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MCAT Gen. Chem Ch.11
| Term | Definition |
|---|---|
| Oxidation | Loss of electrons |
| Reduction | Gain of electrons |
| Oxidation-Reduction (Redox) | Reaction in which both oxidation and reduction are paired together |
| Oxidizing Agen | Facilitates the oxidation of another compound and is reduced itself in the process |
| Reducing Agent | Facilitates the reduction of another compound and is itself oxidized in the process |
| Common Oxidizing Agents Contain: | Oxygen or a similarly electronegative element |
| Common Reducing Agents Contain: | Metal ions or hydrides (H-) |
| Any Free Element Or Diatomic Species Has An Oxidation Number Of: | Zero |
| The Oxidation Number Of A Monoatomic Ion Is: | Equal to the charge of the ion. |
| Group IA Metals In Compounds Have An Oxidation Number Of: | +1 |
| Group II A Metals In Compounds Have An Oxidation Number Of: | +2 |
| Group VIIA Elements In Compounds Have An Oxidation Number Of: | -1 |
| Oxidation State Of Hydrogen Is: | +1 |
| Oxidation State Of Hydrogen When Paired With A Less Electronegative Element Is: | -1 |
| Oxidation State Of Oxygen Is Usually: | -2 |
| Oxidation Of Oxygen In Peroxides Or In Compounds With More Electronegative Elements Is: | -2 |
| Sum Of Oxidation Numbers Of All Atoms Present In A Compound Is: | Equal to overall charge of that compound |
| Steps Of The Half-Reaction Method When Balancing Redox Reactions (First Half): | Separate the two half reactions, balance the atoms of each half-reaction by starting with elements besides H and O. In acidic solutions, balance H and O using water and H+. In basic solutions, balance H and O using water and OH-. |
| Steps Of The Half-Reaction Method When Balancing Redox Reactions (Second Half): | Balance the charges of each half-reaction by adding electrons as necessary to one side of the reaction. Multiply the half-reactions as necessary to obtain the same number of electrons in both half-reactions. |
| Steps Of The Half-Reaction Method When Balancing Redox Reactions (Third Half): | Add the half-reactions while canceling out terms on both sides of the reaction arrow. Confirm that the mass and charge are balanced. |
| Complete Ionic Equation: | Accounts for all of the ions present in a reaction. |
| To Write A Complete Ionic Reaction: | Split all aqueous compounds into their relevant ions. Keep solid salts intact. |
| Net Ionic Equations | Ignore spectator ions to focus only on the species that actually participate in the reaction. To obtain a net ionic reaction, subtract the ions appearing on both sides of the reaction which are called spectator ions. |
| For Reactions That Contain No Aqueous Salts, The Net Ionic Equation Is: | Generally the same as the overall balanced reaction |
| For Double Displacement / Metathesis Reactions That Do Not Form A Solid Salt, There Is: | No net ionic reaction because all ions remain in solution and do not change oxidation number. |
| Disproportionation (Dismutation) Reactions | Type of redox reactions in which one element is both oxidized and reduced, forming at least two molecules containing the element with different oxidation states. |
| Oxidation-reduction Titrations | Similar to acid-base titrations and follow transfer of charge. |
| Indicators Used In Oxidation-Reduction Titrations Change Color: | When certain voltages of solutions are achieved |
| Potentiometric Titration | Form of redox titration in which a voltmeter or external cell measures the electromotive force (emf) of a solution. No indicator is used, and the equivalence point is determined by a sharp change in voltage. |
Created by:
SamB91
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