redox terms
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
|
|
||||
|---|---|---|---|---|---|
| Anode | Where oxidation takes place. In electrolysis, it is the + electrode and anions are attracted here.
🗑
|
||||
| Cathode | Where reduction takes place. In electrolysis, it is the - electrode and cations are attracted here.
🗑
|
||||
| Electrolysis | Passage of electric current through an electrolyte. Amount of discharge is affected by: 1) current; 2) charge on ion, 3) duration of electrolysis.
🗑
|
||||
| Electrolyte | A substance which does not conduct electricity when solid, but does when molten or in aqueous solution and is chemically decomposed in the process.
🗑
|
||||
| Electrolytic cell | Used to make non-spontaneous redox reactions occur by providing energy in the form of electricity from an external source.
🗑
|
||||
| Electroplating | A process of coating one metal with a thin layer of another metal, by electrolysis.
🗑
|
||||
| Half cell | A metal in contact with an aqueous solution of its own ions.
🗑
|
||||
| Oxidation | The loss of electrons
🗑
|
||||
| Oxidizing agent | A substance that readily oxidizes other substances. Oxidizing agents are thus reduced.
🗑
|
||||
| Reactivity | A measure of the readiness of a substance to gain or lose electrons. The stronger the reducing agent or oxidizing agent, the more reactive it is.
🗑
|
||||
| Redox reaction | A reaction in which there is a transfer of electrons, i.e. reduction and oxidation occurring simultaneously.
🗑
|
||||
| Reducing agent | A substance that readily reduces other substances. Reducing agents are thus oxidized.
🗑
|
||||
| Reduction | The gain of electrons
🗑
|
||||
| Salt bridge | Allows the free movement of ions in a voltaic cell. Paper dipped in a saturated solution of KNO3 is an example of a salt bridge.
🗑
|
||||
| Shorthand notation | For a voltaic cell. Example: Cu(s)/Cu2+(aq) || H+(aq) / H2(g)
🗑
|
||||
| Standard conditions | 298 K, 1 atm, 1.0 M.
🗑
|
||||
| Standard electrode potential | The electrode potential of one half-cell compared against another half-cell, by convention, the hydrogen half-cell, which is arbitrarily given a value of 0 V.
🗑
|
||||
| Standard cell potential | Difference between the two standard electrode potentials of the two half cells.
🗑
|
||||
| Standard hydrogen electrode | Arbitrarily assigned a potential of zero. Electrode consists of an inert metal such as platinum dipped into a 1 M solution of HCl, where hydrogen gas at 1 atm flows in.
🗑
|
||||
| Voltaic cell | Two different half-cells connected together to enable to electron transferred during the redox reaction to produce energy in the form of electricity. The electrons are produced at the half-cell that is most easily oxidized.
🗑
|
Review the information in the table. When you are ready to quiz yourself you can hide individual columns or the entire table. Then you can click on the empty cells to reveal the answer. Try to recall what will be displayed before clicking the empty cell.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Created by:
brendanlegel
Popular Chemistry sets