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Synthesis, basic properties, and structure
Although the formula is most commonly written CNBr, the Carbon atom is actually bonded to bromine by a single bond and to nitrogen by a triple bond. The compound is linear and quite polar, but it does not spontaneously ionize in water. Therefore, it dissolves in both water and polar organic solvents.
Cyanogen bromide can be prepared by oxidation of sodium cyanide with bromine, which proceeds via a cyanogen intermediate ((CN)2).
The main uses of cyanogen bromide are to immobilize proteins, fragment proteins by cleaving peptide bonds, and synthesize cyanamides and other molecules.
Cyanogen bromide is often used to immobilize proteins by coupling them to reagents such as agarose for affinity chromatography.  Because of its simplicity and mild pH conditions, cyanogen bromide activation is the most common method for preparing affinity gels. CNBr is also often used because it reacts with the hydroxyl groups on agarose to form cyanate esters and imidocarbonates. These groups are reacted with primary amines in order to couple the protein onto the agarose matrix, as shown in the figure. Because cyanate esters are more reactive than are cyclic imidocarbonates, the amine will react mostly with the ester, yielding isourea derivatives, and partially with the less reactive imidocarbonate, yielding substituted imidocarbonates.
The disadvantages of this approach include the toxicity of cyanogen bromide and its sensitivity to oxidation. Also, cyanogen bromide activation involves the attachment of a ligand to agarose by an isourea bond, which is positively charged at neutral pH and thus unstable. Consequently, isourea derivatives may act as weak anion exchangers.
Cyanogen bromide hydrolyzes peptide bonds at the C-terminus of methionine residues. This reaction is used to reduce the size of polypeptide segments for identification and sequencing.
In CNBr, the electrons on the carbon atom are pulled towards the more electronegative bromine. This leaves the carbon electropositive or electrophilic and vulnerable to attack by electrons on the nucleophilic sulfur in methionine. This attack is followed by the formation of a five-membered ring as opposed to a six-membered ring, which would entail the formation of a double bond in the ring between nitrogen and carbon. This double bond would result in a rigid ring conformation, thereby destabilizing the molecule. Thus, the five-membered ring is formed so that the double bond is outside the ring, as shown in the figure.
Although the nucleophilic sulfur in methionine is responsible for attacking CNBr, the sulfur in cysteine does not behave similarly. If the sulfur in cysteine attacked cyanogen bromide, the bromide ion would deprotonate the cyanide adduct, leaving the sulfur uncharged and the beta carbon of the cysteine not electrophilic. The strongest electrophile would then be the cyanide nitrogen, which, if attacked by water, would yield cyanic acid and the original cysteine.
Cleaving proteins with CNBr requires using a buffer such as 0.1N HCl (hydrochloric acid) or 70% HOF (formic acid).  These are the most common buffers for cleavage. An advantage to HCl is that formic acid causes the formation of formyl esters, which complicates protein characterization. However, formic is still often used because it dissolves most proteins. Also, the oxidation of methionine to methionine sulfoxide, which is inert to CNBr attack, occurs more readily in HCl than in formic acid, possibly because formic acid is a reducing acid. Alternative buffers for cleavage include guanidine or urea in HCl because of their ability to unfold proteins, thereby making methionine more accessible to CNBr. 
Note that water is required for normal peptide bond cleavage of the iminolactone intermediate. In formic acid, cleavage of Met-Ser and Met-Thr bonds is enhanced with increased water concentration because these conditions favor the addition of water across the imine rather than reaction of the side chain hydroxyl with the imine. Lowered pH tends to increase cleavage rates by inhibiting methionine side chain oxidation.
When methionine is followed by serine or threonine, side reactions can occur that destroy the methionine without peptide bond cleavage. Normally, once the iminolactone is formed (refer to figure), water and acid can react with the imine to cleave the peptide bond, forming a homoserine lactone and new N-terminal peptide. However, if the adjacent amino acid to methionine has a hydroxyl or sulfhydryl group, this group can react with the imine to form a homoserine without peptide bond cleavage.  These two cases are shown in the figure.
Cyanogen bromide is also widely used in organic synthesis. As stated earlier, the reagent is prone to attack by nucleophiles such as amines and alcohols because of the electrophilic carbon. In the synthesis of cyanamides and dicyanamides, primary and secondary amines react with CNBr to yield mono- and dialkylcyanamides, which can further react with amines and hydroxylamine to yield guanidines and hydroxyguanidines. In the von Braun reaction, tertiary amines react with CNBr to yield disubstituted cyanamides and an alkyl bromide. CNBr can be used to prepare aryl nitriles, nitriles, anhydrides, and cyanates. It can also serve as a cleaving agent. 
Toxicity, storage, and deactivation
Cyanogen bromide is moisture-sensitive but can be stored under dry conditions at 2 to 8 °C for extended periods of time.
Cyanogen bromide is volatile, and readily absorbed through the skin or gastrointestinal tract. Therefore, toxic exposure may occur by inhalation, physical contact, or ingestion. It is acutely toxic, causing a variety of nonspecific symptoms. Exposure to even small amounts may cause convulsions or death. 
To deactivate CNBr in a solution not exceeding 60 g/L of CNBr (dilute if necessary), the recommended method is to add 1 mol/L NaOH and 1 mol/L NaOCl in volumes of ratio 1:1:2 (CNBr solution:NaOH:NaOCl).  The aqueous alkali hydroxide instantly hydrolyzes CNBr to alkali cyanide and bromide. The cyanide can then be oxidized by sodium or calcium hypochlorite to the less toxic cyanate ion. Note that deactivation is extremely exothermic and may be explosive.
Gross, Erhard & Witkop, Bernhard (1962), " ", The Journal of Biological Chemistry 237 (6): 1856-60,
Inglis, A.S. & Edman, P. (1970), " ", Analytical Biochemistry 37 (1): 73-80,
|This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Cyanogen_bromide". A list of authors is available in Wikipedia.|