Other elements in the group of Bromine · Type of element · Compounds it is used in · Uses for Bromine · Unique info for bromine · location · Bohr Diagram. File bromine (Br) enhanced Bohr diagramweb.net No higher resolution available. 35_bromine_(Br)diagramweb.net ( × diagramweb.net!
What Is Bromine Number
Bromine atomic orbital and chemical bonding information. There are also tutorials on the first thirty-six elements of the periodic table. Bohr diagrams show electrons orbiting the nucleus of an atom somewhat like planets orbit around the sun.
In the Bohr model, electrons are. Bromine at Chemical diagramweb.net Basic Information | Atomic Name: Bromine Symbol: Br Atomic Number: 35 [Bohr Model of Bromine], Number of Energy.In atomic physics, the Rutherford–Bohr model or Bohr model or Bohr diagram, presented by Niels Bohr and Ernest Rutherford in , a system consisting of a small, dense nucleus surrounded by revolving electrons —similar to the structure of the Solar System.
A Bohr diagram is a simplified visual representation of an atom that was developed by Danish physicist Niels Bohr in The diagram depicts the atom as a positively charged nucleus surrounded by electrons that travel in circular orbits about the nucleus in discrete energy levels. already exists as an alternate of this question.
Would you like to make it the primary and merge this question into it? For that, we have electron shell diagrams.
Isotope data for bromine-81 in the Periodic Table Isotopes of Bromine (click to see decay chain): 67 Br 68 Br 69 Br 70 Br 71 Br 72 Br 73 Br 74 Br 75 Br 76 Br 77 Br 78 Br 79 Br 80 Br 81 Br 82 Br 83 Br 84 Br 85 Br 86 Br 87 Br 88 Br 89 Br 90 Br 91 Br 92 Br 93 Br 94 Br 95 Br 96 Br 97 Br. Atomic Number: 35. Atomic symbol: Br. Atomic Weight: 79.904. Electron affinity: -325 kJ/mol. Electron configuration: 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 5. Ionization energies: 1140 kJ/mol.
Bromine, atomic structure
Here are electron shell atom diagrams for the elements, ordered by increasing atomic number. For each electron shell atom diagram, the element symbol is listed in the nucleus.
The electron shells are shown, moving outward from the nucleus. Bohr-Rutherford diagram [ 2 Answers ] Hello, I must find the Bohr-Rutherford diagram for an element.
There are so many types of diagrams that I do not know which one to use.Bohr Model Of Bromine. Bromine :) On EmazeHow to Do Bohr Diagrams | Sciencing
Our editors will review what you’ve submitted and determine whether to revise the article.
Join Britannica's Publishing Partner Program and our community of experts to gain a global audience for your work!Bromine (Br), chemical element, a deep red noxious liquid, and a member of the halogen elements, or Group 17 (Group VIIa) of the periodic table.
| atomic number | 35 |
|---|---|
| atomic weight | [79.901, 79.907] |
| melting point | −7.2 °C (19 °F) |
| boiling point | 59 °C (138 °F) |
| specific gravity | 3.12 at 20 °C (68 °F) |
| oxidation states | −1, +1, +3, +5, +7 |
| electron configuration | (Ar)3d104s24p5 |
History
Bromine was discovered in 1826 by the French chemist Antoine-Jérôme Balard in the residues (bitterns) from the manufacture of sea salt at Montpellier. He liberated the element by passing chlorine through an aqueous solution of the residues, which contained magnesium bromide. Distillation of the material with manganese dioxide and sulfuric acid produced red vapours, which condensed to a dark liquid. The similarity of this procedure to that for making chlorine suggested to Balard that he had obtained a new element similar to chlorine. (The German chemist Justus von Liebig appears to have obtained the element before Balard, but he wrongly considered it to be iodine chloride.) Because of the bad odour of the element, the French Academy of Sciences suggested the name bromine, from the Greek word bromos, meaning “bad smell” or “stench.”
Occurrence and distribution
A rare element, bromine is found in nature dispersed throughout Earth’s crust only in compounds as soluble and insoluble bromides. Some enrichment occurs in ocean water (65 parts per million by weight), in the Dead Sea (approximately 5 grams per litre [0.7 ounce per gallon]), in some thermal springs, and in rare insoluble silver bromide minerals (such as bromyrite, found in Mexico and Chile). Natural salt deposits and brines are the main sources of bromine and its compounds. Jordan, Israel, China, and the United States led the world in bromine production in the early 21st century; other important bromine-producing countries during that period include Japan, Ukraine, and India.
Natural bromine is a mixture of two stable isotopes: bromine-79 (50.54 percent) and bromine-81 (49.46 percent). Of the 17 known radioactive isotopes of the element, bromine-77 has the longest half-life (57 hours).
