Mercury oxide naming

In 1787 William Cruikshank (1745-1795) isolated, but did not identify, strontium from the mineral strontianite he examined. In 1790 Dr. Adair Crawford (1748—1794), an Irish chemist, discovered strontium by accident as he was examining barium chloride. He found a substance other than what he expected and considered it a new mineral. He named the new element strontium and its mineral strontianite after a village in Scotland. In 1808 Sir Humphry Davy treated the ore with hydrochloric acid, which produced strontium chloride. He then mixed mercury oxide with the strontium chloride to form an amalgam alloy of the two metals that collected at the cathode of his electrolysis apparatus. He heated the resulting substance to vaporize the mercury, leaving the strontium metal as a deposit. 

The facts on air composition were expressed most clearly by Scheele, in his booklet Abhandlmg von der Luft und dem Feuer (Treatise on Air and Fire), which was published in 1777 (Scheele 1777). From laboratory scripts it is now known that Scheele discovered oxygen - dephlogisticated air - before Priestley and by similar methods heating silver carbonate, red mercury oxide, salpeter and magnesium nitrate. Scheele also discovered chlorine (CI2), and he named the ingredients of air as Feuerluft (O2) and verdorbene Luft (N2). Scheele found evidence that one unit of oxygen produces one volume of carbon dioxide and defined that... 

Discovery Scheele discovered oxygen, probably in 1772. He prepared oxygen by heating mercury oxide and silver carbonate. The result was published in 1777. In 1774 Priestley discovered oxygen independently. Lavoisier gave the name oxygine to the element. 

The biological eflect of an element is not only dependent on the total concentration, but also highly related to its chemical forms present in biological systems, e.g. the oxidation state, the nature of the ligands or even the molecular structure. Dramatic examples are chromium, tin and mercury, to name just a few. Cr(VI) ions are considered far more toxic than Cr(III). Although the inorganic forms of tin and mercury are less toxic or even do not show toxic... 

Another very interesting application of this increased chemical activity of aluminium when amalgamated with mercury is incorporated in a toy which is sometimes seen on sale under the name of" Daddy Tin Whiskers . This toy consists of an aluminium stamping of a face and a pencil, the core of which is filled with a preparation chiefly composed of a mercury salt. It is operated by rubbing the eyebrows and chin with this special pencil. Shortly afterwards white hairs of aluminium oxide (AlsOj) gather wherever the pencil has touched the aluminium. 

Ozone was discovered in 1785 by the Dutch chemist Van Marum. He observed that when an electric spark passed through oxygen, a product was formed that had a peculiar, irritating odor and that tarnished mercury. Schonhein confirmed Van Marum s observation in 1840 and determined the oxidizing properties of this irritating odor gas. He named it ozone from the Greek word ozo, which means smelling. ... 

William Cruickshank in 1787 and Adair Crawford in 1790 independently detected strontium in the mineral strontianite, small quantities of which are associated with calcium and barium minerals. They determined that the strontianite was an entirely new mineral and was different from baryta and other barium minerals known at the time. In 1808, Sir Humphry Davy isolated strontium by electrolysis of a mixture of moist strontium hydroxide or chloride with mercuric oxide, using a mercury cathode. The element was named after the town Strontian in Scotland where the mineral strontianite was found. 

Then a French pharmacist named Pierre Bayen pointed out to Lavoisier that calx of mercur) , which we would now call mercuric oxide, can be converted to mercury simply by heating, without the need for phlogiston-rich charcoal. Moreover, the gas released in this process was not Black s fixed air, but something quite different. What was this gas That started to become clear to Lavoisier when Joseph Priestley came to dinner. 

A. J. Balard,9 in 1821, also prepared hypobromous acid in a similar manner, namely, by the gradual addition of mercuric oxide of bromine water, and thoroughly shaking the mixture after each addition. Further, quantities of bromine and mercuric oxide can be added until the yellow fluid contains between 6 and 7 parts of HOBr per 100 c.c. The mercuric oxide can be replaced by silver oxide, silver or mercuric nitrate, mercuric acetate, etc. The soln. with 6-7 parts of HOBr per 100 c.c. decomposes at 30°, but more dil. soln. when distilled under ordinary atm. press, give a distillate of bromine followed by a straw-yellow fraction which is a dil. aq. soln. of hypobromous acid. The decomposition is not so pronounced if it be conducted at 40° under a press, of, say, 50 mm. of mercury. 

For use in medicine he directs to use only the first two preparations, though others are used in chemistry. He explains further the preparation of the waters above employed which are merely water solutions of salts named. The mortification of copper, lead, mercury and other metals is similarly described, with products such as verdigris, white lead, corrosive sublimate, or the various oxides, etc. In some cases, as with gold, the processes are elaborate but the fancied results are not capable of rational interpretation.7... 

After washing and drying the capillary, many experimenters simply lower the mercury reservoir enough to stop the flow of mercury, but this procedure can occasionally cause problems. The inevitable metal impurities in mercury can be air-oxidized at the capillary tip, and the oxidation products may change the parameters of the electrode (namely, m and td). There is also a possibility that a small amount of the sample solution may remain in the capillary and then evaporate, leaving a solid residue this will also change the parameters of the electrode, and the residue may be very difficult to remove from the capillary. 

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