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Heating produces highly toxic mercury fumes and oxygen, which increases the fire hazard. Mercury(II) oxide reacts violently with reducing agents, chlorine, hydrogen peroxide, magnesium (when heated), disulfur dichloride and hydrogen trisulfide. Shock-sensitive compounds are formed with metals and elements such as sulfur and phosphorus. [13]
Hydroxides of mercury are poorly characterized, as attempted isolation studies of mercury(II) hydroxide have yielded mercury oxide instead. [62] 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 ...
Mercury oxide can refer to: Mercury(I) oxide (mercurous oxide), Hg 2 O; Mercury(II) oxide (mercuric oxide), HgO; See also. Montroydite, the mineral form of mercury(II ...
Most salts with main group elements tend to contain only Hg(II) and metallic mercury, because the presence of strong Lewis bases destabilizes the intermetallic bond. In appropriate solvents, however, Hg(I) salts with derivatives of amides, pyridines, phosphorus trifluoride, tin(II), and certain other main group elements are all known. [9]
The standard Gibbs free energy of formation (G f °) of a compound is the change of Gibbs free energy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states (the most stable form of the element at 1 bar of pressure and the specified temperature, usually 298.15 K or 25 °C).
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Hg(II) can be alkylated by treatment with diazonium salts in the presence of copper metal. In this way 2-chloromercuri-naphthalene has been prepared. [12] Phenyl(trichloromethyl)mercury can be prepared by generating dichlorocarbene in the presence of phenylmercuric