The correct order of matching of complex compound in column I with the properties in column II:
`{:(,"Column I",,"Column II",),((A),[Cr(NH_(3))_(6)]^(3+),(P),"Tetrahedral and paaramagnetic",),((B),[Co(CN)_(6)]^(3-),(Q),"Octahedral and diamagnetic",),((C ),[Ni(CN)_(4)]^(2-),(R ),"Octahedral and paramagnetic",),((D),[Ni(Cl)_(4)]^(2-),(S),"Square planar and diamagnetic",):}`

Options

A. `A-R, B-Q, C-P, d-S`
B. `A-Q, B-R, C-P, D-S`
C. `A-R, B-Q, C-S, D-P`
D. `A-Q, B-R, C-S, D-P`

Explanation

To solve the problem of matching the complex compounds in Column I with their properties in Column II, we will analyze each complex one by one, determining their geometry and magnetic properties based on the ligands and oxidation states.

### Step-by-step Solution:

1. **Identify the first complex: [Cr(NH₃)₆]³⁺**
- **Oxidation State**: Chromium (Cr) in this complex has an oxidation state of +3.
- **Electron Configuration**: The electron configuration of Cr is [Ar] 3d⁵ 4s¹. For Cr³⁺, it becomes [Ar] 3d³.
- **Unpaired Electrons**: In the 3d³ configuration, there are 3 unpaired electrons.
- **Ligand Type**: NH₃ is a weak field ligand, which means there will be no pairing of electrons.
- **Geometry**: With six ligands, the geometry is octahedral.
- **Magnetic Property**: Since there are unpaired electrons, the complex is paramagnetic.
- **Match**: This corresponds to option R ("Octahedral and paramagnetic").

2. **Identify the second complex: [Co(CN)₆]³⁻**
- **Oxidation State**: Cobalt (Co) in this complex has an oxidation state of +3.
- **Electron Configuration**: The electron configuration of Co is [Ar] 3d⁷ 4s². For Co³⁺, it becomes [Ar] 3d⁶.
- **Unpaired Electrons**: CN⁻ is a strong field ligand, which causes pairing of electrons. Thus, the configuration will have all six electrons paired.
- **Geometry**: With six ligands, the geometry is octahedral.
- **Magnetic Property**: Since there are no unpaired electrons, the complex is diamagnetic.
- **Match**: This corresponds to option Q ("Octahedral and diamagnetic").

3. **Identify the third complex: [Ni(CN)₄]²⁻**
- **Oxidation State**: Nickel (Ni) in this complex has an oxidation state of +2.
- **Electron Configuration**: The electron configuration of Ni is [Ar] 3d⁸ 4s². For Ni²⁺, it becomes [Ar] 3d⁸.
- **Unpaired Electrons**: CN⁻ is a strong field ligand, which causes pairing of electrons. Thus, all electrons will be paired.
- **Geometry**: With four ligands, the geometry is square planar.
- **Magnetic Property**: Since there are no unpaired electrons, the complex is diamagnetic.
- **Match**: This corresponds to option S ("Square planar and diamagnetic").

4. **Identify the fourth complex: [Ni(Cl)₄]²⁻**
- **Oxidation State**: Nickel (Ni) in this complex has an oxidation state of +2.
- **Electron Configuration**: The electron configuration of Ni is [Ar] 3d⁸ 4s². For Ni²⁺, it becomes [Ar] 3d⁸.
- **Unpaired Electrons**: Cl⁻ is a weak field ligand, which means there will be no pairing of electrons. Thus, there will be 2 unpaired electrons.
- **Geometry**: With four ligands, the geometry is tetrahedral.
- **Magnetic Property**: Since there are unpaired electrons, the complex is paramagnetic.
- **Match**: This corresponds to option P ("Tetrahedral and paramagnetic").

### Final Matching:
- A: [Cr(NH₃)₆]³⁺ → R ("Octahedral and paramagnetic")
- B: [Co(CN)₆]³⁻ → Q ("Octahedral and diamagnetic")
- C: [Ni(CN)₄]²⁻ → S ("Square planar and diamagnetic")
- D: [Ni(Cl)₄]²⁻ → P ("Tetrahedral and paramagnetic")

### Conclusion:
The correct order of matching is: A-R, B-Q, C-S, D-P, which corresponds to option C (RQSP).