![]() Lone pair (non-bonded electron) = Number of valance electrons – Number of bonded electrons. In IF 5, iodine contains one lone pair of electrons and fluorine contains three lone pairs of electrons. In the IF 5 structure, both iodine and fluorine contain lone pairs. Only one electron is required to fill up the valence shell. Its valance shell occupies seven electrons. In the case of fluorine, it satisfies the octet rule. Iodine has a total of twelve electrons which include both bond pairs and lone pairs. It needs eighteen electrons to fill up its outermost shell. It holds more than eight electrons in the outermost orbital. In the IF 5 molecule, iodine does not obey the octet rule. This rule explains that to acquire stability an atom can form a bond (ionic or covalent) in such a way that the valence shell contains eight electrons. Due to the presence of lone pair electron in the axial position, the repulsion is minimum and the bond angle is nearly 900. In the IF5 lewis structure, the bond angle is 81.90. The bond angle of the IF 5 lewis structure is given below. The angle formed between two covalent bonds is called the bond angle.
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