Now it's time to consider a component that has a role in the charging system, although it's not considered part of that system.
That component is the battery, which is actually part of the starting system. (In the charging system, the alternator provides the majority of the electricity used, while in the starting system, the battery provides the majority of the electricity.)
Before looking at the batteries in our motor vehicles, lets take a brief look at the history, construction, and operation of batteries in general.
Simply put, a battery is a device that converts chemical energy into electrical energy.
Knowledge on how to make and use a battery has existed since prehistoric times. Archeological evidence indicates some prehistoric people may have made and used batteries, most likely for electroplating metals. Likewise, early philosophers (i.e., scientists) made and used batteries in their study of biology. (Fear arising from the publication of the experiments very probably led Mary Shelley to write Frankenstein.)
While this knowledge has existed for a long time; being discovered, forgotten, and rediscovered repeatedly across human history; putting this technology to wide-spread practical use is relatively recent, within the past century or so.
Basically, a battery consists of two dissimilar materials (the electrodes) separated by a substance (electrolyte) that allows (encourages?) ions to flow from one of the materials to the other. This flow of ions produces electricity.
This can be demonstrated, in a simple exercise used in schools, using a piece of copper, a piece of zinc, and a lemon. An ordinary bare copper wire and a zinc-plated nail or screw will work as electrodes and the citric acid in the lemon serves as the electrolyte. You'll need a good voltmeter (or multimeter) to detect and measure the electricity produced. Alternatively, you can connect several in series to drive a low voltage LED or a small light bulb. (A LED would be best because they will react better to low voltages than most light bulbs.)
The same can be done with a potato, with its phosphoric acid acting as the electrolyte. (You do the same with a can of cola, which also contains phosphoric acid. The aluminum can could serve as one electrode -- and a copper wire as the other -- except soda cans are lined with plastic to prevent interaction between the cola and the aluminum.)
A third possibility is a can of sauerkraut, with a copper wire inserted in the sauerkraut acting as one electrode, the tin-plated can as the other electrode, and the lactic acid in the sauerkraut serving as the electrolyte. (Look up "lemon battery" on Wikipedia if you want to know more.)
These batteries are essentially identical to the common, readily available dry cells used in flashlights, portable electronics, and toys. (Causing significant problems for parents every Christmas when they realized they overlooked the "batteries not included" statement on their children's presents.) People have actually used these to "Macgyver" a source of electricity on emergencies.
The battery we've discussed so far use an electrochemical process, called galvanic corrosion, which is essentially a one-way process. They cannot reasonably be recharged so, once their chemical energy is used up, they have to be disposed of. Adding to this limitation is the galvanic corrosion continues regardless of whether the batteries are being used or stored. Although the process occurs at a slower rate, common carbon-zinc and alkaline batteries continue losing 8-20 percent of their charge per year while in storage, starting with when they are manufactured.
The one-way, expendable nature of these batteries make them less than ideal for our primary uses in motor vehicles. We need batteries that can be discharged and recharged repeatedly. We also need them to be reliable and reasonably inexpensive in terms cost and longevity.
The batteries we use today were, in the old days, called storage batteries and are effectively the same as the batteries first used in cars when manufacturers started including electric starters. The differences between then and now are mostly limited to improvements in design and construction.
The reason we still use this somewhat ancient technology is due to significant existing manufacturing infrastructure and economy of scale, both of which help keep the price down.
Fifty years ago, motor vehicle batteries were simple. They were all flooded lead-acid (cells could be opened to add distilled water when needed) and generally only available in one size, which is known today as BCI Group 24.
Today, there's a bewildering array of size and types, such as sealed, gel, AGM, and so forth. Adding to the confusion is the way various terms are tossed about and combined, with an assumption consumers know what the dealers are talking about. (My example of types actually demonstrates this by combining two distinctly different forms of battery categorization.)
In the next installment of my ramblings, I'll try to sort out and simplify this confusion, as well as go deeper into depth about motor battery technology and use.
