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Bromine Oxide
Bromine can form several different unstable oxides: * Dibromine monoxide (Br2O) * Bromine dioxide (BrO2) * Dibromine trioxide (Br2O3) * Dibromine pentoxide (Br2O5) * Tribromine octoxide (Br3O8) Also, a number of ions are bromine oxides: * Hypobromite (BrO−) * Bromite (BrO2−) * Bromate (BrO3−) * Perbromate (BrO4−) And the bromine monoxide radical: * Bromine oxide (BrO) See also * Oxygen fluoride * Chlorine oxide * Iodine oxide Iodine oxides are chemical compounds of oxygen and iodine. Iodine has only two stable oxides which are isolatable in bulk, iodine tetroxide and iodine pentoxide, but a number of other oxides are formed in trace quantities or have been hypothesized ... {{Chemistry index Bromine compounds Oxides ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Bromine
Bromine is a chemical element with the symbol Br and atomic number 35. It is the third-lightest element in group 17 of the periodic table ( halogens) and is a volatile red-brown liquid at room temperature that evaporates readily to form a similarly coloured vapour. Its properties are intermediate between those of chlorine and iodine. Isolated independently by two chemists, Carl Jacob Löwig (in 1825) and Antoine Jérôme Balard (in 1826), its name was derived from the Ancient Greek (bromos) meaning "stench", referring to its sharp and pungent smell. Elemental bromine is very reactive and thus does not occur as a native element in nature but it occurs in colourless soluble crystalline mineral halide salts, analogous to table salt. In fact, bromine and all the halogens are so reactive that they form bonds in pairs—never in single atoms. While it is rather rare in the Earth's crust, the high solubility of the bromide ion (Br) has caused its accumulation in the oceans. Comme ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Oxide
An oxide () is a chemical compound that contains at least one oxygen atom and one other element in its chemical formula. "Oxide" itself is the dianion of oxygen, an O2– (molecular) ion. with oxygen in the oxidation state of −2. Most of the Earth's crust consists of oxides. Even materials considered pure elements often develop an oxide coating. For example, aluminium foil develops a thin skin of Al2O3 (called a passivation layer) that protects the foil from further corrosion.Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. . Stoichiometry (the measurable relationship between reactants and chemical equations of a equation or reaction) Oxides are extraordinarily diverse in terms of stoichiometries and in terms of the structures of each stoichiometry. Most elements form oxides of more than one stoichiometry. A well known example is carbon monoxide and carbon dioxide.Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Dibromine Monoxide
Dibromine monoxide is the chemical compound composed of bromine and oxygen with the formula Br2O. It is a dark brown solid which is stable below −40 °C and is used in bromination reactions. It is similar to dichlorine monoxide, the monoxide of its halogen neighbor one period higher on the periodic table. The molecule is bent, with C2v molecular symmetry. The Br−O bond length is 1.85 Å and the Br−O−Br bond angle is 112°, similar to dichlorine monoxide. Reactions Dibromine monoxide can be prepared by reacting bromine vapor or a solution of bromine in carbon tetrachloride with mercury(II) oxide at low temperatures: :2 Br2 + 2 HgO → HgBr2·HgO + Br2O It can also be formed by thermal decomposition Thermal decomposition, or thermolysis, is a chemical decomposition caused by heat. The decomposition temperature of a substance is the temperature at which the substance chemically decomposes. The reaction is usually endothermic as heat is re . ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Bromine Dioxide
Bromine dioxide is the chemical compound composed of bromine and oxygen with the formula BrO2. It forms unstable yellow to yellow-orange crystals. It was first isolated by R. Schwarz and M. Schmeißer in 1937 and is hypothesized to be important in the atmospheric reaction of bromine with ozone. It is similar to chlorine dioxide, the dioxide of its halogen neighbor one period higher on the periodic table. Reactions Bromine dioxide is formed when an electric current is passed through a mixture of bromine and oxygen gases at low temperature and pressure. Bromine dioxide can also be formed by the treatment of bromine gas with ozone in trichlorofluoromethane at −50 °C. When mixed with a base, bromine dioxide gives the bromide and bromate anions: :6 BrO2 + 6 NaOH Sodium hydroxide, also known as lye and caustic soda, is an inorganic compound with the formula NaOH. It is a white solid ionic compound consisting of sodium cations and hydroxide anions . Sodium hydroxide ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Dibromine Trioxide
Dibromine trioxide is the chemical compound composed of bromine and oxygen with the formula Br2O3. It is an orange solid that is stable below −40 °C. It has the structure Br−O−BrO2 (bromine bromate). The Br−O−Br bond is bent, with a bond angle of 111.2°, and the Br−O−BrO2 bond length is 1.85 Å. Reactions Dibromine trioxide can be prepared by reacting a solution of bromine in dichloromethane with ozone Ozone (), or trioxygen, is an inorganic molecule with the chemical formula . It is a pale blue gas with a distinctively pungent smell. It is an allotrope of oxygen that is much less stable than the diatomic allotrope , breaking down in the lo ... at low temperatures. It disproportionates in alkali solutions to Br and BrO. References Bromine(V) compounds Sesquioxides Bromine(I) compounds Mixed valence compounds {{inorganic-compound-stub ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Dibromine Pentoxide
