Hope this helps clear the S.S. to Alum. misinfo!
Galvanic Corrosion
Because corrosion is an electrochemical process involving the flow of electric current, corrosion can be generated by a galvanic effect which arises from the contact of dissimilar metals in an electrolyte (an electrolyte is an electrically conductive liquid, I.E. Salt Water). In fact three conditions are required for galvanic corrosion to proceed; the two metals must be widely separated on the galvanic series (Most S.S. and Alum. are very close) they must be in electrical contact and their surfaces must be bridged by an electrically conducting fluid. Removal of any of these three conditions will prevent galvanic corrosion.
The obvious means of prevention is to avoid mixed metal fabrications. Frequently this is not practical, but prevention can also be by removing the electrical contact - this can be achieved by the use of plastic or rubber washers or sleeves, or by ensuring the absence of the electrolyte such as by improvement to draining or by the use of protective hoods. This effect is also dependent upon the relative areas of the dissimilar metals. If the area of the less noble material is large compared to that of the more noble (cathodic) the corrosive effect is greatly reduced, and may in fact become negligible. Conversely a large area of noble metal in contact with a small area of less noble will accelerate the galvanic corrosion rate.
For example it is common practice to fasten aluminium sheets with stainless steel screws, but aluminium screws in a large area of stainless steel are likely to rapidly corrode.
See clear as mud!
Use S.S. anytime you want in Alum.!!!!
Disclaimer'
The above was copied from my College notes, when I was in Metalurgy. circa 1973
