Module 1-4 Unit 2 Flashcards
Oxidation
the loss of electrons
Reduction
the gain of electrons
OIL RIG meaning
Oxidation Is Loss
and
Reduction Is Gain
Redox reaction
When an atom loses an electron (oxidation), it is gained by another atom (reduction), and they must happen simutaneously
Oxidizing Agent
A reactant the oxidizes other reactants
Therefore reduces itself
Reducing agent
A reactant that reduces another reactant
Therefore oxidizes itself
Spontaneous redox reaction
A reaction between a strong OA and a strong RA
OA is above RA on the table
Nonspontaneous redox reaction
A reaction between a weak OA and a weak RA
The Spontineity Rule
The OA must be above the RA on table to be a spontaneous reaction
Half-Reaction
an equation that only shows the reduction or oxidation
Only half of the reaction
Disproportionation Reaction
Redox reaction where some of the atoms of an element are oxidized and the other atoms are reduced.
Some may lose electrons, some may gain electrons in the same reaction
Oxidation number
The charge an atom in a compound would have if electrons were held by the atom with the strongest electronegativity (no sharing)
Oxidation Rules
6
1) pure elements have a charge of 0
2) charge of a single ion is their oxidation number (Ex: Al+3(aq))
3) Hydrogen number is usually +1, but -1 with metals
4) Oxygen is usually -2 (except some)
5) molecular compounds element is assigned a number equal to the negative charge it usually has
6) Sum of all oxidation numbers equal the overall charge of the compound (either neutral or charged)
Oxidation number changes in redox reactions
Increase in oxidation number represents oxidation
Decrease in oxidation number represents reduction
Endpoint
Visible signal in a titration that the reaction has stopped
