Difference between revisions of "Copper(I) oxide"
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(Created page with "{{Chembox | Name = Copper(I) oxide | Reference = | IUPACName = Copper(I) oxide | PIN = | SystematicName = | OtherNames = <!-- Images --> | ImageFile = | ImageSize = | Image...") |
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| Line 5: | Line 5: | ||
| PIN = | | PIN = | ||
| SystematicName = | | SystematicName = | ||
| − | | OtherNames = | + | | OtherNames = Cuprite<br>Cuprous oxide<br>Dicopper oxide<br>Red copper oxide |
<!-- Images --> | <!-- Images --> | ||
| ImageFile = | | ImageFile = | ||
| Line 49: | Line 49: | ||
| Appearance = Brownish-red solid | | Appearance = Brownish-red solid | ||
| BoilingPt = | | BoilingPt = | ||
| − | | BoilingPtC = | + | | BoilingPtC = 1,800 |
| BoilingPt_ref = | | BoilingPt_ref = | ||
| BoilingPt_notes = | | BoilingPt_notes = | ||
| Line 58: | Line 58: | ||
| MolarMass = 143.09 g/mol | | MolarMass = 143.09 g/mol | ||
| MeltingPt = | | MeltingPt = | ||
| − | | MeltingPtC = | + | | MeltingPtC = 1,232 |
| MeltingPt_ref = | | MeltingPt_ref = | ||
| MeltingPt_notes = | | MeltingPt_notes = | ||
| Line 65: | Line 65: | ||
| pKb = | | pKb = | ||
| Solubility = Insoluble | | Solubility = Insoluble | ||
| − | | SolubleOther = | + | | SolubleOther = Reacts with acids, aq. [[ammonia|NH<sub>3</sub>]]<br>Insoluble in alcohols, ethers, halocarbons, hydrocarbons |
| Solvent = | | Solvent = | ||
| VaporPressure = ~0 mmHg | | VaporPressure = ~0 mmHg | ||
| Line 71: | Line 71: | ||
| Section3 = {{Chembox Structure | | Section3 = {{Chembox Structure | ||
| Coordination = | | Coordination = | ||
| − | | CrystalStruct = | + | | CrystalStruct = Cubic |
| MolShape = | | MolShape = | ||
}} | }} | ||
| Line 77: | Line 77: | ||
| DeltaGf = | | DeltaGf = | ||
| DeltaHc = | | DeltaHc = | ||
| − | | DeltaHf = | + | | DeltaHf = −170 kJ·mol<sup>−1</sup> |
| − | | Entropy = | + | | Entropy = 93 J·mol<sup>−1</sup>·K<sup>−1</sup> |
| HeatCapacity = | | HeatCapacity = | ||
}} | }} | ||
| Section5 = {{Chembox Explosive | | Section5 = {{Chembox Explosive | ||
| − | | ShockSens = | + | | ShockSens = Non-explosive |
| − | | FrictionSens = | + | | FrictionSens = Non-explosive |
| − | | DetonationV = | + | | DetonationV = Non-explosive |
| − | | REFactor = | + | | REFactor = Non-explosive |
}} | }} | ||
| Section6 = {{Chembox Hazards | | Section6 = {{Chembox Hazards | ||
| − | | AutoignitionPt = | + | | AutoignitionPt = Non-flammable |
| − | | ExploLimits = | + | | ExploLimits = Non-explosive |
| − | | ExternalMSDS = | + | | ExternalMSDS = [https://www.docdroid.net/ujlhKU3/copperi-oxide-sa.pdf Sigma-Aldrich] |
| − | | FlashPt = | + | | FlashPt = Non-flammable |
| − | | LD50 = | + | | LD50 = 1.340 mg/kg (rat, oral) |
| LC50 = | | LC50 = | ||
| − | | MainHazards = | + | | MainHazards = Toxic |
| NFPA-F = | | NFPA-F = | ||
| NFPA-H = | | NFPA-H = | ||
| Line 105: | Line 105: | ||
| OtherFunction = | | OtherFunction = | ||
| OtherFunction_label = | | OtherFunction_label = | ||
| − | | OtherCompounds = [[Copper( | + | | OtherCompounds = [[Copper(II) oxide]] |
}} | }} | ||
}} | }} | ||
| Line 112: | Line 112: | ||
==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
| + | Copper(I) oxide degrades to [[copper(II) oxide]] in moist air. | ||
| + | : Cu<sub>2</sub>O + ½ O<sub>2</sub> → 2 CuO | ||
| − | + | Cuprous oxide reacts with dilute [[sulfuric acid]] and [[nitric acid]] to produce [[copper(II) sulfate]] and [[copper(II) nitrate]]. | |
| + | Copper(I) oxide dissolves in concentrated aq. [[ammonia]] solution to form the colorless complex [Cu(NH<sub>3</sub>)<sub>2</sub>]<sup>+</sup>, which is easily oxidized in air to the blue [Cu(NH<sub>3</sub>)<sub>4</sub>(H<sub>2</sub>O)<sub>2</sub>]<sup>2+</sup>. It dissolves in [[hydrochloric acid]] to give solutions of CuCl<sub>2</sub><sup>−</sup>. | ||
| + | |||
| + | ===Physical=== | ||
| + | Cuprous oxide is a reddish brown solid, odorless, insoluble in solvents. | ||
==Availability== | ==Availability== | ||
| Line 121: | Line 127: | ||
