What is the hybridization of the central metal ion in the complex [Cu(NH3)4]2+?
Practice Questions
1 question
Q1
What is the hybridization of the central metal ion in the complex [Cu(NH3)4]2+?
sp
sp2
sp3
dsp2
In [Cu(NH3)4]2+, the copper ion undergoes dsp2 hybridization to accommodate four ligands.
Questions & Step-by-step Solutions
1 item
Q
Q: What is the hybridization of the central metal ion in the complex [Cu(NH3)4]2+?
Solution: In [Cu(NH3)4]2+, the copper ion undergoes dsp2 hybridization to accommodate four ligands.
Steps: 6
Step 1: Identify the central metal ion in the complex [Cu(NH3)4]2+. The central metal ion is copper (Cu).
Step 2: Determine the oxidation state of copper in the complex. Since the complex has a 2+ charge and ammonia (NH3) is a neutral ligand, the oxidation state of copper is +2.
Step 3: Find the electron configuration of copper in its +2 oxidation state. The electron configuration of neutral copper (Cu) is [Ar] 3d10 4s1. For Cu2+, it loses two electrons, resulting in [Ar] 3d9.
Step 4: Count the number of ligands attached to the copper ion. There are four ammonia (NH3) ligands attached to the copper ion.
Step 5: Determine the type of hybridization needed to accommodate the four ligands. Since there are four ligands, the hybridization will be based on the d-orbitals and will be dsp2.
Step 6: Conclude that the hybridization of the central metal ion (Cu) in the complex [Cu(NH3)4]2+ is dsp2.
