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	4.12 g cm−3[1]
Melting point	110 °C
Solubility in water	decomposes
Structure[1]
Crystal structure	orthorhombic
Space group	Fddd
Lattice constant	a = 4.748(3) Å, b = 13.96(1) Å, c = 10.86(1) Å
Formula units (Z)	8
Hazards
	NIOSH (US health exposure limits):
PEL (Permissible)	TWA 1 mg/m3 (as Cu)[2]
REL (Recommended)	TWA 1 mg/m3 (as Cu)[2]
IDLH (Immediate danger)	TWA 100 mg/m3 (as Cu)[2]
	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, is the inorganic compound with the chemical formula Cu₂ SO₄. It is a white solid that has attracted little attention, in contrast to copper(II) sulfate. It is an unusual example of a copper(I) compound derived from an oxyanion, illustrated also by the non- or fleeting existence of cuprous nitrate and cuprous perchlorate.[1]

Structure

Cu₂SO₄ crystallizes in the orthorhombic space group Fddd. Each oxygen in a sulfate anion is bridged to another sulfate by a copper atom, and the Cu-O distances are 196 pm. The structure is intermediate between silver sulfate and solid sulfuric acid.[1]

Synthesis

Cuprous sulfate is produced by the reaction of copper metal with sulfuric acid at 200 °C:[3]

{\ce {2Cu + 2 H2SO4 -> Cu2SO4 + SO2 + 2 H2O}}

The small amount of water produced in this reaction is absorbed by the sulfuric acid.

Cu₂SO₄ can also be synthesized by the action of dimethyl sulfate on cuprous oxide:[4]

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

The material is stable in dry air at room temperature but decomposes rapidly in presence of moisture or on heating. It disproportionates upon contact with water:[4]

{\ce {Cu2SO4 + 4 H2O -> Cu + [Cu(H2O)4]SO4}}

It can also be produced by the reaction of copper(II) sulfate and a reducing agent such as sodium thiosulfate.

Structure

Cu₂SO₄ crystallizes in the orthorhombic space group. The Cu-O distances are 196 pm.

References

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. S2CID 101673081.
NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
O. Glemser; R. Sauer (1963). "Copper (I) Sulfate". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2pages=1020. NY,NY: Academic Press.
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.

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[ZKrist-1] 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. S2CID 101673081.

[PGCH-2] NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).

[3] O. Glemser; R. Sauer (1963). "Copper (I) Sulfate". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2pages=1020. NY,NY: Academic Press.

[VoVan-4] 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.