Copper and its compounds are on the Community Right-To-Know List. Reported in EPA TSCA Inventory.

ACGIH TLV: TWA (fume) 0.2 mg/m³; (dust, mist) 1 mg(Cu)/m³
DOT Classification:  8; Label: Corrosive

Cupric chloride anhydrous, with the CAS register number 7447-39-4, is also called as Copper dichloride. The substance is a yellow-brown solid with the chemical formula CuCl₂. Its EINECS register number is 231-210-2. Cupric chloride anhydrous is stable, but reacts violently with potassium and sodium. If contacts with acetylene may form explosive acetylides. Hygroscopic. This is a light brown solid, which slowly absorbs moisture to form a blue-green dihydrate.

Properties: Cupric chloride anhydrous reacts with hydrochloric acid or other chloride sources to form complex ions: the red CuCl₃^-, and the yellow CuCl₄^2-. Using sulfur dioxide as the reductant, copper(II) chloride can be reduced into copper(I) derivatives.

2 CuCl₂ + SO₂ + 2 H₂O → 2 CuCl + 2 HCl + H₂SO₄

Cupric chloride anhydrous will decompose to CuCl and Cl₂ at 1000 °C:

2 CuCl₂ → 2 CuCl + Cl₂

Cupric chloride anhydrous also can form a variety of coordination complexes with ligands such as pyridine and triphenylphosphine oxide:

CuCl₂ + 2 C₅H₅N → [CuCl₂(C₅H₅N)₂] (tetragonal)
CuCl₂ + 2 (C₆H₅)₃P=O → [CuCl₂((C₆H₅)₃P=O)₂] (tetrahedral)

Preparation: Cupric chloride anhydrous may be prepared directly by union of the elements, copper and chlorine. It can also be generated by treatment of the hydroxide, oxide, or copper(II) carbonate with hydrochloric acid. In addition, Cupric chloride anhydrous is prepared commercially by the action of chlorination of copper:

Cu + Cl₂ + 2 H₂O → CuCl₂(H₂O)₂

Uses: Cupric chloride anhydrous can be used as catalyst, antifungal and astringent drug, and feed additive. A major industrial application for Cupric chloride is as a co-catalyst with palladium(II) chloride in the Wacker process. In this process, ethene (ethylene) is converted to ethanal using water and air. During the reaction, PdCl₂ is reduced to Pd, and the CuCl₂ serves to re-oxidize this back to PdCl₂. Air can then oxidize the resultant CuCl back to CuCl₂, completing the cycle.

C₂H₄ + PdCl₂ + H₂O → CH₃CHO + Pd + 2 HCl
Pd + 2 CuCl₂ → 2 CuCl + PdCl₂
4 CuCl + 4 HCl + O₂ → 4 CuCl₂ + 2 H₂O

Cupric chloride anhydrous has a variety of specialized applications in the synthesis of organic compounds. It catalyzes the chlorination in the production of vinyl chloride and dichloroethane. Cupric chloride is also used in pyrotechnics as a blue/green coloring agent. In a flame test, Cupric chloride, like all copper compounds, emit green-blue. Cupric chloride can also oxidize phenols in the presence of oxygen.

When you are using Cupric chloride anhydrous, you should be very cautious about it. The substance is toxic if swallowed and dangerous for the environment. In addition, it is irritating to eyes, respiratory system and skin. Cupric chloride anhydrous is very toxic to aquatic organisms which may cause long-term adverse effects in the aquatic environment. In case of contact with eyes, you can rinse immediately with plenty of water and seek medical advice. Whenever you will use or contact it, you need wear suitable gloves and eye/face protection. In case of accident or if you feel unwell seek medical advice immediately.

You can still convert the following datas into molecular structure:
(1)Canonical SMILES: Cl[Cu]Cl
(2)InChI: InChI=1S/2ClH.Cu/h2*1H;/q;;+2/p-2
(3)InChIKey: ORTQZVOHEJQUHG-UHFFFAOYSA-L

Toxicity of Cupric chloride anhydrous: