Oxidation-Reduction Reactions Flashcards
Oxidation
Loss of electrons
Reduction
Gain of electrons
Oxidation/Reduction with Respect to Oxygen Transfer
Oxidation is the GAIN of oxygen
Reduction is the LOSS of oxygen
Oxidizing Agent
Facilitates the oxidation of another compound. Is itself reduced.
Reducing Agent
Facilitates the reduction of another compound. Is itself oxidized.
Balancing via Half-Reaction Method
1) Separate the two half-reactions
2) Balance the atoms of each half-reaction
3) Balance the charges of each half-reaction by adding electrons as necessary
4) Multiply the half-reactions as necessary to obtain the same number of electrons in both half-reactions
5) Add the half-reactions, cancelling out terms on both sides
Oxidation # Rules
Any free element or diatomic species = 0
Monatomic ion = the charge of the ion
When in compounds, group 1A metals = +1; group 2A metals = +2
When in compounds, group 7A elements = -1, unless combined with an element of greater EN
H = +1 unless it is paired with a less EN element, then = -1
O = -2 except in peroxides, when it = -1, or in compounds with more EN elements
The sum of all oxidation numbers in a compound must = overall charge
Complete Ionic Equation
Accounts for all of the ions present in a reaction. Split all aqueous compounds into their relevant ions. Keep solid salts inact.
Net Ionic Equation
Ignores spectator ions
Disproportionation Reactions
A type of redox reaction in which one element is both oxidized and reduced, forming at least two molecules containing the element with different oxidation states.
REDOX Titrations
Similar in methodology to acid-base titrations, however, these titrations follow transfer of charge.
Potentiometric Titration
A form of REDOX titration in which a voltmeter measures the electromotive force of a solution. No indicator is used, and the equivalence point is determined by a sharp change in voltage.
