Mercury (element)

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Mercury, 80Hg
Pouring liquid mercury bionerd.jpg
Mercury
Appearanceshiny, silvery liquid
Standard atomic weight Ar°(Hg)
Mercury 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
Cd

Hg

Cn
goldmercurythallium
Atomic number (Z)80
Group group 12
Period period 6
Block   d-block
Electron configuration [ Xe ] 4f14 5d10 6s2
Electrons per shell2, 8, 18, 32, 18, 2
Physical properties
Phase at  STP liquid
Melting point 234.3210  K (−38.8290 °C,−37.8922 °F)
Boiling point 629.88 K(356.73 °C,674.11 °F)
Density (near r.t.)13.546 [3]  g/cm3
Triple point 234.3156 K,1.65×10−7 kPa
Critical point 1750 K, 172.00 MPa
Heat of fusion 2.29  kJ/mol
Heat of vaporization 59.11 kJ/mol
Molar heat capacity 27.983 J/(mol·K)
Vapor pressure
P (Pa)1101001 k10 k100 k
at T (K)315350393449523629
Atomic properties
Oxidation states −2 , +1, +2(a mildly basic oxide)
Electronegativity Pauling scale: 2.00
Ionization energies
  • 1st: 1007.1 kJ/mol
  • 2nd: 1810 kJ/mol
  • 3rd: 3300 kJ/mol
Atomic radius empirical:151  pm
Covalent radius 132±5 pm
Van der Waals radius 155 pm
Mercury spectrum visible.png
Spectral lines of mercury
Other properties
Natural occurrence primordial
Crystal structure rhombohedral
Rhombohedral.svg
Thermal expansion 60.4 µm/(m⋅K)(at 25 °C)
Thermal conductivity 8.30 W/(m⋅K)
Electrical resistivity 961 nΩ⋅m(at 25 °C)
Magnetic ordering diamagnetic [4]
Molar magnetic susceptibility −33.44×10−6 cm3/mol(293 K) [5]
Speed of sound liquid: 1451.4 m/s (at 20 °C)
CAS Number 7439-97-6
History
Discovery Ancient Egyptians(before 1500 BCE)
Symbol"Hg": from its Latin name hydrargyrum , itself from Greek hydrárgyros , 'water-silver'
Isotopes of mercury
Main isotopes [6] Decay
abun­dance half-life (t1/2) mode pro­duct
194Hg synth 444 y ε 194Au
195Hgsynth9.9 hε 195Au
196Hg0.15% stable
197Hgsynth64.14 hε 197Au
198Hg10.0%stable
199Hg16.9%stable
200Hg23.1%stable
201Hg13.2%stable
202Hg29.7%stable
203Hgsynth46.612 d β 203Tl
204Hg6.82%stable
Symbol category class.svg  Category: Mercury (element)
| references

Mercury is a chemical element; it has symbol Hg and atomic number 80. It is also known as quicksilver and was formerly named hydrargyrum ( /hˈdrɑːrərəm/ hy-DRAR-jər-əm) from the Greek words hydor (water) and argyros (silver). [7] A heavy, silvery d-block element, mercury is the only metallic element that is known to be liquid at standard temperature and pressure; the only other element that is liquid under these conditions is the halogen bromine, though metals such as caesium,gallium, and rubidium melt just above room temperature.

Contents

Mercury occurs in deposits throughout the world mostly as cinnabar (mercuric sulfide). The red pigment vermilion is obtained by grinding natural cinnabar or synthetic mercuric sulfide. Exposure to mercury and mercury-containing organic compounds is toxic to the nervous system, immune system and kidneys of humans and other animals; mercury poisoning can result from exposure to water-soluble forms of mercury (such as mercuric chloride or methylmercury) either directly or through mechanisms of biomagnification.

Mercury is used in thermometers, barometers, manometers, sphygmomanometers, float valves, mercury switches, mercury relays, fluorescent lamps and other devices, although concerns about the element's toxicity have led to the phasing out of such mercury-containing instruments. [8] It remains in use in scientific research applications and in amalgam for dental restoration in some locales. It is also used in fluorescent lighting. Electricity passed through mercury vapor in a fluorescent lamp produces short-wave ultraviolet light, which then causes the phosphor in the tube to fluoresce, making visible light.

Properties

Physical properties

An old pound coin (density ~7.6 g/cm ) floats on mercury due to the combination of the buoyant force and surface tension. Pound-coin-floating-in-mercury.jpg
An old pound coin (density ~7.6 g/cm ) floats on mercury due to the combination of the buoyant force and surface tension.

Mercury is a heavy, silvery-white metal that is liquid at room temperature. Compared to other metals, it is a poor conductor of heat, but a fair conductor of electricity. [10]

It has a freezing point of −38.83 °C and a boiling point of 356.73 °C, [11] [12] [13] both the lowest of any stable metal, although preliminary experiments on copernicium and flerovium have indicated that they have even lower boiling points. [14] This effect is due to lanthanide contraction and relativistic contraction reducing the radius of the outermost electrons, and thus weakening the metallic bonding in mercury. [11] Upon freezing, the volume of mercury decreases by 3.59% and its density changes from 13.69 g/cm3 when liquid to 14.184 g/cm3 when solid. The coefficient of volume expansion is 181.59 × 10−6 at 0 °C, 181.71 × 10−6 at 20 °C and 182.50 × 10−6 at 100 °C (per °C). Solid mercury is malleable and ductile, and can be cut with a knife. [15]

Table of thermal and physical properties of liquid mercury: [16] [17]

Temperature (°C)Density (kg/m^3)Specific heat (kJ/kg K)Kinematic viscosity (m^2/s)Conductivity (W/m K)Thermal diffusivity (m^2/s)Prandtl NumberBulk modulus (K^-1)
013628.220.14031.24E-078.24.30E-060.02880.000181
2013579.040.13941.14E-078.694.61E-060.02490.000181
5013505.840.13861.04E-079.45.02E-060.02070.000181
10013384.580.13739.28E-0810.515.72E-060.01620.000181
15013264.280.13658.53E-0811.496.35E-060.01340.000181
20013144.940.1578.02E-0812.346.91E-060.01160.000181
25013025.60.13577.65E-0813.077.41E-060.01030.000183
315.5128470.1346.73E-0814.028.15E-060.00830.000186

Chemical properties

Mercury does not react with most acids, such as dilute sulfuric acid, although oxidizing acids such as concentrated sulfuric acid and nitric acid or aqua regia dissolve it to give sulfate, nitrate, and chloride. Like silver, mercury reacts with atmospheric hydrogen sulfide. Mercury reacts with solid sulfur flakes, which are used in mercury spill kits to absorb mercury (spill kits also use activated carbon and powdered zinc). [18]

Amalgams

Mercury-discharge spectral calibration lamp Mercury discharge tube.jpg
Mercury-discharge spectral calibration lamp

Mercury dissolves many metals such as gold and silver to form amalgams. Iron is an exception, and iron flasks have traditionally been used to transport the material. [19] Several other first row transition metals with the exception of manganese, copper and zinc are also resistant in forming amalgams. Other elements that do not readily form amalgams with mercury include platinum. [20] [21] Sodium amalgam is a common reducing agent in organic synthesis, and is also used in high-pressure sodium lamps.

Mercury readily combines with aluminium to form a mercury-aluminium amalgam when the two pure metals come into contact. Since the amalgam destroys the aluminium oxide layer which protects metallic aluminium from oxidizing in-depth (as in iron rusting), even small amounts of mercury can seriously corrode aluminium. For this reason, mercury is not allowed aboard an aircraft under most circumstances because of the risk of it forming an amalgam with exposed aluminium parts in the aircraft. [22]

Mercury embrittlement is the most common type of liquid metal embrittlement, as mercury is a natural component of some hydrocarbon reservoirs and will come into contact with petroleum processing equipment under normal conditions. [23]

Isotopes

There are seven stable isotopes of mercury, with 202
Hg
being the most abundant (29.86%). The longest-lived radioisotopes are 194
Hg
with a half-life of 444 years, and 203
Hg
with a half-life of 46.612 days. Most of the remaining radioisotopes have half-lives that are less than a day. 206
Hg
occurs naturally in tiny traces as an intermediate decay product of 238
U
. 199
Hg
and 201
Hg
are the most often studied NMR-active nuclei, having spins of 12 and 32 respectively. [10]

Etymology

The symbol for the planet Mercury () has been used since ancient times to represent the element Mercury symbol (fixed width).svg
The symbol for the planet Mercury (☿) has been used since ancient times to represent the element

"Hg" is the modern chemical symbol for mercury. It is an abbreviation of hydrargyrum, a romanized form of the ancient Greek name for mercury, ὑδράργυρος (hydrargyros). Hydrargyros is a Greek compound word meaning "water-silver", from ὑδρ- (hydr-), the root of ὕδωρ (hydor) "water", and ἄργυρος (argyros) "silver". [7] Like the English name quicksilver ("living-silver"), this name was due to mercury's liquid and shiny properties. [24]

The modern English name "mercury" comes from the planet Mercury. In medieval alchemy, the seven known metals—quicksilver, gold, silver, copper, iron, lead, and tin—were associated with the seven planets. Quicksilver was associated with the fastest planet, which had been named after the Roman god Mercury, who was associated with speed and mobility. The astrological symbol for the planet became one of the alchemical symbols for the metal, and "Mercury" became an alternative name for the metal. Mercury is the only metal for which the alchemical planetary name survives, as it was decided it was preferable to "quicksilver" as a chemical name. [25] [26]

History

Mercury was found in Egyptian tombs that date from 1500 BC; [27] cinnabar, the most common natural source of mercury, has been in use since the Neolithic Age. [28]

In China and Tibet, mercury use was thought to prolong life, heal fractures, and maintain generally good health, although it is now known that exposure to mercury vapor leads to serious adverse health effects. [29] The first emperor of a unified China, Qín Shǐ Huáng Dì—allegedly buried in a tomb that contained rivers of flowing mercury on a model of the land he ruled, representative of the rivers of China—was reportedly killed by drinking a mercury and powdered jade mixture formulated by Qin alchemists intended as an elixir of immortality. [30] [31] Khumarawayh ibn Ahmad ibn Tulun, the second Tulunid ruler of Egypt (r. 884–896), known for his extravagance and profligacy, reportedly built a basin filled with mercury, on which he would lie on top of air-filled cushions and be rocked to sleep. [32]