==Preparation== | ==Preparation== | ||
| − | Reduction of copper(II) solutions with [[sulfur dioxide]] will yield this compound. | + | Reduction of copper(II) solutions with [[sulfur dioxide]] will yield this compound. |
| − | + | Aqueous [[Copper(I) chloride|cuprous chloride]] solutions react with base like sodium hydroxide to give copper(I) oxide. | |
| + | In all procedures, the color of the product is highly sensitive to the procedural details. | ||
| − | == | + | ==Projects== |
| + | *Copper compound collecting | ||
| + | *Make copper metal | ||
| + | *Make copper complexes | ||
| + | ==Handling== | ||
===Safety=== | ===Safety=== | ||
| + | Copper(I) oxide is an irritant, so avoid handling it directly. | ||
===Storage=== | ===Storage=== | ||
| + | Copper(I) oxide should be kept in air-tight bottles, plastic or glass. | ||
===Disposal=== | ===Disposal=== | ||
| + | Reduce it to metallic copper with a reducing agent, which can be recycled. | ||
==References== | ==References== | ||
<references/> | <references/> | ||
===Relevant Sciencemadness threads=== | ===Relevant Sciencemadness threads=== | ||
| + | *[https://www.sciencemadness.org/whisper/viewthread.php?tid=74058 Preparation of Copper (I) oxide from copper?] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=3105 how to produce Cu2O at home] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=22534 Sintering Cu2O] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=5131 Fehlings and Cu2O...] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=13798 How we could synthesis and stabilized Cu2O] | ||
| + | |||
| + | [[Category:Chemical compounds]] | ||
| + | [[Category:Inorganic compounds]] | ||
| + | [[Category:Copper compounds]] | ||
| + | [[Category:Oxides]] | ||
| + | [[Category:Air-sensitive materials]] | ||
| + | [[Category:Materials unstable in acidic solution]] | ||
| + | [[Category:Pigments]] | ||
| + | [[Category:Insoluble compounds]] | ||
Latest revision as of 08:22, 5 August 2021
| Names | |
|---|---|
| IUPAC name
Copper(I) oxide
| |
| Other names
Cuprite
Cuprous oxide Dicopper oxide Red copper oxide | |
| Properties | |
| Cu2O | |
| Molar mass | 143.09 g/mol |
| Appearance | Brownish-red solid |
| Odor | Odorless |
| Density | 6.0 g/cm3 |
| Melting point | 1,232 °C (2,250 °F; 1,505 K) |
| Boiling point | 1,800 °C (3,270 °F; 2,070 K) |
| Insoluble | |
| Solubility | Reacts with acids, aq. NH3 Insoluble in alcohols, ethers, halocarbons, hydrocarbons |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std molar
entropy (S |
93 J·mol−1·K−1 |
| Std enthalpy of
formation (ΔfH |
−170 kJ·mol−1 |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
1.340 mg/kg (rat, oral) |
| Related compounds | |
| Related compounds
|
Copper(II) oxide |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Copper(I) oxide or cuprous oxide is the inorganic compound with the formula Cu2O.
Contents
Properties
Chemical
Copper(I) oxide degrades to copper(II) oxide in moist air.
- Cu2O + ½ O2 → 2 CuO
Cuprous oxide reacts with dilute sulfuric acid and nitric acid to produce copper(II) sulfate and copper(II) nitrate.
Copper(I) oxide dissolves in concentrated aq. ammonia solution to form the colorless complex [Cu(NH3)2]+, which is easily oxidized in air to the blue [Cu(NH3)4(H2O)2]2+. It dissolves in hydrochloric acid to give solutions of CuCl2−.
Physical
Cuprous oxide is a reddish brown solid, odorless, insoluble in solvents.
Availability
Is is sold by chemical suppliers. Can also be bought online.
Preparation
Reduction of copper(II) solutions with sulfur dioxide will yield this compound.
Aqueous cuprous chloride solutions react with base like sodium hydroxide to give copper(I) oxide.
In all procedures, the color of the product is highly sensitive to the procedural details.
Projects
- Copper compound collecting
- Make copper metal
- Make copper complexes
Handling
Safety
Copper(I) oxide is an irritant, so avoid handling it directly.
Storage
Copper(I) oxide should be kept in air-tight bottles, plastic or glass.
Disposal
Reduce it to metallic copper with a reducing agent, which can be recycled.
