| Names | |
|---|---|
| Other names Cuprous hydroxide; Copper monohydroxide | |
| Identifiers | |
3D model (JSmol) | |
| ChemSpider | |
PubChem CID | |
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| Properties | |
| CuOH | |
| Molar mass | 80.55 g/mol |
| 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). | |
Copper(I) hydroxide is the hydroxide of the metal copper with the chemical formula of CuOH. It is a mild, highly unstable alkali. The color of pure CuOH is yellow or orange-yellow, [2] but it usually appears rather dark red because of impurities. It is extremely easily oxidized even at room temperature. It is useful for some industrial processes and in preventing condensation of formaldehyde. It is also an important reactant and intermediate for several important products including Cu2O3 [3] and Cu(OH)2. Additionally, it can act as a catalyst in the synthesis pyrimidopyrrolidone derivatives. [4]
The dissociation of Cu(OH)2− leads to the formation of CuOH.
The dissociation energy required for this reaction is 62 ± 3 kcal/mol. [3]
Another method is by the double displacement of CuCl and NaOH:
Notably, this method is rarely used because the CuOH produced will gradually dehydrate and eventually turn into Cu2O.
CuOH can be a linear molecule of the symmetry group C∞v. For the linear structure, the bond distance of the Cu-O bond has been found to be 1.788 Å and the distance of the O-H bond has been found to be 0.952 Å. The CuOH bond angle was measured as 180°. [3]
There is also the possibility of a formed CuOH with the point group Cs. This has been found to have increased stability compared to the linear geometry. In this case, the bond distance of the Cu-O bond was 1.818 Å and the bond distance of the O-H bond was 0.960 Å. The bond angle for this geometry was 131.9°. The compound is highly ionic in character, which is why this angle is not exactly 120°. [3]
CuOH has been characterized spectroscopically using intracavity laser spectroscopy, [5] single vibronic level emission, [6] and microwave spectroscopic detection. [7]
Similar to iron(II) hydroxide , copper(I) hydroxide can easily oxidise into copper(II) hydroxide:
Cu(OH)2 is used as a fungicide for agriculture, as a mordant, as a source for copper salts, and for the manufacturing of rayon. [8]
CuOH can act as a catalyst. It has been found to be useful in the reaction of heterocyclic ketene aminals (an important building block) with diazoesters. This reaction is used to synthesize pyrimidopyrrolidone derivatives with high yields and mild reaction conditions needed. [4] As a catalyst in these reactions, it is used with potassium tert-butoxide and argon with tert-butyl hydroperoxide and dichloroethane. 25 examples of these reactions were successfully performed. [4] Chemicals in the pyrrolidone family have been useful for drug development, including pharmaceuticals for the neuroprotection after strokes and in anti-seizure medications. Although these are psychoactive drugs, they tend to have fewer side effects than their counterparts. The mechanisms by which these drugs work have yet to be established. [9]
CuOH is an important intermediate in the formation of copper(I) oxide (Cu2O). [3] The Cu2O compound has versatile applications such as for use in solar cells, [10] for the oxidation of fiberglass, [11] and for use in lithium ion batteries. [12] It has even been shown to have a useful application in the development of DNA biosensors for the hepatitis B virus. [13] Notably, it has been found that both CuOH and Cu(OH)2 must be simultaneously present for the synthesis of Cu2O. [3]
Cu+ and Cu2+ are the most common oxidation states of copper although Cu3+ and Cu4+ have also been reported. Cu2+ tends to form stable compounds whereas Cu+ usually forms unstable compounds such as CuOH. One exception to this is Cu2O, which is much more stable. However, aside from this compound, compounds containing Cu+ have not been studied as extensively as Cu2+ compounds due to their relative instability. This includes CuOH. [14]
Hydroxide is a diatomic anion with chemical formula OH−. It consists of an oxygen and hydrogen atom held together by a single covalent bond, and carries a negative electric charge. It is an important but usually minor constituent of water. It functions as a base, a ligand, a nucleophile, and a catalyst. The hydroxide ion forms salts, some of which dissociate in aqueous solution, liberating solvated hydroxide ions. Sodium hydroxide is a multi-million-ton per annum commodity chemical. The corresponding electrically neutral compound HO• is the hydroxyl radical. The corresponding covalently bound group –OH of atoms is the hydroxy group. Both the hydroxide ion and hydroxy group are nucleophiles and can act as catalysts in organic chemistry.
Inorganic chemistry deals with synthesis and behavior of inorganic and organometallic compounds. This field covers chemical compounds that are not carbon-based, which are the subjects of organic chemistry. The distinction between the two disciplines is far from absolute, as there is much overlap in the subdiscipline of organometallic chemistry. It has applications in every aspect of the chemical industry, including catalysis, materials science, pigments, surfactants, coatings, medications, fuels, and agriculture.
Iron(III) chloride describes the inorganic compounds with the formula FeCl3(H2O)x. Also called ferric chloride, these compounds are available both in anhydrous and hydrated forms which are both hygroscopic. They are common sources of iron in its +3 oxidation state. The anhydrous derivative is a Lewis acid, while the hydrate is a mild oxidizing agent. It is used as a water cleaner and as an etchant for metals.
Copper(II) nitrate describes any member of the family of inorganic compounds with the formula Cu(NO3)2(H2O)x. The hydrates are blue solids. Anhydrous copper nitrate forms blue-green crystals and sublimes in a vacuum at 150-200 °C. Common hydrates are the hemipentahydrate and trihydrate.
