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Classified as a cyclic diketone, it is a derivative of 1,3-cyclohexanedione. It is a white solid that is soluble in water, as well as ethanol and methanol . It once was used as a reagent to test for the aldehyde functional group .
These compounds usually form the -1, +1, +3 and +5 oxidation states. Bromine is intermediate in reactivity between chlorine and iodine, and is one of the most reactive elements. Bond energies to bromine tend to be lower than those to chlorine but higher than those to iodine, and bromine is a weaker oxidising agent than chlorine but a stronger ...
For 1,2- and 1,4-disubstituted cyclohexane, a trans configuration, the diaxial conformation is effectively prevented by its high steric strain. For 1,3-disubstituted cyclohexanes, the cis form is diequatorial and the flipped conformation suffers additional steric interaction between the two axial groups.
1,4-Cyclohexadiene is an organic compound with the formula C 6 H 8. It is a colourless, flammable liquid that is of academic interest as a prototype of a large class of related compounds called terpenoids, an example being γ-terpinene. An isomer of this compound is 1,3-cyclohexadiene.
Compared with its isomer cyclohexa-1,4-diene, cyclohexa-1,3-diene is about 1.6 kJ/mol more stable. [5] Cyclohexadiene and its derivatives form (diene)iron tricarbonyl complexes. Illustrative is [(C 6 H 8)Fe(CO) 3], an orange liquid. This complex reacts with hydride-abstracting reagents to give the cyclohexadienyl derivative [(C 6 H 7)Fe(CO) 3 ...
A prominent example is the carbon dioxide dimer, [4] which is likely to be relevant to Venus atmosphere. [5] Excimers and exciplexes are excited structures with a short lifetime. For example, noble gases do not form stable dimers, but they do form the excimers Ar 2 *, Kr 2 * and Xe 2 * under high pressure and electrical stimulation. [6]
Bromine trifluoride (BrF 3) is a yellow-green liquid that conducts electricity — it self-ionises to form [BrF 2] + and [BrF 4] −. It reacts with many metals and metal oxides to form similar ionised entities; with other metals, it forms the metal fluoride plus free bromine and oxygen ; and with water, it forms hydrofluoric acid and ...
Bromine is more electronegative than carbon (2.9 vs 2.5). Consequently, the carbon in a carbon–bromine bond is electrophilic, i.e. alkyl bromides are alkylating agents. [2] Carbon–halogen bond strengths, or bond dissociation energies are of 115, 83.7, 72.1, and 57.6 kcal/mol for bonded to fluorine, chlorine, bromine, or iodine, respectively ...