Match the complexes given in column `-I` and the magnetic properties given in column `-II` and select the correct answer using the code below the lists `:`
`{:("Column " I,,"Column " I,,),(("Complexes"),,("Magnetic properties"),,),((a)[NiCl_(2)(PPh_(3))_(2)],,(p)"Paramagnetic with 1 unpaired electrons",,),((b)V(CO)_(6),,(q)"Paramagnetic with 2 unparied electrons",,),((c )[Cr(CN)_(6)]^(4-),,(r)"Paramagnetic with 3 unpaired electrons",,),((d)Ni(CO)_(4),,(s)"Diamagnetic",,):}`
Codes `:`

Options

A. `{:(,"(a)","(b)","(c)","(d)"),(,p,q,r,s):}`
B. `{:(,"(a)","(b)","(c)","(d)"),(,q,p,q,s):}`
C. `{:(,"(a)","(b)","(c)","(d)"),(,p,p,q,r):}`
D. `{:(,"(a)","(b)","(c)","(d)"),(,p,r,q,s):}`

Explanation

To solve the problem of matching the complexes in Column I with their corresponding magnetic properties in Column II, we will analyze each complex one by one, determining their oxidation states, electronic configurations, and magnetic properties.

### Step-by-Step Solution:

1. **Complex (a): NiCl₂(PPh₃)₂**
- **Oxidation State Calculation**:
- Let the oxidation state of Ni be \( x \).
- The equation becomes: \( x + 2(-1) + 2(0) = 0 \) (since PPh₃ is a neutral ligand).
- Thus, \( x = +2 \).
- **Electronic Configuration**:
- Ni in +2 state: \( \text{Ni}^{2+} \) has the configuration \( [Ar] 3d^8 \).
- **Magnetic Properties**:
- Since PPh₃ and Cl⁻ are weak field ligands, there will be no pairing of electrons.
- Therefore, it is **paramagnetic** with **2 unpaired electrons**.
- **Match**: (a) → (q)

2. **Complex (b): V(CO)₆**
- **Oxidation State Calculation**:
- The oxidation state of V is 0 (since CO is a neutral ligand).
- **Electronic Configuration**:
- V has the configuration \( [Ar] 4s^2 3d^3 \).
- **Magnetic Properties**:
- CO is a strong field ligand, and thus there will be no pairing of electrons.
- Therefore, it is **paramagnetic** with **3 unpaired electrons**.
- **Match**: (b) → (r)

3. **Complex (c): Cr(CN)₆⁴⁻**
- **Oxidation State Calculation**:
- Let the oxidation state of Cr be \( x \).
- The equation becomes: \( x + 6(-1) = -4 \).
- Thus, \( x = +2 \).
- **Electronic Configuration**:
- Cr in +2 state: \( [Ar] 4s^1 3d^5 \).
- **Magnetic Properties**:
- CN⁻ is a strong field ligand, which causes pairing of electrons.
- Therefore, it is **diamagnetic** (no unpaired electrons).
- **Match**: (c) → (s)

4. **Complex (d): Ni(CO)₄**
- **Oxidation State Calculation**:
- The oxidation state of Ni is 0 (since CO is a neutral ligand).
- **Electronic Configuration**:
- Ni has the configuration \( [Ar] 4s^2 3d^8 \).
- **Magnetic Properties**:
- CO is a strong field ligand, which causes pairing of electrons.
- Therefore, it is **diamagnetic** (no unpaired electrons).
- **Match**: (d) → (s)

### Final Matches:
- (a) → (q)
- (b) → (r)
- (c) → (s)
- (d) → (s)

### Summary of Matches:
- a - q: Paramagnetic with 2 unpaired electrons
- b - r: Paramagnetic with 3 unpaired electrons
- c - s: Diamagnetic
- d - s: Diamagnetic