k3 [al(c2o4)3] hybridization state? According to. VBT theory Slove on the page plzzzz
Question:
Find the hybridization state of K₃[Al(C₂O₄)₃] according to VBT.
Solution:
Given complex:
K₃[Al(C₂O₄)₃]
Complex ion = [Al(C₂O₄)₃]³⁻
Central metal atom = Al
Ligand = Oxalate ion (C₂O₄)²⁻
Oxalate is a bidentate ligand.
One oxalate ligand donates 2 lone pairs.
Number of oxalate ligands = 3
Therefore,
Coordination number = 3 × 2
= 6
Now determine oxidation state of Al:
Let oxidation state of Al = x
x + 3(-2) = -3
x – 6 = -3
x = +3
So metal ion is:
Al³⁺
Electronic configuration of Al:
Al = 1s² 2s² 2p⁶ 3s² 3p¹
Electronic configuration of Al³⁺:
Al³⁺ = 1s² 2s² 2p⁶
For coordination number 6,
hybridization can be:
d²sp³ or sp³d²
Since Al³⁺ has no occupied 3d electrons,
outer orbitals are used:
3s + 3p + 2d
Therefore,
Hybridization = sp³d²
Geometry = Octahedral
Final Answer:
Hybridization of K₃[Al(C₂O₄)₃] = sp³d²
Geometry = Octahedral
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The hybridization of the complex ion [Al(C₂O₄)₃]³⁻ according to VBT is d²sp³, and the geometry is octahedral.
Let’s solve the hybridization of the coordination complex K₃[Al(C₂O₄)₃] step-by-step using Valence Bond Theory (VBT) in easy language and with proper reasoning on one page.
📘 What is the Hybridization of K₃[Al(C₂O₄)₃] According to VBT?
🔹 Step 1: Identify the Central Metal Ion
The central metal is Aluminium (Al).
K₃[Al(C₂O₄)₃] means:
- 3 potassium ions (K⁺)
- 1 complex ion: [Al(C₂O₄)₃]³⁻
So, Al³⁺ is the central ion in the complex.
🔹 Step 2: Write Electronic Configuration of Al³⁺
Atomic number of Al = 13
So, Al: 1s² 2s² 2p⁶ 3s² 3p¹
Al³⁺ means 3 electrons removed → from 3s and 3p
So, Al³⁺ = 1s² 2s² 2p⁶ → [Ne] → completely filled 2nd shell, no electrons in 3rd shell.
👉 It has no unpaired electrons but can still form coordination bonds by accepting lone pairs.
🔹 Step 3: Identify the Ligand and Its Type
Oxalate ion (C₂O₄²⁻) is a bidentate ligand (donates 2 lone pairs per ligand).
We have 3 oxalate ligands → total 6 donor atoms (6 bonds).
So, the coordination number = 6
🔹 Step 4: Hybridization Required
Coordination number 6 → needs 6 orbitals to bond.
According to VBT:
| Coordination Number | Hybridization | Geometry |
|---|---|---|
| 6 | d²sp³ | Octahedral |
👉 So, Al³⁺ will use:
- 2 empty d-orbitals
- 1 s-orbital
- 3 p-orbitals
Total = 6 orbitals = d²sp³ hybridization
🔹 Step 5: Final Answer with Geometry
- Hybridization of Al³⁺ = d²sp³
- Geometry = Octahedral
- Magnetism = Diamagnetic (no unpaired electrons)
✅ Final Answer:
The hybridization of the complex ion [Al(C₂O₄)₃]³⁻ according to VBT is d²sp³, and the geometry is octahedral.
