Match the complexed listed column `-I` with type of hybridisation listed in column `-II` and select the correct answer using the code given below the lists `:`
`{:(,"Column"-I,,"Column"-II,),((a),[AuF_(4)]^(-),,(p)" "dsp^(2)"hybridisation",),((b),[Cu(CN)_(4)]^(3-),,(q)" "sp^(3)"hybridisation",),((c ),[Co(NH_(3))_(6)]^(3+),,(r)" "sp^(3)d^(2)"hybridisation",),((d),[Fe(H_(2)O)_(5)NO]^(2+),,(s)" "d^(2)sp^(3)"hybridisation",):}`

Options

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

Explanation

To solve the problem of matching the complexes in Column I with their corresponding hybridization types in Column II, we will analyze each complex individually and determine their hybridization based on the oxidation states and the nature of the ligands involved.

### Step-by-Step Solution:

1. **Identify the Complex: [AuF₄]⁻**
- **Oxidation State of Au**: In this complex, the oxidation state of Au is +3.
- **Electron Configuration**: The electron configuration of Au in +3 oxidation state is 5d⁸ (6s is empty).
- **Hybridization**: Since Au has 8 electrons in the d-orbitals and can utilize the s and p orbitals for bonding, it undergoes **dsp² hybridization**.
- **Match**: This corresponds to option (p).

2. **Identify the Complex: [Cu(CN)₄]³⁻**
- **Oxidation State of Cu**: In this complex, the oxidation state of Cu is +1.
- **Electron Configuration**: The electron configuration of Cu in +1 oxidation state is 3d¹⁰ (4s is empty).
- **Hybridization**: With a completely filled d-orbital, Cu can only use its s and p orbitals for bonding, leading to **sp³ hybridization**.
- **Match**: This corresponds to option (q).

3. **Identify the Complex: [Co(NH₃)₆]³⁺**
- **Oxidation State of Co**: In this complex, the oxidation state of Co is +3.
- **Electron Configuration**: The electron configuration of Co in +3 oxidation state is 3d⁵.
- **Hybridization**: NH₃ is a strong field ligand, which causes pairing of electrons. Therefore, Co can use the paired d-orbitals along with s and p orbitals, leading to **d²sp³ hybridization**.
- **Match**: This corresponds to option (s).

4. **Identify the Complex: [Fe(H₂O)₅NO]²⁺**
- **Oxidation State of Fe**: In this complex, the oxidation state of Fe is +2.
- **Electron Configuration**: The electron configuration of Fe in +2 oxidation state is 3d⁶.
- **Hybridization**: H₂O is a weak field ligand, which does not cause pairing of electrons. Therefore, Fe uses its s and p orbitals along with the d-orbitals, leading to **sp³d² hybridization**.
- **Match**: This corresponds to option (r).

### Summary of Matches:
- (a) [AuF₄]⁻ → (p) dsp² hybridization
- (b) [Cu(CN)₄]³⁻ → (q) sp³ hybridization
- (c) [Co(NH₃)₆]³⁺ → (s) d²sp³ hybridization
- (d) [Fe(H₂O)₅NO]²⁺ → (r) sp³d² hybridization

### Final Answer:
The correct matching is:
- a → p
- b → q
- c → s
- d → r

Thus, the answer code is **P Q S R**.