Why Pbcl4 Is Less Stable Than Sncl4?
As We Move Down the Group from C to Pb, the Stability of +4 Oxidation State Decreases While That of +2 Oxidation State Increases Due to the Same Inert Pair...
As we move down the group from C to Pb, the stability of +4 oxidation state decreases while that of +2 oxidation state increases due to the same inert pair effect. ... Therefore, for Pb +2 oxidation state becomes more stable than +4 oxidation state and vice-versa for Sn.
Why is pbcl4 less stable?
Pb has electronic configuration [Xe] 4f14 5d10 6s2 6p2. Due to poor shielding of 6s2 electrons by inner d and f electrons, it is difficult to remove 6s2 electrons (inert pair). Thus, due to inert pair effect, the +2 oxidation state is more stable than +4 oxidation state. Hence, PbCl4 is less stable than PbCl2.
Why sncl4 is less stable than SnCl2?
Sncl2 is more stable than sncl4. According, to the rule more charge has higher tendency to polarise the surrounding atom which tends to introduce a covalent character in molecule. sncl4 tends to have higher positive charge and its size is smaller. Hence, sncl4 is covelant and sncl2 is iocnic and stable.
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