Why does the octet rule not hold for many compounds containing elements in the row of the periodic table?

Question

Edit.. periodic table and beyond?

Answer 1

d orbitals start to get filled and the five d orbitals can hold 10 electrons. Octet rule is not valid but aufbau principle comes into play.Hope you have learnt a bit of advanced atomic struture to be able to understand my answer

Answer 2

The Octet Rule does not hold for those because, since n>2. When n=3, there are a lot more valence orbitals available.

n=2: 2s 2p -----> 4 valence orbitals available, which means a max of 8 electrons.

n=3: 3s 3p 3d -----> 9 valence orbitals available, which means a max of 18 electrons.

I just learned this AGAIN yesterday in my college chemistry lecture class.

Answer 3

Past group 2, and in the d block elements the octet rule brakes down. This is because the 3rd. shell can hold more than 8 electrons, though they are more stable and more common.

Answer 4

if they can tap into the d block you can get hypervalent compounds. in certain situations you even get hyperligous compounds.