In November 2014 "large quantities" of mercury were discovered in a chamber 60 feet below the 1800-year-old pyramid known as the "Temple of the Feathered Serpent," "the third largest pyramid of Teotihuacan," Mexico along with "jade statues, jaguar remains, a box filled with carved shells and rubber balls". [33]

Aristotle recounts that Daedalus made a wooden statue of Venus move by pouring quicksilver in its interior. [34] In Greek mythology Daedalus gave the appearance of voice in his statues using quicksilver. The ancient Greeks used cinnabar (mercury sulfide) in ointments; the ancient Egyptians and the Romans used it in cosmetics. In Lamanai, once a major city of the Maya civilization, a pool of mercury was found under a marker in a Mesoamerican ballcourt. [35] [36] By 500 BC mercury was used to make amalgams (Medieval Latin amalgama, "alloy of mercury") with other metals. [37]

Alchemists thought of mercury as the First Matter from which all metals were formed. They believed that different metals could be produced by varying the quality and quantity of sulfur contained within the mercury. The purest of these was gold, and mercury was called for in attempts at the transmutation of base (or impure) metals into gold, which was the goal of many alchemists. [25]

The mines in Almadén (Spain), Monte Amiata (Italy), and Idrija (now Slovenia) dominated mercury production from the opening of the mine in Almadén 2500 years ago, until new deposits were found at the end of the 19th century. [38]

Occurrence

Mercury is an extremely rare element in Earth's crust, having an average crustal abundance by mass of only 0.08 parts per million (ppm). [39] Because it does not blend geochemically with those elements that constitute the majority of the crustal mass, mercury ores can be extraordinarily concentrated considering the element's abundance in ordinary rock. The richest mercury ores contain up to 2.5% mercury by mass, and even the leanest concentrated deposits are at least 0.1% mercury (12,000 times average crustal abundance). It is found either as a native metal (rare) or in cinnabar, metacinnabar, sphalerite, corderoite, livingstonite and other minerals, with cinnabar (HgS) being the most common ore. [40] [41] Mercury ores often occur in hot springs or other volcanic regions. [42]

Beginning in 1558, with the invention of the patio process to extract silver from ore using mercury, mercury became an essential resource in the economy of Spain and its American colonies. Mercury was used to extract silver from the lucrative mines in New Spain and Peru. Initially, the Spanish Crown's mines in Almadén in Southern Spain supplied all the mercury for the colonies. [43] Mercury deposits were discovered in the New World, and more than 100,000 tons of mercury were mined from the region of Huancavelica, Peru, over the course of three centuries following the discovery of deposits there in 1563. The patio process and later pan amalgamation process continued to create great demand for mercury to treat silver ores until the late 19th century. [44]

Native mercury with cinnabar, Socrates mine, Sonoma County, California. Cinnabar sometimes alters to native mercury in the oxidized zone of mercury deposits. Mercury-27128.jpg
Native mercury with cinnabar, Socrates mine, Sonoma County, California. Cinnabar sometimes alters to native mercury in the oxidized zone of mercury deposits.

Former mines in Italy, the United States and Mexico, which once produced a large proportion of the world supply, have now been completely mined out or, in the case of Slovenia (Idrija) and Spain (Almadén), shut down due to the fall of the price of mercury. Nevada's McDermitt Mine, the last mercury mine in the United States, closed in 1992. The price of mercury has been highly volatile over the years and in 2006 was $650 per 76-pound (34.46 kg) flask. [45]

Mercury is extracted by heating cinnabar in a current of air and condensing the vapor. The equation for this extraction is:

HgS + O2 → Hg + SO2
Evolution of mercury price (U.S.) and production (worldwide) HgProductionPrice.png
Evolution of mercury price (U.S.) and production (worldwide)

In 2020, China was the top producer of mercury, providing 88% of the world output (2200 out of 2500 tonnes), followed by Tajikistan (178 t), Russia (50 t) and Mexico (32 t). [46]

Because of the high toxicity of mercury, both the mining of cinnabar and refining for mercury are hazardous and historic causes of mercury poisoning. [47] In China, prison labor was used by a private mining company as recently as the 1950s to develop new cinnabar mines. Thousands of prisoners were used by the Luo Xi mining company to establish new tunnels. [48] Worker health in functioning mines is at high risk.

A newspaper claimed that an unidentified European Union directive calling for energy-efficient lightbulbs to be made mandatory by 2012 encouraged China to re-open cinnabar mines to obtain the mercury required for CFL bulb manufacture. Environmental dangers have been a concern, particularly in the southern cities of Foshan and Guangzhou, and in Guizhou province in the southwest. [48]

Abandoned mercury mine processing sites often contain very hazardous waste piles of roasted cinnabar calcines. Water run-off from such sites is a recognized source of ecological damage. Former mercury mines may be suited for constructive re-use; for example, in 1976 Santa Clara County, California purchased the historic Almaden Quicksilver Mine and created a county park on the site, after conducting extensive safety and environmental analysis of the property. [49]

Chemistry

All known mercury compounds exhibit one of two positive oxidation states: I and II. Experiments have failed to unequivocally demonstrate any higher oxidation states: both the claimed 1976 electrosynthesis of an unstable Hg(III) species and 2007 cryogenic isolation of HgF4 have disputed interpretations and remain difficult (if not impossible) to reproduce. [50]

Compounds of mercury(I)

Unlike its lighter neighbors, cadmium and zinc, mercury usually forms simple stable compounds with metal-metal bonds. Most mercury(I) compounds are diamagnetic and feature the dimeric cation, Hg2+
2
. Stable derivatives include the chloride and nitrate. Treatment of Hg(I) compounds complexation with strong ligands such as sulfide, cyanide, etc. and induces disproportionation to Hg2+
and elemental mercury. [51] Mercury(I) chloride, a colorless solid also known as calomel, is really the compound with the formula Hg2Cl2, with the connectivity Cl-Hg-Hg-Cl. It reacts with chlorine to give mercuric chloride, which resists further oxidation. Mercury(I) hydride, a colorless gas, has the formula HgH, containing no Hg-Hg bond; however, the gas has only ever been observed as isolated molecules. [52]

Indicative of its tendency to bond to itself, mercury forms mercury polycations, which consist of linear chains of mercury centers, capped with a positive charge. One example is Hg2+
3
(AsF
6
)

2
. [53]

Compounds of mercury(II)

Mercury(II) is the most common oxidation state and is the main one in nature as well. All four mercuric halides are known and have been demonstrated to form linear coordination geometry, despite mercury's tendency to form tetrahedral molecular geometry with other ligands. This behavior is similar to the Ag+ ion. The best known mercury halide is mercury(II) chloride, an easily sublimating white solid. [54]

Mercury(II) oxide, the main oxide of mercury, arises when the metal is exposed to air for long periods at elevated temperatures. It reverts to the elements upon heating near 400 °C, as was demonstrated by Joseph Priestley in an early synthesis of pure oxygen. [18] Hydroxides of mercury are poorly characterized, as attempted isolation studies of mercury(II) hydroxide have yielded mercury oxide instead. [55]

Being a soft metal, mercury forms very stable derivatives with the heavier chalcogens. Preeminent is mercury(II) sulfide, HgS, which occurs in nature as the ore cinnabar and is the brilliant pigment vermilion. Like ZnS, HgS crystallizes in two forms, the reddish cubic form and the black zinc blende form. [10] The latter sometimes occurs naturally as metacinnabar. [41] Mercury(II) selenide (HgSe) and mercury(II) telluride (HgTe) are also known, these as well as various derivatives, e.g. mercury cadmium telluride and mercury zinc telluride being semiconductors useful as infrared detector materials. [56]

Mercury(II) salts form a variety of complex derivatives with ammonia. These include Millon's base (Hg2N+), the one-dimensional polymer (salts of HgNH+
2
)
n
), and "fusible white precipitate" or [Hg(NH3)2]Cl2. Known as Nessler's reagent, potassium tetraiodomercurate(II) (HgI2−
4
) is still occasionally used to test for ammonia owing to its tendency to form the deeply colored iodide salt of Millon's base. [57]

Mercury fulminate is a detonator widely used in explosives. [10]

Organomercury compounds

Organic mercury compounds are historically important but are of little industrial value in the western world. Mercury(II) salts are a rare example of simple metal complexes that react directly with aromatic rings. Organomercury compounds are always divalent and usually two-coordinate and linear geometry. Unlike organocadmium and organozinc compounds, organomercury compounds do not react with water. They usually have the formula HgR2, which are often volatile, or HgRX, which are often solids, where R is aryl or alkyl and X is usually halide or acetate. Methylmercury, a generic term for compounds with the formula CH3HgX, is a dangerous family of compounds that are often found in polluted water. [58] They arise by a process known as biomethylation.

Applications

The bulb of a mercury-in-glass thermometer Maximum thermometer close up 2.JPG
The bulb of a mercury-in-glass thermometer

Mercury is used primarily for the manufacture of industrial chemicals or for electrical and electronic applications. It is used in some liquid-in-glass thermometers, especially those used to measure high temperatures. A still increasing amount is used as gaseous mercury in fluorescent lamps, while most of the other applications are slowly being phased out due to health and safety regulations. In some applications, mercury is replaced with less toxic but considerably more expensive Galinstan alloy. [59]

Medicine

Amalgam filling Amalgam.jpg
Amalgam filling

Historical and folk

Mercury and its compounds have been used in medicine, although they are much less common today than they once were, now that the toxic effects of mercury and its compounds are more widely understood. An example of the early therapeutic application of mercury of was published in 1787 by James Lind. [60]

The first edition of the Merck's Manual (1899) featured many then-medically relevant mercuric compounds, such as mercury-ammonium chloride, yellow mercury proto-iodide, calomel, and mercuric chloride, among others. [61]

Mercury in the form of one of its common ores, cinnabar, is used in various traditional medicines, especially in traditional Chinese medicine. Review of its safety has found that cinnabar can lead to significant mercury intoxication when heated, consumed in overdose, or taken long term, and can have adverse effects at therapeutic doses, though effects from therapeutic doses are typically reversible. Although this form of mercury appears to be less toxic than other forms, its use in traditional Chinese medicine has not yet been justified, as the therapeutic basis for the use of cinnabar is not clear. [62]

