Difference between revisions of "Copper(II) chloride"
From Sciencemadness Wiki
| Line 1: | Line 1: | ||
| − | + | {{Chembox | |
| − | '''Copper(II) chloride''', also known as '''cupric chloride''', is an ionic compound of [[copper]] and [[chlorine]] with the formula CuCl<sub>2</sub>. It is a brown solid when anhydrous, but turns a brilliant turquoise color when hydrated. | + | | Name = Copper(II) chloride |
| + | | Reference = | ||
| + | | IUPACName = Copper(II) chloride | ||
| + | | PIN = | ||
| + | | SystematicName = | ||
| + | | OtherNames = Copper dichloride<br>Cupric chloride<br>Cupric dichloride | ||
| + | <!-- Images --> | ||
| + | | ImageFile = | ||
| + | | ImageSize = | ||
| + | | ImageAlt = | ||
| + | | ImageName = | ||
| + | | ImageFile1 = Copper(II) chloride anhydrous by Zyklon-A.png | ||
| + | | ImageSize1 = 270 | ||
| + | | ImageAlt1 = | ||
| + | | ImageName1 = | ||
| + | | ImageCaption1 = Anhydrous copper (II) chloride | ||
| + | | ImageFile2 = CuCl2 Dihydrate.jpg | ||
| + | | ImageSize2 = 270 | ||
| + | | ImageAlt2 = | ||
| + | | ImageName2 = | ||
| + | | ImageCaption2 = Pieces of copper(II) chloride dihydrate | ||
| + | | ImageFile3 = | ||
| + | | ImageSize3 = | ||
| + | | ImageAlt3 = | ||
| + | | ImageName3 = | ||
| + | | ImageFileL1 = | ||
| + | | ImageSizeL1 = | ||
| + | | ImageAltL1 = | ||
| + | | ImageNameL1 = | ||
| + | | ImageFileR1 = | ||
| + | | ImageSizeR1 = | ||
| + | | ImageAltR1 = | ||
| + | | ImageNameR1 = | ||
| + | | ImageFileL2 = | ||
| + | | ImageSizeL2 = | ||
| + | | ImageAltL2 = | ||
| + | | ImageNameL2 = | ||
| + | | ImageFileR2 = | ||
| + | | ImageSizeR2 = | ||
| + | | ImageAltR2 = | ||
| + | | ImageNameR2 = | ||
| + | <!-- Sections --> | ||
| + | | Section1 = {{Chembox Identifiers | ||
| + | | 3DMet = | ||
| + | | Abbreviations = | ||
| + | | SMILES = | ||
| + | }} | ||
| + | | Section2 = {{Chembox Properties | ||
| + | | AtmosphericOHRateConstant = | ||
| + | | Appearance = Brown solid (anhydrous)<br>Blue-green solid (dihydrate) | ||
| + | | BoilingPt = | ||
| + | | BoilingPtC = 993 | ||
| + | | BoilingPt_ref = | ||
| + | | BoilingPt_notes = (anhydrous, decomposes) | ||
| + | | Density = 3.386 g/cm<sup>3</sup> (anhydrous)<br>2.51 g/cm<sup>3</sup> (dihydrate) | ||
| + | | Formula = CuCl<sub>2</sub> (anhydrous)<br>CuCl<sub>2</sub>·2H<sub>2</sub>O (dihydrate) | ||
| + | | HenryConstant = | ||
| + | | LogP = | ||
| + | | MolarMass = 134.45 g/mol (anhydrous)<br>170.48 g/mol (dihydrate) | ||
| + | | MeltingPt = | ||
| + | | MeltingPtC = | ||
| + | | MeltingPt_ref = | ||
| + | | MeltingPt_notes = ''anhydrous''<br>498 °C (928 °F; 771 K)<hr>''dihydrate''<br>100 °C (212 °F; 373 K) (dehydrates) | ||
| + | | Odor = Odorless | ||
| + | | pKa = | ||
| + | | pKb = | ||
| + | | Solubility = 70.6 g/100 mL (0 °C)<br>75.7 g/100 mL (25 °C)<br>107.9 g/100 mL (100 °C) | ||
| + | | SolubleOther = Soluble in [[acetone]] | ||
| + | | Solubility1 = 53 g/100 mL (15 °C) | ||
| + | | Solvent1 = ethanol | ||
| + | | Solubility2 = 68 g/100 mL (15 °C) | ||
| + | | Solvent2 = methanol | ||
| + | | VaporPressure = | ||
| + | }} | ||
| + | | Section3 = {{Chembox Structure | ||
| + | | Coordination = Octahedral | ||
| + | | CrystalStruct = distorted CdI<sub>2</sub> structure | ||
| + | | MolShape = | ||
| + | }} | ||
| + | | Section4 = {{Chembox Thermochemistry | ||
| + | | DeltaGf = | ||
| + | | DeltaHc = | ||
| + | | DeltaHf = | ||
| + | | Entropy = | ||
| + | | HeatCapacity = | ||
| + | }} | ||
| + | | Section5 = {{Chembox Explosive | ||
| + | | ShockSens = | ||
| + | | FrictionSens = | ||
| + | | DetonationV = | ||
| + | | REFactor = | ||
