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Shweta Thakur posted an Question
August 26, 2020 • 00:25 am
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30 points
30 points
- IIT JAM
- Chemistry (CY)
Why cr with +6 oxidation state is less stable than w with +6 oxidation state coxmhau uh bbdk t ngdroli h inear et + h@aagu hro ped
hy yd6loch lhutas, hithus ola mov av& Dat Page 3 sttom gt). toswis most calle tho Mo Sd ce mat W 3d,4d, Sw Coxmhau uh bbdk t nGdroli H inear et + h@AAgu HRO ped oA)
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Priyanshu kumar Best Answer
Shweta here we see the IE factors....the sum of total IE in same group for various metals is less for heavier elements...so down the group +6 OS stability increases....
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For lighter elements in this OS the sum of IE is more...so it is less stable
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In transition metals like p block elements inert pair effect have no role
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https://youtu.be/fMAvPFE8lbQ check this short video shweta
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got it sir
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Suman Kumar![best-answer]()
in group 6, Mo(VI) and W(VI) are found to be more stable than Cr(VI) because. This easier availability of d and s electron occurs as higher energy d and s orbital like 4d,5d,3s and 4s allow the orbital to loss electron easily and form stable higher oxidation state
3d electrons are better attracted to the nucleus. Indeed, the 3d orbitals do not contain radial nodes and their electrons are thus closer to the nucleus. The radial nodes in 4d and higher d-orbitals ‘add distance’ between the nucleus and the corresponding d-electrons (do not copy that wording: it is bad). It is this proximity to the nucleus and the consequential lesser extension of the orbitals into space that draws electrons into them, destabilising the higher oxidation states and stabilising slightly lower ones.