Draw the structure of the $[Cr(CO)_6]$ complex.
(N/A) The central metal atom is Chromium $(Cr)$ with an atomic number of $24$. The electronic configuration of $Cr$ is $[Ar] 3d^5 4s^1$.
In the $[Cr(CO)_6]$ complex,the oxidation state of $Cr$ is $0$.
$CO$ is a strong field ligand,which causes pairing of electrons in the $3d$ orbitals.
The hybridization involved is $d^2sp^3$,which corresponds to an octahedral geometry.
The structure consists of a central $Cr$ atom surrounded by six $CO$ ligands arranged at the corners of an octahedron.
In the $[Cr(CO)_6]$ complex,the oxidation state of $Cr$ is $0$.
$CO$ is a strong field ligand,which causes pairing of electrons in the $3d$ orbitals.
The hybridization involved is $d^2sp^3$,which corresponds to an octahedral geometry.
The structure consists of a central $Cr$ atom surrounded by six $CO$ ligands arranged at the corners of an octahedron.
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Similar Questions
Match List-$I$ with List-$II$:
List-$I$ List-$II$ $A. K_2[Ni(CN)_4]$ $I. sp^3$ $B. [Ni(CO)_4]$ $II. sp^3d^2$ $C. [Co(NH_3)_6]Cl_3$ $III. dsp^2$ $D. Na_3[CoF_6]$ $IV. d^2sp^3$
Choose the correct answer from the options given below:
| List-$I$ | List-$II$ |
| $A. K_2[Ni(CN)_4]$ | $I. sp^3$ |
| $B. [Ni(CO)_4]$ | $II. sp^3d^2$ |
| $C. [Co(NH_3)_6]Cl_3$ | $III. dsp^2$ |
| $D. Na_3[CoF_6]$ | $IV. d^2sp^3$ |
Choose the correct answer from the options given below:
The geometries of some complex ions are given below. Select the correct answer.
$(1) [Ag(NH_3)_2]^+ - \text{Linear}$
$(2) [MnCl_4]^{2-} - \text{Tetrahedral}$
$(3) [Cu(NH_3)_4]^{2+} - \text{Square planar}$
$(4) [Ni(CN)_4]^{2-} - \text{Square planar}$
$(1) [Ag(NH_3)_2]^+ - \text{Linear}$
$(2) [MnCl_4]^{2-} - \text{Tetrahedral}$
$(3) [Cu(NH_3)_4]^{2+} - \text{Square planar}$
$(4) [Ni(CN)_4]^{2-} - \text{Square planar}$
Difficult
View SolutionThe shape of the $[Fe(CN)_6]^{4-}$ ion is:
Medium
View SolutionOn the basis of valence bond theory,discuss the geometrical shapes and magnetic properties of the following $4$-coordinated complexes:
$(i)$ $[NiCl_{4}]^{2-}$
$(ii)$ $[Ni(CN)_{4}]^{2-}$
$(iii)$ $[Ni(CO)_{4}]$
$(iv)$ $MnO_{4}^{-}$
$(i)$ $[NiCl_{4}]^{2-}$
$(ii)$ $[Ni(CN)_{4}]^{2-}$
$(iii)$ $[Ni(CO)_{4}]$
$(iv)$ $MnO_{4}^{-}$
Medium
View SolutionStatement $1$: $[Ti(H_2O)_6]^{4+}$ is coloured while $[Sc(H_2O)_6]^{3+}$ is colourless.
Statement $2$: $d-d$ transition is not possible in $[Sc(H_2O)_6]^{3+}$.
Statement $2$: $d-d$ transition is not possible in $[Sc(H_2O)_6]^{3+}$.
Medium
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