In the meanwhile, look up "Battery (electricity)" in Wikipedia to explore more information on batteries. (As before, following the links in this article could lead to discussions chock full of chemistry and mathematics.) Also,
Scientific American has a good overview, written in everyday English.
Before closing, I'd like to touch on two areas affected by what I've discussed above, which may be important to people reading this.
The first area is marine corrosion, which is a very important concern among boat owners and operators, leading to significant and possibly catastrophic damage. The galvanic process for batteries is exactly the same as one form of corrosion attacking boats.
Any time two different metals exist on a boat, they can create what amounts to a battery. The speed with which this causes corrosion is determined by the metals, whether they are below or above the waterline, in fresh or sea water, and whether or not the two metals are electrically connected. (Sacrificial zinc anodes are used to redirect the corrosion towards those anodes instead of other, more important and valuable components.)
One person I know severely shortened the life of his new boat, which he often used in salt water, by using stainless steel fasteners below the waterline on the aluminum hull. The aluminum hull protected the stainless steel fasteners by acting as a sacrificial anode, resulting in the hull being rapidly eaten away by galvanic corrosion.
While galvanic corrosion is a constant, on-going process varying only in terms of the speed with which it happens, a related form of marine corrosion -- electrolytic corrosion -- is just as detrimental.
As we've seen, galvanic corrosion creates electricity as an output. On the other hand, electrolytic corrosion is a form of electroplating, requiring an input of electrical current to occur.
Electrolytic corrosion is almost always the result of improper wiring, either within the boat itself or other nearby boats in a harbor.
The second area is galvanic corrosion in fasteners used to hold buildings together.
Decades ago, wood was pressure-treated using chromate copper arsenate (CCA). Irrational public fear about the arsenic component led to the use of CCA being heavily restricted and effectively phased out in the U.S.
The copper component in CCA did interact with building fasteners, causing some galvanic corrosion. However, the amount of copper in CCA is relatively small, limiting the rate of corrosion to the point where there was little concern in terms of the expected life of buildings. (The possibility of failure was much greater due to common rust, as compared to CCA.)
The issue of wood rot didn't go away with the ban on CCA so manufacturers had to use a other chemicals for pressure treating wood, such as alkaline copper quaternary (ACQ). Unfortunately, all available replacement chemicals either had significantly higher copper content, were prohibitively expensive, or ineffective against some forms of wood rot and insect infestation.
During the transition period, builders continued using the same fasteners on ACQ wood that they had used with CCA wood. The higher copper content resulted in greatly accelerated galvanic corrosion affecting the fasteners. (Galvanized fasteners only slowed things a bit because copper loves zinc, eating through it quickly before going on to attack the steel in the fastener.)
In one documented case, a builder went back to inspect houses he'd built less than a decade before and discovered the ACQ had corrode the sill plate fasteners to the point where gravity was effectively the only thing holding the houses on their foundations. I fully expect, in the near future if it hasn't already happened, a relatively mild wind storm or earthquake to cause a large number of these houses to come off their foundations while leaving older buildings in place.
The problems with ACQ and similar pressure treatment chemical has led to the larger variety of significantly more expensive fasteners, typically coated with plastic, appearing on the lumber yard and big box shelves.
This is the reason I insist on CCA wood in the house I'm building. I also use the more expensive plastic-coated fasteners to help extend the house's expected life span.
A comedian once said, "Every time a rat dies in Canada, we lose something else to eat." To that I'd add, "Every time the people in California have a hissy fit, we lose something useful and our lives get more expensive and complicated."
Okay, I'm done with my ranting โฆ someone else can have the soapbox.
1970 Explorer Class A on a 1969 Dodge M300 chassis with 318 cu. in. (split year)
1972 Executive Class A on a Dodge M375 chassis with 413 cu. in.
1973 Explorer Class A on a Dodge RM350 (R4) chassis with 318 engine & tranny from 1970 Explorer Class A