1 / 8

Ch 12 Electrolysis in water

Ch 12 Electrolysis in water. Electrolysis is a fairly simple process. There are two plates in a solution, and an electric current is sent through. The plates are the cathode, where reduction takes place, and the anode, where oxidation takes place. cathode-reduction anode-oxidation.

marci
Download Presentation

Ch 12 Electrolysis in water

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Ch 12 Electrolysis in water Electrolysis is a fairly simple process. There are two plates in a solution, and an electric current is sent through. The plates are the cathode, where reduction takes place, and the anode, where oxidation takes place. cathode-reduction anode-oxidation

  2. Rules for cathode reaction A cation may be reduced to a metal Cu+ + 1 e- Cu Or water way be reduce to hydrogen 2 H2O + 2 e- H2+ 2 OH- Transition metals tend to reduce before water, main group metals tend to reduce after

  3. Rules for anode reactions An anion nonmetal may be oxidized to a nonmetal 2 Cl- Cl2+ 2 e- Water may be oxidized to oxygen 2 H2O  O2+ 4 H++ 4 e- Chlorine, bromine and iodine will oxidize before oxygen. That is it.

  4. Rules for molten binary salts Molten means melted, with no water. These are straightforward and easy! Molten magnesium chloride is electrolysized MgCl2 Mg + Cl2

  5. examples Aqueous calcium bromide is electrolyzed Aqueous chromium (III) nitrate is electrolyzed Aqueous cobalt (II) bromide electrolyzed Molten sodium chloride is electrolyzed

  6. Ch 13 Complex ion reactions Formation of complex ions Common complex ions metals Fe Co Ni Cr Cu Zn Ag Al Common ligands NH3 CN- OH-SCN- General rule: the number of ligands will be twice the charge of the metal ion

  7. Example Iron (III) chloride reacts with potassium cyanide Fe3+ + CN- Fe(CN)63+ How did I get the charge? Iron is 3+ , 6 cyanides at 1-

  8. Examples Zinc (I) fluoride reacts with sodium thiocyanate Concentrated ammonia is reacted with cobalt (III) iodide Barium hydroxide reacts with nickel (II) nitrate

More Related