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When we pass electricity through water it breaks into hydrogen and oxygen gas.

$$\ce{2H2O -> 2H2 + O2}$$

What I couldn't understand is how the electrical energy is converted to breaking the bonds of water molecule. I've searched a lot but couldn't find any satisfactory answers on how the energy conversion happens.

Few thoughts :

  1. The fast moving electrons from the battery hit the water molecules breaking them into hydrogen and oxygen ions.
  2. I think above idea is incorrect as pure water is an insulator and blocks passage of electrons. Then it might have to do with the electric field that exists through out the water between the anode and cathode. Does this electric field somehow transfer energy to the water molecules and split them ?
  3. Above idea makes sense to me as we can think of each $\ce{H2O}$ molecule as a dipole $\ce{2H+-O^2-}$, so it can interact with electric field.
  4. I feel all above ideas are silly and there is some sophisticated way to reason this which I don't know yet.
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Electrolysis of pure water is very difficult, but adding only a small amount of ions make the process easily achieved. In most places, there are enough minerals in the water that the ionic strength or conductivity of the water is great enough for electrolysis to effectively occur without needing to add additional ions to the water

Water dissociates into H+ ions and $\ce{OH–}$ ions; the $\ce{H+}$ ions are attracted to the negative electrode (the cathode) and are converted (reduced) to a hydrogen atom ($\ce{H}$) (i.e. $\ce{e- + H+ -> H}$). This is highly unstable and immediately reacts with another hydrogen atom to produce $\ce{H2}$, molecular hydrogen gas. At the other electrode (the anode), oxidation occurs. The $\ce{OH-}$ ions are attracted to the positive electrode where they are oxidized to form oxygen gas ($\ce{O2}$) and hydrogen ions ($\ce{H+}$). However, if chloride is present, it will oxidize (instead of the $\ce{OH–}$ ions) and form chlorine gas, which will then react with the water to form hypochlorous acid.

The cathode reaction is: $\ce{2H+ + 2e- (cathode) →H2 (g)}$
The anode reaction is: $\ce{2OH– → 4e-(anode) +O2 + 2H+}$
The overall reaction is: $\ce{2H2O → 2H2 (g) + O2 (g)}$

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  • $\begingroup$ Thank you. I know the reactions and gases that form at each terminal. But I still don't understand how the electrical energy is converted into breaking the bonds. For example, in an incandescent light bulb, the fast moving electrons hit the atoms in filament and make them vibrate. (converting electrical energy into vibrations of atoms). I'm wondering if something like this happens in electrolysis too.. $\endgroup$ – rsadhvika Feb 15 '17 at 13:47
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    $\begingroup$ The electical energy is used to ionise the water into H+ and OH- and under the electric field they move towards cathode and anode respectively and react there. For eg : H+ ion moves towards cathode under electric field and reacts with electrons present on the negatively charged cathode to form hydrogen gas. Also, for pure water a huge potential is required to ionise water,so some salts are added to promote flow of current and ionise the water molecules $\endgroup$ – user41346 Feb 15 '17 at 14:17

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