Copper(I) sulfate

Copper(I) sulfate
Names
	Other names Copper(I) sulphate; Cuprous sulfate; Dicopper sulfate
Identifiers
CAS Number	17599-81-4;
3D model (JSmol)	Interactive image;
ChemSpider	118749;
ECHA InfoCard	100.159.746
PubChem CID	134737;
CompTox Dashboard (EPA)	DTXSID30889663 ;
	InChI InChI=1S/2Cu.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2+1;/p-2 Key: WIVXEZIMDUGYRW-UHFFFAOYSA-L; InChI=1/2Cu.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2+1;/p-2 Key: WIVXEZIMDUGYRW-NUQVWONBAI;
	SMILES [O-]S(=O)(=O)[O-].[Cu+].[Cu+];
Properties
Chemical formula	Cu2SO4
Molar mass	223.15 g mol−1
Appearance	White
Density	3.6 g cm−3
Melting point	110 °C
Solubility in water	Water-soluble
Hazards
	NIOSH (US health exposure limits):
PEL (Permissible)	TWA 1 mg/m3 (as Cu)[1]
REL (Recommended)	TWA 1 mg/m3 (as Cu)[1]
IDLH (Immediate danger)	TWA 100 mg/m3 (as Cu)[1]
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
	Infobox references

Copper(I) sulfate, also known as cuprous sulfate and dicopper sulfate, is the chemical compound with the chemical formula Cu₂ SO₄ and a molar mass of 223.15 g mol⁻¹. It is an unstable compound as copper(I) compounds are generally unstable and is more commonly found in the CuSO₄ state. It is white in color at room temperature and is water-soluble. Due to the low-stability of the compound there are currently not many applications to date.

Synthesis

Anhydrous Cu₂SO₄, can be synthesized at approximately around 75% purity by the action of dimethyl sulfate on Cu₂O following the formula:[2]

{\ce {Cu2O + (CH3O)2SO2 -> Cu2SO4 + (CH3)2O}}

The material is fairly stable in dry air at room temperature but decomposes rapidly in presence of moisture or on heating. Due to its instability the material starts to decompose when heated or if water is present to Cu SO₄ and follows the formula:[2]

{\ce {Cu2SO4 ->[{\ce {H2O}}] Cu + CuSO4}}

Around temperatures of 300 °C it is not likely for any Cu₂SO₄ to be present as the structure is just not stable enough.

It can also be prepared by reducing copper(II) sulfate solution with a reducing agent like solution sodium bisulfite or sodium thiosulfate to reduce Cu²⁺ to Cu⁺. This is visibly noticeable as the blue CuSO₄ will begin to turn colorless when the cuprous ion is formed.

Structure

Cu₂SO₄ crystallizes in the orthorhombic space group Fddd with cubic closest pack cell unit properties a = 474.8, b = 1396, and c = 1086 pm, Z = 8, Dx = 4.12 g cm⁻³. The structure is formed by the tendency of Cu(I) to form two collinear sp bonds to oxygen atoms which result in short O–Cu–O groups with the O–Cu bond length being approximately 196vpm. Due to the bonding properties of the Cu(I) metal the structure is built of layers of composition Cu₂SO_4. Due to the loss of only one electron and the bonding properties of copper(I) the structure is built up from four oxygen atoms of each sulfate group bonding to four other sulfate groups of the same layer via symmetrical O–Cu–O bridging.[3] Due to its unstable nature it is difficult to obtain an accurate 3D structure, but was first successfully done in 1987 by Berthold, Born, and Wartchow.

Applications

No current common uses due to stability issues. However, its more common copper(II) sulfate form has various current uses from production of fungicides and insecticides, growth stimulation in agriculture, soil sterilization, disinfection, preservatives, antiseptics, pharmaceuticals, disease prevention, mold protection, gas purification and coloring, textiles, public health and medicine, agriculture, and chemistry.

References

NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
Vo Van, Kim; Habashi, Faith (1972). "Identification and Thermal Stability of Copper(I) Sulfate". Can. J. Chem. 50 (23): 3872–3875. doi:10.1139/v72-610.
Berthold, H. J.; Born, J.; Wartchow, R. (1988). "The crystal structure of copper(I)sulfate Cu₂SO₄ – The first structure of a simple cuprous oxo-salt". Z. Kristallogr. Cryst. Mater. 183: 309–318. doi:10.1524/zkri.1988.183.14.309.

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[PGCH-1] NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).

[VoVan-2] Vo Van, Kim; Habashi, Faith (1972). "Identification and Thermal Stability of Copper(I) Sulfate". Can. J. Chem. 50 (23): 3872–3875. doi:10.1139/v72-610.

[ZKrist-3] Berthold, H. J.; Born, J.; Wartchow, R. (1988). "The crystal structure of copper(I)sulfate Cu₂SO₄ – The first structure of a simple cuprous oxo-salt". Z. Kristallogr. Cryst. Mater. 183: 309–318. doi:10.1524/zkri.1988.183.14.309.