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+2 oxidationstate of lead is more stablethan +4 oxidation state . Give reasons.

Answer» <html><body><p></p>Solution :Among the elements of group 14, carbon does not have d- or f-electrons . Therefore , it does not show inert pair <a href="https://interviewquestions.tuteehub.com/tag/effect-966056" style="font-weight:bold;" target="_blank" title="Click to know more about EFFECT">EFFECT</a>. Consequently, it shows an oxidationstate of`+4`due to the presenceof <a href="https://interviewquestions.tuteehub.com/tag/two-714195" style="font-weight:bold;" target="_blank" title="Click to know more about TWO">TWO</a> electrons in the s- andtwo electronsin the p-orbitalof thevalenceshell. In contrast , all other elements from Ge to Pb containeither dor both d- and f-electron increases, the inertpair effect becomesmore and more prominent. In other words,as we move dow the group from Ge to Pb, the <a href="https://interviewquestions.tuteehub.com/tag/stability-651358" style="font-weight:bold;" target="_blank" title="Click to know more about STABILITY">STABILITY</a> of +2 oxidation stateincreases whilethat of `+4` oxidationstate decreases.Therefore , the tendencyof Ge, <a href="https://interviewquestions.tuteehub.com/tag/sn-646415" style="font-weight:bold;" target="_blank" title="Click to know more about SN">SN</a> and Pb to <a href="https://interviewquestions.tuteehub.com/tag/exhibit-447130" style="font-weight:bold;" target="_blank" title="Click to know more about EXHIBIT">EXHIBIT</a> +2 oxidation state increases with increasing atomic number in group 14.</body></html>


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