Dibromine pentoxide is the chemical compound composed of bromine and oxygen with the formula Br2O5. It is a colorless solid that is stable below −20 °C. It has the structure O2Br−O−BrO2, the Br−O−Br bond is bent with bond angle 121.2°. Each BrO3 group is pyramidal with the bromine atom at the apex. Reactions Dibromine pentoxide can be prepared by reacting a solution of bromine in dichloromethane with ozone at low temperatures and recrystallized from propionitrile Propionitrile, also known as ethyl cyanide and propanenitrile, is an organic compound with the formula CH3CH2CN. It is a simple aliphatic nitrile. The compound is a colourless, water-soluble liquid. It is used as a solvent and a precursor to oth .... References Bromine(V) compounds Oxides {{inorganic-compound-stub ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Hypobromite
The hypobromite ion, also called alkaline bromine water, is BrO−. Bromine is in the +1 oxidation state. The Br–O bond length is 1.82 Å. Hypobromite is the bromine compound analogous to hypochlorites found in common bleaches, and in immune cells. In many ways, hypobromite functions in the same manner as hypochlorite, and is also used as a germicide and antiparasitic in both industrial applications, and in the immune system. Preparation Hypobromite salts form upon treating bromine with aqueous alkali, such as sodium or potassium hydroxide. At 20 °C the reaction is rapid. : Br2 + 2 OH−(aq) → Br− + BrO− + H2O In this reaction the bromine disproportionates (some undergoes reduction and some oxidation) from oxidation state 0 (Br2) to oxidation state −1 (Br−) and oxidation state +1 (BrO−). Sodium hypobromite can be isolated as an orange solid. A secondary reaction, where hypobromite spontaneously disproportionates to bromide (bromine oxidation state −1) a ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Bromous Acid
Bromous acid is the inorganic compound with the formula of HBrO2. It is an unstable compound, although salts of its conjugate base – bromites – have been isolated. In acidic solution, bromites decompose to bromine.Egon Wiberg, Arnold Frederick Holleman (2001) ''Inorganic Chemistry'', Elsevier Discovery In 1905, Richards A. H. proved the existence of bromous acid through a series of experiments involving silver nitrate (AgNO3) and bromine. The reaction of excess cold aqueous to form hypobromous acid (HBrO), silver bromide (AgBr) and nitric acid (HNO3): :Br2 + AgNO3 + H2O → HBrO + AgBr + HNO3 Richards discovered that the effect of adding excess liquid bromine in a concentrated silver nitrate (AgNO3) resulted in a different reaction mechanism. From numbers of equivalent portions of acid bromine formed from the previous reaction, the ratio between oxygen and bromine was calculated, with the exact value of O:Br (0.149975:0.3745), suggesting the acid compound contains two oxyg ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Bromate
The bromate anion, BrO, is a bromine-based oxoanion. A bromate is a chemical compound that contains this ion. Examples of bromates include sodium bromate, (), and potassium bromate, (). Bromates are formed many different ways in municipal drinking water. The most common is the reaction of ozone and bromide: : Br + → BrO Electrochemical processes, such as electrolysis of brine without a membrane operating to form hypochlorite, will also produce bromate when bromide ion is present in the brine solution. Photoactivation (sunlight exposure) will encourage liquid or gaseous bromine to generate bromate in bromide-containing water. In laboratories bromates can be synthesized by dissolving in a concentrated solution of potassium hydroxide (KOH). The following reactions will take place (via the intermediate creation of hypobromite): : + 2 OH− → Br + BrO + :3 BrO → BrO + 2 Br Human health issues Bromate in drinking water is undesirable because it is a suspected huma ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Perbromate
In chemistry, the perbromate ion is the anion having the chemical formula . It is an oxyanion of bromine, the conjugate base of perbromic acid, in which bromine has the oxidation state +7. Unlike its chlorine () and iodine () analogs, it is difficult to synthesize. It has tetrahedral molecular geometry. The term perbromate also refers to a compound that contains the anion or the functional group. The perbromate ion is a strong oxidizing agent. The reduction potential for the / Br− couple is +0.68 V at pH 14. This is comparable to selenite's reduction potential. Synthesis Attempted syntheses of perbromates were unsuccessful until 1968, when it was finally obtained by the beta decay of selenium-83 in a selenate salt: : → + β− Subsequently, it was successfully synthesized again by the electrolysis of , although only in low yield. Later, it was obtained by the oxidation of bromate with xenon difluoride. Once perbromates are obtained, perbromic acid can b ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Oxygen Fluoride
Oxygen fluorides are compounds of elements oxygen and fluorine with the general formula , where ''n'' = 1 to 6. Many different oxygen fluorides are known: *oxygen difluoride () * dioxygen difluoride () * trioxygen difluoride or ozone difluoride () * tetraoxygen difluoride () * pentaoxygen difluoride () * hexaoxygen difluoride () *dioxygen monofluoride or fluoroperoxyl () Oxygen fluorides are strong oxidizing agents with high energy and can release their energy either instantaneously or at a controlled rate. Thus, these compounds attracted much attention as potential fuels in jet propulsion systems. Synthesis Here are some synthesis methods and reactions of the three most common oxygen fluorides – oxygen difluoride (), dioxygen difluoride () and ozone difluoride (). Oxygen difluoride () A common preparative method involves fluorination of sodium hydroxide: : is a colorless gas at room temperature and a yellow liquid below 128 K. Oxygen difluoride has an irritati ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
