In complex A, there is more number of unpaired electron therefore, it exhibits the highest paramagnetic behaviour.


Hence, the correct option is A.

Introduction:
Paramagnetic behavior refers to the property of a substance to be attracted to an external magnetic field. It is observed in compounds that have unpaired electrons. In this context, we will analyze the given complexes and determine which one exhibits the highest paramagnetic behavior.

Analysis:
To determine the paramagnetic behavior, we need to consider the number of unpaired electrons present in each complex. The complex with the highest number of unpaired electrons will exhibit the highest paramagnetic behavior.

Let's analyze each complex individually:

[Co(ox)2(OH)2]-:
- The oxidation state of cobalt (Co) in this complex is +3.
- The ligands are oxalate (ox) and hydroxide (OH).
- Cobalt has a d^6 electron configuration, and in the +3 oxidation state, it loses three electrons.
- The oxalate ligands are neutral, and each contributes two electrons to the coordination sphere.
- The hydroxide ligands are also neutral, and each contributes one electron.
- Therefore, the total number of electrons in the coordination sphere is 6 + 2 + 2 + 2 = 12.
- As cobalt has a d^6 configuration, all the electrons are paired, resulting in zero unpaired electrons.
- Hence, this complex is diamagnetic.

[Ti(NH3)6]3:
- The oxidation state of titanium (Ti) in this complex is +3.
- The ligands are ammonia (NH3).
- Titanium has a d^1 electron configuration, and in the +3 oxidation state, it loses three electrons.
- Each ammonia ligand is a neutral donor and contributes one electron.
- Therefore, the total number of electrons in the coordination sphere is 1 + 1 + 1 + 1 + 1 + 1 = 6.
- As titanium has a d^1 configuration, there is one unpaired electron.
- Hence, this complex is paramagnetic.

[V(gly)2(OH)2(NH3)2]:
- The oxidation state of vanadium (V) in this complex is +3.
- The ligands are glycine (gly), hydroxide (OH), and ammonia (NH3).
- Vanadium has a d^2 electron configuration, and in the +3 oxidation state, it loses three electrons.
- The glycine ligands are neutral, and each contributes two electrons to the coordination sphere.
- The hydroxide ligands are also neutral, and each contributes one electron.
- The ammonia ligands are neutral, and each contributes one electron.
- Therefore, the total number of electrons in the coordination sphere is 2 + 2 + 1 + 1 + 1 + 1 = 8.
- As vanadium has a d^2 configuration, there are two unpaired electrons.
- Hence, this complex is paramagnetic.

[Fe(en)(bpy)(NH3)2]2:
- The oxidation state of iron (Fe) in this complex is +2.
- The ligands are ethylenediamine (en), bipyridine (bpy), and ammonia (NH3).
- Iron has a d^6 electron configuration, and in the +2 oxidation state, it loses two electrons.
- The ethy