Two complexes [Cr(H_2O)_6]Cl_3 (A) and [Cr(N | vedclass

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(A) The colour observed is the complementary colour of the light absorbed by the complex.$ \Delta_0 $ is calculated from the energy of the absorbed li

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$ \Delta_0 $ values of $(A)$ and $(B)$ are calculated from the energies of violet and yellow light,respectively

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(A) The colour observed is the complementary colour of the light absorbed by the complex.$ \Delta_0 $ is calculated from the energy of the absorbed light,not the emitted (observed) light.Since $(A)$ is violet,it absorbs yellow light,and since $(B)$ is yellow,it absorbs violet light.Therefore,the statement that $ \Delta_0 $ values are calculated from the energies of violet and yellow light respectively is incorrect.

List-$I$ (Electronic configuration of tetrahedral metal ion)	List-$II$ (Crystal Field Stabilization Energy $(\Delta_t)$)
$A$. $d^2$	$I$. $-0.6$
$B$. $d^4$	$II$. $-0.8$
$C$. $d^6$	$III$. $-1.2$
$D$. $d^8$	$IV$. $-0.4$

Two complexes $[Cr(H_2O)_6]Cl_3 \ (A)$ and $[Cr(NH_3)_6]Cl_3 \ (B)$ are violet and yellow coloured respectively. The incorrect statement regarding them is

Similar Questions

Match the $LIST$-$I$ with $LIST$-$II$:

List-$I$ (Electronic configuration of tetrahedral metal ion) List-$II$ (Crystal Field Stabilization Energy $(\Delta_t)$)

$A$. $d^2$ $I$. $-0.6$

$B$. $d^4$ $II$. $-0.8$

$C$. $d^6$ $III$. $-1.2$

$D$. $d^8$ $IV$. $-0.4$

Among the following species,the one which causes the highest $CFSE, \Delta _0$ as a ligand is

An ion $M^{2+}$ forms the complexes $[M(H_2O)_6]^{2+}$,$[M(en)_3]^{2+}$,and $[MBr_6]^{4-}$. Match the complex with the appropriate colour.

The correct order of ligands in the spectrochemical series is

Which of the following complexes has the maximum number of unpaired electrons in the $e_g$ set of orbitals?

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