Compounds can't act as oxidizing as well as reducing
Dear student
Compounds can act as both oxidising or reducing in most cases.
Example SO2 , oxidation number of S= +4, when it converts to S, oxidation number = 0, however in SO3, ox. number=+6
since sulphur has empty d orbital so it can show higher oxidation state.
Same goes for Mn and Cl
Aluminium on the other hand does not have d- orbital thus the highest oxidation state it can exhibit is +3. So, it can only act as a reducing agent.
option d
Regards
Compounds can act as both oxidising or reducing in most cases.
Example SO2 , oxidation number of S= +4, when it converts to S, oxidation number = 0, however in SO3, ox. number=+6
since sulphur has empty d orbital so it can show higher oxidation state.
Same goes for Mn and Cl
Aluminium on the other hand does not have d- orbital thus the highest oxidation state it can exhibit is +3. So, it can only act as a reducing agent.
option d
Regards