Question

why pbcl4 act as strong oxidizing agent

Answer 1

student-name Rohit Kumar asked in Chemistry
why pbcl4 act as strong oxidizing agent
1 Follow 0
student-name Avni Johari answered this
625 helpful votes in Chemistry, Class XI-Science
This happens because +2 oxidation state is more stable than +4 oxidation state due to the 'inert pair effect'. As we go down the group, the size of the atom increases as d and f electrons are far away from the nucleus. This makes the s electrons more tightly bound to the nucleus due to which they are reluctant to take part in chemical reactions. They act as an inert pair of electrons and this leads to increased stability of +2 oxidation state in group 14 elements. Instead of losing 4 electrons (2 from s orbital and 2 from p), they only tend to lose the p orbital electrons. Hence Pb4+ can easily gain 2 electrons to form more stable Pb2+ ions thereby acting as a strong oxidising agent.

Answer 2

Hey dear,

● Answer -
- Pb has electronic configuration [Xe] 4f14 5d10 6s2 6p2.
- It's s electrons are more strongly held that p electrons.
- Thus, it loses two p-electrons to form stable PCl2 and can also lose 2 s-electrons to form less stable PCl4.
- PCl4 being less stable easily gets converted to PCl2 while other reactant gets oxidized.


Hope this helps you..