Tetrabromomethane

Tetrabromomethane has two polymorphs: crystalline II or β below 46.9 °C (320.0 K) and crystalline I or α above 46.9 °C. Monoclinic polymorph has space group C2/c with lattice constants: a = 20.9, b = 12.1, c = 21.2 (.10⁻¹ nm), β = 110.5°.^[4] Bond energy of C-Br is 235 kJ.mol⁻¹.^[5]

Due to its symmetrically substituted tetrahedral structure, its dipole moment is 0 Debye. Critical temperature is 439 °C (712 K) and critical pressure is 4.26 MPa.^[4]

Plastic crystallinity

The high temperature α phase is known as a plastic crystal phase. Roughly speaking, the CBr₄ are situated on the corners of the cubic unit cell as well as on the centers of its faces in an fcc arrangement. It was thought in the past that the molecules could rotate more or less freely (a 'rotor phase'), so that on a time average they would look like spheres. Recent work ^[6] has shown, however, that the molecules are restricted to only 6 possible orientations (Frenkel disorder). Moreover, they cannot take these orientations entirely independently from each other because in some cases the bromine atoms of neighboring molecules would point at each other leading to impossibly short distances. This rules out certain orientational combinations when two neighbor molecules are considered. Even for the remaining combinations displacive changes occur that better accommodate neighbor to neighbor distances. The combination of censored Frenkel disorder and displacive disorder implies a considerable amount of disorder inside the crystal which leads to highly structured sheets of diffuse scattered intensity in X-ray diffraction. In fact, it is the structure in the diffuse intensity that provides the information about the details of the structure.

Chemical reactions

In combination with triphenylphosphine, CBr₄ is used in the Appel reaction, which converts alcohols to alkyl bromides. Similarly, CBr₄ is used in combination with triphenylphosphine in the first step of the Corey-Fuchs reaction, which converts aldehydes into terminal alkynes. It is significantly less stable than lighter tetrahalomethanes.

It is prepared by methane bromination using HBr or Br₂. It can be also prepared by more economical reaction of tetrachloromethane with aluminium bromide at 100 °C.^[5]

Uses

It is used as a solvent for greases, waxes and oils, in plastic and rubber industry for blowing and vulcanization, further for polymerization, as a sedative and as an intermediate in manufacturing agrochemicals. Due to its non-flammability it is used as an ingredient in fire-resistant chemicals. It is also used for separating minerals because of its high density.

References

↑ "carbon tetrabromide - Compound Summary". PubChem Compound. USA: National Center for Biotechnology Information. 26 March 2005. Identification. Retrieved 18 June 2012.
↑ "Carbon compounds: carbon tetrabromide". Retrieved 22 February 2013.
1 2 3 4 "NIOSH Pocket Guide to Chemical Hazards #0106". National Institute for Occupational Safety and Health (NIOSH).
1 2 F. Brezina, J. Mollin, R. Pastorek, Z. Sindelar. Chemicke tabulky anorganickych sloucenin (Chemical tables of inorganic compounds). SNTL, 1986.
1 2 N. N. Greenwood, A. Earnshaw. Chemie prvku (Chemistry of the Elements). Informatorium, Prague, 1993.
↑ Coupled orientational and displacive degrees of freedom in the high-temperature plastic phase of the carbon tetrabromide α-CBr4 Jacob C. W. Folmer, Ray L. Withers, T. R. Welberry, and James D. Martin. Physical Review B 77 in press

External links

Bromine compounds

AgBr AlBr₃ AmBr₃ AsBr₃ AuBr₃ BBr₃ B₂Br₄ BaBr₂ BeBr₂ BiBr₃ BrCl CsBr BrF₃ BrF₅ HBr IBr KBr LiBr BrN₃ NaBr BrO₂ RbBr TlBr CaBr₂ CdBr₂ CoBr₂ CuBr₂ EuBr₂ FeBr₂ GeBr₂ HgBr₂ Hg₂Br₂ MgBr₂ MnBr₂ NiBr₂ Br₂O Br₂O₃ Br₂O₅ PbBr₂ PdBr₂ PtBr₂ S₂Br₂ Se₂Br₂ SnBr₂ SrBr₂ TeBr₂ YbBr₂ ZnBr₂ CeBr₃ CrBr₃ CsBr₃ DyBr₃ ErBr₃ EuBr₃ FeBr₃ GaBr₃ GdBr₃ HoBr₃ InBr InBr₃ IrBr₃ LaBr₃ LuBr₃ MoBr₃ NBr₃ NdBr₃ PBr₃ PrBr₃ ReBr₃ SbBr₃ SmBr₃ TbBr₃ TmBr₃ UBr₃ VBr₃ YBr₃ YbBr₃ GeBr₄ HfBr₄ PbBr₄ SeBr₄ SiBr₄ SnBr₄ TeBr₄ ThBr₄ TiBr₄ UBr₄ WBr₄ ZrBr₄ NbBr₅ PBr₅ TaBr₅ UBr₅ WBr₅ CBr₄ CrBr₂ DyBr₂ HfBr₂ HfBr₃

Chemical formulas

Halomethanes

Monosubstituted	CH₃F CH₃Cl CH₃Br CH₃I

Disubstituted	CH₂F₂ CH₂ClF CH₂BrF CH₂FI CH₂Cl₂ CH₂BrCl CH₂ClI CH₂Br₂ CH₂BrI CH₂I₂

Trisubstituted	CHF₃ CHClF₂ CHBrF₂ CHF₂I CHCl₂F CHBrClF CHClFI CHBr₂F CHBrFI CHFI₂ CHCl₃ CHBrCl₂ CHCl₂I CHBr₂Cl CHBrClI CHClI₂ CHBr₃ CHBr₂I CHBrI₂ CHI₃

Tetrasubstituted	CF₄ CClF₃ CBrF₃ CF₃I CCl₂F₂ CBrClF₂ CClF₂I CBr₂F₂ CBrF₂I CF₂I₂ CCl₃F CBrCl₂F CCl₂FI CBr₂ClF C*BrClFI CClFI₂ CBr₃F CBr₂FI CBrFI₂ CFI₃ CCl₄ CBrCl₃ CCl₃I CBr₂Cl₂ CBrCl₂I CCl₂I₂ CBr₃Cl CBr₂ClI CBrClI₂ CClI₃ CBr₄ CBr₃I CBr₂I₂ CBrI₃ CI₄

* Chiral compound.

Inorganic compounds of carbon and related ions

Compounds	CBr₄ CCl₄ CF CF₄ CI₄ CO CO₂ CO₃ COS CS CS₂ CSe₂ C₃O₂ C₃S₂ SiC

Carbon ions	Carbides [:C≡C:]^2–, [::C::]^4–, [:C=C=C:]^4– Cyanides [:C≡N:]^– Cyanates [:O-C≡N:]^– Thiocyanates [:S-C≡N:]^– Fulminates [:C≡N-O:]^– Thiofulminates [:C≡N-S:]^–

Oxides and related	Oxides Metal carbonyls Carbonic acid Bicarbonates Carbonates

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