Cyclopropene is an organic compound with the formula C3H4. It is the simplest cycloalkene. Because the ring is highly strained, cyclopropene is difficult to prepare and highly reactive. This colorless gas has been the subject for many fundamental studies of bonding and reactivity. It does not occur naturally, but derivatives are known in some fatty acids. Derivatives of cyclopropene are used commercially to control ripening of some fruit.
Cuprate loosely refers to a material that can be viewed as containing anionic copper complexes. Examples include tetrachloridocuprate ([CuCl4]2−), the superconductor YBa2Cu3O7, and the organocuprates (e.g., dimethylcuprate [Cu(CH3)2]−). The term cuprates derives from the Latin word for copper, cuprum. The term is mainly used in three contexts: oxide materials, anionic coordination complexes, and anionic organocopper compounds.
Lead(II) chloride (PbCl2) is an inorganic compound which is a white solid under ambient conditions. It is poorly soluble in water. Lead(II) chloride is one of the most important lead-based reagents. It also occurs naturally in the form of the mineral cotunnite.
Copper(I) chloride, commonly called cuprous chloride, is the lower chloride of copper, with the formula CuCl. The substance is a white solid sparingly soluble in water, but very soluble in concentrated hydrochloric acid. Impure samples appear green due to the presence of copper(II) chloride (CuCl2).
Copper(II) chloride, also known as cupric chloride, is an inorganic compound with the chemical formula CuCl2. The monoclinic yellowish-brown anhydrous form slowly absorbs moisture to form the orthorhombic blue-green dihydrate CuCl2·2H2O, with two water molecules of hydration. It is industrially produced for use as a co-catalyst in the Wacker process.
Organotin chemistry is the scientific study of the synthesis and properties of organotin compounds or stannanes, which are organometallic compounds containing tin carbon bonds. The first organotin compound was diethyltin diiodide, discovered by Edward Frankland in 1849. The area grew rapidly in the 1900s, especially after the discovery of the Grignard reagents, which are useful for producing Sn–C bonds. The area remains rich with many applications in industry and continuing activity in the research laboratory.
Diazonium compounds or diazonium salts are a group of organic compounds sharing a common functional group [R−N+≡N]X− where R can be any organic group, such as an alkyl or an aryl, and X is an inorganic or organic anion, such as a halide.
A salt metathesis reaction, sometimes called a double displacement reaction, is a chemical process involving the exchange of bonds between two reacting chemical species which results in the creation of products with similar or identical bonding affiliations. This reaction is represented by the general scheme:
Copper(II) hydroxide is the hydroxide of copper with the chemical formula of Cu(OH)2. It is a pale greenish blue or bluish green solid. Some forms of copper(II) hydroxide are sold as "stabilized" copper(II) hydroxide, although they likely consist of a mixture of copper(II) carbonate and hydroxide. Cupric hydroxide is a strong base, although its low solubility in water makes this hard to observe directly.
Copper(II) acetate, also referred to as cupric acetate, is the chemical compound with the formula Cu(OAc)2 where AcO− is acetate (CH
3CO−
2). The hydrated derivative, Cu2(OAc)4(H2O)2, which contains one molecule of water for each copper atom, is available commercially. Anhydrous copper(II) acetate is a dark green crystalline solid, whereas Cu2(OAc)4(H2O)2 is more bluish-green. Since ancient times, copper acetates of some form have been used as fungicides and green pigments. Today, copper acetates are used as reagents for the synthesis of various inorganic and organic compounds. Copper acetate, like all copper compounds, emits a blue-green glow in a flame.
Organosilicon chemistry is the study of organometallic compounds containing carbon–silicon bonds, to which they are called organosilicon compounds. Most organosilicon compounds are similar to the ordinary organic compounds, being colourless, flammable, hydrophobic, and stable to air. Silicon carbide is an inorganic compound.
A boronic acid is an organic compound related to boric acid in which one of the three hydroxyl groups is replaced by an alkyl or aryl group. As a compound containing a carbon–boron bond, members of this class thus belong to the larger class of organoboranes.
Organosilver chemistry is the study of organometallic compounds containing a carbon to silver chemical bond. The theme is less developed than organocopper chemistry.
Dicopper chloride trihydroxide is the chemical compound with the formula Cu2(OH)3Cl. It is often referred to as tribasic copper chloride (TBCC), copper trihydroxyl chloride or copper hydroxychloride. It is a greenish crystalline solid encountered in mineral deposits, metal corrosion products, industrial products, art and archeological objects, and some living systems. It was originally manufactured on an industrial scale as a precipitated material used as either a chemical intermediate or a fungicide. Since 1994, a purified, crystallized product has been produced at the scale of thousands of tons per year, and used extensively as a nutritional supplement for animals.
The Chan–Lam coupling reaction – also known as the Chan–Evans–Lam coupling is a cross-coupling reaction between an aryl boronic acid and an alcohol or an amine to form the corresponding secondary aryl amines or aryl ethers, respectively. The Chan–Lam coupling is catalyzed by copper complexes. It can be conducted in air at room temperature. The more popular Buchwald–Hartwig coupling relies on the use of palladium.
Transition metal dithiocarbamate complexes are coordination complexes containing one or more dithiocarbamate ligand, which are typically abbreviated R2dtc−. Many complexes are known. Several homoleptic derivatives have the formula M(R2dtc)n where n = 2 and 3.