Mercury(I) chloride (also known as calomel or mercurous chloride) has been used in traditional medicine as a diuretic, topical disinfectant, and laxative. Mercury(II) chloride (also known as mercuric chloride or corrosive sublimate) was once used to treat syphilis (along with other mercury compounds), although it is so toxic that sometimes the symptoms of its toxicity were confused with those of the syphilis it was believed to treat. [63] It is also used as a disinfectant. Blue mass, a pill or syrup in which mercury is the main ingredient, was prescribed throughout the 19th century for numerous conditions including constipation, depression, child-bearing and toothaches. [64] In the early 20th century, mercury was administered to children yearly as a laxative and dewormer, and it was used in teething powders for infants. The mercury-containing organohalide merbromin (sometimes sold as Mercurochrome) is still widely used but has been banned in some countries, such as the U.S. [65]

Contemporary

Mercury is an ingredient in dental amalgams. [66]

Thiomersal (called Thimerosal in the United States) is an organic compound used as a preservative in vaccines, although this use is in decline. [67] Although it was widely speculated that this mercury-based preservative could cause or trigger autism in children, no evidence supports any such link. [68] Nevertheless, thiomersal has been removed from, or reduced to trace amounts in all U.S. vaccines recommended for children 6 years of age and under, with the exception of the inactivated influenza vaccine. [67] Merbromin (Mercurochrome), another mercury compound, is a topical antiseptic used for minor cuts and scrapes in some countries. Today, the use of mercury in medicine has greatly declined in all respects, especially in developed countries. [69]

Mercury is still used in some diuretics, although substitutes such as thiazides now exist for most therapeutic uses. [70] In 2003, mercury compounds were found in some over-the-counter drugs, including topical antiseptics, stimulant laxatives, diaper-rash ointment, eye drops, and nasal sprays. The FDA has "inadequate data to establish general recognition of the safety and effectiveness" of the mercury ingredients in these products. [71]

Production of chlorine and caustic soda

Chlorine is produced from sodium chloride (common salt, NaCl) using electrolysis to separate the metallic sodium from the chlorine gas. Usually the salt is dissolved in water to produce a brine. By-products of any such chloralkali process are hydrogen (H2) and sodium hydroxide (NaOH), which is commonly called caustic soda or lye. By far the largest use of mercury [72] [73] in the late 20th century was in the mercury cell process (also called the Castner-Kellner process) where metallic sodium is formed as an amalgam at a cathode made from mercury; this sodium is then reacted with water to produce sodium hydroxide. [74] Many of the industrial mercury releases of the 20th century came from this process, although modern plants claim to be safe in this regard. [73] From the 1960s onward, the majority of industrial plants moved away from mercury cell processes towards diaphragm cell technologies to produce chlorine, though 11% of the chlorine made in the United States was still produced with the mercury cell method as of 2005. [75]

Laboratory uses

Thermometers

Thermometers containing mercury were invented in the early 18th century by Daniel Gabriel Fahrenheit, though earlier attempts at making temperature-measuring instruments filled with quicksilver had been described in the 1650s. [76] :23 Fahrenheit's mercury thermometer was based off an earlier design that used alcohol rather than mercury; the mercury thermometer was significantly more accurate than those using alcohol. [77] From the early 21st century onwards, the use of mercury thermometers has been declining, and mercury-containing instruments have been banned in many jurisdictions following the 1998 Protocol on Heavy Metals. [78] [79] Modern alternatives to mercury thermometers include resistance thermometers, thermocouples, and thermistor sensors that output to a digital display. [80]

Mirrors

Some transit telescopes use a basin of mercury to form a flat and absolutely horizontal mirror, useful in determining an absolute vertical or perpendicular reference. Concave horizontal parabolic mirrors may be formed by rotating liquid mercury on a disk, the parabolic form of the liquid thus formed reflecting and focusing incident light. Such liquid-mirror telescopes are cheaper than conventional large mirror telescopes by up to a factor of 100, but the mirror cannot be tilted and always points straight up. [81] [82] [83]

Electrochemistry

Liquid mercury is part of a popular secondary reference electrode (called the calomel electrode) in electrochemistry as an alternative to the standard hydrogen electrode. The calomel electrode is used to work out the electrode potential of half cells. [84] The triple point of mercury, −38.8344 °C, is a fixed point used as a temperature standard for the International Temperature Scale (ITS-90). [10]

Polarography and crystallography

In polarography, both the dropping mercury electrode [85] and the hanging mercury drop electrode [86] use elemental mercury. This use allows a new uncontaminated electrode to be available for each measurement or each new experiment.

Mercury-containing compounds are also of use in the field of structural biology. Mercuric compounds such as mercury(II) chloride or potassium tetraiodomercurate(II) can be added to protein crystals in an effort to create heavy atom derivatives that can be used to solve the phase problem in X-ray crystallography via isomorphous replacement or anomalous scattering methods. [87]

Niche uses

Gaseous mercury is used in mercury-vapor lamps and some "neon sign" type advertising signs and fluorescent lamps. Those low-pressure lamps emit very spectrally narrow lines, which are traditionally used in optical spectroscopy for calibration of spectral position. Commercial calibration lamps are sold for this purpose; reflecting a fluorescent ceiling light into a spectrometer is a common calibration practice. [88] Gaseous mercury is also found in some electron tubes, including ignitrons, thyratrons, and mercury arc rectifiers. [89] It is also used in specialist medical care lamps for skin tanning and disinfection. [90] Gaseous mercury is added to cold cathode argon-filled lamps to increase the ionization and electrical conductivity. An argon-filled lamp without mercury will have dull spots and will fail to light correctly. Lighting containing mercury can be bombarded/oven pumped only once. When added to neon filled tubes, inconsistent red and blue spots are produced in the light emissions until the initial burning-in process is completed; eventually it will light a consistent dull off-blue color. [91]

The Deep Space Atomic Clock (DSAC) under development by the Jet Propulsion Laboratory utilises mercury in a linear ion-trap-based clock. The novel use of mercury permits the creation of compact atomic clocks with low energy requirements ideal for space probes and Mars missions. [92]

Skin whitening

Mercury is effective as an active ingredient in skin whitening compounds used to depigment skin. [93] The Minamata Convention on Mercury limits the concentration of mercury in such whiteners to 1 part per million. However, as of 2022, many commercially sold whitener products continue to exceed that limit, and are considered toxic. [94]

Firearms

Mercury(II) fulminate is a primary explosive, which has mainly been used as a primer of a cartridge in firearms throughout the 19th and 20th centuries. [95]

Historic uses

A single-pole, single-throw (SPST) mercury switch Mercury Switch without housing.jpg
A single-pole, single-throw (SPST) mercury switch
Mercury manometer to measure pressure Barometer mercury column hg.jpg
Mercury manometer to measure pressure

Many historic applications made use of the peculiar physical properties of mercury, especially as a dense liquid and a liquid metal:

Other applications made use of the chemical properties of mercury:

Toxicity and safety

Mercury
Hazards
GHS labelling:
GHS-pictogram-skull.svg GHS-pictogram-silhouette.svg GHS-pictogram-pollu.svg
Danger
H330, H360D, H372, H410
P201, P233, P260, P273, P280, P304, P308, P310, P313, P340, P391, P403 [122]
NFPA 704 (fire diamond)
NFPA 704.svgHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
0
0

Mercury can be absorbed through the skin and mucous membranes and mercury vapors can be inhaled, so containers of mercury are securely sealed to avoid spills and evaporation. Heating of mercury, or of compounds of mercury that may decompose when heated, should be carried out with adequate ventilation in order to minimize exposure to mercury vapor. The most toxic forms of mercury are its organic compounds, such as dimethylmercury and methylmercury. Mercury can cause both chronic and acute poisoning. [123] [124]

Releases in the environment

Amount of atmospheric mercury deposited at Wyoming's Upper Fremont Glacier over the last 270 years Mercury in Ice Core Upper Fremont Glacier.svg
Amount of atmospheric mercury deposited at Wyoming's Upper Fremont Glacier over the last 270 years

Preindustrial deposition rates of mercury from the atmosphere may be about 4 ng per 1 L of ice deposited. Volcanic eruptions and related natural sources are responsible for approximately half of atmospheric mercury emissions. [125]

Atmospheric mercury contamination in outdoor urban air at the start of the 21st century was measured at 0.01–0.02 μg/m3. A 2001 study measured mercury levels in 12 indoor sites chosen to represent a cross-section of building types, locations and ages in the New York area. This study found mercury concentrations significantly elevated over outdoor concentrations, at a range of 0.0065 – 0.523 μg/m3. The average was 0.069 μg/m3. [126]

Half of mercury emissions are attributed to mankind. The sources can be divided into the following estimated percentages: [127]

The above percentages are estimates of the global human-caused mercury emissions in 2000, excluding biomass burning, an important source in some regions. [127]

A serious industrial disaster was the dumping of waste mercury compounds into Minamata Bay, Japan, between 1932 and 1968. It is estimated that over 3,000 people suffered various deformities, severe mercury poisoning symptoms or death from what became known as Minamata disease. [129] [130]

China is estimated to produce 50% of the mercury emissions, most of which result from the production of vinyl chloride. [131]

Joss paper burning on the street, a common tradition practiced in Asia, Hong Kong, 2023

Mercury also enters into the environment through the improper disposal of mercury-containing products. [132] Due to health concerns (see below), toxics use reduction efforts are cutting back or eliminating mercury in such products. For example, the amount of mercury sold in thermostats in the United States decreased from 14.5 tons in 2004 to 3.9 tons in 2007. [133]

The tobacco plant readily absorbs and accumulates heavy metals such as mercury from the surrounding soil into its leaves. These are subsequently inhaled during tobacco smoking. [134] While mercury is a constituent of tobacco smoke, [135] studies have largely failed to discover a significant correlation between smoking and Hg uptake by humans compared to sources such as occupational exposure, fish consumption, and amalgam tooth fillings. [136]

A less well-known source of mercury is the burning of joss paper, [137] which is a common tradition practiced in Asia, including China, [138] Vietnam, Hong Kong, Thailand, Taiwan and Malaysia. [139]

Spill cleanup

Mercury spills pose an immediate threat to people handling the material, in addition to being an environmental hazard if the material is not contained properly. This is of particular concern for visible mercury, or mercury in liquid state, as its unusual appearance and behavior for a metal makes it an attractive nuisance to the uninformed. [140] Procedures have been developed to contain mercury spills, as well as recommendations on appropriate responses based on the conditions of a spill. [141] [142] Tracking liquid mercury away from the site of a spill is a major concern in liquid mercury spills; regulations emphasize containment of the visible mercury as the first course of action, followed by monitoring of mercury vapors and vapor cleanup. Several products are sold as mercury spill adsorbents, ranging from metal salts to polymers and zeolites. [143]

Sediment contamination

Sediments within large urban-industrial estuaries act as an important sink for point source and diffuse mercury pollution within catchments. [144] A 2015 study of foreshore sediments from the Thames estuary measured total mercury at 0.01 to 12.07 mg/kg with mean of 2.10 mg/kg and median of 0.85 mg/kg (n=351). [144] The highest mercury concentrations were shown to occur in and around the city of London in association with fine grain muds and high total organic carbon content. [144] The strong affinity of mercury for carbon rich sediments has also been observed in salt marsh sediments of the River Mersey, with a mean concentration of 2 mg/kg, up to 5 mg/kg. [145] These concentrations are far higher than those in the salt marsh river creek sediments of New Jersey and mangroves of Southern China, which exhibit low mercury concentrations of about 0.2 mg/kg. [146] [147]

Occupational exposure

EPA workers clean up residential mercury spill in 2004 EPA workers clean up residential mercury spill (3986684199).jpg
EPA workers clean up residential mercury spill in 2004

Due to the health effects of mercury exposure, industrial and commercial uses are regulated in many countries. The World Health Organization, [148] OSHA, and NIOSH all treat mercury as an occupational hazard; both OSHA and NIOSH, among other regulatory agencies, have established specific occupational exposure limits on the element and its derivative compounds in liquid and vapor form. [149] [150] Environmental releases and disposal of mercury are regulated in the U.S. primarily by the United States Environmental Protection Agency.

