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pbi4 exist or not

Answer Save. 4 Answers. Nov 26 2020 05:22 AM. The Questions and Answers of PbI4 does not exist why ? Solution.pdf Next Previous. See the answer. Dear User, Pb exist as Pb(IV) in PbI 4. Q.14 Suggest reasons why the B-F … Lead (II) iodide, which has PbI2 as its chemical formula, exists only this way and not in the form PbI4 as someone might guess. Pbl 4 does not exist because Pb-I bond initially formed during the reaction of Pb with I 2 does not release enough energy to unpair 6s 2 electrons and excite one of them to higher orbital to have 4 unpaired electrons around it. This problem has been solved! are solved by group of students and teacher of IIT JAM, which is also the largest student community of IIT JAM. A high-boiling liquid, bp 202–204 ° C burns with a yellow, sooty flame. Related Questions. WCP. Expert Answer 100% (2 ratings) Previous question Next question Get more help from Chegg. Question: While SnI4 Is Quite Stable, PbI4 Does Not Exist As A Stable Compound. If the answer is not available please wait for a while and a community member will probably answer this soon. Why is PbI4 not possible whereas PbCl4 exists? So whenever a Pb compound is formed in +4 oxidation state then it would try to oxidise the counter anion and by this process it gets reduced to +2 oxidation state. Relevance. COMEDK 2014: The non existence of PbI4 and PbBr4 is due to (A) highly oxidizing nature of Pb4+ ions (B) highly reducing nature of I- and Br- ions (C) While PO2 and PbCl4 exist, PbBr2 and PbI4 do not. Chlorine is a stronger oxidising agent and so can easily oxidise lead from +2 oxidation state to +4 oxidation state, therefore, PbCl4 exists whereas PbBr4 and Pbl4 do not exist because bromine and iodine are weaker oxidising agents and so cannot oxidise Pb2+ to Pb4+. Favorite Answer. Question from P-Block elements (Group-13 and Group-14),chemistry why? PbI does not exist. While SnI4 is quite stable, PbI4 does not exist as a stable compound. Why? Because of Inert Pair Effect Pb prefers to exist in 2+ oxidation state. While PO2 and PbCl4 exist, PbBr2 and PbI4 do not. Pb 4+ being a strong acid (strong oxidant) will take up electrons from soft base (have fairly good reducing power) I- to oxidise … +4 oxidation state is less stable and therefore gets reduced to +2.PbI 4 does not exist because the iodide ion reduces Pb(IV) to Pb(II) and itself gets oxidised to I 2 and therefore PbI 2 is formed. Neither are good electrolytes. Why? why? P b C l 4 exists but P b B r 4 and P b I 4 do not because P b − I and P b − B r bonds initially formed during the reaction do not release enough energy to unpair 6 s 2 electrons and excite one of them to higher orbital to have four unpaired electrons around lead atom. Expert's Answer. 1 decade ago. There are, however PbI2 and PbI4. Sodium fusion indicates that halogens, nitrogen, and sulfur are not present. 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