Difference between revisions of "Nickel(II) perchlorate"
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Can be prepared by reacting [[nickel(II) oxide]] with [[perchloric acid]], followed by recrystallization. | Can be prepared by reacting [[nickel(II) oxide]] with [[perchloric acid]], followed by recrystallization. | ||
| − | : NiO + 2 HClO<sub>4</sub> → Ni(ClO<sub>4</sub>)<sub>2</sub> + | + | : NiO + 2 HClO<sub>4</sub> → Ni(ClO<sub>4</sub>)<sub>2</sub> + H<sub>2</sub>O |
Another route involves adding a solution of [[nickel(II) sulfate]] in a solution of [[barium perchlorate]]: | Another route involves adding a solution of [[nickel(II) sulfate]] in a solution of [[barium perchlorate]]: | ||
| Line 129: | Line 129: | ||
: NiSO<sub>4</sub> + Ba(ClO<sub>4</sub>)<sub>2</sub> → Ni(ClO<sub>4</sub>)<sub>2</sub> + BaSO<sub>4</sub>↓ | : NiSO<sub>4</sub> + Ba(ClO<sub>4</sub>)<sub>2</sub> → Ni(ClO<sub>4</sub>)<sub>2</sub> + BaSO<sub>4</sub>↓ | ||
| − | This route produces the hexahydrate form. Anhydrous nickel perchlorate cannot be produced by heating | + | This route produces the hexahydrate form. Anhydrous nickel perchlorate cannot be produced by heating nickel(II) perchlorate hexahydrate, since it decomposes upon heating. |
==Projects== | ==Projects== | ||
Latest revision as of 20:43, 16 November 2020
| Names | |
|---|---|
| IUPAC name
Nickel(II) perchlorate
| |
| Other names
Nickel diperchlorate
| |
| Properties | |
| Ni(ClO4)2 (anhydrous) Ni(ClO4)2·6H2O (hexahydrate) | |
| Molar mass | 257.59 g/mol (anhydrous) 365.68 g/mol (hexahydrate) |
| Appearance | Greenish solid |
| Odor | Odorless |
| Melting point | 140 °C (284 °F; 413 K) (hexahydrate) |
| 22.25 g/100 ml (0 °C) 25.06 g/100 ml (20 °C) 27.37 g/100 ml (45 °C) | |
| Solubility | Soluble in acetone, ethanol, methanol Insoluble in halocarbons |
| Vapor pressure | ~0 mmHg |
| Hazards | |
| Safety data sheet | Sigma-Aldrich (hexahydrate) |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Nickel(II) chloride Nickel(II) chlorate Nickel(II) nitrate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Nickel(II) nitrate is the chemical compound with the formula Ni(ClO4)2. It is commonly available as the hexahydrate form, Ni(ClO4)2·6H2O.
Contents
Properties
Chemical
Nickel(II) perchlorate will form complex with amines, which are powerful energetic compounds.
Physical
Nickel(II) perchlorate is a greenish hygroscopic solid, soluble in water.
Availability
Nickel(II) perchlorate is sold by chemical suppliers.
Preparation
Can be prepared by reacting nickel(II) oxide with perchloric acid, followed by recrystallization.
- NiO + 2 HClO4 → Ni(ClO4)2 + H2O
Another route involves adding a solution of nickel(II) sulfate in a solution of barium perchlorate:
- NiSO4 + Ba(ClO4)2 → Ni(ClO4)2 + BaSO4↓
This route produces the hexahydrate form. Anhydrous nickel perchlorate cannot be produced by heating nickel(II) perchlorate hexahydrate, since it decomposes upon heating.
Projects
- Make tris(ethylenediamine)nickel perchlorate[1]
- Make nickel hexamine perchlorate
- Make nickel hydrazine perchlorate
Handling
Safety
Nickel(II) perchlorate is a powerful oxidizing agent. In contact with strong acids, it will ignite organic material on contact. If a cotton or paper is soaked in nickel perchlorate and left to dry, the resulting material will burn very rapidly in contact with open flame, almost explode.
Since it's a nickel compound, it is irritating to the eyes, skin, respiratory tract, and is also a known allergen and carcinogen.
Storage
In closed plastic (HDPE or PTFE) or glass bottles, in a dry place, away from combustible materials and metallic powders.
Disposal
Nickel perchlorate should be reduced to chloride, then precipitated into an insoluble form and taken to waste disposal centers.