Fish

Fish and shellfish have a natural tendency to concentrate mercury in their bodies, often in the form of methylmercury, a highly toxic organic compound of mercury. Species of fish that are high on the food chain, such as shark, swordfish, king mackerel, bluefin tuna, albacore tuna, and tilefish contain higher concentrations of mercury than others. Because mercury and methylmercury are fat soluble, they primarily accumulate in the viscera, although they are also found throughout the muscle tissue. [151] Mercury presence in fish muscles can be studied using non-lethal muscle biopsies. [152] Mercury present in prey fish accumulates in the predator that consumes them. Since fish are less efficient at depurating than accumulating methylmercury, methylmercury concentrations in the fish tissue increase over time. Thus species that are high on the food chain amass body burdens of mercury that can be ten times higher than the species they consume. This process is called biomagnification. Mercury poisoning happened this way in Minamata, Japan, now called Minamata disease. [129] [130]

Cosmetics

Some facial creams contain dangerous levels of mercury. Most contain comparatively non-toxic inorganic mercury, but products containing highly toxic organic mercury have been encountered. [153] [154] New York City residents have been found to be exposed to significant levels of inorganic mercury compounds through the use of skin care products. [155]

Effects and symptoms of mercury poisoning

Toxic effects include damage to the brain, kidneys and lungs. Mercury poisoning can result in several diseases, including acrodynia (pink disease), Hunter-Russell syndrome, and Minamata disease. Symptoms typically include sensory impairment (vision, hearing, speech), disturbed sensation and a lack of coordination. The type and degree of symptoms exhibited depend upon the individual toxin, the dose, and the method and duration of exposure. Case–control studies have shown effects such as tremors, impaired cognitive skills, and sleep disturbance in workers with chronic exposure to mercury vapor even at low concentrations in the range 0.7–42 μg/m3. [156] [157]

A study has shown that acute exposure (4–8 hours) to calculated elemental mercury levels of 1.1 to 44 mg/m3 resulted in chest pain, dyspnea, cough, hemoptysis, impairment of pulmonary function, and evidence of interstitial pneumonitis. [123] Acute exposure to mercury vapor has been shown to result in profound central nervous system effects, including psychotic reactions characterized by delirium, hallucinations, and suicidal tendency. Occupational exposure has resulted in broad-ranging functional disturbance, including erethism, irritability, excitability, excessive shyness, and insomnia. With continuing exposure, a fine tremor develops and may escalate to violent muscular spasms. Tremor initially involves the hands and later spreads to the eyelids, lips, and tongue. Long-term, low-level exposure has been associated with more subtle symptoms of erethism, including fatigue, irritability, loss of memory, vivid dreams and depression. [124] [158]

Treatment

Research on the treatment of mercury poisoning is limited. Currently available drugs for acute mercurial poisoning include chelators N-acetyl-D, L-penicillamine (NAP), British Anti-Lewisite (BAL), 2,3-dimercapto-1-propanesulfonic acid (DMPS), and dimercaptosuccinic acid (DMSA). In one small study including 11 construction workers exposed to elemental mercury, patients were treated with DMSA and NAP. [159] Chelation therapy with both drugs resulted in the mobilization of a small fraction of the total estimated body mercury. DMSA was able to increase the excretion of mercury to a greater extent than NAP. [159]

Regulations

International

140 countries agreed in the Minamata Convention on Mercury by the United Nations Environment Programme (UNEP) to prevent mercury vapor emissions. [160] The convention was signed on 10 October 2013. [161]

United States

In the United States, the Environmental Protection Agency is charged with regulating and managing mercury contamination. Several laws give the EPA this authority, including the Clean Air Act, the Clean Water Act, the Resource Conservation and Recovery Act, and the Safe Drinking Water Act. Additionally, the Mercury-Containing and Rechargeable Battery Management Act, passed in 1996, phases out the use of mercury in batteries, and provides for the efficient and cost-effective disposal of many types of used batteries. [162] North America contributed approximately 11% of the total global anthropogenic mercury emissions in 1995. [163]

The United States Clean Air Act, passed in 1990, put mercury on a list of toxic pollutants that need to be controlled to the greatest possible extent. Thus, industries that release high concentrations of mercury into the environment agreed to install maximum achievable control technologies (MACT). In March 2005, the EPA promulgated a regulation [164] that added power plants to the list of sources that should be controlled and instituted a national cap and trade system. States were given until November 2006 to impose stricter controls, but after a legal challenge from several states, the regulations were struck down by a federal appeals court on 8 February 2008. The rule was deemed not sufficient to protect the health of persons living near coal-fired power plants, given the negative effects documented in the EPA Study Report to Congress of 1998. [165] However newer data published in 2015 showed that after introduction of the stricter controls mercury declined sharply, indicating that the Clean Air Act had its intended impact. [166]

The EPA announced new rules for coal-fired power plants on 22 December 2011. [167] Cement kilns that burn hazardous waste are held to a looser standard than are standard hazardous waste incinerators in the United States, and as a result are a disproportionate source of mercury pollution. [168]

European Union

In the European Union, the directive on the Restriction of the Use of Certain Hazardous Substances in Electrical and Electronic Equipment (see RoHS) bans mercury from certain electrical and electronic products, and limits the amount of mercury in other products to less than 1000 ppm. [169] There are restrictions for mercury concentration in packaging (the limit is 100 ppm for sum of mercury, lead, hexavalent chromium and cadmium) and batteries (the limit is 5 ppm). [170] In July 2007, the European Union also banned mercury in non-electrical measuring devices, such as thermometers and barometers. The ban applies to new devices only, and contains exemptions for the health care sector and a two-year grace period for manufacturers of barometers. [171]

Scandinavia

Norway enacted a total ban on the use of mercury in the manufacturing and import/export of mercury products, effective 1 January 2008. [172] In 2002, several lakes in Norway were found to have a poor state of mercury pollution, with an excess of 1 μg/g of mercury in their sediment. [173] In 2008, Norway's Minister of Environment Development Erik Solheim said: "Mercury is among the most dangerous environmental toxins. Satisfactory alternatives to Hg in products are available, and it is therefore fitting to induce a ban." [174] Products containing mercury were banned in Sweden in 2009, [175] [176] while elemental mercury has been banned from manufacture and use in all but a few applications (such as certain energy-saving light sources and amalgam dental fillings) in Denmark since 2008. [177]

See also

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<span class="mw-page-title-main">Mercury poisoning</span> Poisoning caused by mercury chemicals

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<span class="mw-page-title-main">Mercury(II) chloride</span> Chemical compound known as corrosive sublimate

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<span class="mw-page-title-main">Methylmercury</span> Toxic chemical compound

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<span class="mw-page-title-main">Amalgam (chemistry)</span> Alloy of mercury with another metal

An amalgam is an alloy of mercury with another metal. It may be a liquid, a soft paste or a solid, depending upon the proportion of mercury. These alloys are formed through metallic bonding, with the electrostatic attractive force of the conduction electrons working to bind all the positively charged metal ions together into a crystal lattice structure. Almost all metals can form amalgams with mercury, the notable exceptions being iron, platinum, tungsten, and tantalum. Silver-mercury amalgams are important in dentistry, and gold-mercury amalgam is used in the extraction of gold from ore. Dentistry has used alloys of mercury with metals such as silver, copper, indium, tin and zinc.

<span class="mw-page-title-main">Mercury in fish</span>

The presence of mercury in fish is a health concern for people who eat them, especially for women who are or may become pregnant, nursing mothers, and young children. Fish and shellfish concentrate mercury in their bodies, often in the form of methylmercury, a highly toxic organomercury compound. This element is known to bioaccumulate in humans, so bioaccumulation in seafood carries over into human populations, where it can result in mercury poisoning. Mercury is dangerous to both natural ecosystems and humans because it is a metal known to be highly toxic, especially due to its neurotoxic ability to damage the central nervous system.

<span class="mw-page-title-main">Mercury cycle</span>

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<span class="mw-page-title-main">Mercury regulation in the United States</span>

Mercury regulation in the United States limit the maximum concentrations of mercury (Hg) that is permitted in air, water, soil, food and drugs. The regulations are promulgated by agencies such as the Environmental Protection Agency (EPA) and Food and Drug Administration (FDA), as well as a variety of state and local authorities. EPA published the Mercury and Air Toxics Standards (MATS) regulation in 2012; the first federal standards requiring power plants to limit emissions of mercury and other toxic gases.

Hurair Vasken Aposhian was a Ph.D. toxicologist and an emeritus professor of molecular and cell biology at the University of Arizona, a post he held beginning in 1975. He is also a former professor of pharmacology at the medical school at said university. He received his bachelor's degree in chemistry, at Brown University, 1948. He received a master's degree and a PhD in physiological chemistry at the University of Rochester, where he published some scientific studies about the synthesis of isoalloxazine ring-containing compounds. He did a postdoctoral with Nobel Laureate Arthur Kornberg in the department of biochemistry at Stanford University School of Medicine. He has done sabbatical scholar-in-residence at MIT and at the University of California at San Diego. He is best known for his pioneering work on Succimer and Unithiol in the treatment of arsenic, mercury, lead and other heavy metals leading to FDA approval of succimer in childhood lead poisoning at levels over 40 ug/dl. Previous posts he had held include at Vanderbilt, Tufts University, and the University of Maryland. His views about mercury in vaccines and in dental amalgams go against the consensus of the medical community and are controversial.

