Allessandro Volta produced the world’s first electric battery in 1799, although he only reported his achievement a year later. He reputedly said ‘I myself, joking aside, am amazed. Amazed how pure and simple electricity caused by the contact of metals could have produced so much excitement.’ We still marvel at the flow of electrons inside battery cells, and dedicate this post to explaining how this works.
Electricity is the Flow or Electrons Plain and Simple
A battery comprises one or more electrochemical cells. Each of these contains two electrodes, with an electrolyte filter between them. One of these electrodes contains electrons holding charge.
When stored electricity flows from the battery through an external device, the electrons move to the other electrode. Meanwhile a counterbalancing flow of ions occurs within the battery. When the flow of electrons inside the battery cell ceases, the battery is flat.
Most battery types are rechargeable nowadays. In electrochemical terms this means sending the electrons back to the original terminal. The electrodes are generally different types of metals to induce this process.
Reverse Flow of Electrons Inside Battery Cells
Rechargeable batteries have chemistry allowing reverse electron flow. This reinstates the cell(s) to their original state, so they can start delivering electricity again. However, this process is not perfect, because each ‘cycle’ wears the electrodes out a little. Driving a battery too hard speeds this process.
There are two take-away lessons to learn from this. In the first instance, we should only recharge batteries when they are low. And secondly, we should never ‘drive a battery too hard’ by overloading it. Longer battery life depends on us respecting this.
Scientists continue to explore ways to make better batteries that last longer. Much of this work focuses on exploring new electrodes and electrolytes. This one of the themes we follow on this blog, and we find it a constantly expanding world.
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