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Chloroform, [10] or trichloromethane (often abbreviated as TCM), is an organochloride with the formula C H Cl 3 and a common solvent. It is a volatile , colorless, sweet-smelling, dense liquid produced on a large scale as a precursor to refrigerants and PTFE . [ 11 ]
2 CuCl 2 → 2 CuCl + Cl 2 The reported melting point of copper(II) chloride of 498 °C (928 °F) is a melt of a mixture of copper(I) chloride and copper(II) chloride. The true melting point of 630 °C (1,166 °F) can be extrapolated by using the melting points of the mixtures of CuCl and CuCl 2 .
[1] [2] [3] Introduced by Gilbert N. Lewis in his 1916 article The Atom and the Molecule, a Lewis structure can be drawn for any covalently bonded molecule, as well as coordination compounds. [4] Lewis structures extend the concept of the electron dot diagram by adding lines between atoms to represent shared pairs in a chemical bond.
The naming of is group is derived from the methyl group (which has the formula –CH 3), by replacing each hydrogen atom by a chlorine atom. Compounds with this group are a subclass of the organochlorines. Some notable examples of compounds with this group are trichloromethane H– CCl 3, 1,1,1-trichloroethane H 3 C – CCl 3, and chloral HOC ...
The organic compound 1,1,1-trichloroethane, also known as methyl chloroform and chlorothene, is a chloroalkane with the chemical formula CH 3 CCl 3. It is an isomer of 1,1,2-trichloroethane . A colourless and sweet-smelling liquid, it was once produced industrially in large quantities for use as a solvent . [ 5 ]
1,1,2-Trichloroethane, vinyl trichloride or 1,1,2-TCA, is an organochloride solvent with the molecular formula C 2 H 3 Cl 3 and the structural formula CH 2 Cl—CHCl 2. It is a colourless, sweet-smelling liquid that does not dissolve in water, but is soluble in most organic solvents. It is an isomer of 1,1,1-trichloroethane, and a byproduct of ...
[10] [11] The phase diagram for the anhydrous system KCl / CuCl 2 shows potassium trichloridocuprate KCuCl 3 as a congruently-melting compound, but not K 2 CuCl 4. [12] The dihydrate decomposes on heating above 93 °C to KCl, KCuCl 3 and water. [13] [14] The doubts were put to rest when successful dehydration was achieved by T. J. Nolan and ...
CCl 4 + Na 2 SiF 6 → CCl 3 F + CCl 2 F 2 + CCl 3 F + NaCl + SiF 4 CCl 4 + BrF 3 → BrF + CCl 2 F 2 + CCl 3 F. Trichlorofluoromethane was included in the production moratorium in the Montreal Protocol of 1987. It is assigned an ozone depletion potential of 1.0, and U.S. production was ended on January 1, 1996. [6]