<span class="mw-page-title-main">Mercury pollution in the ocean</span> Mercury contamination in sea and sediments

Mercury is a heavy metal that cycles through the atmosphere, water, and soil in various forms to different parts of the world. Due to this natural mercury cycle, irrespective of which part of the world releases mercury it could affect an entirely different part of the world making mercury pollution a global concern. Mercury pollution is now identified as a global problem and awareness has been raised on an international action plan to minimize anthropogenic mercury emissions and clean up mercury pollution. The 2002 Global Mercury Assessment concluded that "International actions to address the global mercury problem should not be delayed". Among many environments that are under the impact of mercury pollution, the ocean is one which cannot be neglected as it has the ability to act as a "storage closet" for mercury. According to a recent model study the total anthropogenic mercury released into the ocean is estimated to be around 80,000 to 45,000 metric tons and two-thirds of this amount is estimated to be found in waters shallower than 1000m level where much consumable fish live. Mercury can bioaccumulate in marine food chains in the form of highly toxic methylmercury which can cause health risks to human seafood consumers. According to statistics, about 66% of global fish consumption comes from the ocean. Therefore, it is important to monitor and regulate oceanic mercury levels to prevent more and more mercury from reaching the human population through seafood consumption.

References

  1. "Standard Atomic Weights: Mercury". CIAAW. 2011.
  2. Prohaska, Thomas; Irrgeher, Johanna; Benefield, Jacqueline; Böhlke, John K.; Chesson, Lesley A.; Coplen, Tyler B.; Ding, Tiping; Dunn, Philip J. H.; Gröning, Manfred; Holden, Norman E.; Meijer, Harro A. J. (4 May 2022). "Standard atomic weights of the elements 2021 (IUPAC Technical Report)". Pure and Applied Chemistry. doi:10.1515/pac-2019-0603. ISSN   1365-3075.
  3. Fehlauer, H.; Bettin, H. (2004). "Density of mercury—measurements and reference values". Metrologia. 41 (2): S16–S22. doi:10.1088/0026-1394/41/2/S02 . Retrieved 8 July 2023.
  4. "Magnetic Susceptibility of the Elements And Inorganic Compounds" (PDF). www-d0.fnal.gov. Fermi National Accelerator Laboratory: DØ Experiment (lagacy document). Archived from the original (PDF) on 24 March 2004. Retrieved 18 February 2015.
  5. Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN   0-8493-0464-4.
  6. Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi:10.1088/1674-1137/abddae.
  7. 1 2 "Definition of hydrargyrum | Dictionary.com". Archived from the original on 12 August 2014. Retrieved 22 December 2022. Random House Webster's Unabridged Dictionary .
  8. "What is EPA doing about mercury air emissions?". United States Environmental Protection Agency (EPA). Archived from the original on 8 February 2007. Retrieved 1 May 2007.
  9. "New 12-sided pound coin to enter circulation in March". BBC News. 1 January 2017. Retrieved 2 January 2017.
  10. 1 2 3 4 5 6 Hammond, C. R. "The Elements" (PDF). Archived from the original (PDF) on 26 June 2008. in Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN   0-8493-0486-5.
  11. 1 2 Norrby, L.J. (1991). "Why is mercury liquid? Or, why do relativistic effects not get into chemistry textbooks?". Journal of Chemical Education. 68 (2): 110. Bibcode:1991JChEd..68..110N. doi:10.1021/ed068p110. S2CID   96003717.
  12. Senese, F. "Why is mercury a liquid at STP?". General Chemistry Online at Frostburg State University. Archived from the original on 4 April 2007. Retrieved 1 May 2007.
  13. Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. pp. 4.125–4.126. ISBN   0-8493-0486-5.
  14. "Dynamic Periodic Table". www.ptable.com. Archived from the original on 20 November 2016. Retrieved 22 November 2016.
  15. Simons, E. N. (1968). Guide to Uncommon Metals. Frederick Muller. p. 111.
  16. Holman, Jack P. (2002). Heat Transfer (9th ed.). New York, NY: cGraw-Hill Companies, Inc. pp. 600–606. ISBN   978-0-07-240655-9.
  17. Incropera, Frank P. (2007). Fundamentals of Heat and Mass Transfer (6th ed.). Hoboken, NJ: John Wiley and Sons, Inc. pp. 941–950. ISBN   978-0-471-45728-2.
  18. 1 2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN   978-0-08-037941-8.
  19. Swackhamer, Barry (26 November 2011). "Mercury Storage Vault". The Historic Marker Database. Retrieved 11 December 2023.
  20. Gmelin, Leopold (1852). Hand book of chemistry. Cavendish Society. pp. 103 (Na), 110 (W), 122 (Zn), 128 (Fe), 247 (Au), 338 (Pt). Archived from the original on 9 May 2013. Retrieved 30 December 2012.
  21. Soratur, S. H. (2002). Essentials of Dental Materials. Jaypee Brothers Publishers. p. 14. ISBN   978-81-7179-989-3.
  22. Vargel, C.; Jacques, M.; Schmidt, M. P. (2004). Corrosion of Aluminium. Elsevier. p. 158. ISBN   978-0-08-044495-6.
  23. Case, Raymundo; McIntyre, Dale R. (14 March 2010). Mercury Liquid Metal Embrittlement Of Alloys For Oil And Gas Production And Processing.
  24. Webster's Revised Unabridged Dictionary. Springfield, Mass.: G. & C. Merriam. 1913. OCLC   800618302 . Retrieved 27 December 2023.
  25. 1 2 Stillman, J. M. (2003). Story of Alchemy and Early Chemistry. Kessinger Publishing. pp. 7–9. ISBN   978-0-7661-3230-6. OCLC   233637688.
  26. Maurice Crosland (2004) Historical Studies in the Language of Chemistry
  27. "Mercury and the environment — Basic facts". Environment Canada, Federal Government of Canada. 2004. Archived from the original on 16 September 2011. Retrieved 27 March 2008.
  28. Martín Gil, J.; Martín Gil, F. J.; Delibes de Castro, G.; Zapatero Magdaleno, P.; Sarabia Herrero, F. J. (1995). "The first known use of vermillion". Experientia. 51 (8): 759–761. doi:10.1007/BF01922425. ISSN   0014-4754. PMID   7649232. S2CID   21900879.
  29. "Mercury — Element of the ancients". Center for Environmental Health Sciences, Dartmouth College. Archived from the original on 2 December 2012. Retrieved 9 April 2012.
  30. "Qin Shihuang". Ministry of Culture, People's Republic of China. 2003. Archived from the original on 4 July 2008. Retrieved 27 March 2008.
  31. Wright, David Curtis (2001). The History of China . Greenwood Publishing Group. p. 49. ISBN   978-0-313-30940-3.
  32. Sobernheim, Moritz (1987). "Khumārawaih". In Houtsma, Martijn Theodoor (ed.). E.J. Brill's first encyclopaedia of Islam, 1913–1936, Volume IV: 'Itk–Kwaṭṭa. Leiden: BRILL. p. 973. ISBN   978-90-04-08265-6. Archived from the original on 3 June 2016.
  33. 1 2 Yuhas, Alan (24 April 2015). "Liquid mercury found under Mexican pyramid could lead to king's tomb". The Guardian. ISSN   0261-3077. Archived from the original on 1 December 2016. Retrieved 22 November 2016.
  34. Hicks, R. D. (1907). "Chapter 3". Aristotle De Anima. Cambridge: Cambridge University Press. Text
  35. Pendergast, David M. (6 August 1982). "Ancient maya mercury". Science. 217 (4559): 533–535. Bibcode:1982Sci...217..533P. doi:10.1126/science.217.4559.533. PMID   17820542. S2CID   39473822.
  36. "Lamanai". Archived from the original on 11 June 2011. Retrieved 17 June 2011.
  37. Hesse, R W (2007). Jewelrymaking through history. Greenwood Publishing Group. p. 120. ISBN   978-0-313-33507-5.
  38. Eisler, R. (2006). Mercury hazards to living organisms. CRC Press. ISBN   978-0-8493-9212-2.
  39. Ehrlich, H. L.; Newman, D. K. (2008). Geomicrobiology. CRC Press. p. 265. ISBN   978-0-8493-7906-2.
  40. Rytuba, James J (2003). "Mercury from mineral deposits and potential environmental impact". Environmental Geology. 43 (3): 326–338. doi:10.1007/s00254-002-0629-5. S2CID   127179672.
  41. 1 2 "Metacinnabar". Mindat.org. Retrieved 16 November 2023.
  42. "Mercury Recycling in the United States in 2000" (PDF). USGS. Archived (PDF) from the original on 26 March 2009. Retrieved 7 July 2009.
  43. Burkholder, M. & Johnson, L. (2008). Colonial Latin America. Oxford University Press. pp. 157–159. ISBN   978-0-19-504542-0.
  44. Jamieson, R W (2000). Domestic Architecture and Power. Springer. p. 33. ISBN   978-0-306-46176-7.
  45. Brooks, W. E. (2007). "Mercury" (PDF). U.S. Geological Survey. Archived (PDF) from the original on 27 May 2008. Retrieved 30 May 2008.
  46. "World Mineral Production" (PDF). p. 48. Retrieved 22 November 2023.
  47. "Thank President Obama and Administrator Jackson for protecting us from toxic mercury". Act.credoaction.com. 21 December 2011. Archived from the original on 1 May 2012. Retrieved 30 December 2012.
  48. 1 2 Sheridan, M. (3 May 2009). "'Green' Lightbulbs Poison Workers: hundreds of factory staff are being made ill by mercury used in bulbs destined for the West". The Sunday Times (of London, UK). Archived from the original on 17 May 2009.
  49. Boulland M (2006). New Almaden. Arcadia Publishing. p. 8. ISBN   978-0-7385-3131-1.
  50. For a general overview, see Riedel, S.; Kaupp, M. (2009). "The Highest Oxidation States of the Transition Metal Elements". Coordination Chemistry Reviews. 253 (5–6): 606–624. doi:10.1016/j.ccr.2008.07.014.

