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Question
Rationalise the given statement and give a chemical reaction:
Lead (II) chloride reacts with Cl2 to give PbCl4.
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Solution
Lead belongs to group 14 of the periodic table. The two oxidation states displayed by this group is +2 and +4. On moving down the group, the +2 oxidation state becomes more stable and the +4 oxidation state becomes less stable. This is because of the inert pair effect. Hence, PbCl4 is much less stable than PbCl2. However, the formation of PbCl4 takes place when chlorine gas is bubbled through a saturated solution of PlCl2.
\[\ce{PbCl_{2(s)} + Cl_{2(g)} -> PbCl_{4(l)}}\]
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