Final answer:
CrO3 acts as an oxidizing agent by going from a +5 to +7 oxidation state, gaining electrons, while WO3 does not typically act as an oxidizing agent due to the stability of tungsten in its typical oxidation state.
Step-by-step explanation:
The question revolves around the difference in ionization energy and coordination aspects between chromium trioxide (CrO3) and tungsten trioxide (WO3). In a reaction environment, CrO3 exhibits a change where the chromium atom goes from a +5 to a +7 oxidation state, indicating its ability to act as an oxidizing agent.
This is because CrO3 is capable of accepting electrons, as it goes from CrO3 to CrO4-, gaining two electrons in the process. Conversely, WO3 does not typically act as an oxidizing agent due to the relative stability of tungsten in the +6 oxidation state and lesser ease in changing oxidation states compared to chromium.
Accordingly, the difference in ionization energy and coordination aspects between CrO3 and WO3 contributes to the fact that: b) CrO3 is an oxidizing agent, while WO3 is not.
This is in line with the general trend that elements of the second and third transition series, such as tungsten, are more stable in higher oxidation states and have a larger atomic radius, making it more challenging to remove electrons compared to elements of the first series, like chromium.