In the complex ion $\left[Cu\left(CN\right)_{4}\right]^{3-}$ the hybridization state, oxidation state and number of unpaired electrons of copper are respectively
- $dsp^{2},+1,1$
- $sp^{3},+1,Zero$
- $sp^{3},+2,1$
- $dsp^{3}, +2, Zero$
The Correct Option is B
Solution and Explanation
$cu^{+}$ ground state=CN $\left(-\right)$is strong field ligand, $\Delta$ is high
Hybridisation $=sp^{3};$oxidation state of Cu = +1
Number of unpaired electron = 0
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Concepts Used:
Coordination Compounds
A coordination compound holds a central metal atom or ion surrounded by various oppositely charged ions or neutral molecules. These molecules or ions are re-bonded to the metal atom or ion by a coordinate bond.
Coordination entity:
A coordination entity composes of a central metal atom or ion bonded to a fixed number of ions or molecules.
Ligands:
A molecule, ion, or group which is bonded to the metal atom or ion in a complex or coordination compound by a coordinate bond is commonly called a ligand. It may be either neutral, positively, or negatively charged.