    The claimed 1976 synthesis is Deming, Richard L.; Allred, A. L.; Dahl, Alan R.; Herlinger, Albert W.; Kestner, Mark O. (July 1976). "Tripositive mercury. Low temperature electrochemical oxidation of 1,4,8,11-tetraazacyclotetradecanemercury(II) tetrafluoroborate". Journal of the American Chemical Society. 98 (14): 4132–4137. doi:10.1021/ja00430a020; but note that Reidel & Kaupp cite more recent work arguing that the cyclam ligand is instead oxidized.

    The claimed 2007 isolation is Xuefang Wang; Andrews, Lester; Riedel, Sebastian; Kaupp, Martin (2007). "Mercury Is a Transition Metal: The First Experimental Evidence for HgF4". Angew. Chem. Int. Ed. 46 (44): 8371–8375. doi:10.1002/anie.200703710. PMID   17899620, but the spectral identifications are disputed in Rooms, J. F.; Wilson, A. V.; Harvey, I.; Bridgeman, A. J.; Young, N. A. (2008). "Mercury-fluorine interactions: a matrix isolation investigation of Hg⋯F2, HgF2 and HgF4 in argon matrices". Phys Chem Chem Phys. 10 (31): 4594–605. Bibcode:2008PCCP...10.4594R. doi:10.1039/b805608k. PMID   18665309.

