Germanium chloride

Base Information

• Chemical Name: Germanium chloride
• CAS No.: 10038-98-9
• Molecular Formula: Cl4Ge
• Molecular Weight: 214.402
• Hs Code.: 2827 39 85
• European Community (EC) Number: 233-116-7
• NSC Number: 132053
• UNII: YSV1R803C0
• DSSTox Substance ID: DTXSID1044350
• Nikkaji Number: J95.193E
• Wikipedia: Germanium tetrachloride,Germanium(IV) chloride,Germanium_tetrachloride
• Mol file: 10038-98-9.mol

Synonyms:Germaniumchloride (GeCl4) (6CI,7CI,8CI);Germanium chloride;Germanium(IV) chloride;NSC 132053;Tetrachlorogermane;

Chemical Property of Germanium chloride

Chemical Property:

• Appearance/Colour: Colorless transparent oily liquid
• Vapor Pressure: 76 mm Hg ( 20 °C)
• Melting Point: -49.5 °C
• Refractive Index: 1.4644
• Boiling Point: 83 °C(lit.)
• Flash Point: 83.1°C
• PSA: 0.00000
• Density: 1.844 g/mL at 25 °C
• LogP: 2.37720
• Storage Temp.: Store below +30°C.
• Sensitive.: Moisture Sensitive
• Solubility.: Soluble in ether, benzene, chloroform, carbon tetrachloride. Ins
• Water Solubility.: DECOMPOSES
• Hydrogen Bond Donor Count: 0
• Hydrogen Bond Acceptor Count: 0
• Rotatable Bond Count: 0
• Exact Mass: 215.793638
• Heavy Atom Count: 5
• Complexity: 19.1

Purity/Quality:

99.9% ^*data from raw suppliers

Germanium(IV) chloride (99.99%-Ge) PURATREM ^*data from reagent suppliers

Safty Information:

• Pictogram(s): C
• Hazard Codes: C
• Statements: 14-34-67-40-37
• Safety Statements: 26-27-36-45-8-36/37/39-25

MSDS Files:

SDS file from LookChem

Useful:

• Chemical Classes: Metals -> Metalloid Compounds (Germanium)
• Canonical SMILES: Cl[Ge](Cl)(Cl)Cl
• Physical Properties: Colorless liquid; density 1.879 g/cm3 at 20°C and 1.844 g/cm3 at 30°C; refractive index 1.464; solidifies at –49.5°C; decomposes in water; soluble in alcohol, ether, benzene, chloroform and carbon tetrachloride; insoluble in concentrated hydrochloric and sulfuric acids.
• Physical properties: Colorless liquid; density 1.879 g/cm3 at 20°C and 1.844 g/cm3 at 30°C; refractive index 1.464; boils at 86.5°C; solidifies at -49.5°C; decomposes in water; soluble in alcohol, ether, benzene, chloroform and carbon tetrachloride; insoluble in concentrated hydrochloric and sulfuric acids.
• Uses: It is used as a catalyst in the conversion of carbohydrates into 5-hydroxymethylfurfural in ionic liquids, as a reducing agent in combination with triphenylphosphine (TPP) for the reduction of alpha-bromo carboxylic acid derivatives, and in the production of pure germanium. It also finds use as an intermediate for several optical processes. It is one of the most important dopants in silica glass for optical fibers. It is employed in the preparation of germanium dioxide which is used for wide camera lens, microscopy, IR-transparent glasses/windows/lenses, and for the core of fiber-optic lines. Germanium(IV) chloride is used in the microwave preparation of Ge2Cl6, a colorless crystalline material which was included in a further study of low-valent germanium compounds.1 Germanium(IV) chloride is used in the preparation of many germanium compounds.

Technology Process of Germanium chloride

There total 111 articles about Germanium chloride which guide to synthetic route it. The literature collected by LookChem mainly comes from the sharing of users and the free literature resources found by Internet computing technology. We keep the original model of the professional version of literature to make it easier and faster for users to retrieve and use. At the same time, we analyze and calculate the most feasible synthesis route with the highest yield for your reference as below:

synthetic route:

Reference yield: 100.0%

germanium (7440-56-4) → germaniumtetrachloride (10038-98-9)

Guidance literature:

In melt; Electrolysis; electrolysis in AlCl3-NaCl-KCl, NaCl-KCl, NaCl-PbCl2, LiCl-KCl, or NaCl-AlCl3 melts;; condensation of the anodic gas; purity 99.9%;

Reference yield: 50.0%

tetrachloromethane (56-23-5) + germanium (7440-56-4) → germaniumtetrachloride (10038-98-9) + trichloro(trichloromethyl)germane (25105-16-2)

Guidance literature:

reaction of germanium atoms with organic halide by co-condensation under vac. at 77 K; GC-MASS;

DOI:10.1246/cl.1987.1105

Reference yield: 15.0%

germanium (7440-56-4) + chloroform (67-66-3,8013-54-5) → germaniumtetrachloride (10038-98-9) + Dichlormethyltrichlorgerman (21572-22-5)

Guidance literature:

reaction of germanium atoms with organic halide by co-condensation under vac. at 77 K; GC-MASS;

DOI:10.1246/cl.1987.1105

upstream raw materials:

germanium

Iodine monochloride

dichloromethane

GeCl₃[N(CH₃)2]

Downstream raw materials:

germanium

diethylaluminium chloride

ethyl germanium trichloride

2-Methyl-1-trichlorgermyl-propan

Refernces

Syntheses, X-ray structures, and redox behaviour of the group 14 bis-boraamidinates MPhB(μ-N-t-Bu)₂₂ (M = Ge, Sn) and Li₂MPhB(μ-N-t-Bu)₂₂ (M = Sn, Pb)

10.1139/V08-183

The research presents a comprehensive study on the syntheses, X-ray structures, and redox behavior of group 14 bis-boraamidinates, specifically focusing on the complexes M[PhB(m-N-t-Bu)2]2 (where M = Ge, Sn) and Li2M[PhB(m-N-t-Bu)2]2 (where M = Sn, Pb). The purpose of the study was to investigate the redox transformations of these complexes and to explore the possibility of accessing cation radicals {M[PhB(m-N-t-Bu)2]2}+ (M = Si, Ge, Sn) through mild oxidation of the corresponding neutral precursors. The researchers used a variety of chemicals in their experiments, including PhBCl2, GeCl4, SnCl4, SnCl2, PbI2, t-BuNH2, SO2Cl2, and LiN(H)-tBu, among others. The conclusions drawn from the research were that the germanium complex was inert towards oxidizing agents, while the tin complex could be oxidized to form a thermally unstable blue radical cation. The study also characterized the structural and fluctional behavior of the synthesized heterotrimetallic complexes, revealing novel polycyclic arrangements and unique bonding modes within these complexes. The findings provide valuable insights into the electronic structures and potential applications of these group 14 complexes, highlighting the differences in their redox properties compared to their isoelectronic group 13 counterparts.