. Antoine-Laurent Lavoisier and Joseph Priestley used this reaction in their study of oxygen.

There are relatively few mercury(I) or mercurous compounds. The mercury(I) ion, Hg22+, is diatomic and stable. Mercury(I) chloride, Hg2Cl2 (commonly known as calomel), is probably the most important univalent compound. It is used in antiseptic salves. Mercury(II) chloride, HgCl2 (also called bichloride of mercury or corrosive sublimate), is perhaps the commonest bivalent compound. Although extremely toxic, this odourless, colourless substance has a wide variety of appliCATions.

In agriculture it is used as a fungicide; in medicine it is sometimes employed as a topical antiseptic in concentrations of one part per 2,000 parts of water; and in the chemical industry it serves as a CATalyst in the manufacture of vinyl chloride and as a starting material in the production of other mercury compounds. Mercury(II) oxide, HgO, provides elemental mercury for the preparation of various organic mercury compounds and certain inorganic mercury salts. This red or yellow crystalline solid is also used as an electrode (mixed with graphite) in zinc-mercuric oxide electric cells and in mercury batteries. Mercury(II) sulfide, HgS, is a black or red crystalline solid used chiefly as a pigment in paints, rubber, and plastics. The red form of the compound, occurring as the mineral cinnabar, is the world's primary source of mercury.

atomic number 80 atomic weight 200.59 melting point -38.87 C (-37.97 F) boiling point 356.9 C (674 F) specific gravity 13.5 (20 C [68 F]) valence 1, 2 electronic config. 2-8-18-32-18-2 or (Xe)4f 145d106s2 Mercury forms the mercury(II) ion Hg2+ and the mercury(I) ion (Hg2) 2+. In the latter, two electrons are shared in a covalent bond between the two metal atoms. The mercury(I) ion shows little tendency to form complexes, whereas the mercury(II) ion does form them. In contrast to mercury(II) compounds, which are usually covalent, all the common mercury(I) salts are ionic, and the soluble compounds--e.g., mercury(I) nitrate, Hg2 (NO3) 2--show normal properties of ionic compounds, such as ease of dissociation or breakup into separate ions.

Mercury is exceptional in that, unlike zinc or cadmium, it does not react easily with oxygen on heating, and mercury(II) oxide does not show the acid property of forming salts (mercurates), whereas zinc oxide does this readily. Mercury is again anomalous in that it does not produce hydrogen, as do zinc and cadmium, upon treatment with dilute acids. With fairly concentrated nitric acid, zinc and cadmium evolve oxides of nitrogen and form zinc or cadmium nitrates; mercury gives both mercury(II) nitrate, Hg(NO3)2, and mercury(I) nitrate, Hg2(NO3)2.

A further characteristic of mercury that is uncommon among metals is its readiness to form stable compounds containing a mercury-carbon bond or a mercury-nitrogen bond. As a result, mercury forms a wide variety of organic compounds (compounds that always contain carbon, usually also hydrogen, and often one or more of the elements oxygen, nitrogen, sulfur). On the whole, therefore, the zinc group elements do not show a smooth gradation of properties, mainly because of the number of anomalous properties of mercury, which in many respects shows a greater similarity to silver than to zinc and cadmium.

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