Physical and chemical properties
Bromine Ionic Charge
Free bromine is a reddish brown liquid with an appreciable vapour pressure at room temperature. Bromine vapour is amber in colour. Bromine has a pungent odour and is irritating to the skin, eyes, and respiratory system. Exposure to concentrated bromine vapour, even for a short time, may be fatal. Like the other halogens, bromine exists as diatomic molecules in all aggregation states.
About 3.41 grams (0.12 ounce) of bromine dissolve in 100 millilitres (0.1 quart) of water at room temperature. The solution is known as bromine water. Like chlorine water, it is a good oxidizing agent, and it is more useful because it does not decompose so readily. It liberates free iodine from iodide-containing solutions and sulfur from hydrogen sulfide. Sulfurous acid is oxidized by bromine water to sulfuric acid. In sunlight bromine water decomposes, with release of oxygen, as in the following equation:
From bromine water a hydrate (a clathrate) can be isolated that contains 172 water molecules and 20 cavities capable of accommodating the bromine molecules. Bromine dissolves in aqueous alkali hydroxide solutions, giving bromides, hypobromites, or bromates, depending on the temperature. Bromine is readily extracted from water by organic solvents such as carbon tetrachloride, chloroform, or carbon disulfide, in which it is very soluble. In the organic solvents it gives an orange solution.
The electron affinity of bromine is high and is similar to that of chlorine. It is, however, a less powerful oxidizing agent, chiefly because of the weaker hydration of the bromide ion as compared with the chloride ion. Similarly, a metal-bromine bond is weaker than the corresponding metal-chlorine bond, and this difference is reflected in the chemical reactivity of bromine, which lies between that of chlorine and that of iodine. An organic bromo compound resembles the corresponding chloro derivative but is usually more dense, less volatile, less combustible, and less stable.
Bromine combines violently with the alkali metals and with phosphorus, arsenic, aluminum, and antimony but less violently with certain other metals. Bromine displaces hydrogen from saturated hydrocarbons and adds to unsaturated hydrocarbons, though not as readily as chlorine does.
The most stable oxidation state of the element is −1, in which bromine occurs naturally. But oxidation states of 0 (elemental bromine, Br2), +1 (hypobromite, BrO−), +3 (bromite, BrO−2), +5 (bromate, BrO−3), and +7 (perbromate, BrO−4) are also known. The first ionization energy of bromine is high, and compounds containing bromine in positive oxidation numbers are stabilized by appropriate ligands, mainly oxygen and fluorine. Compounds with the oxidation numbers +1, +3, +4, +5, and +7 all contain covalent bonds.
Production and use
The chief commercial source of bromine is ocean water, from which the element is extracted by means of chemical displacement (oxidation) by chlorine in the presence of sulfuric acid through the reaction
The product of the reaction is a dilute solution of bromine, from which the element is removed by blowing air through it. The free bromine is then mixed with sulfur dioxide, and the mixed gases are passed up a tower down which water is trickling. The following reaction takes place in the tower:
resulting in a mixture of acids that is much richer in bromide ion than seawater. A second treatment with chlorine liberates bromine, which is freed from chlorine and purified by passage over moist iron filings.
Commercial bromine generally contains up to 0.3 percent chlorine. It is usually stored in glass bottles or in barrels coated with lead or Monel metal.
The industrial usage of bromine had been dominated by the compound ethylene bromide (C2H4Br2), which once was added to gasoline with tetraethyl lead to prevent deposition of lead in the engine. Since the renunciation of leaded gasoline, bromine compounds have mainly been used in flame retardants, but ethylene bromide is still an important compound because of its use to destroy nematodes and other pests in soils. Bromine is also used in the production of catalysts, such as aluminum bromide.
Bromine has other uses, as in making various dyes and the compounds tetrabromoethane (C2H2Br4) and bromoform (CHBr3), which are used as liquids in gauges because of their high specific gravity. Until the development of barbiturates in the early 20th century, bromides of potassium, sodium, calcium, strontium, lithium, and ammonium were used widely in medicine because of their sedative action. Silver bromide (AgBr), an important component of photographic film, is, like silver chloride and iodide, light sensitive. Traces of potassium bromate (KBrO3) are added to wheat flour to improve baking. Other bromine compounds of significance include hydrogen bromide (HBr), a colourless gas used as a reducing agent and a catalyst in organic reactions. A solution of the gas in water is called hydrobromic acid, a strong acid that resembles hydrochloric acid in its activity toward metals and their oxides and hydroxides.
Bromine Atomic Number And Symbol
Bromine Element
- key people
- related topics