  51. Henderson, W. (2000). Main group chemistry. Great Britain: Royal Society of Chemistry. p. 162. ISBN   978-0-85404-617-1. Archived from the original on 13 May 2016.
  52. Knight, Lon B. (1971). "Hyperfine Interaction, Chemical Bonding, and Isotope Effect in ZnH, CdH, and HgH Molecules". The Journal of Chemical Physics. 55 (5): 2061–2070. Bibcode:1971JChPh..55.2061K. doi:10.1063/1.1676373.
  53. Brown, I. D.; Gillespie, R. J.; Morgan, K. R.; Tun, Z.; Ummat, P. K. (1984). "Preparation and crystal structure of mercury hexafluoroniobate (Hg
    3
    NbF
    6
    ) and mercury hexafluorotantalate (Hg
    3
    TaF
    6
    ): mercury layer compounds". Inorganic Chemistry. 23 (26): 4506–4508. doi:10.1021/ic00194a020.
  54. Chisholm, Hugh, ed. (1911). "Corrosive Sublimate"  . Encyclopædia Britannica . Vol. 7 (11th ed.). Cambridge University Press. p. 197.
  55. Anderegg, G.; Schwarzenbach, G.; Padmoyo, M.; Borg, Ö. F. (1958). "Monomolekular gelöstes Quecksilberhydroxyd und seine Basizität". Helvetica Chimica Acta. 41 (4): 988–996. doi:10.1002/hlca.19580410411.
  56. Rogalski, A (2000). Infrared detectors. CRC Press. p. 507. ISBN   978-90-5699-203-3.
  57. Vogel, Arthur I.; Svehla, G. (1979), Vogel's Textbook of Macro and Semimicro Qualitative Inorganic Analysis (5th ed.), London: Longman, p. 319, ISBN   0-582-44367-9 via the Internet Archive
  58. Committee on the Toxicological Effects of Methylmercury; Board on Environmental Studies and Toxicology; Commission on Life Sciences; National Research Council (2000). Toxicological effects of methylmercury. National Academies Press. ISBN   978-0-309-07140-6.
  59. Surmann, P; Zeyat, H (November 2005). "Voltammetric analysis using a self-renewable non-mercury electrode". Analytical and Bioanalytical Chemistry. 383 (6): 1009–13. doi:10.1007/s00216-005-0069-7. PMID   16228199. S2CID   22732411.
  60. Lind, J (1787). "An Account of the Efficacy of Mercury in the Cure of Inflammatory Diseases, and the Dysentery". The London Medical Journal. 8 (Pt 1): 43–56. ISSN   0952-4177. PMC   5545546 . PMID   29139904.
  61. Merck's Manual 1899 (1st ed.). Archived from the original on 24 August 2013. Retrieved 16 June 2013.
  62. Liu J; Shi JZ; Yu LM; Goyer RA; Waalkes MP (2008). "Mercury in traditional medicines: is cinnabar toxicologically similar to common mercurials?". Exp. Biol. Med. (Maywood). 233 (7): 810–7. doi:10.3181/0712-MR-336. PMC   2755212 . PMID   18445765.
  63. Pimple KD, Pedroni JA, Berdon V (9 July 2002). "Syphilis in history". Poynter Center for the Study of Ethics and American Institutions at Indiana University-Bloomington. Archived from the original on 16 February 2005. Retrieved 17 April 2005.
  64. 1 2 Mayell, H. (17 July 2007). "Did Mercury in "Little Blue Pills" Make Abraham Lincoln Erratic?". National Geographic News . Archived from the original on 22 May 2008. Retrieved 15 June 2008.
  65. "What happened to Mercurochrome?". 23 July 2004. Archived from the original on 11 April 2009. Retrieved 7 July 2009.
  66. "Dental Amalgam Fillings". Silver Spring, MD: U.S. Food and Drug Administration (FDA). 29 September 2020.
  67. 1 2 "Thimerosal in Vaccines". Food and Drug Administration / Center for Biologics Evaluation and Research. 6 September 2007. Archived from the original on 29 September 2007. Retrieved 1 October 2007.
  68. Parker SK, Schwartz B, Todd J, Pickering LK (2004). "Thimerosal-containing vaccines and autistic spectrum disorder: a critical review of published original data". Pediatrics. 114 (3): 793–804. CiteSeerX   10.1.1.327.363 . doi:10.1542/peds.2004-0434. PMID   15342856. S2CID   1752023.
    Erratum: Parker SK, Todd J, Schwartz B, Pickering LK (January 2005). "Thimerosal-containing vaccines and autistic spectrum disorder: a critical review of published original data". Pediatrics. 115 (1): 200. doi:10.1542/peds.2004-2402. PMID   15630018. S2CID   26700143.
  69. "Quantitative and Qualitative Analysis of Mercury Compounds in the List". Federal Food, Drug, and Cosmetic Act (FD&C Act). U.S. Food and Drug Administration. 30 April 2009.
  70. Beyer KH (September 1993). "Chlorothiazide. How the thiazides evolved as antihypertensive therapy". Hypertension. 22 (3): 388–91. doi: 10.1161/01.hyp.22.3.388 . PMID   8349332.
  71. "Title 21—Food and Drugs Chapter I—Food and Drug Administration Department of Health and Human Services Subchapter D—Drugs for Human Use Code of federal regulations". United States Food and Drug Administration. Archived from the original on 13 March 2007. Retrieved 1 May 2007.
  72. "The CRB Commodity Yearbook (annual)". The CRB Commodity Yearbook: 173. 2000. ISSN   1076-2906.
  73. 1 2 Leopold, B. R. (2002). "Chapter 3: Manufacturing Processes Involving Mercury. Use and Release of Mercury in the United States" (PDF). National Risk Management Research Laboratory, Office of Research and Development, U.S. Environmental Protection Agency, Cincinnati, Ohio. Archived from the original (PDF) on 21 June 2007. Retrieved 1 May 2007.
  74. "Chlorine Online Diagram of mercury cell process". Euro Chlor. Archived from the original on 2 September 2006. Retrieved 15 September 2006.
  75. O'Brien, Thomas F.; Bommaraju, Tilak V.; Hine, Fumio, eds. (2005). "History of the Chlor-Alkali Industry". Handbook of Chlor-Alkali Technology. Boston, MA: Springer. pp. 17–36. doi:10.1007/0-306-48624-5_2. ISBN   978-0-306-48624-1 . Retrieved 5 October 2020.
  76. Middleton, W. E. K. (1966). A history of the thermometer and its use in meteorology. Johns Hopkins Press. ISBN   9780801871535.
  77. Grigull, Ulrich (1966). Fahrenheit, a Pioneer of Exact Thermometry. (The Proceedings of the 8th International Heat Transfer Conference, San Francisco, 1966, Vol. 1, pp. 9–18.)
  78. "Protocol on Heavy Metals". UNECE. Retrieved 10 August 2014.
  79. "Mercury Reduction Act of 2003". United States. Congress. Senate. Committee on Environment and Public Works. Retrieved 6 June 2009.
  80. "Mercury Thermometer Alternatives: Hg Alternatives". nist.gov. National Institute of Standards and Technology. 29 November 2021. Retrieved 22 December 2023.
  81. "Liquid-mirror telescope set to give stargazing a new spin". Govert Schilling. 14 March 2003. Archived from the original on 18 August 2003. Retrieved 11 October 2008.
  82. Gibson, B. K. (1991). "Liquid Mirror Telescopes: History". Journal of the Royal Astronomical Society of Canada. 85: 158. Bibcode:1991JRASC..85..158G.
  83. "Laval University Liquid mirrors and adaptive optics group". Archived from the original on 18 September 2011. Retrieved 24 June 2011.
  84. Brans, Y W; Hay W W (1995). Physiological monitoring and instrument diagnosis in perinatal and neonatal medicine. CUP Archive. p. 175. ISBN   978-0-521-41951-2.
  85. Zoski, Cynthia G. (7 February 2007). Handbook of Electrochemistry. Elsevier Science. ISBN   978-0-444-51958-0.
  86. Kissinger, Peter; Heineman, William R. (23 January 1996). Laboratory Techniques in Electroanalytical Chemistry, Second Edition, Revised and Expanded (2nd ed.). CRC. ISBN   978-0-8247-9445-3.
  87. Pike, Ashley C. W.; Garman, Elspeth F.; Krojer, Tobias; von Delft, Frank; Carpenter, Elisabeth P. (1 March 2016). "An overview of heavy-atom derivatization of protein crystals". Acta Crystallographica. Section D, Structural Biology. 72 (Pt 3): 303–318. Bibcode:2016AcCrD..72..303P. doi:10.1107/S2059798316000401. ISSN   2059-7983. PMC   4784662 . PMID   26960118.
  88. Hopkinson, G. R.; Goodman, T. M.; Prince, S. R. (2004). A guide to the use and calibration of detector array equipment. SPIE Press. p. 125. Bibcode:2004gucd.book.....H. ISBN   978-0-8194-5532-1.
  89. Howatson A H (1965). "Chapter 8". An Introduction to Gas Discharges. Oxford: Pergamon Press. ISBN   978-0-08-020575-5.
  90. Milo G E; Casto B C (1990). Transformation of human diploid fibroblasts. CRC Press. p. 104. ISBN   978-0-8493-4956-0.
  91. Shionoya, S. (1999). Phosphor handbook. CRC Press. p. 363. ISBN   978-0-8493-7560-6.
  92. Robert L. Tjoelker; et al. (2016). "Mercury Ion Clock for a NASA Technology Demonstration Mission". IEEE Transactions on Ultrasonics, Ferroelectrics, and Frequency Control. 63 (7): 1034–1043. Bibcode:2016ITUFF..63.1034T. doi:10.1109/TUFFC.2016.2543738. PMID   27019481. S2CID   3245467.
  93. Mohammed, Terry; Mohammed, Elisabeth; Bascombe, Shermel (9 October 2017). "The evaluation of total mercury and arsenic in skin bleaching creams commonly used in Trinidad and Tobago and their potential risk to the people of the Caribbean". Journal of Public Health Research. 6 (3): 1097. doi:10.4081/jphr.2017.1097. PMC   5736993 . PMID   29291194.
  94. Meera Senthilingam, "Skin whitening creams containing high levels of mercury continue to be sold on the world's biggest e-commerce sites, new report finds", 9 March 2022, CNN https://www.cnn.com/2022/03/09/world/zmwg-skin-whitening-creams-mercury-ecommerce-sites-intl-cmd/index.html
  95. Wisniak, Jaime (2012). "Edward Charles Howard. Explosives, meteorites, and sugar". Educación Química. Universidad Nacional Autonoma de Mexico. 23 (2): 230–239. doi: 10.1016/s0187-893x(17)30114-3 . ISSN   0187-893X.
  96. Healy, Paul F.; Blainey, Marc G. (2011). "Ancient Maya Mosaic Mirrors: Function, Symbolism, And Meaning". Ancient Mesoamerica. 22 (2): 229–244 (241). doi:10.1017/S0956536111000241. S2CID   162282151.
  97. Lew K. (2008). Mercury. The Rosen Publishing Group. p. 10. ISBN   978-1-4042-1780-5.
  98. Pearson L. F. (2003). Lighthouses. Osprey Publishing. p. 29. ISBN   978-0-7478-0556-4.
  99. Ramanathan E. AIEEE Chemistry. Sura Books. p. 251. ISBN   978-81-7254-293-1.
  100. Shelton, C. (2004). Electrical Installations. Nelson Thornes. p. 260. ISBN   978-0-7487-7979-6.
  101. Eckert, J. P. (October 1953). "A Survey of Digital Computer Memory Systems". Proceedings of the IRE. 41 (10): 1393–1406. doi:10.1109/JRPROC.1953.274316.
  102. van Delft, Dirk; Kes, Peter (1 September 2010). "The discovery of superconductivity". Physics Today . Archived from the original on 14 November 2023. Retrieved 6 December 2023.
  103. Tresca, Cesare; Profeta, Gianni; Marini, Giovanni; Bachelet, Giovanni B.; Sanna, Antonio; Calandra, Matteo; Boeri, Lilia (3 November 2022). "Why mercury is a superconductor". Physical Review B. 106 (18). arXiv: 2111.13867 . Bibcode:2022PhRvB.106r0501T. doi:10.1103/PhysRevB.106.L180501. hdl: 11573/1659661 . ISSN   2469-9950. S2CID   244715089.
  104. Berlincourt, T. G. & Hake, R. R. (1962). "Pulsed-Magnetic-Field Studies of Superconducting Transition Metal Alloys at High and Low Current Densities". Bulletin of the American Physical Society. II-7: 408.
  105. "Popular Science". The Popular Science Monthly. Bonnier Corporation. 118 (3): 40. 1931. ISSN   0161-7370.
  106. Mueller, Grover C. (September 1929). Cheaper Power from Quicksilver. Popular Science.
  107. "Mercury as a Working Fluid". Museum of Retro Technology. 13 November 2008. Archived from the original on 21 February 2011.
  108. James Collier; Geoffrey F. Hewitt (1987). Introduction to Nuclear Power. Taylor & Francis. p. 64. ISBN   978-1-56032-682-3.
  109. "Glenn Contributions to Deep Space 1". NASA. 21 May 2008. Archived from the original on 1 October 2009. Retrieved 7 July 2009.
  110. "Electric space propulsion". The Internet Encyclopedia of Science. David Darling. Archived from the original on 30 May 2009. Retrieved 7 July 2009.
  111. "IMERC Fact Sheet: Mercury Use in Batteries". Northeast Waste Management Officials' Association. January 2010. Archived from the original on 29 November 2012. Retrieved 20 June 2013.
  112. Mercury Silvering, archived from the original on 4 March 2005, retrieved 12 February 2010.
  113. "Organotin Compounds in the Environment". Open Chemist. Archived from the original on 10 March 2007.
  114. Smart, N. A. (1968). "Use and residues of mercury compounds in agriculture". Residue Reviews / Rückstands-Berichte. Vol. 23. pp. 1–36. doi:10.1007/978-1-4615-8437-7_1. ISBN   978-1-4615-8439-1. PMID   4875698.{{cite book}}: |journal= ignored (help)
  115. Gray, T. (22 September 2004). "The Amazing Rusting Aluminum". Popular Science. Archived from the original on 20 July 2009. Retrieved 7 July 2009.
  116. Francis, G. W. (1849). Chemical Experiments. D. Francis. p. 62.
  117. Castles, W. T.; Kimball, V. F. (2005). Firearms and Their Use. Kessinger Publishing. p. 104. ISBN   978-1-4179-8957-7.
  118. Lee, J. D. (1999). Concise Inorganic Chemistry. Wiley-Blackwell. ISBN   978-0-632-05293-6.
  119. Waldron, H. A. (1983). "Did the Mad Hatter have mercury poisoning?". Br. Med. J. (Clin. Res. Ed.). 287 (6409): 1961. doi:10.1136/bmj.287.6409.1961. PMC   1550196 . PMID   6418283.
