Why Does NH3 Form Complex Ions with Transition Elements But NH4 Does Not?

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NH3 readily forms complex ions with transition elements due to its ability to act as a Lewis base, donating a lone pair of electrons to form coordinate bonds. In contrast, NH4+ does not form such complexes because it lacks the lone pair necessary for bonding; the additional hydrogen atom in NH4+ results in a fully occupied valence shell, leaving no unpaired electrons available for bonding interactions. This difference in electron configuration and bonding capability explains the contrasting behavior of NH3 and NH4+ in complex ion formation.
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I am taking this correspondence course, i ran into this question and I think i know the answer but I'm not sure.
Why is it that NH3 readily forms complex ions with the transition elements but NH4 does not?
I think it is because of the extra bond with Hydrogen, therefore there is less unpaired d electrons but I'm not sure.
 
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