[Greenport]

Say one sets up an electrolysis chamber for the purpose of splitting apart either molten table salt or an aqueous solution of it...

When the NaCl comes into contact with the cathode, the Na(+) will be attracted to the cathode and break off of the Cl(-).

Or in the same way, when the ion comes into contact with the anode, the Cl(-) would go to the anode and the Na(+) breaks off.

What concerns me is what happens after the molecules split apart. Do they travel to the other electrode? or are they just released right where they are?

For instance, if the NaCl hits the cathode, of course the Na(+) will stay there but will the Cl(-) somehow find its way to the anode? Or does it just stay in the same chamber? (And why or why not?)

If that is the case then couldn't positively or negatively charged atoms be transferred over long distances electrically in this manner, as long as there was a current?

[Arkcon]

In aqueous solution or molten, you can assume the Na+ and Cl- ions are already apart, and swimming, if you will, freely.  But the electrolysis adds something to the mix, that just dissolving or melting doesn't, do you know what that is?  And what reaction takes place?

[Greenport]

Thanks for your comment. That does help me a little to understand how it works. I believe that the reaction you are speaking of is a redox (reduction and oxidation), but other than electricity (and perhaps hydrogen & oxygen) Im not sure what else is added.

So in your explanation where they are already broken apart (that makes sense to me, since, they'd be dissolved in that case), does that mean that both Sodium and Chlorine would be released into BOTH chambers?

[Borek]

Yep, at the same time. Current flows which means electrons have to go past the electrode/solution or electrode/molten salt phase boundary. It means chemical reaction (reduction/oxidation) happening - and you will always need two simultaneous reactions to keep your solution/molten salt electrically neutral.

[Greenport]

Then how is it that electrolysis of water (with an electrolyte in it of course) yields Hydrogen gas on one end and Oxygen gas on the other?

[Arkcon]

Then how is it that electrolysis of water (with an electrolyte in it of course) yields Hydrogen gas on one end and Oxygen gas on the other?

What is the difference between say, H⁺ -- one of the porducts of water's dissociation, and H₂ -- the product of it's electrolysis?  What's changed, and how?

I believe that the reaction you are speaking of is a redox (reduction and oxidation), but other than electricity (and perhaps hydrogen & oxygen) Im not sure what else is added.

Can you write a red-ox reaction, using the "electricity" that's been added?  It doesn't enter as bolts of lightning, how is it added?

[Greenport]

Well, H⁺ is a cation, which (technically) wants to be reduced. However since hydrogen's orbital only has a possible two electrons, it can really go either way (and often does). Thus, hydrogen reacts with other hydrogen cations to form H₂. This usually happens so quickly that we would not have free H+ hanging around very long and thus H₂ would be the product.

The H₂O would break apart into two free H⁺ cations and one O^- anion. The H⁺ would combine to H₂ and the O^- molecules would combine to form O2.

And as much as I hate to say it, I really am not 100% sure what is coming out of the end of the wires then - perhaps positively and negatively charged ions of hydrogen and/or oxygen? No, that doesn't seem right.

[Arkcon]

Well, H⁺ is a cation, which (technically) wants to be reduced. However since hydrogen's orbital only has a possible two electrons, it can really go either way (and often does). Thus, hydrogen reacts with other hydrogen cations to form H₂. This usually happens so quickly that we would not have free H+ hanging around very long and thus H₂ would be the product.

H⁺ + H⁺ --> H₂ ?  Ummm...no, that's not it.

And as much as I hate to say it, I really am not 100% sure what is coming out of the end of the wires then - perhaps positively and negatively charged ions of hydrogen and/or oxygen? No, that doesn't seem right.

I realize it can be a little daunting to figure out, if the wires are corrected to a DC generator, or a rectifier.  But what if the wires used for electrolysis get the electricity from a chemical battery?  Do you know how a chemical battery works?

[Borek]

http://www.chembuddy.com/?left=pH-calculation&right=water-ion-product

[LQ43]

Then how is it that electrolysis of water (with an electrolyte in it of course) yields Hydrogen gas on one end and Oxygen gas on the other?

The H₂O would break apart into two free H⁺ cations and one O^- anion. The H⁺ would combine to H₂ and the O^- molecules would combine to form O2.

You are on the right track with thinking about the oxidation - reduction of water to produce H2 and O2 gas. But as Borek has hinted, the dissociation of water is very small, so WHY would H2O break apart to give ions to produce these gases? In oxidation - reduction reactions, what is transferred?

Please think about Arkon's question and the meaning of current or electricity

It doesn't enter as bolts of lightning, how is it added?

Do you have a standard reduction potential table in your textbook? It might make more sense to you as you understand the above

[Borek]

You are on the right track with thinking about the oxidation - reduction of water to produce H2 and O2 gas. But as Borek has hinted, the dissociation of water is very small, so WHY would H2O break apart to give ions to produce these gases?

First of all I was hinting to the fact that water dissociation is not producing 2H⁺ and O^2-

[Greenport]

oy' well I'm reading some chapters on this topic to get more info..