Difference between revisions of "Mercury(II) oxide"
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| SolubleOther = Reacts with acids<br>Insoluble in [[acetone]], alcohols, [[ammonia]], ethers, | | SolubleOther = Reacts with acids<br>Insoluble in [[acetone]], alcohols, [[ammonia]], ethers, | ||
| Solvent = | | Solvent = | ||
| − | | VaporPressure = | + | | VaporPressure = ~0 mmHg |
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| Section3 = {{Chembox Structure | | Section3 = {{Chembox Structure | ||
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| OtherFunction = | | OtherFunction = | ||
| OtherFunction_label = | | OtherFunction_label = | ||
| − | | OtherCompounds = [[Zinc oxide]] | + | | OtherCompounds = [[Zinc oxide]]<br>[[Cadmium oxide]] |
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==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
| − | Mercury oxide | + | Mercury(II) oxide reacts with most acids to give mercury salts, making it the basic precursor for any mercury compound. |
===Physical=== | ===Physical=== | ||
| − | Mercury(II) oxide is a dense red or orange solid, insoluble in water | + | Mercury(II) oxide is a dense red or orange solid, insoluble in water and organic solvents. |
==Availability== | ==Availability== | ||
| Line 125: | Line 125: | ||
==Preparation== | ==Preparation== | ||
| − | Mercuric oxide can be made via pyrolysis of [[mercury(II) nitrate]] below 500 °C. | + | Mercuric oxide can be made via pyrolysis of [[mercury(II) nitrate]] at temperature above 360 °C, but below 500 °C. |
| + | |||
| + | : Hg(NO<sub>3</sub>)<sub>2</sub> → HgO + 2 NO<sub>2</sub> + ½ O<sub>2</sub> | ||
| + | |||
| + | An less hazardous route involves hydrolyzing [[mercury(II) sulfate]] in water using [[sodium hydroxide]] in a 1:2 molar ratio:<ref>https://www.youtube.com/watch?v=k5mYdz7IWl8</ref> | ||
| + | |||
| + | : HgSO<sub>4</sub> + 2 NaOH → HgO + Na<sub>2</sub>SO<sub>4</sub> + H<sub>2</sub>O | ||
| + | |||
| + | However, the HgO obtained through this route is difficult to purify, as it's difficult to dry and contains lots of unreacted mercuric sulfate. | ||
==Projects== | ==Projects== | ||
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<references/> | <references/> | ||
===Relevant Sciencemadness threads=== | ===Relevant Sciencemadness threads=== | ||
| + | *[https://www.sciencemadness.org/whisper/viewthread.php?tid=158643 Mercuric oxide from mercuric sulfate] | ||
*[http://www.sciencemadness.org/talk/viewthread.php?tid=61769 Mercury Oxide?] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=61769 Mercury Oxide?] | ||
*[http://www.sciencemadness.org/talk/viewthread.php?tid=3842 Mercury Oxides] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=3842 Mercury Oxides] | ||
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[[Category:Things that should NOT be messed with except by professionals]] | [[Category:Things that should NOT be messed with except by professionals]] | ||
[[Category:Contact poisons]] | [[Category:Contact poisons]] | ||
| + | [[Category:Neurotoxins]] | ||
Latest revision as of 21:26, 16 October 2022
| Names | |
|---|---|
| IUPAC name
Mercury(II) oxide
| |
| Other names
Mercuric oxide
Montroydite Red mercuric oxide Red mercury | |
| Properties | |
| HgO | |
| Molar mass | 216.59 g/mol |
| Appearance | Yellow or red solid |
| Odor | Odorless |
| Density | 11.14 g/cm3 |
| Melting point | 500 °C (932 °F; 773 K) (decomposes) |
| Boiling point | Decomposes |
| 0.0053 g/100 ml (25 °C) 0.0395 g/100 ml (100 °C) | |
| Solubility | Reacts with acids Insoluble in acetone, alcohols, ammonia, ethers, |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std molar
entropy (S |
70 J·mol−1·K−1 |
| Std enthalpy of
formation (ΔfH |
−90 kJ/mol |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
18 mg/kg (rat, oral) |
| Related compounds | |
| Related compounds
|
Zinc oxide Cadmium oxide |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Mercury(II) oxide, or mercuric oxide is a red or orange solid, with the formula HgO.
Contents
Properties
Chemical
Mercury(II) oxide reacts with most acids to give mercury salts, making it the basic precursor for any mercury compound.
Physical
Mercury(II) oxide is a dense red or orange solid, insoluble in water and organic solvents.
Availability
Mercuric oxide can be found in the cathode of old mercury batteries.
Mercury oxide can be bought from chemical suppliers, though it's not easy to get hold of.
Mercury and mercury compounds cannot be freely acquired in EU.
Preparation
Mercuric oxide can be made via pyrolysis of mercury(II) nitrate at temperature above 360 °C, but below 500 °C.
- Hg(NO3)2 → HgO + 2 NO2 + ½ O2
An less hazardous route involves hydrolyzing mercury(II) sulfate in water using sodium hydroxide in a 1:2 molar ratio:[1]
- HgSO4 + 2 NaOH → HgO + Na2SO4 + H2O
However, the HgO obtained through this route is difficult to purify, as it's difficult to dry and contains lots of unreacted mercuric sulfate.
Projects
- Make mercury(II) chloride
- Make elemental mercury
Handling
Safety
Mercury(II) oxide is extremely toxic. Ingestion may be fatal.
Storage
In closed glass or plastic bottles, away from acids.
Disposal
Mercury(II) oxide should be converted to an insoluble mercury compound, such as mercury sulfide, then taken to hazardous waste disposal centers.
References
Relevant Sciencemadness threads
- Articles containing unverified chemical infoboxes
- Chembox articles without image
- Chemical compounds
- Inorganic compounds
- Mercury compounds
- Oxides
- Materials unstable in acidic solution
- Things that can kill you very quickly
- Things that should NOT be messed with except by professionals
- Contact poisons
- Neurotoxins
