The chlorine has gone to form sodium chloride. In this equation, the Cl and Br have swapped places:. This type of reaction happens with all the halogens. A more reactive halogen displaces a less reactive halogen from a solution of one of its salts.
If you test different combinations of the halogens and their salts, you can work out a reactivity series for Group The slideshow shows what happens when chlorine, bromine and iodine are added to various halogen salts:.
Adding chlorine, bromine and iodine to halogen salts. Chlorine water is added to three solutions. The result of adding chlorine to the three solutions. Incompatible materials: Reducing agents, alkali metals, powdered metals, aluminum, stainless steel, iron, copper, organic materials, bromine will attack some types of plastics, rubber, and coatings, aldehydes, ketones, arsenic powder, amines, amides, phenols, alcohol, reacts violently with: ammonia, azides, ozone.
Safety Data Sheet. Product Number: , Version 5. Instability and Reactivity Hazards: Strong oxidizer. Reacts with alkalies, reactive metals, and other reducing agents. Acetaldehyde: Combination of acetaldehyde with bromine, chlorine, fluorine, or iodine can be violent.
During the drop-wise addition of bromine into a ml. When the temperature of the reactants exceeded 40 deg C, the flask exploded. Bromine vapor reacts with warm aluminum foil with brilliant incandescence.
The reaction is vigorous, even at 15 deg C. Ammonia plus bromine with heat explodes due to the formation of extremely sensitive nitrogen tribromide. Antimony is spontaneously flammable in fluorine, chlorine, or bromine. With iodine, the reaction produces heat, which can cause flame or even an explosion if the quantities are great enough. At ordinary temperatures, cesium monoxide plus bromine, chlorine, fluorine or iodine reacts with incandescence. At temperatures above deg C.
Chlorine and iodine act similarly. Addition of bromine to a mixture of chlorotrifluoroethylene and oxygen causes an explosion. One of the products of the reaction is chlorotrifluoroethylene peroxide, which explodes when heated. Cuprous acetylide is spontaneously flammable with bromine vapor, chlorine gas or fine iodine. The use of dimethyl formamide as a solvent in one of the catalysis reactions of olefins and bromine resulted in the operation of a rupture disk on an autoclave.
The investigation indicated that there was a highly exothermic reaction between dimethyl formamide and bromine. In one instance mixing 40 cc of bromine and cc of dimethyl formamide resulted in an increase of temperature to above deg C and an increase in pressure to above psi.
A mixture of ethyl phosphine and bromine, chlorine, or nitric acid fuming explodes. Bromine unites with fluorine at ordinary temperatures with luminous flame, forming bromine trifluoride. Iron carbide burns in chlorine below deg C with incandescence and behaves similarly with bromine at about deg C. Bromine has been added dropwise at deg C to a solution of isobutyrophenone in carbon tetrachloride. The flask was then packed in ice. After 15 minutes, the flask exploded. The reaction between potassium and bromine gas is vigorous with incandescence.
A violent explosion will occur if potassium is brought in contact with liquid bromine. The system bromine-plus-sodium, however, requres a small impact to cause an explosion. The system bromine-plus-lithium requires a much larger impact to explode it.
The other halogens, apart from fluorine, behave similarly. Fluorine reacts explosively with all hydrocarbons - including alkenes - to give carbon and hydrogen fluoride. If you are interested in the reaction with, say, chlorine, all you have to do is to replace Br by Cl. The reaction is an example of electrophilic addition. The bromine is a very "polarizable" molecule and the approaching pi bond in the ethene induces a dipole in the bromine molecule.
If you draw this mechanism in an exam, write the words "induced dipole" next to the bromine molecule - to show that you understand what's going on.
In the first stage of the reaction, one of the bromine atoms becomes attached to both carbon atoms, with the positive charge being found on the bromine atom. A bromonium ion is formed. Figure: Step 1 in mechanism of addition of Bromine to ethene. The bromonium ion is then attacked from the back by a bromide ion formed in a nearby reaction.
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