| + | }} | ||
| + | | Section6 = {{Chembox Hazards | ||
| + | | AutoignitionPt = | ||
| + | | ExploLimits = | ||
| + | | ExternalMSDS = [https://www.docdroid.net/6jd0ecm/copperii-chloride-sa.pdf.html Sigma-Aldrich] (anhydrous)<br>[https://www.docdroid.net/v9jTMCL/copperii-chloride-dihydrate-sa.pdf.html Sigma-Aldrich] (dihydrate) | ||
| + | | FlashPt = Non-flammable | ||
| + | | LD50 = | ||
| + | | LC50 = | ||
| + | | MainHazards = Irritant<br>Corrosive | ||
| + | | NFPA-F = | ||
| + | | NFPA-H = | ||
| + | | NFPA-R = | ||
| + | | NFPA-S = | ||
| + | }} | ||
| + | | Section7 = {{Chembox Related | ||
| + | | OtherAnions = | ||
| + | | OtherCations = | ||
| + | | OtherFunction = | ||
| + | | OtherFunction_label = | ||
| + | | OtherCompounds = [[Copper(I) chloride]] | ||
| + | }} | ||
| + | }} | ||
| + | '''Copper(II) chloride''', also known as '''cupric chloride''', is an ionic compound of [[copper]] and [[chlorine]] with the formula '''CuCl<sub>2</sub>'''. It is a brown solid when anhydrous, but turns a brilliant turquoise color when hydrated. | ||
==Properties== | ==Properties== | ||
===Physical properties=== | ===Physical properties=== | ||
| − | Copper(II) chloride is a brown powder that turns red when molten. Its melting point is 498 °C. | + | [[File:Copper(II)_chloride_crystals_by No Tears Only Dreams Now.jpg|thumb|250px|Still-wet CuCl<sub>2</sub> crystals grown on the inside of a beaker.]] |
| + | Copper(II) chloride is a brown powder that turns red when molten. Its melting point is 498 °C. Copper(II) chloride is hygroscopic and absorbs water in open air to form the dihydrate, which is a neutral tetracoordinate [[Coordination complex|complex]]. The material normally exists as a brilliant turquoise powder, but thin, transparent, fragile crystals may be grown. In the presense of excess chloride ions, it will form a greener colored acidic copper(II) chloride, in which the water ligands are substituted for [[chloride]] ions. [[Tetrachlorocupric acid]] is formed. | ||
===Chemical properties=== | ===Chemical properties=== | ||
Copper(II) chloride can oxidize and dissolve [[aluminium]], owing to the formation of the [[tetrachlorocuprate]] ion. Besides this, it is a moderate oxidizer and will also dissolve other reactive metals such as [[zinc]] and [[magnesium]]. It is also useful in organic synthesis because it can chlorinate the alpha position of [[Carbonyl|carbonyls]]. In the presence of oxygen, it can also oxidize [[phenols]]. | Copper(II) chloride can oxidize and dissolve [[aluminium]], owing to the formation of the [[tetrachlorocuprate]] ion. Besides this, it is a moderate oxidizer and will also dissolve other reactive metals such as [[zinc]] and [[magnesium]]. It is also useful in organic synthesis because it can chlorinate the alpha position of [[Carbonyl|carbonyls]]. In the presence of oxygen, it can also oxidize [[phenols]]. | ||
| + | |||
| + | Copper(II) chloride burns at low temperature with a deep blue flame (or green, depending on impurities). If the flame temperature is too high, it breaks down and gives a more greenish flame color. For this reason, it cannot be used in fireworks to obtain blue flame. | ||
==Availability== | ==Availability== | ||
| − | Copper chloride can be purchased from chemical suppliers. [http://www.sciencecompany.com/Cupric-Chloride-100g-P6404.aspx ScienceCompany] sells 100 g of copper(II) chloride dihydrate at 11.95$. | + | Copper chloride can be purchased from chemical suppliers or online from eBay and Amazon. [http://www.sciencecompany.com/Cupric-Chloride-100g-P6404.aspx ScienceCompany] sells 100 g of copper(II) chloride dihydrate at 11.95$. |
