Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
10 Cards in this Set
- Front
- Back
- 3rd side (hint)
|
Oxidtion numbers |
Uncombined element: 0 Hydrogen: +1 Oxygen: -2 |
|
|
|
Change in oxidation number |
Increase = oxidation = red agent Decrease = reduction = ox agent |
|
|
|
Balancing REDOX in acidic conditions |
1. half-equations 2. Balance elements (not O or H) 3. Balance O atoms w/ H2O 4. Balance H w/ H+ 5. Balance charges w/ e- |
|
|
|
Winkler method |
1. add manganese (II) salts 2Mn^(2+) + 02 + 4OH(-) --> 2MnO2 + 2H2O
2. Add acidified iodine ions MnO2 + 2I(-) + 4H(+) --> Mn^(2+) + I2 + 2H2O
3. Titrate iodine w/sodium thiosulfate in presence of starch S2O3^(2-) + I2 --> S4O6 ^(2-) + 2I(-) |
|
|
|
Electrochemical cells |
Voltaic/Galvanic: cathode +ive Electrolysis: cathode -ive
|
|
|
|
MNEMONICS |
OILRIG - source of e- Red Cat |
Temperatures Electrode Pressure Concentration |
|
|
Electrode reduction potential |
SHE (Standard Hydrogen Electrode) •Pt electrode •E* = 0 V •1M H(+) •298K •100kPa
Standard reduction potential •298 K •100 kPa •1M concentration sol^ •pure substances •if no solid metal; Pt electrode |
|
|
|
Electrolysis |
q = I * t 1 mole of e- = 1 Faraday =96 500 c Mass = Mr * moles |
|
|
|
Salt bridge |
Salt bridge enables -ve q to be carried in opposite direction to that of the e- to neutralize any build up q and mantain e.m.f. |
|
|
|
Standard electrode potential |
Voltage obtained when half cell is connected to the SHE |
Definition |
