As we can see in this question.
The stability depends on the charge density of the metal Ion that is in the central.
the charge density of Fe 3+ is more than Fe 2+.
that's why,
K3[Fe(CN)6] is more stable than K4[Fe(CN)6].
It states that the one will be more stable who has the highest charge on the central atom and then the highest stability of complex.
Answer:
K₄[Fe(CN)₆ ]₂ is more stable than k₃[Fe(CN)₆]
Explanation:
As we know that factors affecting thermodynamic satability of complex
(1) oxidation no of central metal Or charge density of metal ∝ stability
So,(I) K₄[Fe(CN)₆]₂
Let fe has oxidation no. x
we know that k have (+1) oxidation no.
and (CN) have (-1) oxidation no.
So Fe have +4 oxidation no. in complex K₄[Fe(CN)₆]₂
Now, (II) k₃[Fe(CN)₆]
let Fe has oxidation no. x
and we know k have (+1) oxidation no.
(CN) have (-1) oxidation .
so Fe have +3 oxidation no. in complex k₃[Fe(CN)₆]
so clearly, ,(I) K₄[Fe(CN)₆]₂ is more stable than k₃[Fe(CN)₆]
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in other case , When at the place of k₄[CN)₆]₂ is k₄[CN)₆] then, k₃[(CN)₆] will be more stable
because in complex k₄[Fe(CN)₆] central metal (Fe) have only +2 oxidation state or charge density
k₄[CN)₆] = 1*4+ x + 6*(-1)=0
k₃[Fe(CN)₆] = 1*3+ x + 6*(-1)
so, , in complex k₃[Fe(CN)₆] central metal (Fe) have +3 oxidation state or charge density .
So, in this case k₃[Fe(CN)₆] will be more stable than k₄[Fe(CN)₆]
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Answers & Comments
ANSWER ⤵️
As we can see in this question.
The stability depends on the charge density of the metal Ion that is in the central.
the charge density of Fe 3+ is more than Fe 2+.
that's why,
K3[Fe(CN)6] is more stable than K4[Fe(CN)6].
It states that the one will be more stable who has the highest charge on the central atom and then the highest stability of complex.
Answer:
K₄[Fe(CN)₆ ]₂ is more stable than k₃[Fe(CN)₆]
Explanation:
As we know that factors affecting thermodynamic satability of complex
(1) oxidation no of central metal Or charge density of metal ∝ stability
So,(I) K₄[Fe(CN)₆]₂
Let fe has oxidation no. x
we know that k have (+1) oxidation no.
and (CN) have (-1) oxidation no.
So Fe have +4 oxidation no. in complex K₄[Fe(CN)₆]₂
Now, (II) k₃[Fe(CN)₆]
let Fe has oxidation no. x
and we know k have (+1) oxidation no.
(CN) have (-1) oxidation .
so Fe have +3 oxidation no. in complex k₃[Fe(CN)₆]
so clearly, ,(I) K₄[Fe(CN)₆]₂ is more stable than k₃[Fe(CN)₆]
______________________________
_______________________________
in other case , When at the place of k₄[CN)₆]₂ is k₄[CN)₆] then, k₃[(CN)₆] will be more stable
because in complex k₄[Fe(CN)₆] central metal (Fe) have only +2 oxidation state or charge density
k₄[CN)₆] = 1*4+ x + 6*(-1)=0
k₃[Fe(CN)₆] = 1*3+ x + 6*(-1)
so, , in complex k₃[Fe(CN)₆] central metal (Fe) have +3 oxidation state or charge density .
So, in this case k₃[Fe(CN)₆] will be more stable than k₄[Fe(CN)₆]