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[2] [7] The heat of formation is c. 24 kilocalories (100 kJ) per mol. [7] It is a semiconductor with a reported bandgap of c. 3.2eV, [9] however, a thin zinc nitride film prepared by electrolysis of molten salt mixture containing Li 3 N with a zinc electrode showed a band-gap of 1.01 eV. [10] Zinc nitride reacts violently with water to form ...
Zinc compounds are noteworthy for their nondescript appearance and behavior: they are generally colorless (unlike compounds of other elements with oxidation number +2, which are colored), do not readily engage in redox reactions, and generally adopt symmetrical structures. [1] [2] [3] [4]
Platinum nitride and osmium nitride may contain N 2 units, and as such should not be called nitrides. [11] [12] Nitrides of heavier members from group 11 and 12 are less stable than copper nitride (Cu 3 N) and zinc nitride (Zn 3 N 2): dry silver nitride (Ag 3 N) is a contact explosive which may detonate from the slightest touch, even a falling ...
[1] Side effects of alcohols applied to the skin include skin irritation. [2] Care should be taken with electrocautery, as ethanol is flammable. [1] Types of alcohol used include ethanol, denatured ethanol, 1-propanol, and isopropyl alcohol. [6] [7] Alcohols are effective against a range of microorganisms, though they do not inactivate spores. [7]
Titanium-nitride coatings can also be deposited by thermal spraying whereas TiN powders are produced by nitridation of titanium with nitrogen or ammonia at 1200 °C. [ 7 ] Bulk ceramic objects can be fabricated by packing powdered metallic titanium into the desired shape, compressing it to the proper density, then igniting it in an atmosphere ...
Cyanogen is typically generated from cyanide compounds. One laboratory method entails thermal decomposition of mercuric cyanide: . 2 Hg(CN) 2 → (CN) 2 + Hg 2 (CN) 2 Or, one can combine solutions of copper(II) salts (such as copper(II) sulfate) with cyanides; an unstable copper(II) cyanide is formed which rapidly decomposes into copper(I) cyanide and cyanogen.
Mononuclear complexes feature terminal nitride ligands, typically with short M-N distances consistent with metal ligand multiple bonds. For example, in the anion in PPh 4 [MoNCl 4], the Mo-N distance is 163.7 pm. The occurrence of terminal nitrido ligands follow the patterns seen for oxo complexes: they are more common for early and heavier metals.
The oxynitrides are a group of inorganic compounds containing oxygen and nitrogen not bound to each other, instead combined with other non-metallic or metallic elements. Some of these are oxosalts with oxygen replaced by nitrogen.