Electrochem: RA, OA, OX # Flashcards
(21 cards)
Define Reduction
Process where species GAINS electrons
- electrons present as reactants
LEO
Define Oxidation
Metals that corrode (rust) undergo oxidation where species LOSE electrons
-Electrons present as products
GER
Define Redox Reactions
Reduction and Oxidation must occur together in a complete reaction
Define Oxidizing Agent
the species that is reduced (gains e) causes oxidation
Define Reducing Agent
the species that is oxidized (losses e) causing reduction
When making Redox Reactions note:
- Ionic compounds break into their ions including water
- Molecular compounds stay as molecules
- Acids contain H+
Spontaneous Reaction
- Reaction between OA and RA occur
- OA is higher in ranking
Non-Spontaneous Reaction
- No reaction occurs between OA and RA
- RA is higher in ranking
SOA ion will have most reactions with?
the other RA metals
SRA metal will have the most reactions with?
OA ions
Define Oxidation Numbers
- Made up numbers that don’t follow the rule of bonding
- explains exchange of electrons
- can be pos., neg, or fractions
Ox # for elements
0
Ox # for O2
-2
Ox# for H
+1 (except in non-metals where it is -1)
In peroxides (H2O2) Ox # for O2 is
-1
Ox # for ions w/ charge
based on their ionic charge (Fe2+= 2+)
Total OX # for neutral compounds
sum must be 0
When compound does not have H or O2, start with what element?
the element that is more electronegative and use their ionic charge, must still have sum of 0
Ox # increases
Oxidation (RA)
Ox # decreases
Reduction (OA)
What is it called when OA and RA are the same?
Disporportionation (h2o)
