I've learnt in class that charges store up on capacitor plates (the electrons). But why don't the electrons just jump across capacitor, what stops them? At first I thought perhaps it might just be the air molecules, as they are insulating and have no charge carriers, the electrons wouldn't have enough energy to barge their way through.

How about if I had a capacitor in a vacuum though? Would the electrons just be able to leap across the capacitor because there is nothing there to stop them? If this were the case however, the capacitor could theoretically be any separation and the electrons would simply float across, which seems absurd, so there must be something stopping the electrons from leaving?

  • $\begingroup$ What makes you think that a vacuum is a conductor? A vacuum is a better insulter than air. Generally, it is the ion content of the medium that determines conductivity. (excluding known elemental conductors, like copper.) For example, pure water is a fairly good insulter. Impurities and things like salt, which breaks into its component ions, are generally why we think of water as conductive. -See: google.com/… and en.wikipedia.org/wiki/… $\endgroup$
    – CoilKid
    Mar 13, 2015 at 23:57

2 Answers 2


This is quite an interesting question.

First - air is a (poor) conductor. See this earlier answer for some details on how well (or poorly) air conducts (especially when the relative humidity increases).

Next - vacuum as an insulator. You are right that once electrons are "in space", a vacuum doesn't provide much impediment. This is why cathode ray tubes (old TVs, oscilloscopes) and other vacuum tubes could work. But you might know that these typically contain a hot cathode: a filament that is heated, and that then gives off ("evaporates") electrons. The hotter the filament, the more electrons. This is a good way to regulate current in vacuum tubes (to this day, it's how X ray tubes work!).

The analogy of "boiling off" the electrons is quite good. Just as water, when heated, will evaporate more vigorously, so electrons will escape material more readily when they are hot. And just as some liquids have lower boiling points than others, different materials have different "work functions" - the amount of energy that an electron needs to be given before it can escape.

This was demonstrated, of course, in the early 1900's when it was shown that shining light of a certain wavelength or shorter could excite electrons and cause them to escape from metals (the photoelectric effect) but that longer wavelength light, regardless of intensity, could not. This was actually later understood to be caused by the particle nature of light and one of the first piece of experimental evidence of quantum mechanics (for which Einstein got a Nobel prize).

Back to the electrons and their work function. I wrote an answer about this a while ago: that was actually more detailed, looking at the velocity distribution of electrons that do escape. Taking a step back from that, electrons in a metal behave a bit like a gas: they move around randomly, bump into each other, and their velocities follow the Boltzmann distribution. This means there are always a few highly energetic ones around - more when the metal is hot. There is a natural energy barrier keeping the electrons bound to the metal, and electrons with energy greater than that can and will escape. This is described in this wiki article.

Perhaps you have already understood that a capacitor in vacuum can also lose charge when exposed to light: so if you want your vacuum capacitor to hold charge for a long time, you have to keep it cold and dark.


The same question could be asked about electrons in atoms. Why on Earth do they remain bound to the nucleus instead of floating around freely? The answer to this question and to yours is that the nucleus (in the case of atoms) and the metal (in your case) is offering a quite cozy place for the electrons to be and leaving it is quite costly in term of energy.

From an energetic point of view, electrons have to move across a huge barrier to go to the other side and in normal capacitors the applied potential difference is simply not enough to provide this missing energy.

Sometimes however, the applied voltage can reach what is called the breakdown voltage which is a voltage that is strong enough to help the electrons climb the energetic barrier and cross the gap: this generates a spark that is not often wanted. This voltage breakdown can be due to either a too high voltage to begin with or a change in the external conditions (humidity, damaging of the electrodes etc..) that will lower the barrier to cross.

Lastly, you are right to say that the vacuum is conducting in some sense (at least in the sense that an electron in vacuum with a certain speed does not need a constant supply of energy to continue moving) and the presence of some atoms that do not favour charge transport in air can worsen the crossing of the gap. Experiments have shown that the breakdown voltage was lowered as the quality of the vacuum was increased.

  • $\begingroup$ I thought the electrons were roughly bound to nucleus because of electrostatic force (nucleus being positive)? But in the case of capacitor, don't the electrons gather all on one plate, and instead of having an attractive electrostatic force, you have repulsive because you have a buildup of negative charge? And why does such an energetic barrier exist that prevents the electrons from jumping across? thanks $\endgroup$ Mar 14, 2015 at 0:12
  • $\begingroup$ the build up of the potential difference created between two capacitor plates (because of the charge accumulation you talk about) is only as much as what you put in with your DC or AC generator. If we call this potential difference $V$, then if $eV < \Delta E$, where $\Delta E = E_{vacuum} - E_{metal}$ is the height of the energetic barrier to cross the vacuum gap, then your electrons have no reason (and no physical mean) to go to the other side. This is both because of the electrostatic interaction and some chemical bonding that the electrons do not want to leave the metal. $\endgroup$
    – gatsu
    Mar 14, 2015 at 9:39

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