Consider the following statements and arrange in the order of the true/false as given in the codes.
`S_1`:Both `[Co(o x )_3]^(3-)` and `[CoF_6]^(3-)` are paramagnetic.
`S_2`:`CoCl_(3)3NH_3`( Six Coordination Number ) complex is non-conducting.
`S_3`:The number of possible geometrical isomers for the complex `[Pt(NO_2)(cl) (OH)(NH_3)]` is six.
`S_4`:The oxidation state of iron in brown ring complex `[Fe(H_2O)_5NO^+`] `SO_4` is + 1 Where NO is `NO^(+)`

Options

A. F T T F
B. T T T T
C. F T F T
D. T T T F

Explanation

To solve the problem, we need to analyze each statement and determine whether it is true or false. We will then arrange the statements in the order of true/false.

### Step-by-Step Solution:

1. **Analyze Statement S1:**
- **Statement:** Both \([Co(o x )_3]^{3-}\) and \([CoF_6]^{3-}\) are paramagnetic.
- **Analysis:**
- For \([Co(o x )_3]^{3-}\): Cobalt in this complex is in the +3 oxidation state, which gives it a \(3d^6\) configuration. Since oxalate is a strong field ligand, it causes pairing of electrons. Thus, this complex is **diamagnetic** (no unpaired electrons).
- For \([CoF_6]^{3-}\): Cobalt is also in the +3 oxidation state here. Fluoride is a weak field ligand, so it does not cause pairing, resulting in unpaired electrons. Therefore, this complex is **paramagnetic**.
- **Conclusion:** Since one is diamagnetic and the other is paramagnetic, **S1 is false**.

2. **Analyze Statement S2:**
- **Statement:** CoCl\(_3\)·3NH\(_3\) (Six Coordination Number) complex is non-conducting.
- **Analysis:**
- This complex is neutral because both CoCl\(_3\) and NH\(_3\) are neutral overall. Neutral complexes do not dissociate into ions in solution, making them non-conducting.
- **Conclusion:** **S2 is true**.

3. **Analyze Statement S3:**
- **Statement:** The number of possible geometrical isomers for the complex \([Pt(NO_2)(Cl)(OH)(NH_3)]\) is six.
- **Analysis:**
- This complex has a coordination number of 4 and contains different ligands (NO\(_2\), Cl, OH, NH\(_3\)). The maximum number of geometrical isomers for a square planar complex with 4 different ligands is 2 (cis and trans). Therefore, the total number of geometrical isomers is not six.
- **Conclusion:** **S3 is false**.

4. **Analyze Statement S4:**
- **Statement:** The oxidation state of iron in the brown ring complex \([Fe(H_2O)_5NO^+]SO_4\) is +1 where NO is \(NO^+\).
- **Analysis:**
- In the complex, the sulfate ion (SO\(_4^{2-}\)) has a charge of -2. The overall charge of the complex is +2. The charge from \(NO^+\) contributes +1. The water molecules are neutral. Therefore, if we let the oxidation state of Fe be \(x\):
\[ x + 0 + 1 = +2 \implies x = +1 \]
- **Conclusion:** **S4 is true**.

### Final Arrangement:
- **S1:** False
- **S2:** True
- **S3:** False
- **S4:** True

Thus, the order of true/false statements is: **False, True, False, True**.

### Final Answer:
The correct order is: **False, True, False, True**.