Chemistry Module #16-FINAL CHAPTER
About this set
Created by:
ScoutFinch on May 24, 2010
Subjects:
chemistry, Potters School, The Potter's School
Description:
For Chemistry with Mrs.Weeks at TPS
Classes:
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50 terms
Terms | Definitions |
|---|---|
 Oxidation Number | The charge that an atom in a molecule would develop if the most electronegative atoms in the molecule took the shared electrons from the less electronegative atoms |
| Oxidation numbers treat all compounds as | ionic |
| Oxidation numbers | aren't real |
| Oxidation numbers do not | have any significance in the real world |
| The sum of all oxidation numbers | in a molecule must equal the charge of that molecule |
| Rule #1 | When a substance has only one type of atom, the oxidation number for that atom = the charge of the substance divided by the number of atoms present |
| Rule #2 | Group 1A metals always have a +1 O. # in molecules that have more than 1 type of atom |
| Rule #3 | Group 2A metals always have a +2 O. # in molecules that have more than 1 type of atom |
| Rule #4 | Fluorine always has a -1 O. # in molecules that have more than 1 type of atom |
| Rule #5a | When with 1 other atom that is a metal, H has a -1 O. # |
| Rule #5b | When with other multiple atoms, H has a +1 O. # |
| Rule #6 | Oxygen has an -2 O.# in molecules that have more than 1 type of atom |
| Rule #7 | If all else fails, apply the O. # as the same as what the atom would take in an ionic compound. Groups 3A, 6A and 7A work best. |
| Oxidation | the process by which an atom loses electrons |
| Reduction | the process by which an atom gains electrons |
| LEO says GER | lose electrons oxidation, gain electrons reduction |
| when an atom undergoes reduction | we say that it has been reduced |
| when an atom undergoes oxidation | we say that it has been oxidized |
| If any 2 atoms change oxidation numbers in a reaction | it is a redox reaction |
| Electricity | is just electrons traveling through a wire |
| voltmeter | indicates the voltage of a battery |
| salt bridge | cancels out + or - charge that develops in an anode or cathode |
| a salt bridge contains | an aqeuous ionic compound and is necessary for the proper working of the battery |
| anode | negative side of the battery |
| cathode | positive side of the battery |
| anions | negative ions |
| cation | source of positive charges |
| galvanic cell | battery as described in Module 16 |
| metal strips conducting electrons | electrodes |
| Lead-acid battery | car battery |
| in lead acid battery, reactants | PbO2, Pb and H2SO4 (aq) |
| in lead acid battery, products | PbSO4, H2O |
| when you recharge a battery, | you reverse the reaction, converting produscts to reactant |
| dry cell battery | contains no aqueous solutions |
| dry cell battery used in flashlights | alkaline cell because the salt bridge uses KOH, a base |
| in alkaline batteries, the inner construction of the battery is broken down | which means it can not recharge |
| redox reactions are often useful, | but can be harmful (rust, corrosion) |
| corrosion is | oxidation |
| use the 7 rules of determining ox. numbers as a | hierarchy |
| what happened in exp. 16.1 | citric acid oxidized iodine to 5+ in order to form the blue starch compound, it needed to be 0 |
| anodes go on the | left |
| cathodes go on the | right |
| car battery is | rechargeable |
| dry cell battery | no aq solution |
| the anode must be made of | metal in equation |
| cathode does not need to be made of | metal in equation |
| cations | + ions |
| anions | - ions |
| all batteries are not | galvanic cells |
| h2so4 is a reactant | in a lead acid battery |
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