==Preparation== | ==Preparation== | ||
| − | Copper(II) chloride can be produced by adding copper metal to a mixture of [[hydrochloric acid]] and [[hydrogen peroxide]]. Copper is resistant to attack by pure hydrochloric acid and other non-oxidizing acids, so an [[oxidizer]] must be added to promote dissolution (in this case, hydrogen peroxide). | + | Copper(II) chloride can be produced by adding copper metal to a mixture of [[hydrochloric acid]] and [[hydrogen peroxide]]. Copper is resistant to attack by pure hydrochloric acid and other non-oxidizing acids, so an [[oxidizer]] must be added to promote dissolution (in this case, hydrogen peroxide). [[Copper(II) oxide]] or hydroxide can be used instead of copper metal. |
| + | |||
| + | Totally anhydrous copper(II) chloride can be made by passing dry [[chlorine]] gas over hot [[copper]] metal. | ||
==Projects== | ==Projects== | ||
| + | *Make [[copper(I) chloride]] | ||
*Make the [[trichlorocuprate]] ion | *Make the [[trichlorocuprate]] ion | ||
| − | *Make blue fire | + | *Make blue-green fire |
| + | *Moisture indicator | ||
==Handling== | ==Handling== | ||
===Safety=== | ===Safety=== | ||
| − | Copper(II) chloride is toxic and corrosive, so protection should be worn when handling the compound. | + | Copper(II) chloride is toxic and corrosive, so proper protection, such as gloves should be worn when handling the compound. |
===Storage=== | ===Storage=== | ||
| − | Copper(II) chloride should be stored in closed containers, to keep it dry. The anhydrous form should be kept in sealed containers. | + | Copper(II) chloride should be stored in closed containers, to keep it dry. The anhydrous form should be kept in sealed containers or in a desiccator. |
===Disposal=== | ===Disposal=== | ||
| − | Copper(II) chloride must be reduced with another metal, such as iron to form iron(II) chloride | + | Copper(II) chloride must be reduced to copper metal with with another more reactive metal, such as [[iron]] or [[zinc]] to form [[iron(II) chloride]] or [[zinc chloride]] which are less toxic, before being disposed of. |
==References== | ==References== | ||
| Line 33: | Line 153: | ||
===Relevant Sciencemadness threads=== | ===Relevant Sciencemadness threads=== | ||
*[http://www.sciencemadness.org/talk/viewthread.php?tid=18710 copper II chloride crystals] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=18710 copper II chloride crystals] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=24784 Making copper chloride] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=15485 copper II chloride anhydrous] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=27395 Making Copper Chloride] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=35340 Copper (II) chloride - green flame for fireworks] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=65762 Tried to make Copper Chloride, help.] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=23838 CuCl2 from copper sulfate ?] | ||
[[Category:Chemical compounds]] | [[Category:Chemical compounds]] | ||
| Line 41: | Line 167: | ||
[[Category:Halides]] | [[Category:Halides]] | ||
[[Category:Chemicals for crystal growing]] | [[Category:Chemicals for crystal growing]] | ||
| + | [[Category:Easily prepared chemicals]] | ||
Revision as of 16:31, 21 December 2016
_chloride_anhydrous_by_Zyklon-A.png) Anhydrous copper (II) chloride
| |
 Pieces of copper(II) chloride dihydrate
| |
| Names | |
|---|---|
| IUPAC name
Copper(II) chloride
| |
| Other names
Copper dichloride
Cupric chloride Cupric dichloride | |
| Properties | |
