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Statement I: Pb^(4+) compounds are stron...

Statement I: `Pb^(4+)` compounds are stronger oxidizing agents than `Sn^(4+)` compounds.
Statement II:The higher oxidation states for the group 14 elements are more stable for the heavier members of the group due to ‘inert pair effect’.

A

Statement-1 is True, Statement-2 is True and Statement-2 is a correct explanation for Statement-1

B

Statement-1 is True, Statement-2 is True and Statement-2 is NOT a correct explanation for Statement-1

C

Statement-1 is True, Statement-2 is False

D

Statement-1 is False, Statement-2 is True

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Assertion (A) : Pb^(+4) compounds are stronger oxidiising agents than Sn^(4+) compounds . Reason (R): The higher oxidation states for group 14 elements are more stable for the heavier members of the group due to inert pair effect .

Assertion (A) : Pb^(+4) compounds are stronger oxidiising agents than Sn^(4+) compounds . Reason (R): The higher oxidation states for group 14 elements are more stable for the heavier members of the group due to inert pair effect .

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Ge (II) compounds are powerful reducing agents whereas Pb(IV) compound are strong oxidants. It can be due to

Why are Mn^(2+) compounds more stable than Fe^(2+) toward oxidation to their +3 state?

What are the common oxidation states exhibited by the elements of group 14 and which state is more stable for Pb ?

The +1 oxidation state in group 13 and +2 oxidation state in group 14 becomes more and more stable with increased atomic number. Explain.

Ni (II) compounds are thermodynamically more stable than Pt(II) compounds but the order is reverse in case of + 4 oxidation states. Why?

Assertion : Cr(VI) in the form of dichromate in acidic medium is a strong oxidising agent where MoO_3 and WO_3 are not. Reason: In d-block elements higher oxidation states are favoured by heavier members.

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VMC MODULES ENGLISH-p-BLOCK ELEMENTS-1-LEVEL 2
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