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![[Post New]](/templates/default/images/icon_minipost_new.gif) 16 Feb 2008 19:00:37 IST
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With reference to oxides of 15 th group element The oxide in higher oxidation of the element is more acididc than tat of lower oxidation state. Their acidic character decreases down the group. Can u pls xplain d abov statement..
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16 Feb 2008 19:02:16 IST
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as the oxidation state increases acidic nature also increases. it is fact
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16 Feb 2008 19:06:43 IST
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as the oxidation state increases,the positive charge on thethe element increases,tendencyto accept electrons increases, and thus acidic character increases..
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16 Feb 2008 19:10:19 IST
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Good answer @yuiop
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well the above answers are logical but not correct...
the actual reason is inert pair effect....
we knw that grp 15 elements general configuration is ns2 ns3
and by the defination of INERT PAIR EFFECT:
s-electrons don't participate as we go down the group so..commpare the stability:
Sb+3 < Sb +5
Bi +3 > Bi+5
bcoz Bi wouldn't want its s-electrons to participate...so it'll be stable in +3 state only.
its oxides wil be sesquioxides ie....in the form on X2O3..(X=element of grp 15)
now as per the question...
Bi in Bi2O3 will be in +3 oxidation state...which is less stable than +5..
so it will act as a strong reducing agent and get oxidized itself...
STRONG REDUCING AGENT ie... more BASIC NATURE...
more the tendency to reduce more is the BASIC NATURE and more less is the Acidic nature....
and now when it comes to Sb2O3... it is iin +3 oxidation state whichz more stable than +5 oxidation state..so it won't act as an reducing agent(it will be acidic..)...
hence Bi2O3 will show basic nature.. and not Sb2O3 acidic.....
trend of stability:
As+5 > Sb +5 > Bi+5
As+3 < Sb +3
Bi2O3 will be the most basic...
u can never count out inert pair effect...it must always be given priority...
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16 Feb 2008 22:45:13 IST
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@svj29 dude ...tat was jus an execellent answer..... .....................n xactly wht i needed !!!! Thank u so much....i realy wish i cud rate u mor.... Cheers !! 
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