  120. Alpers, C. N.; Hunerlach, M. P.; May, J. Y.; Hothem, R. L. "Mercury Contamination from Historical Gold Mining in California". U.S. Geological Survey. Archived from the original on 22 February 2008. Retrieved 26 February 2008.
  121. "Mercury amalgamation". Corrosion Doctors. Archived from the original on 19 May 2009. Retrieved 7 July 2009.
  122. "Mercury 294594". Sigma-Aldrich.
  123. 1 2 McFarland, RB & Reigel, H (1978). "Chronic Mercury Poisoning from a Single Brief Exposure". J. Occup. Med. 20 (8): 532–4. doi:10.1097/00043764-197808000-00003. PMID   690736.
  124. 1 2 Mercury, Environmental Health Criteria monograph No. 001, Geneva: World Health Organization, 1976, ISBN   92-4-154061-3
  125. "Glacial Ice Cores Reveal A Record of Natural and Anthropogenic Atmospheric Mercury Deposition for the Last 270 Years". United States Geological Survey (USGS). Archived from the original on 4 July 2007. Retrieved 1 May 2007.
  126. "Indoor Air Mercury" (PDF). Northeast Waste Management Officials' Association. May 2003. Archived from the original (PDF) on 25 March 2009. Retrieved 7 July 2009.
  127. 1 2 3 Pacyna E G; Pacyna J M; Steenhuisen F; Wilson S (2006). "Global anthropogenic mercury emission inventory for 2000". Atmos Environ. 40 (22): 4048. Bibcode:2006AtmEn..40.4048P. doi:10.1016/j.atmosenv.2006.03.041.
  128. Maprani, Antu C.; Al, Tom A.; MacQuarrie, Kerry T.; Dalziel, John A.; Shaw, Sean A.; Yeats, Phillip A. (2005). "Determination of Mercury Evasion in a Contaminated Headwater Stream". Environmental Science & Technology. 39 (6): 1679–87. Bibcode:2005EnST...39.1679M. doi:10.1021/es048962j. PMID   15819225.
  129. 1 2 "Minamata Disease The History and Measures". Ministry of the Environment, Government of Japan. Archived from the original on 24 June 2009. Retrieved 7 July 2009.
  130. 1 2 Dennis Normile (27 September 2013). "In Minamata, Mercury Still Divides". Science. 341 (6153): 1446–7. Bibcode:2013Sci...341.1446N. doi:10.1126/science.341.6153.1446. PMID   24072902.
  131. Ciriminna, Rosaria; Falletta, Ermelinda; Della Pina, Cristina; Teles, Joaquim Henrique; Pagliaro, Mario (2016). "Industrial Applications of Gold Catalysis". Angewandte Chemie International Edition. 55 (46): 1433–7851. doi:10.1002/anie.201604656. hdl: 2434/463818 . PMID   27624999. S2CID   28730917.
  132. "Mercury-containing Products". United States Environmental Protection Agency (EPA). Archived from the original on 12 February 2007. Retrieved 1 May 2007.
  133. "IMERC Fact Sheet: Mercury Use in Thermostats" (PDF). Northeast Waste Management Officials' Association. January 2010. Archived from the original (PDF) on 17 June 2012.
  134. Pourkhabbaz, A.; Pourkhabbaz, H. (2012). "Investigation of Toxic Metals in the Tobacco of Different Iranian Cigarette Brands and Related Health Issues". Iranian Journal of Basic Medical Sciences. 15 (1): 636–644. PMC   3586865 . PMID   23493960.
  135. Talhout, Reinskje; Schulz, Thomas; Florek, Ewa; Van Benthem, Jan; Wester, Piet; Opperhuizen, Antoon (2011). "Hazardous Compounds in Tobacco Smoke". International Journal of Environmental Research and Public Health. 8 (12): 613–628. doi: 10.3390/ijerph8020613 . ISSN   1660-4601. PMC   3084482 . PMID   21556207.
  136. Bernhard D, Rossmann A, Wick G (2005). "Metals in Cigarette Smoke". IUBMB Life. 57 (12): 805–809. doi: 10.1080/15216540500459667 . PMID   16393783. S2CID   35694266.
  137. Shen, Huazhen; Tsai, Cheng-Mou; Yuan, Chung-Shin; Jen, Yi-Hsiu; Ie, Iau-Ren (2017). "How incense and joss paper burning during the worship activities influences ambient mercury concentrations in indoor and outdoor environments of an Asian temple?". Chemosphere. 167: 530–540. Bibcode:2017Chmsp.167..530S. doi:10.1016/j.chemosphere.2016.09.159. PMID   27764746.
  138. Lin, Chunshui; Huang, Ru-Jin; Duan, Jing; Zhong, Haobin; Xu, Wei; Wu, Yunfei; Zhang, Renjian (2022). "Large contribution from worship activities to the atmospheric soot particles in northwest China". Environmental Pollution. 299: 118907. doi:10.1016/j.envpol.2022.118907. PMID   35091017. S2CID   246355499.
  139. "Parkinson's disease in occupational exposure to joss paper, a report of two cases".
  140. Azziz-Baumgartner, E; Luber, G; Schurz-Rogers, H; Backer, L; Belson, M; Kieszak, S; Caldwell, K; Lee, B; Jones, R (2007). "Exposure assessment of a mercury spill in a Nevada school -- 2004". Clin Toxicol. 45 (4): 391–395. doi:10.1080/15563650601031569. PMID   17486480. S2CID   33770481.
  141. "Mercury: Spills, Disposal and Site Cleanup". Environmental Protection Agency. Archived from the original on 13 May 2008. Retrieved 11 August 2007.
  142. "Action Levels for Elemental Mercury Spills" (PDF). www.atsdr.cdc.gov. 22 March 2012.
  143. Yu, Jin-Gang; Yue, Bao-Yu; Wu, Xiong-Wei; Liu, Qi; Jiao, Fei-Peng; Jiang, Xin-Yu; Chen, Xiao-Qing (1 December 2015). "Removal of mercury by adsorption: a review". Environmental Science and Pollution Research. 23 (6): 5056–5076. doi:10.1007/s11356-015-5880-x. PMID   26620868. S2CID   28365564.
  144. 1 2 3 Vane, C.H.; Beriro, D.J.; Turner, G.H. (2015). "Rise and fall of mercury (Hg) pollution in sediment cores of the Thames Estuary, London, UK". Earth and Environmental Science Transactions of the Royal Society of Edinburgh. 105 (4): 285–296. doi: 10.1017/S1755691015000158 . ISSN   1755-6910.
  145. Vane, C.H.; Jones, D.G.; Lister, T.R. (2009). "Mercury contamination in surface sediments and sediment cores of the Mersey Estuary, UK" (PDF). Marine Pollution Bulletin. 58 (6): 940–946. Bibcode:2009MarPB..58..940V. doi:10.1016/j.marpolbul.2009.03.006. ISSN   0025-326X. PMID   19356771.
  146. Vane, C.H.; Harrison, I.; Kim, A.W.; Moss-Hayes, V.; Vickers, B.P.; Horton, B.P. (2008). "Status of organic pollutants in surface sediments of Barnegat Bay-Little Egg Harbor Estuary, New Jersey, USA" (PDF). Marine Pollution Bulletin. 56 (10): 1802–1808. Bibcode:2008MarPB..56.1802V. doi:10.1016/j.marpolbul.2008.07.004. ISSN   0025-326X. PMID   18715597.
  147. Vane, C.H.; Harrison, I.; Kim, A.W.; Moss-Hayes, V.; Vickers, B.P.; Hong, K. (2009). "Organic and metal contamination in surface mangrove sediments of South China" (PDF). Marine Pollution Bulletin. 58 (1): 134–144. Bibcode:2009MarPB..58..134V. doi:10.1016/j.marpolbul.2008.09.024. ISSN   0025-326X. PMID   18990413.
  148. "Mercury and health". World Health Organization. 31 March 2017. Retrieved 22 December 2023.
  149. "1910.1000 TABLE Z-2". Occupational Safety and Health Administration. 23 June 2006. Retrieved 22 December 2023.
  150. "Mercury compounds [except (organo) alkyls] (as Hg)". Centers for Disease Control and Prevention. The National Institute for Occupational Safety and Health. 30 October 2019. Retrieved 22 December 2023.
  151. Cocoros, Glenn; Cahn, Phyllis H.; Siler, William (November 1973). "Mercury concentrations in fish, plankton and water from three Western Atlantic estuaries". Journal of Fish Biology. 5 (6): 641–647. Bibcode:1973JFBio...5..641C. doi:10.1111/j.1095-8649.1973.tb04500.x.
  152. "How We Do Things at IISD-ELA: Collecting a fish muscle biopsy". IISD. 30 September 2015. Retrieved 7 July 2020.
  153. Mole, Beth (20 December 2019). "Woman had 524x the normal level of mercury in her blood from skin cream use". ArsTechnica. Retrieved 20 July 2021.
  154. Mudan, Anita, Copan L, Wang R, et al. (20 December 2019). "Notes from the Field: Methylmercury Toxicity from a Skin Lightening Cream Obtained from Mexico — California, 2019". Morbidity and Mortality Weekly Report. 68 (50): 1166–1167. doi:10.15585/mmwr.mm6850a4. PMC   6936160 . PMID   31856147.
  155. McKelvey W; Jeffery N; Clark N; Kass D; Parsons PJ. 2010 (2011). "Population-Based Inorganic Mercury Biomonitoring and the Identification of Skin Care Products as a Source of Exposure in New York City". Environ Health Perspect. 119 (2): 203–9. doi:10.1289/ehp.1002396. PMC   3040607 . PMID   20923743.{{cite journal}}: CS1 maint: numeric names: authors list (link)
  156. Ngim, CH; Foo, SC; Boey, KW; Keyaratnam, J (1992). "Chronic neurobehavioral effects of elemental mercury in dentists". British Journal of Industrial Medicine. 49 (11): 782–90. doi:10.1136/oem.49.11.782. PMC   1039326 . PMID   1463679.
  157. Liang, Y. X.; Sun, R. K.; Sun, Y.; Chen, Z. Q.; Li, L. H. (1993). "Psychological effects of low exposure to mercury vapor: Application of computer-administered neurobehavioral evaluation system". Environmental Research. 60 (2): 320–7. Bibcode:1993ER.....60..320L. doi:10.1006/enrs.1993.1040. PMID   8472661.
  158. Inorganic mercury, Environmental Health Criteria monograph No. 118, Geneva: World Health Organization, 1991, ISBN   92-4-157118-7
  159. 1 2 Bluhm, RE; Bobbitt, RG; Welch, LW; Wood, AJJ; Bonfiglio, JF; Sarzen, C; Heath, AJ; Branch, RA (1992). "Elemental Mercury Vapour Toxicity, Treatment, and Prognosis After Acute, Intensive Exposure in Chloralkali Plant Workers. Part I: History, Neuropsychological Findings and Chelator effects". Hum Exp Toxicol. 11 (3): 201–10. Bibcode:1992HETox..11..201B. doi:10.1177/096032719201100308. PMID   1352115. S2CID   43524794.
  160. "Minamata Convention Agreed by Nations". United Nations Environment Program. Archived from the original on 30 January 2013. Retrieved 19 January 2013.
  161. Section, United Nations News Service (19 January 2013). "UN News — Governments at UN forum agree on legally-binding treaty to curb mercury pollution". UN News Service Section. Archived from the original on 16 October 2016. Retrieved 22 November 2016.
  162. "Mercury: Laws and regulations". United States Environmental Protection Agency. 16 April 2008. Archived from the original on 13 May 2008. Retrieved 30 May 2008.
  163. "Reductions in Mercury Emissions". International Joint Commission on the Great Lakes. Archived from the original on 28 August 2008. Retrieved 21 July 2008.
  164. "Clean Air Mercury Rule". United States Environmental Protection Agency (EPA). Archived from the original on 30 June 2007. Retrieved 1 May 2007.
  165. "State of New Jersey et al., Petitioners vs. Environmental Protection Agency (Case No. 05-1097)" (PDF). United States Court of Appeals for the District of Columbia Circuit. Argued 6 December 2007, Decided 8 February 2008. Archived (PDF) from the original on 3 February 2011. Retrieved 30 May 2008.
  166. Castro MS, Sherwell J (2015). "Effectiveness of Emission Controls to Reduce the Atmospheric Concentrations of Mercury". Environmental Science & Technology . 49 (24): 14000–14007. Bibcode:2015EnST...4914000C. doi:10.1021/acs.est.5b03576. PMID   26606506.
  167. "Oldest, dirtiest power plants told to clean up". Boston Globe. 22 December 2011. Archived from the original on 14 July 2014. Retrieved 2 January 2012.
  168. Howard Berkes (10 November 2011). "EPA Regulations Give Kilns Permission To Pollute". NPR. Archived from the original on 17 November 2011. Retrieved 2 January 2012.
  169. "Directive 2002/95/EC on the Restriction of the Use of Certain Hazardous Substances in Electrical and Electronic Equipment". 27 January 2003. Article 4 Paragraph 1. e.g. "Member States shall ensure that, from July 1, 2006, new electrical and electronic equipment put on the market does not contain lead, mercury, cadmium, hexavalent chromium, polybrominated biphenyls (PBB) or polybrominated diphenyl ethers (PBDE)."
  170. "Mercury compounds in European Union". EIA Track. 2007. Archived from the original on 28 April 2008. Retrieved 30 May 2008.
  171. Jones H. (10 July 2007). "EU bans mercury in barometers, thermometers". Reuters. Archived from the original on 3 January 2009. Retrieved 12 September 2017.
  172. "Norway to ban mercury". EU Business. 21 December 2007. Archived from the original on 21 January 2008. Retrieved 30 May 2008.
  173. Berg, T; Fjeld, E; Steinnes, E (2006). "Atmospheric mercury in Norway: contributions from different sources". The Science of the Total Environment. 368 (1): 3–9. Bibcode:2006ScTEn.368....3B. doi:10.1016/j.scitotenv.2005.09.059. PMID   16310836.
  174. Edlich, Richard F; Rhoads, Samantha K.; Cantrell, Holly S.; Azavedo, Sabrina M.; Newkirk, Anthony T. Banning Mercury Amalgam in the United States (PDF) (Report). USA: Food and Drug Administration. Archived from the original (PDF) on 1 November 2013.
  175. "Sweden to ban mercury". The Local. 14 January 2009. Archived from the original on 28 August 2016. Retrieved 22 November 2016.
  176. "Sweden may be forced to lift ban on mercury". The Local. 21 April 2012. Archived from the original on 28 August 2016. Retrieved 22 November 2016.
  177. "Survey of mercury and mercury compounds" (PDF). Miljøstyrelsen. 2014. Retrieved 21 December 2023.

Further reading