CHEM 101 Lecture Notes - Lecture 25: Cyano Radical, Lewis Structure, Covalent Bond
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How to do it - an example . Thus, lewis reasoned that when electrons congregated to form molecules they had to do so in pairs. Thus, he proposed electron pair bonds (single = 2, double = 4, triple = 6) and lone pairs. When it was realized that so-called free radical, i. e. , odd-electron molecules and ions, did exist, lewis had to deal with these molecules. His approach to constructing the structure of odd-electron molecules is not the same as the method we will use below, but will get to the same resultant structures and possibly have the advantage of being a bit more straight-forward. [by the way, free radicals are unstable and thus readily bond with other free radical species so that the two odd electrons will for an electron-pair covalent bond. ] One approach to constructing the lewis structure of odd-electron species:
