Preparation of copper(i) chloride lab report

(III). The relative stabilities of each oxidation state depend on the nature of ligands and anions as

well as the nature of the solvent medium. In this experiment, the copper(I) ions once formed, react

with chloride ions to form the insoluble copper(I) chloride.

Glacial acetic acid is a dangerous liquid and must be used in a fume cupboard.

➢ EXPLANATION OF ANY INSTRUMENTAL TECHNIQUE BEING USED IN

Based on the introduction, the overall balanced chemical equation is given. Copper begins

to have a +2 charge in the compound copper (II) chloride dihydrate, then it reacts with HCl to form

tetrachlorocuprate (II) ion. The metallic copper metal then is pulled an electron from the solution

to form a complex of copper wherein its charge is +1. By then, copper (I) chloride is already

The deionized water is added slowly with continuous stirring in the process, then HCl to

the copper(II) chloride solution. Dilute the suspension of copper(I) chloride so formed with about

half the sulfurous acid solution, allow the precipitate to settle, and decant most of the supernatant

Copper(I) chloride (quite commonly called cuprous chloride), is the lower chloride of copper, with the formula CuCl. It occurs naturally as the mineral nantokite. It is a white solid which is almost insoluble in water, and which tends to oxidise in air to green CuCl2. It is a Lewis acid which reacts with suitable ligands such as ammonia or chloride ion to form complexes, many of which are water-soluble. It is even able to form a stable complex with carbon monoxide.

In aqueous solution, CuCl would be unstable with respect to disproportionation into Cu and CuCl2, but its low solubility allows it to be a stable compound.

Chemical Properties

Copper(I) chloride is a Lewis acid, classified as soft according to the Hard-Soft Acid-Base concept. Thus it tends to form stable complexes with soft Lewis bases such as triphenylphosphine:

CuCl + PPh3 → [CuCl(PPh3)]4 (Ph = phenyl)

Although CuCl is insoluble in water, it dissolves in aqueous solutions containing suitable donor molecules. It readily forms complexes with halide ions, for example forming H3O+ CuCl2- with concentrated hydrochloric acid. It also dissolves readily in solutions containing CN-, S2O32- or NH3

Solutions of CuCl in HCl or NH3 absorb carbon monoxide to form colourless complexes such as the crystalline halogen-bridged dimer [CuCl(CO)]2. The same HCl solution can also react with acetylene gas to form [CuCl(C2H2)], while an NH3 solution of CuCl forms an explosive acetylide with acetylene. Complexes of CuCl with alkenes can be made by reduction of CuCl2 by sulfur dioxide in the presence of the alkene in alcohol solution. Complexes with chelating alkenes such as 1,5-cyclooctadiene are particularly stable:

CuCl reacts with organometallic compounds such as methyllithium (CH3Li) to form "Gilman reagents" such as (CH3)2CuLi, which find extensive use in organic synthesis. Grignard reagents react similarly.

Preparation

Copper(I) chloride may be prepared by the reduction of copper(II) salts such as CuSO4 using sulfur dioxide or copper metal. SO2 may be prepared in situ from sodium bisulfite (NaHSO3) or sodium metabisulfite (Na2S2O5) and acid. The reduction is carried out in hydrochloric acid, and the resulting CuCl2- complex is diluted to precipitate white CuCl (by driving the equilibrium using Le Chatelier's principle).

(1) NaHSO3( aq) + HCl ( aq) → SO2( aq) + NaCl + H2O( l)

(2) 2 CuSO4( aq) + SO2( aq) + 2 H2O( l) + 4 HCl( aq) → 2 HCuCl2( aq) + 3 H2SO4( aq)

(3) HCuCl2( aq) + H2O( l) → CuCl( s) + H3O+( aq) + Cl-( aq)

Uses

A major chemical use for copper(I) chloride is as a catalyst for a variety of organic reactions. Compared to other "soft" Lewis acids, it is much more affordable than non-toxic silver(I) chloride and palladium(II) chloride, and much less toxic than lead(II) chloride and mercury(II) chloride. In addition, it can undergo redox chemistry via copper(II) or copper(III) intermediates. This combination of properties make copper(I) salts invaluable reagents.

One such application is in the Sandmeyer reaction. Treatment of an arenediazonium salt with CuCl leads to an aryl chloride, for example:

The reaction has wide scope, and usually gives good yields.

The observation that copper(I) halides catalyse 1,4-addition of Grignard reagents to alpha,beta-unsaturated ketones led to the development of organocuprate reagents that are widely used today in organic synthesis :

Although other copper(I) compounds such as copper(I) iodide are now more often used for this type of reaction, there are cases where copper(I) chloride is particularly effective:

Here, Bu indicates an n- butyl group. Without CuCl, the Grignard reagent alone gives a mixture of 1,2 and 1,4-addition products (i.e., the butyl adds at the closer to the C=O).

Copper(I) chloride is also an intermediate formed from copper(II) chloride in the Wacker process.

Precautions

Copper salts do have some toxicity and should be handled with care; wear gloves and goggles. Avoid bringing CuCl into contact with alkynes.

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