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In Vietnam, the use of laughing gas as a recreational substance began in the 2000s due to its affordability. The balloons used for inhaling the gas are called funky balls [26] and are widely available in bars, pubs, and online for home delivery. This trend is most noticeable in urban areas and social gatherings frequented by young adults.
Nitrous oxide (dinitrogen oxide or dinitrogen monoxide), commonly known as laughing gas, nitrous, or factitious air, among others, [4] is a chemical compound, an oxide of nitrogen with the formula N 2 O. At room temperature, it is a colourless non-flammable gas, and has a slightly sweet scent and taste. [4]
Onset of effect is typically within half a minute, and the effect lasts for about a minute. [1] Nitrous oxide was discovered between 1772 and 1793 and used for anesthesia in 1844. [3] It is on the World Health Organization's List of Essential Medicines. [4] It often comes as a 50/50 mixture with oxygen. [1]
The polarizing effect of Zn 2+ is part of the reason why zinc is found in enzymes such as carbonic anhydrase. Structure of a monomeric zinc dialkyldithiophosphate No fluoro complexes are known, but complexes with the other halides and with pseudohalides , [ZnX 3 ] − and [ZnX 4 ] 2− can be prepared.
In gas nitriding the donor is a nitrogen-rich gas, usually ammonia (NH 3), which is why it is sometimes known as ammonia nitriding. [2] When ammonia comes into contact with the heated work piece it dissociates into nitrogen and hydrogen. The nitrogen then diffuses onto the surface of the material creating a nitride layer.
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 ...
Zinc nitrate has no large scale application but is used on a laboratory scale for the synthesis of coordination polymers. [4] Its controlled decomposition to zinc oxide has also been used for the generation of various ZnO based structures, including nanowires.
It can also be formed by heating zinc to 600 °C in a current of ammonia; the by-product is hydrogen gas. [3] [5] 3 Zn + 2 NH 3 → Zn 3 N 2 + 3 H 2. The decomposition of Zinc Nitride into the elements at the same temperature is a competing reaction. [6] At 700 °C Zinc Nitride decomposes. [1]