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But in graphene, the pi electron clouds can slosh back and forth. Electrons may accumulate in some regions (making them negative) and deplete in others (making them positive). Click the "Toggle Bonds" button to see this.
Now, if along one sheet of graphene the net charge is + - + it can induce a wave of - + - charge on a parallel sheet of graphene. The + areas on one sheet then attract the - areas on the other (and vice versa). This attraction can pull sheets together in a weaker form of "van der Waals" bonding.
The resulting stacks of graphene form graphite. Because of the weak bonding, sheets can slide and pull apart. So, in addition to being an electrical conductor, graphite is a lubricant.
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