Rationalize the given statements and give chemical reactions:

(a) Lead (II) chloride reacts with Cl2 to give PbCl4.

(b) Lead (IV) chloride is highly unstable towards heat.

(c) Lead is known not to form an iodide, PbI4.

Asked by Pragya Singh | 11 months ago |  56

##### Solution :-

(a) In the periodic table, lead is in group 14. This group's oxidation states are +2 and +4. The +2 oxidation state gets more stable as one move down the group, whereas the +4 oxidation state becomes less stable. The inert pair effect is responsible for this. Consequently, $$PbCl_4$$ has a lower stability than $$PbCl_2$$ . When chlorine gas is bubbled through a saturated solution of $$PbCl_2$$,$$PbCl_4$$ is formed. The reaction is given below:

(b) This occurs due to the inert pair effect as you move along group IV. Because Pb(IV) is very unstable, it can be reduced to Pb when heated (II). The reaction is given below:

(c) As far as we know, lead does not produce PbI4 .The oxidation of Pb (+4) occurs in nature, while the reduction of $$I^{-}$$takes place in nature. Combining
Pb(IV) with iodide ion does not result in stability. The iodide ion is a powerful reducing agent in the environment. $$I^{-}$$is oxidised to I2 by Pb(IV), which is then reduced to Pb (II). The reaction is given below:

Answered by Abhisek | 11 months ago

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