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24 Cards in this Set
- Front
- Back
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Single-replacement reactions are all ________ __________. |
Redox reactions |
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What do the terms spontaneous and non spontaneous mean? |
Spontaneous: a reaction happens immediately, like in a battery Non spontaneous: reactions don't happen immediately, but may be forced to react with added electricity. |
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What is a redox table? |
A table consisting of balanced half reactions. These can be read as a reduction reaction by reading from left to right, or as oxidation by reading right to left. The entity on the left is the OA and the entity on the right is the RA. On the left, OA is strongest on the bottom and weakest on the top. On the right, RA is weakest on the bottom and strongest at the top. |
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What is the spontaneity rule? |
If the reducing agent is higher on the table than the oxidizing agent, it is spontaneous. If the oxidizing agent is higher on the table than the reducing agent, it is non spontaneous. |
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If given a reaction with the reactant side but not the product side, how do you find out if the reaction will occur? |
1. Locate the entities on the Standard Reduction Potentials table. One should be on the left, one should be on the right. 2. If the one on the left (OA) is higher than the one on the right, then it is non spontaneous. 3. If the one on the right (RA) is higher than the one on the left, then it is spontaneous. |
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When given the names of two entities and asked if they will react, how do you discover whether or not a reaction will occur? |
1. Write out all entities involved. 2. Find which one is the strongest reducing agent (SRA) and which one is the strongest oxidizing agent (SOA) by finding them on the table. 3. apply spontaneity rules 4. If asked to write the reaction, write the two half reactions (SRA is backwards) and combine for the net reaction |
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When given the results of several experimental reactions, how do you construct a redox table from them. |
1. Indentify which entities are the RA and which are the OA 2. The atoms are generally the RA, and the ions are generally the OA. 3. Write out a statement of which entity is above which entity based on spontaneity rules. 4. Based on this, and using logic, write out the balanced half reactions in correct order. |
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What is an electrochemical cell? |
Any device that uses a redox reaction to either produce or use electricity. |
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What are the two basic components of an electrochemical cell? |
Electrodes: anode and a cathode. Usually two metals, sometimes graphite. One electrode may be the container of the cell. Electrolyte: solution of dissolved ions that conduct electricity. Sometimes a paste |
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What is there in order to let electrons move from anode to cathode? |
An external conducting pathway, often a wire |
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What is a voltaic cell? |
An electrochemical cell that produces electricity as the result of spontaneous redox reactions. E.g. a battery |
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What is an electrolytic cell? |
an electrochemical cell that uses energy to drive nonspontaneous redox reactions. e.g. electroplating and metal purifying. |
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What is a battery? |
A group of two or more electric cells connected to each other. |
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What is a galvanic/voltaic cell? |
Electric cells adapted for scientific study. It is made up of two beakers, each with its own electrolyte and electrode. They represent the half reactions of the redox reaction. A wire connects them to allow electrons to move from the anode to cathode. A salt bridge prevents a positive charge on the anode side and a negative charge on the cathode side so that the redox reaction may continue going. |
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What is a primary cell? |
A battery that cannot be recharged. |
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What is a secondary cell? |
A battery that can be recharged. |
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When given cell notation, how do you draw a voltaic cell? |
1. The entity on the far left is the anode. The entity on the middle left is the electrolyte. 2. The entity on the far right is the cathode. the entity on the middle right is the electrolyte. 3. Draw two beakers, each with a strip of metal, anode on the left, cathode on the right. Label them. 4. Draw the wire and the salt bridge. 5. write in the electrolytes 6. indicate the direction of ions from the salt bridge 7. Indicate direction of electrons |
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What is the difference between a voltaic and electrolytic cell in terms of: spontaneous? |
voltaic: yes electrolytic: no |
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What is the difference between a voltaic and electrolytic cell in terms of: cell potential? |
voltaic: positive electrolytic: negative |
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What is the difference between a voltaic and electrolytic cell in terms of: cathode? |
voltaic: positive electrolytic: negative both; strongest oxidizing agent present undergoes a reduction |
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What is the difference between a voltaic and electrolytic cell in terms of: anode? |
voltaic; negative electrolytic: positive both: strongest reducing agent present undergoes an oxidation |
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What is the difference between a voltaic and electrolytic cell in terms of: direction of electron movement? |
both: anode to cathode |
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What is the difference between a voltaic and electrolytic cell in terms of: direction of ion movement? |
both: anions to anode and cations to cathode |
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When given the cell notation of a voltaic cell, how do you write the reactions and find the cell potential? |
1. anode (SRA) is on the left, cathode (SOA) is on the right. 2. write the oxidation for the anode and the reduction for the cathode. 3. Use standard reduction potentials to find potentials of the half reaction. remember that the oxidation half reaction has its sign flipped. 4. add potentials. should be positive. don't forget units. |
