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Zinc nitride reacts violently with water to form ammonia and zinc oxide. [3] [4] Zn 3 N 2 + 3 H 2 O → 3 ZnO + 2 NH 3. Zinc nitride reacts with lithium (produced in an electrochemical cell) by insertion. The initial reaction is the irreversible conversion into LiZn in a matrix of beta-Li 3 N. These products then can be converted reversibly and ...
In its compounds, Zn 2+ ions have an electronic configuration [Ar] 3d 10.As such, Zn 2+ tends to have a symmetrical coordination geometry in both its complexes and compounds. In both ZnO and ZnS, zinc is bound tetrahedrally bound to four ligands (oxide and sulfide, respectively).
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 ...
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
Zinc nitrate is usually prepared by dissolving zinc metal, zinc oxide, or related materials in nitric acid: Zn + 2 HNO 3 → Zn(NO 3) 2 + H 2 ZnO + 2 HNO 3 → Zn(NO 3) 2 + H 2 O. These reactions are accompanied by the hydration of the zinc nitrate.
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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.
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