In lecture I was taught that, in a galvanic cell at standard conditions, platinum is often used as an inert electrode when the species being oxidized or reduced exists only in solution, because platinum is "inert," which means it is very stable at its oxidation state and resists reduction or oxidation. This concept confuses me, because "Reduction" means to lose charge, a.k.a. gain an electron(s). When the electrode has an electron passing through it in order to be transferred to another material, isn't it being reduced, albeit for a very miniscule amount of time?
For example, consider a galvanic cell with platinum electrodes and an iron wire. If we were to examine the cell at an instant and examine the platinum electrodes/wire, we would see a charge of -1 on some of the platinum atoms and iron wire, correct?
What I'd like to imagine is that, while platinum is capable of having a negative charge because of the room for electrons in its d-block, the species being reduced in the half-cell will always have a higher affinity for accepting the electron due to its higher standard reduction potential. This still leaves me confused on why platinum is willing to accept the electron and thus making platinum a medium for electron transfer in the first place, though. This all applies to the iron wire (or any other element that may be used for electron transfer) as well, but I would like to tackle the case of platinum overall.