Talk:Electrochemistry
From Academic Kids
The article states:
- For example, oxygen has 6 positively charged protons, and thus in the neutral state would also have 6 (negatively charged) electrons. In dihydrogen monoxide (ie, water), each oxygen atom can be viewed as surrendering two electrons, one to each of two hydrogen atoms. The oxidation state of each oxygen atom in water then is -2, and of each hydrogen atom in water is +1.
- In the nomeclature of chemistry, the substance losing electrons is said to be the reductant and is oxidized' by the the other substance(s) in the reaction which gain the electrons.
- The substance gaining the electrons is said to be the oxidant and is said to be reduced (by the reductant).
Now I always thought that the oxygen takes (rather than gives up) two electrons from the hydrogen atoms. Thus the oxygen has a negative charge, and the hydrogens have a positive charge. I believe the article is contradicting itself as it current stands. Can someone who took chemistry more recently than me comment on this? -- ansible
- I think you are right, and it should be: each oxygen atom can be viewed as getting two electrons, one from each of two hydrogen atoms.
It seems to me that the focus of the whole article is wrong, because it deals with redox reactions and oxidation states.
A better definition of electrochemistry would be:
Electrochemistry is the science of the reactions that can take place at the interface of an electronic conductor (the electrode, which can be a metal or a semiconductor including graphite) and an ionic conductor (the electrolyte). -- Nick B.
WHERE IS THE Electrochemistry? that's redox!!!
Agree with last comment. It is really stub article. Need to be re-writed.
(Kaverin)
I added some introduction to start the article to deal with electrochemistry. But still it is a bad stub, which focuses on oxidation and reduction instead on the main points which would inclulde an electrochemical cell with electrodes and electrolyte.
