1. After studying this Power Points Presentation will be able to- Learning Objectives: Learn about interhalogen compounds

2. Element - The Halogen At is radioactive and unstable. Electronic configuration Covalent radius (Å) Ionic radius E.A.B.P.E.N.Dissociation energy  H hyd of anion F He 2s 2 2p 5 0.721.36-333-1884158-515 Cl Ne 3s 2 3 p 5 0.99 1.81 -348-353243-381 Br Ar 4s 2 4 p 5 1.141.95-324582.8192-347 I Kr 5s 2 5 p 5 1.332.16-2951832.5150-305 At Xe 6s 2 6 p 5 1.45 -- 2.2--

3. Interhalogen compounds All are of the type XX’ n where n = odd nos. X’ is always the lighter halogen since the smaller halogen X’ are bonded around the larger X. As the ratio of the radius of X to that of X’ increases, n also increases. IF 7 IF 5 ICl 3 IClIBr BrF 5 BrF 3 BrClBrI ClF 3 ClF

4. Preparation The interhalogen compounds can be prepared by direction combination or by the action of halogen on lower interhalogen compounds. The product formed depends upon some specific conditions For example:

5. Properties Some properties of interhalogen compounds are given in Table:

6. Uses These compounds can be used as non aqueous solvents. Interhalogen compounds are very useful fluorinating agents. ClF 3 and BrF 3 are used for the production of UF 6 in the enrichment of 235 U. U(s) + 3ClF 3 (l) → UF 6 (g) + 3ClF(g