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(C) The atomic number of cobalt $(Co)$ is $27$. The electronic configuration of $Co$ is $[Ar] 3d^7 4s^2$.In the $[CoF_6]^{3-}$ complex,the oxidation s

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$4$

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(C) The atomic number of cobalt $(Co)$ is $27$. The electronic configuration of $Co$ is $[Ar] 3d^7 4s^2$.In the $[CoF_6]^{3-}$ complex,the oxidation state of $Co$ is $x + 6(-1) = -3$,so $x = +3$.The electronic configuration of $Co^{3+}$ is $[Ar] 3d^6$.In the $3d$ subshell,the $6$ electrons are distributed as follows: one orbital is doubly occupied,and the remaining four orbitals are singly occupied.Therefore,there are $4$ unpaired electrons present in the $Co^{3+}$ ion prior to hybridization.

How many unpaired electrons are present in the cobalt ion in the $+3$ oxidation state prior to hybridization in the $[CoF_6]^{3-}$ complex ion?

Similar Questions

Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory:
$(i)$ $[Fe(CN)_6]^{4-}$
$(ii)$ $[FeF_6]^{3-}$
$(iii)$ $[Co(C_2O_4)_3]^{3-}$
$(iv)$ $[CoF_6]^{3-}$

Statement $1$: $[Ti(H_2O)_6]^{4+}$ is coloured while $[Sc(H_2O)_6]^{3+}$ is colourless.
Statement $2$: $d-d$ transition is not possible in $[Sc(H_2O)_6]^{3+}$.

Write the limitations of Valence Bond Theory $(VBT)$.

In the complex $cis-[Cr(en)_2Cl_2]^+$,the oxidation state of $Cr$,the type of $d$-orbital involved in the valence shell,and the coordination number are respectively:

$A$ square planar complex is formed by the hybridization of which atomic orbitals?

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