recipes for a rechargeable electrochemical soup,
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, though,
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, battery researchers must beware of side reactions that can spoil everything.
“There’s the chemical reaction you want — the one that stores energy and releases it,
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,” Crabtree says. “But there are dozens of other … reactions that also take place.” Those side reactions can disable a battery,
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, lead to a risk of catastrophic discharge. (Consider the recent fires in Samsung’s Galaxy Note 7 smartphones.)
Early versions of the lithium-ion battery from the 1970s carried an anode made of pure lithium metal. Through repeated use, lithium ions were stripped off and replated onto the anode,
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, creating fingerlike extensions that reached across to the cathode,
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, shorting out the battery. Today’s lithium-ion batteries have an anode made of graphite (a form of carbon) so that loose lithium ions can snuggle in between sheets of carbon atoms.
Lithium-ion batteries were originally developed with small electronics in mind; they weren’t designed for storing electricity on the grid or powering electric vehicles. Electric cars need lots of power, a quick burst of energy to move from stop to start. Electric car manufacturers now bundle thousands of such batteries together to provide power for up to 200 miles before recharging, but that range still falls far short of what a tank of gas can offer. And lithium-ion batteries drain too quickly to feed long hours of demand on the grid.
Simply popping more batteries into a car or the grid isn’t the answer,
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, Crabtree says. Stockpiling doesn’t improve the charging

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