Chem Test 4 Terms
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43 terms
Terms | Definitions |
|---|---|
 Absorption | The incorporation of a molecule into the host molecule |
| Adsorption | The accumulation of molecules on the surface of a solid or liquid |
| Digestion | When a precipitate is allowed to stand in the presence of the hot solution from which it was precipitated, the large crystals grow at the expense of the small ones. Process of crystal trying to fix itself |
| Gravimetric analysis | Process of precipitating something out of solution to measure how much was in soln |
| Homogeneous precipitation | the precipitating agent is synthesized in the solution rather than added mechanically |
| Nucleation | small particles come together on dust to form a stable solid |
| Peptization | occurs when a coagulated precipitate converts back to its original dispersed state |
| Precipitate | The insoluble solid that forms during the reaction |
| Saturated solution | Solution contains maximum number of dissolved particles |
| Supersaturated solution | Solution exceeds the maximum number of dissolved particles. |
| Anode | on the left; where oxidation occurs |
| Cathode | on the right; where reduction occurs |
| Coulomb | SI unit that measures electricity |
| Ampere | SI unit that measures electrical current; equivalent to 1 C/sec |
| Current | the flow of electrons in a cell |
| Potential, Eo | Cell potential is determined by the tendency of the ions to give off or take electrons |
| Electrode | Either the anode or the cathode; connection between the chemical reaction and the external circuit. |
| Faraday constant | unit of electricity 96,87 coulombs eq-1 |
| Galvanic/Voltaic cell | Batteries that store energy; spontaneous rxns; produce electrical energy |
| Electrolytic Cell | Require an external source of energy; nonspontaneous |
| Half-reaction | the oxidation or reduction component of a redox reaction |
| Joule | SI unit of energy |
| Nernst equation | E=E^o- .0592/n log(([C]^c [D]^d)/([A]^a [B]^b )) |
| Oxidation | loss of electrons |
| Reduction | gain of electrons |
| Oxidizing agent | the species that gets reduced |
| Reducing agent | the species that gets oxidized |
| Voltmeter | placed between the electrodes to measure the difference in the potentials |
| Reaction quotient | the relative proportion of products and reactants present in the reaction mixture at some instant of time other than equilibrium. |
| redox reaction | occurs between a reducing and an oxidizing agent |
| salt bridge | allows charge transfer through the solutions but prevents mixing of the solutions |
| standard reduction potential | potential of half reaction used to determine cell potential |
| Calomel electrode | commonly used reference electrode. Hg | Hg2Cl2 |
| Combination electrode | An electrode that contains both the indicator and the reference electrode |
| Glass electrode | Good at binding H+ ions and therefore measuring pH |
| Indicator electrode | potential is determined by the analyte; measures the analyte |
| Ion-selective electrode | converts the activity of a specific ion into electric potential |
| Reference electrode | Constant potential; completes the cell but does not respond to the analyte |
| Junction potential | liquid junction between two dissimilar solutions prevents mixing. salt bridge |
| Potentiometry | measures the voltage; focuses on low-resistance circuits. |
| Voltametry | Measures the electrical current; focuses on high-resistance circuits |
| SCE (saturated calomel electrode) | commonly used reference electrode. Hg | Hg2Cl2 with solid KI |
| Silver-silver chloride electrode | Ag | AgCl common reference electrode |
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