Pbcl 4 is less stable than pbcl2
Answers
Answered by
3
Answer:
answer is explained in image
Attachments:
Answered by
25
Answer:
Explanation:
As Pb belongs to 4th Group it shows variable oxidation states that are +2 and +4
It's Electronic Configuration is ns²np²
When we move down the group we find that lower oxidation state is more stable than higher one due to inert pair effect so in case of Pb due to the inert pair effect +4 oxidation state of Pb is less stable than +2 state of Pb
So to gain more stability Pb ( +4 ) gains 2 more electrons to become Pb ( +4 ) which is more stable .
Similar questions