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Its bromide and chloride salts [5] can be made from cycloheptatriene and bromine or phosphorus pentachloride, respectively. [6] It is a regular heptagonal, planar, cyclic ion. It has 6 π-electrons (4n + 2, where n = 1), which fulfills Hückel's rule of aromaticity. It can coordinate as a ligand to metal atoms.
A pentachloride is a compound or ion that contains five chlorine atoms or ions. Common pentachlorides include: Antimony pentachloride, SbCl 5; Arsenic pentachloride, AsCl 5; Molybdenum pentachloride, MoCl 5; Niobium pentachloride, NbCl 5; Phosphorus pentachloride, PCl 5; Protactinium pentachloride, PaCl 5; Osmium pentachloride, OsCl 5; Rhenium ...
Bond energies to bromine tend to be lower than those to chlorine but higher than those to iodine, and bromine is a weaker oxidising agent than chlorine but a stronger one than iodine. This can be seen from the standard electrode potentials of the X 2 /X − couples (F, +2.866 V; Cl, +1.395 V; Br, +1.087 V; I, +0.615 V; At, approximately +0.3 V).
Bond energies to bromine tend to be lower than those to chlorine but higher than those to iodine, and bromine is a weaker oxidising agent than chlorine but a stronger one than iodine. This can be seen from the standard electrode potentials of the X 2 /X − couples (F, +2.866 V; Cl, +1.395 V; Br, +1.087 V; I, +0.615 V; At, approximately +0.3 V).
One can test for a bromide ion by adding an oxidizer. One method uses dilute HNO 3. Balard and Löwig's method can be used to extract bromine from seawater and certain brines. For samples testing for sufficient bromide concentration, addition of chlorine produces bromine (Br 2): [7] Cl 2 + 2 Br − → 2 Cl − + Br 2
Bromine pentafluoride, Br F 5, is an interhalogen compound and a fluoride of bromine.It is a strong fluorinating agent.. BrF 5 finds use in oxygen isotope analysis. Laser ablation of solid silicates in the presence of BrF 5 releases O 2 for subsequent analysis. [2]
The reaction proceeds via the unstable molybdenum(V) bromide, which releases bromine at room temperature. [7] MoCl 5 is a good Lewis acid toward non-oxidizable ligands. It forms an adduct with chloride to form [MoCl 6] −. In organic synthesis, the compound finds occasional use in chlorinations, deoxygenation, and oxidative coupling reactions. [8]
The sum of oxidation states in the ion equals its charge (as it equals zero for a neutral molecule). Also in anions, the formal (ionic) charges have to be considered when nonzero. For sulfate this is exemplified with the skeletal or Lewis structures (top), compared with the bond-order formula of all oxygens equivalent and fulfilling the octet ...