Answer
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Hint: Cyanide ion is a strong ligand and strong ligands splits up the d-orbitals more.
${{t}_{2}}g$ should be filled with at least one electron in each orbitals to fill up in the higher ${{e}_{g}}$ orbital.
Complete step by step answer:
In the question it is given, a complex of Co. Co is the central metal atom and the cyanide ions are the ligands that are surrounding the Co atom, there are six cyanide ions and hence we can say that it is an octahedral complex.
- According to the spectrochemical series the cyanide ion is one of the strongest ligands carrying a charge of -1.
- And now we have to know that the Co is in which oxidation state, either we can find through the calculation method but here it is already given in the options that it is a $3{{d}^{6}}$ system.
- If it wasn’t given, then we calculate the oxidation State and find the ${{d}^{n}}$ system to which the complex belongs to.
For that in the complex give the oxidation number of Co as x.
${{\left[ Co{{\left( CN \right)}_{6}} \right]}^{3-}}$-oxidation state- $x+\left( -1 \right)(6)=-3$, x = 3
So here Co is in +3 oxidation state.
The electronic configuration of Co is -$\left[ Ar \right]3{{d}^{7}}4{{s}^{2}}$
In +3 state, it will have a configuration as $\left[ Ar \right]3{{d}^{6}}$
So the system is ${{d}^{6}}$ system.
- Now we know that in d orbitals are divided into 2 levels, ${{t}_{2}}g$ having a set of 3 orbitals ${{d}_{xy}},{{d}_{yz}},{{d}_{xz}}$ and ${{e}_{g}}$ with two orbitals ${{d}_{{{x}^{2}}-{{y}^{2}}}},{{d}_{{{z}^{2}}}}$
- As this complex is an octahedral complex, ${{t}_{2}}g$ will be the orbital with lower energy level and ${{e}_{g}}$ is the higher energy level
- As $C{{N}^{-}}$ is a strong ligand it splits up, ${{t}_{2}}g$ and ${{e}_{g}}$ in a greater energy, splitting energy is greater than the pairing energy. Pairing energy is energy required for the electrons to pair in an orbital before filling the higher energy state.
Splitting energy $\rangle $ Pairing energy
Hence the electrons pair up in the ${{t}_{2}}g$ orbital, So, the correct answer is “Option B”.
Note: If the given complex was tetrahedral i.e. with four ligands surrounding the central metal atom then the orbital with lower energy is – e and higher energy is ${{t}_{2}}$. So according to the question requirement the orbital splitting should be taken care of, and if the ligand was water, Cl etc. then they are weak ligands and splitting energy is less than the pairing energy. Hence the electrons will move to the higher orbital state without pairing.
${{t}_{2}}g$ should be filled with at least one electron in each orbitals to fill up in the higher ${{e}_{g}}$ orbital.
Complete step by step answer:
In the question it is given, a complex of Co. Co is the central metal atom and the cyanide ions are the ligands that are surrounding the Co atom, there are six cyanide ions and hence we can say that it is an octahedral complex.
- According to the spectrochemical series the cyanide ion is one of the strongest ligands carrying a charge of -1.
- And now we have to know that the Co is in which oxidation state, either we can find through the calculation method but here it is already given in the options that it is a $3{{d}^{6}}$ system.
- If it wasn’t given, then we calculate the oxidation State and find the ${{d}^{n}}$ system to which the complex belongs to.
For that in the complex give the oxidation number of Co as x.
${{\left[ Co{{\left( CN \right)}_{6}} \right]}^{3-}}$-oxidation state- $x+\left( -1 \right)(6)=-3$, x = 3
So here Co is in +3 oxidation state.
The electronic configuration of Co is -$\left[ Ar \right]3{{d}^{7}}4{{s}^{2}}$
In +3 state, it will have a configuration as $\left[ Ar \right]3{{d}^{6}}$
So the system is ${{d}^{6}}$ system.
- Now we know that in d orbitals are divided into 2 levels, ${{t}_{2}}g$ having a set of 3 orbitals ${{d}_{xy}},{{d}_{yz}},{{d}_{xz}}$ and ${{e}_{g}}$ with two orbitals ${{d}_{{{x}^{2}}-{{y}^{2}}}},{{d}_{{{z}^{2}}}}$
- As this complex is an octahedral complex, ${{t}_{2}}g$ will be the orbital with lower energy level and ${{e}_{g}}$ is the higher energy level
- As $C{{N}^{-}}$ is a strong ligand it splits up, ${{t}_{2}}g$ and ${{e}_{g}}$ in a greater energy, splitting energy is greater than the pairing energy. Pairing energy is energy required for the electrons to pair in an orbital before filling the higher energy state.
Splitting energy $\rangle $ Pairing energy
Hence the electrons pair up in the ${{t}_{2}}g$ orbital, So, the correct answer is “Option B”.
Note: If the given complex was tetrahedral i.e. with four ligands surrounding the central metal atom then the orbital with lower energy is – e and higher energy is ${{t}_{2}}$. So according to the question requirement the orbital splitting should be taken care of, and if the ligand was water, Cl etc. then they are weak ligands and splitting energy is less than the pairing energy. Hence the electrons will move to the higher orbital state without pairing.