Question:
Which of the following have tetrahedral structures?
Which of the following have tetrahedral structures?
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For $d^8$ configuration of central metal ions like $\text{Ni}^{2+}$:
- Strong-field ligands (e.g., $\text{CN}^-$) result in square planar geometry ($\text{dsp}^2$).
- Weak-field ligands (e.g., $\text{Cl}^-$) result in tetrahedral geometry ($\text{sp}^3$).
- Strong-field ligands (e.g., $\text{CN}^-$) result in square planar geometry ($\text{dsp}^2$).
- Weak-field ligands (e.g., $\text{Cl}^-$) result in tetrahedral geometry ($\text{sp}^3$).
Updated On: May 28, 2026
- $[\text{Ni}(\text{CN})_4]^{2-}$
- $[\text{Ni}(\text{CO})_4]$
- $[\text{NiCl}_4]^{2-}$
- $\text{CrO}_4^{2-}$
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The Correct Option is B, C, D
Solution and Explanation
Step 1: Understanding the Question:
We need to determine which of the given coordination complexes and molecular ions possess a tetrahedral spatial geometry.
Step 2: Detailed Explanation:
Let us analyze the geometry and hybridization of each species:
- (A) $[\text{Ni}(\text{CN})_4]^{2-}$:
Nickel is in the $+2$ oxidation state ($\text{Ni}^{2+}$, $3d^8$ configuration).
Cyanide ($\text{CN}^-$) is a strong-field ligand, which forces the pairing of $3d$ electrons.
This frees up one $3d$ orbital, leading to $\text{dsp}^2$ hybridization and a square planar geometry. (Not tetrahedral)
- (B) $[\text{Ni}(\text{CO})_4]$:
Nickel is in the $0$ oxidation state ($\text{Ni}^0$, $3d^8 4s^2$ configuration).
Carbon monoxide ($\text{CO}$) is an exceptionally strong-field ligand, causing the relocation of the two $4s$ electrons into the $3d$ subshell.
This results in a filled $3d^{10}$ configuration, leaving the $4s$ and $4p$ orbitals vacant for $\text{sp}^3$ hybridization, producing a tetrahedral structure. (Tetrahedral)
- (C) $[\text{NiCl}_4]^{2-}$:
Nickel is in the $+2$ oxidation state ($\text{Ni}^{2+}$, $3d^8$ configuration).
Chloride ($\text{Cl}^-$) is a weak-field ligand and cannot cause electron pairing.
The empty $4s$ and $4p$ orbitals undergo $\text{sp}^3$ hybridization, resulting in a tetrahedral geometry. (Tetrahedral)
- (D) $\text{CrO}_4^{2-}$ (chromate ion):
Chromium is in the $+6$ oxidation state ($\text{Cr}^{6+}$, $3d^0 4s^0$ configuration).
It undergoes $\text{d}^3\text{s}$ (or $\text{sp}^3$) hybridization utilizing empty $d$-orbitals, forming four equivalent $\sigma$ bonds with oxygen atoms in a highly symmetric tetrahedral shape. (Tetrahedral)
Thus, (B), (C), and (D) have tetrahedral structures.
Step 3: Final Answer:
The correct options are (B), (C), and (D).
We need to determine which of the given coordination complexes and molecular ions possess a tetrahedral spatial geometry.
Step 2: Detailed Explanation:
Let us analyze the geometry and hybridization of each species:
- (A) $[\text{Ni}(\text{CN})_4]^{2-}$:
Nickel is in the $+2$ oxidation state ($\text{Ni}^{2+}$, $3d^8$ configuration).
Cyanide ($\text{CN}^-$) is a strong-field ligand, which forces the pairing of $3d$ electrons.
This frees up one $3d$ orbital, leading to $\text{dsp}^2$ hybridization and a square planar geometry. (Not tetrahedral)
- (B) $[\text{Ni}(\text{CO})_4]$:
Nickel is in the $0$ oxidation state ($\text{Ni}^0$, $3d^8 4s^2$ configuration).
Carbon monoxide ($\text{CO}$) is an exceptionally strong-field ligand, causing the relocation of the two $4s$ electrons into the $3d$ subshell.
This results in a filled $3d^{10}$ configuration, leaving the $4s$ and $4p$ orbitals vacant for $\text{sp}^3$ hybridization, producing a tetrahedral structure. (Tetrahedral)
- (C) $[\text{NiCl}_4]^{2-}$:
Nickel is in the $+2$ oxidation state ($\text{Ni}^{2+}$, $3d^8$ configuration).
Chloride ($\text{Cl}^-$) is a weak-field ligand and cannot cause electron pairing.
The empty $4s$ and $4p$ orbitals undergo $\text{sp}^3$ hybridization, resulting in a tetrahedral geometry. (Tetrahedral)
- (D) $\text{CrO}_4^{2-}$ (chromate ion):
Chromium is in the $+6$ oxidation state ($\text{Cr}^{6+}$, $3d^0 4s^0$ configuration).
It undergoes $\text{d}^3\text{s}$ (or $\text{sp}^3$) hybridization utilizing empty $d$-orbitals, forming four equivalent $\sigma$ bonds with oxygen atoms in a highly symmetric tetrahedral shape. (Tetrahedral)
Thus, (B), (C), and (D) have tetrahedral structures.
Step 3: Final Answer:
The correct options are (B), (C), and (D).
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