Bromine Atomic Number

1. Bromine Atomic Number 81
2. Bromine Atomic Number Of Neutrons

1. Complete and detailed technical data about the element Bromine in the Periodic Table. Atomic Number: 35: Atomic Weight: 79.904: Density: 3.12 g/cm 3: Melting.
2. Bromine (Br) Atomic Data for Bromine (Br) Atomic Number = 35 Atomic Weight = 79.904 Reference E95: Isotope: Mass: Abundance: Spin: Mag Moment: 79 Br.
3. Apart from these, some pseudohalides are also known, such as cyanogen bromide (BrCN), bromine thiocyanate (BrSCN), and bromine azide (BrN3). Bromine forms a monofluoride and monochloride, as well as a trifluoride and pentafluoride. Bromine has an atomic number of 35 and is part of the halogen group of elements and is considered a diatomic non-metal. The chemical symbol for Rubidium is Rb.

Atomic Number of Bromine is 35.

A potassium atom (atomic number 19) and a bromine atom (atomic number 35) can form a chemical bond through a transfer of one electron. The potassium ion that forms has 18 electrons. What best describes the bromide ion that forms? It is a negative ion that has one less valence electron than a neutral bromine atom.

Chemical symbol for Bromine is Br. Number of protons in Bromine is 35. Atomic weight of Bromine is 79.904 u or g/mol. Melting point of Bromine is -7,3 °C and its the boiling point is 58,8 °C.

About Bromine

Bromine is a toxic oily liquid of intense red color, known for its strong unpleasant smell. That is why its name comes from a Greek word meaning stench. This chemical element exists in our cells in the form of bromide, but in large doses it has very strong irritating and toxic properties so it should be avoided. Bromine belongs to the group of halogens. In nature, it can be found in some deposits in the soils, which are in abundance in North America and China, as well as in the Dead Sea. This chemical element is used in chemical industry for producing insecticides, pesticides, sedatives, and other chemicals. The compounds of this chemical element are added to various materials to reduce their flammability.

Uses of Bromine

Bromine, a reddish-brown element with symbol Br, is used in making dyes, in pharmaceuticals, in flame-retardants, in medicines, and in agricultural chemicals. Hydrogen bromide, a colorless compound with the formula HBr, is used as a catalyst in organic chemistry. It is also important in the production of inorganic and organic bromine alloys. Tetrabromoethane (C2H2Br4) and Bromoform (CHBr3) are used as liquids in gauges. Silver bromide, a compound with the formula AgBr, is mainly used in photographic films. Bromine monochloride, a compound with formula BrCl, is employed in analytical chemistry and industrial cooling water systems.

Compounds with Bromine

• HBr: Hydrogen bromide
• AgBr: Silver bromide
• BrN₃: Bromine azide
• BrCl: Bromine monochloride
• BrF: Bromine monofluoride
• BrSCN: Bromine thiocyanate
• BrCN: Cyanogen bromide
• BrF₃: Bromine trifluoride
• BrF₅: Bromine pentafluoride
• HOBrO: Bromous acid
• HOBrO₂: Bromic acid
• HOBrO₃: Perbromic acid
• HOBr: Hypobromous acid
• BrOBrO₃: Bromine perbromate
• C₂H₄Br₂: Ethylene bromide
• C₂H₂Br₄: Tetrabromoethane
• CHBr₃: Bromoform
• KBrO₃: Potassium bromate
• CBrC_lF₂: Bromochlorodifluoromethane
• CBrF₃: Bromotrifluoromethane
• CH₂BrC_l: Bromochloromethane

Properties of Bromine Element

What is the Boiling Point of Bromine?

Bromine boiling point is 58,8 °C. Boiling point of Bromine in Kelvin is 332 K.

What is the Melting Point of Bromine?

Bromine melting point is -7,3 °C. Melting point of Bromine in Kelvin is 265.8 K.

How Abundant is Bromine?

Abundant value of Bromine is 2.4 mg/kg.

What is the State of Bromine at Standard Temperature and Pressure (STP)?

State of Bromine is Liquid at standard temperature and pressure at 0℃ and one atmosphere pressure.

When was Bromine Discovered?

Bromine was discovered in 1826.

Our editors will review what you’ve submitted and determine whether to revise the article. Power automate onenote. Wireless apps for mac.

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.

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

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. Microsoft office x for mac. 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 Atomic Number 81

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 Of Neutrons