In the complexes $[Fe {(H_{2} O)}_{6}]^{+ 3}, [Fe {(CN)}_{6}]^{3 -}, [Fe {(C_{2} O_{4})}_{3}]^{3 -} and {[{FeCl}_{6}]}^{3 -}$ , more stability is shown by :

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Solution

Stability of complex comparison:
The stability comparison among the given complexes can be done on the basis of the chelation.
The complexes forming chelation rings among structures are said to be more stable than the others.
Only the complexes having bident or polydentate ligand can form a chelate complex.
Generally, metal chelates are more stable than non-chelates complexes.
$[Fe {(H_{2} O)}_{6}]^{+ 3}$
For this complex the ligand $H_{2} O$ is monodentate forming an octahedral complex hence, there is no chelate ring formation happens in the structure which can be shown as;
$[Fe {(CN)}_{6}]^{- 3}$
For the given complex also the ligand $CN$ is monodentate hence forming an octahedral complex but with no chelation, which can be shown as;
${[Fe {(C_{2} O_{4})}_{3}]}^{3 -}$
For this complex, Oxalate is a bidentate ligand and forms a five-member ring with a metal atom.
Hence among the given complexes, ${[Fe {(C_{2} O_{4})}_{3}]}^{3 -}$ complex is more stable. the structure for which can be shown as;
${[{FeCl}_{6}]}^{- 3}$
For this complex the ligand $Cl$ is monodentate, forming an octahedral complex hence there is no chelate ring formation happens in the structure which can be shown as;
Hence, In the complexes $[Fe {(H_{2} O)}_{6}]^{+ 3}, [Fe {(CN)}_{6}]^{3 -}, [Fe {(C_{2} O_{4})}_{3}]^{3 -} and {[{FeCl}_{6}]}^{3 -}$ , more stability is shown by: ${[Fe {(C_{2} O_{4})}_{3}]}^{3 -}$ .

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Similar questions

Q. In the complex

[F e (H_{2} O)_{6}]^{3 +}

[F e (S C N)_{6}]^{3 -}

[F e (C_{2} O_{4})_{3}]^{3 -}

and

[F e C l_{6}]^{3 -}

, more stability is shown by :

Complete the following table

Element	Atomic number $(Z)$	Mass number $(A)$	Number of protons	Number of electrons $(e)$	Number of neutrons $(n)$
$F$

Q. Which of the following is more stable complex and why?

{[C o {(N H_{3})}_{6}]}^{3 +}

and

{[C o {(e n)}_{3}]}^{3 +}

Q. In the complexes

[F e (H_{2} O)_{6}]^{3 +}, [F e (C N)_{6}]^{3 -}, [F e (C_{2} O_{4})_{3}]^{3 -}

and

[F e C l_{6}]^{3 -}

, more stability is shown by :

Consider a $70 %$ efficient hydrogen-oxygen cell working under the standard condition at $1$ bar and $298$ K. Its cell reaction is

$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l)$

The work derived from the cell on the consumption of $1.0 \times 10^{- 3}$ $mol of H_{2} (g)$ is used to compress $1.00 mol$ of a monoatomic ideal gas in a thermally insulated container. What is the change in the temperature (in $K$ ) of the ideal gas?

The standard reduction potentials for the two half-cells are given below

$O_{2} (g) + 4 H^{+} (aq) + 4 e^{-} \to 2 H_{2} O (l)$ , $E^{0}$ = $1.23 V$

$2 H^{+} (aq) + 2 e^{-} \to H_{2} (g)$ , $E^{0}$ = $0.00 V$

Use $F = 96500 {Cmol}^{- 1}$ , $R = 8.314 {Jmol}^{- 1} K^{- 1}$ .

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In the complexes [Fe(H2O)6]+3,[Fe(CN)6]3−,[Fe(C2O4)3]3−and[FeCl6]3−, more stability is shown by :

In the complexes $[Fe {(H_{2} O)}_{6}]^{+ 3}, [Fe {(CN)}_{6}]^{3 -}, [Fe {(C_{2} O_{4})}_{3}]^{3 -} and {[{FeCl}_{6}]}^{3 -}$ , more stability is shown by :