Tetraamminecopper(II) sulfate: Difference between revisions
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| verifiedrevid = |
| verifiedrevid = 447611336 |
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| Name = Tetraamminecopper(II) sulfate monohydrate |
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| ImageFile = |
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| ImageFile1 = CuN4aq.png |
| ImageFile1 = CuN4aq.png |
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| ImageName1 = Ball-and-stick model of the |
| ImageName1 = Ball-and-stick model of the Tetramine copper(II) cation |
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| ImageCaption1 = Tetraamminecopper(II) sulfate monohydrate<br>{{legend|rgb(256, 128, 80)|[[Copper]], Cu}}{{legend|red|[[Oxygen]], O}}{{legend|blue|[[Nitrogen]], N}}{{legend|yellow|[[Sulfur]], S}}{{legend|white|[[Hydrogen]], H}} |
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| ImageCaption2 = Tetraamminecopper(II) sulfate monohydrate crystals |
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| ImageFile2 = Copper tetrammine sulfate.jpg |
| ImageFile2 = Copper tetrammine sulfate.jpg |
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| IUPACName = |
| IUPACName = Tetraammineaquacopper(II) sulfate |
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| OtherNames = |
| OtherNames = {{ubl|Cuprammonium(II) sulfate|Cuprammonium(II) sulfate monohydrate|Cupric sulfate, ammoniated|Tetraamminecopper(II) sulfate monohydrate}} |
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| SystematicName = |
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| Section1 = {{Chembox Identifiers |
| Section1 = {{Chembox Identifiers |
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| CASNo_Ref = {{cascite|correct|??}} |
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| CASNo = 14283-05-7 |
| CASNo = 14283-05-7 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = YMW7182547 |
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| SMILES = [OH2+][Cu-3]([NH3+])([NH3+])([NH3+])[NH3+].[O-][S+2]([O-])([O-])[O-]}} |
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| Section2 = {{Chembox Properties |
| Section2 = {{Chembox Properties |
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| Formula = [Cu( |
| Formula = {{chem2|[Cu(NH3)4(H2O)]SO4}} |
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| MolarMass = |
| MolarMass = 245.79 g/mol (monohydrate) |
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| Appearance = dark blue-purple solution or crystals |
| Appearance = dark blue-purple solution or crystals |
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| Odor = Ammonia |
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| Density = 1.81 g/cm<sup>3</sup> |
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| MeltingPt = |
| MeltingPt = |
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| BoilingPtC = 330 |
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| BoilingPt_ref = |
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| Solubility = 18.5 g/(100 g) (21.5 °C)<ref name=Brauer/>}} |
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| Section3 = {{Chembox Hazards |
| Section3 = {{Chembox Hazards |
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| MainHazards = |
| MainHazards = |
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| FlashPt = |
| FlashPt = |
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| AutoignitionPt = |
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| Autoignition = }} |
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}} |
}} |
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| Section4 = |
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| Section5 = |
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| Section6 = |
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[[File:Сульфат тетраамминмеди.jpg|alt=Tetraamminecopper(II) sulfate|thumb|Tetraaminecopper(II) sulfate monohydrate milled]] |
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[[File:Иодид тетраамиинмеди.jpg|alt=Tetraamminecopper(II) iodide|thumb|Analogous compound with different anion: tetraamminecopper(II) iodide monohydrate]] |
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⚫ | '''Tetraamminecopper(II) sulfate monohydrate''', or more precisely '''tetraammineaquacopper(II) sulfate''', is the [[salt (chemistry)|salt]] with the formula {{chem2|[Cu(NH3)4]SO4*H2O|auto=1}}, or more precisely {{chem2|[[copper|Cu]]([[ammonia|NH3]])4([[water|H2O]])][[sulfate|SO4]]}}. This dark blue to purple solid is a [[sulfuric acid]] salt of the [[Complex (chemistry)|metal complex]] {{chem2|[Cu(NH3)4(H2O)](2+)}} (tetraammineaquacopper(II) [[cation]]). It is closely related to [[Schweizer's reagent]], which is used for the production of [[cellulose]] fibers in the production of [[rayon]]. |
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==Synthesis== |
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⚫ | '''Tetraamminecopper(II) sulfate''' is the [[ |
