Select the correct statement from the following?

Options

A. `[Sc(H_(2)O)_(6)]^(3+) and [Ti(H_(2)O)_(6)]^(3+)` both are colourless
B. `[Co(NH_(3))_(4)Br_(2)]Cl` show ionization isomers and geometrical isomers
C. `[Pd(NO_(2))_(2)(NH_(3))_(2)]` is square planar and shows geometrical as well as linkage isomers
D. Both (2) and (3) are correct

Answer

To solve the question, we need to analyze the statements regarding the complexes mentioned and determine which ones are correct. Let's break this down step by step.

### Step 1: Analyze the first statement about Scandium and Titanium complexes

1. **Scandium Complex**:
- Scandium in the +3 oxidation state has the electron configuration of Argon (Ar), which means it has no unpaired electrons. Therefore, it is colorless.

2. **Titanium Complex**:
- Titanium in the +3 oxidation state has the electron configuration of Argon 3d¹, which means it has one unpaired electron. Therefore, it is colored.

**Conclusion**: The statement claiming both complexes are colorless is incorrect because the titanium complex is colored.

### Step 2: Analyze the second statement about Cobalt Complex

1. **Cobalt Complex**:
- The complex is described as tetraamino-dibromo-chloro cobalt.
- It has the potential to show both ionization isomerism (by shifting ions between the complex and counter ions) and geometrical isomerism (cis and trans forms due to the arrangement of ligands around the cobalt center).

**Conclusion**: This statement is correct as it can indeed show both types of isomerism.

### Step 3: Analyze the third statement about Palladium Complex

1. **Palladium Complex**:
- The complex is described as di-nitro and di-amino palladium.
- It is stated to be square planar and can show both geometrical isomerism (cis and trans) and linkage isomerism (due to the nitro group being able to coordinate through nitrogen or oxygen).

**Conclusion**: This statement is also correct as it can show both types of isomerism.

### Final Conclusion

Based on the analysis:
- The first statement is incorrect.
- The second and third statements are correct.

Thus, the correct answer is that statements 2 and 3 are correct.

### Answer: Option D (Statements 2 and 3 are correct)

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