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chem redox turell
redox terms
| Question | Answer |
|---|---|
| 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. |
Created by:
brendanlegel
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