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This compound can be prepared by adding concentrated [[aqueous solution]] of [[ammonia]] to a [[saturated solution|saturated]] aqueous solution of [[copper(II) sulfate pentahydrate]] followed by precipitation of the product with [[ethanol]] or [[isopropanol]].<ref name=Brauer>Editor G.Brauer "Tetraamminecopper (II) Sulfate" Handbook of Preparative Inorganic Chemistry, 2nd Ed., Academic Press, 1965, New York. Vol. 2. p. 1021.</ref> |
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:{{chem2|4 NH3 + CuSO4*5H2O → [Cu(NH3)4(H2O)]SO4 + 4 H2O}} |
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==Chemical reaction and solubility== |
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==Preparation, structure, properties== |
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This compound can be prepared by treating concentrated [[ammonia]] solution, NH<sub>3</sub>, to a [[wiktionary:saturated|saturated]] aqueous [[solution]] of [[copper sulfate]] [Cu(H<sub>2</sub>O)<sub>6</sub>]SO<sub>4</sub> until all the copper(II) hydroxide that is initially formed redissolves into a deep blue solution. The deep blue crystalline solid tends to hydrolyse and lose ammonia ligands upon standing in air. |
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The deep blue crystalline solid tends to [[hydrolyse]] and evolve (release) ammonia upon standing in air.<ref name=Brauer/> It is fairly soluble in water. The brilliant dark blue-violet color of tetraamminecopper(II) sulfate solution is due to presence of {{chem2|[Cu(NH3)4](2+)}} (tetraamminecopper(II) cation). Often, the dark blue-violet color is used as a positive test to verify the presence of {{chem2|Cu(2+)}} in a solution. |
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== Structure and properties == |
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The solid state structure of tetraamminecopper(II) sulfate monohydrate confirms that the compound is a [[salt (chemistry)|salt]]. The [[Metal complex|complex]] [[cation]] is {{chem2|[Cu(NH3)4(H2O)](2+)}} (tetraammineaquacopper(II) cation), which has a [[square pyramidal molecular geometry]]. The [[copper|Cu]]-[[nitrogen|N]] and Cu-[[oxygen|O]] bond length are about 210 and 233 [[picometre|pm]], respectively, as determined by [[X-ray crystallography]].<ref>{{cite journal|author=B. Morosin|title=The Crystal Structures of Copper Tetraammine Complexes. A. Cu(NH<sub>3</sub>)<sub>4</sub>SO<sub>4</sub><sup>.</sup>H<sub>2</sub>O and Cu(NH<sub>3</sub>)<sub>4</sub>SeO<sub>4</sub>|journal=Acta Crystallographica|year=1969|volume=B25|issue=1 |pages=19–30|doi=10.1107/S0567740869001725|bibcode=1969AcCrB..25...19M}}</ref> The correct concentrations of [[ammonia]] and [[copper(II) sulfate]] solution needed to synthesize the complex can be determined by [[colorimetry]]. The combination of the correct concentrations will produce the highest [[absorbance]] read out on the [[Colorimeter (chemistry)|colorimeter]] and as a result the formula of the complex can be verified. |
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In the solid state, the salt consists of the [Cu(NH<sub>3</sub>)<sub>4</sub>H<sub>2</sub>O]<sup>2+</sup> cation, which has a square pyramidal molecular geometry. The Cu-N and Cu-O distances are about 210 and 233 pm.<ref>Morosin "The crystal structures of copper tetraammine complexes. A. Cu(NH3)4SO2.H2O and Cu(NH3)4SeO4" Acta Cryst. (1969). B25, 19-30 {{doi|10.1107/S0567740869001725}}</ref> |
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==Corrosion== |
==Corrosion== |
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The |
The characteristic deep blue colour of the tetraammine complex is found in [[brass]] and [[copper alloys]] where attack from ammonia has occurred, leading to cracking. The problem was first found in [[Cartridge (firearms)|ammunition cartridge]] cases when they were stored near [[animal waste]], which produced trace amounts of ammonia. This type of corrosion is known as [[season cracking]]. |
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==Uses== |
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[[File:Tetramminecopper sulfate.JPG|thumb|A container containing an ammonia solution of tetraamminecopper(II) sulfate]] |
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The closely related [[Schweizer's reagent]] is used for the production of [[cuprammonium rayon]]. |
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==References== |
==References== |
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<references/> |
<references/> |
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==External links== |
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*[http://www.npi.gov.au/database/substance-info/profiles/27.html National Pollutant Inventory - Copper and compounds fact sheet] |
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*[https://secure.strem.com/catalog/printer.php?type=msds&catalog_number=29-6600 Material Safety Data Sheet (MSDS)] |
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[[Category:Sulfates]] |
[[Category:Sulfates]] |
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[[Category:Ammine complexes]] |
[[Category:Ammine complexes]] |
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{{inorganic-compound-stub}} |
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[[de:Tetramminkupfersulfat]] |
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[[nl:Tetramminekoper(II)sulfaat]] |