Facts about mercury
A heavy, silvery d-block element, mercury is easily obtained from cinnabar (HgS) which is widely used as a pigment. Mercury is still largely used in the electrochemical cell although it causes environmental pollution. It is also used for making thermometers, barometers, manometers, sphygmomanometers, float valves, etc.
Where is mercury found?
It is a very rare element found in the Earth’s crust but man discovered mercury in ancient times. It is found mostly in native forms or ores such as cinnabar (HgS), metacinnabar, sphalerite, corderoite, and livingstonite.
Most of the ores contain about one percent of Hg but ores from Spin contain 12 to 14 percent of Hg. Therefore, spin is the largest depositor of metal. It is also found at a very low level in the biosphere and in fossil fuels such as coal, oil, and natural gas.
The major mercury-producing countries were Spain, Italy, United States, Mexico, China, Kyrgyzstan, and Algeria.
Due to the fall in price, most of these countries shut down the production of mercury. Production of mercury from mining is still occurring in a number of countries such as Spain, China, Kyrgyzstan, and Algeria.
The extraction of mercury is relatively very simple. The crushed cinnabar (HgS) is concentrated by flotation.
It can obtain by heating HgS in the air (600 °C) followed by decomposition.
2HgS + 3O2 → 2HgO + 2SO2
2HgO → 2Hg + O2
- It may be purified by dropping a thin stream of impure Hg through a column of dilute nitric acid.
- Some dimercury (I) nitrate is produced.
- It reacts with the impure metal to produce its nitrate and liberate Hg.
- The process is repeated several times to gain desired purity level of mercury.
A better and most widely used technique is the distillation of impure mercury under a vacuum.
A heavy silvery-white metal, mercury has filled d-subshell. Therefore, it behaves more like a representative element rather than a transition metal.
The characteristic oxidation state of Hg is +2. It also formed dimercury or Hg2+2 with oxidation state +1.
|Discovery||discovered approx 1500BC|
|Origin of the name||named according to the planet, Mercury|
|Electron per shell||2, 8, 18, 32, 18, 2|
|Electronic configuration||[Xe] 4f14 5d10 6s2|
|Appearance||shiny, silvery liquid|
|State at 20°C||Liquid|
|Melting point||−38.8290 °C|
|Boiling point||356.73 °C|
|Critical temperature||1750 K|
|Atomic radius, non-bonded||2.23 Å|
|Covalent radius||1.32 Å|
|Common oxidation number||+1 and +2|
|Molar heat capacity||27.983 Jmol−1 K−1|
|Electron affinity (kJ mol−1)||Unknown|
|Electronegativity||2.00 according to the Pauling scale|
|Ionization energy (kJ/mol)||1st||2nd||3rd|
Electron configuration of mercury
Mercury in the periodic table
It is placed in place in group 12 and period 6 of the periodic table with valence shell electronic configuration 4f14 5d10 6s2. It is a d-block metal placed along with zinc and cadmium.
Compounds of mercury
The large difference between the 1st and 2nd ionization energies suggests that mercury formed chemical compounds in +1 and +2 oxidation states. A univalent state of Hg appears in the form of Hg2+2.
The study of mercury chemistry is incomplete without an appreciation of Hg (I) and Hg (II) equilibria. The redox potentials of different couples are given below the table,
|Equilibrium reaction||Redox potential (volt)|
|Hg2+2 + 2e → 2Hg||+0.789|
|2Hg+2 + 2e → Hg2+2||0.920|
|Hg+2 + 2e → Hg||+0.854|
|Hg2+2 → Hg + Hg+2||+0.131|
From the above table, only those oxidants with redox potential within the range +0.789 to +0.854 volt can oxidize metallic mercury to a dimercury (I) state.
From a practical viewpoint, we cannot find any oxidant whose potential lies in the range of +0.789 to +0.854. Therefore, direct oxidation of Hg to the dimercury (I) state is not possible. Most of the chemical compounds are formed in Hg (II) state.
Mercury (II) oxide
Mercury (II) oxide is a red or yellow colour chemical compound depending upon the particle size.
- The red form is obtained by slow heating of Hg in oxygen at about 350 °C. It is also obtained by heating Hg(NO3)2.
- A yellow form of HgO is obtained with the addition of alkali to the Hg (II) solution.
The oxide, HgO is weakly basic and dissolved in acids to form salts.
Mercury (II) sulfide
It is obtained in a red and black variety. The stable red variety is a costly pigment. The sulfide is very insoluble and can be brought into solution by boiling with aqua regia.
Chloride, bromide, and Iodide
On boiling with ammonia solution it gives an infusible white precipitate of Hg(NH2)Cl which is hydrolyzed to give Millon’s base. It reacts with gaseous ammonia to form a fusible white precipitate of HgCl2, 2NH3.
The solubility of halides in an aqueous solution decreases in the order of HgF2 > HgCl2 > HgBr2 > HgI2.
Nitrate and Sulfate
Mercury (II) nitrate and sulfate are obtained through the action of nitric acid or sulfuric acid on metallic Hg.
These are soluble water and stable in presence of acids.
6 Hg + 8 HNO3 → 3 Hg2(NO3)2 + 4 H2O + 2 NO
3 Hg2(NO3)2 + 8 HNO3 → 6 Hg(NO3)2 + 2 NO + 4 H2O
2 Hg + 2 H2SO4 → Hg2SO4 + SO2 + 2 H2O
What is mercury used for?
Elemental mercury was known in ancient India, China, Egypt, and Greece. Indian Ayurveda describes the extraction process of pure mercury from its ore cinnabar. They used it mostly on medicine and cosmetics.
Today the use of mercury is reduced due to its toxic effect on the environment and human health.
- It is still largely used in electrolytic cells for the production of caustic soda (NaOH) and chlorine gas.
- Liquid mercury is used in a secondary reference electrode such as a calomel electrode in electrochemistry. It is used for calculating the cell’s potential.
- It is used in electrical and electronic industries for making AC rectifiers and Hg vapour lamps.
- In the laboratory, it is widely used for making thermometers, barometers, manometers, sphygmomanometers, float valves, etc.
- The compounds such as phenyl mercury (II) acetate and other organomercury compounds have been used as fungicides and germicides.
- The amalgamation process is used for the extraction of precious metals such as silver and gold. It is gradually replaced by the cyanide process.
- Liquid mercury is used as a coolant in some nuclear power reactors.
How much mercury is toxic?
It is toxic due to its low vapour pressure and easily enters our body unless precaution is taken.
It produces several types of diseases such as tumors, headaches, inflammation of the bladder, loss of memory, and other brain disorders.
Alfred Stock was a victim of such type of mercury poisoning during the constant handling of vacuum pumps in connection with his research on boron and silicon hydride.
Mercury effects on the environment
Elemental mercury enters the sewage water through different types of industries and affects our environment in several ways.
These species are entered into plankton and thereafter our food chain via fishes. Organomercurials also enter into sewage water and our food chain through pesticides and fungicides.
The methyl mercury cation comes from the food chain attached to cell membranes and brain tissues. They are retained their position for a long period of time.
It may be inhabited the normal function of the brain. O.5 ppm level of CH3Hg+ in the blood is sufficient to disrupt normal physiological functioning.
The normal level of mercury in water is 0.001 to 0.0001 ppm but sewage effluent increases this level to 10 times greater. Ultimately it converted to CH3Hg+ and enter our food chain by causing a tragedy like Minamata.
The most tragic report of mercury poisoning came from Iraq in 1972 where 450 people died after consuming wheat-containing Hg pesticides.