| CuCl2 (anhydrous) CuCl2·2H2O (dihydrate) | |
| Molar mass | 134.45 g/mol (anhydrous) 170.48 g/mol (dihydrate) |
| Appearance | Brown solid (anhydrous) Blue-green solid (dihydrate) |
| Odor | Odorless |
| Density | 3.386 g/cm3 (anhydrous) 2.51 g/cm3 (dihydrate) |
| Melting point | anhydrous 498 °C (928 °F; 771 K) dihydrate 100 °C (212 °F; 373 K) (dehydrates) |
| Boiling point | 993 °C (1,819 °F; 1,266 K) (anhydrous, decomposes) |
| 70.6 g/100 mL (0 °C) 75.7 g/100 mL (25 °C) 107.9 g/100 mL (100 °C) | |
| Solubility | Soluble in acetone |
| Solubility in ethanol | 53 g/100 mL (15 °C) |
| Solubility in methanol | 68 g/100 mL (15 °C) |
| Hazards | |
| Safety data sheet | Sigma-Aldrich (anhydrous) Sigma-Aldrich (dihydrate) |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Copper(I) chloride |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Copper(II) chloride, also known as cupric chloride, is an ionic compound of copper and chlorine with the formula CuCl2. It is a brown solid when anhydrous, but turns a brilliant turquoise color when hydrated.
Contents
Properties
Physical properties
_chloride_crystals_by_No_Tears_Only_Dreams_Now.jpg)
Copper(II) chloride is a brown powder that turns red when molten. Its melting point is 498 °C. Copper(II) chloride is hygroscopic and absorbs water in open air to form the dihydrate, which is a neutral tetracoordinate complex. The material normally exists as a brilliant turquoise powder, but thin, transparent, fragile crystals may be grown. In the presense of excess chloride ions, it will form a greener colored acidic copper(II) chloride, in which the water ligands are substituted for chloride ions. Tetrachlorocupric acid is formed.
Chemical properties
Copper(II) chloride can oxidize and dissolve aluminium, owing to the formation of the tetrachlorocuprate ion. Besides this, it is a moderate oxidizer and will also dissolve other reactive metals such as zinc and magnesium. It is also useful in organic synthesis because it can chlorinate the alpha position of carbonyls. In the presence of oxygen, it can also oxidize phenols.
Copper(II) chloride burns at low temperature with a deep blue flame (or green, depending on impurities). If the flame temperature is too high, it breaks down and gives a more greenish flame color. For this reason, it cannot be used in fireworks to obtain blue flame.
Availability
Copper chloride can be purchased from chemical suppliers or online from eBay and Amazon. ScienceCompany sells 100 g of copper(II) chloride dihydrate at 11.95$.
Preparation
Copper(II) chloride can be produced by adding copper metal to a mixture of hydrochloric acid and hydrogen peroxide. Copper is resistant to attack by pure hydrochloric acid and other non-oxidizing acids, so an oxidizer must be added to promote dissolution (in this case, hydrogen peroxide). Copper(II) oxide or hydroxide can be used instead of copper metal.
Totally anhydrous copper(II) chloride can be made by passing dry chlorine gas over hot copper metal.
Projects
- Make copper(I) chloride
- Make the trichlorocuprate ion
- Make blue-green fire
- Moisture indicator
Handling
Safety
Copper(II) chloride is toxic and corrosive, so proper protection, such as gloves should be worn when handling the compound.
Storage
Copper(II) chloride should be stored in closed containers, to keep it dry. The anhydrous form should be kept in sealed containers or in a desiccator.
Disposal
Copper(II) chloride must be reduced to copper metal with with another more reactive metal, such as iron or zinc to form iron(II) chloride or zinc chloride which are less toxic, before being disposed of.
