Limitations of octet rule

1.	Limitations of octet rule
Answer» 1 . Elements like H and He exist since they donot complete their octet. They complete their duplate. 2 . Formation of hypervalent compound i.e. compounds having more than 8 electrons in their valence shell. Eg. SiF6 , in this Si have 12 shared pair electrons ( 6 of Si and 6 of F) .3 . Formation of compound having less than 8 electrons in their valence shell. Eg. AlCl3, in which aluminum donot complete their octet, after been combined with three Cl, it has only 6 electrons in its valence shell<br>It cannot be applied to the nonmetals after silicon in the Periodic Table. These elements can “expand their octet” and have more than eight valence electrons around the central atom. Molecules with an odd number of electrons such as NO and NO₂ cannot satisfy the octet rule.<br>????

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