Download PMS4P4 Reduction potentials

PM S4 P4 Solve problems and analyse information to calculate the potential E º requirement of
named electrochemical processes using tables of standard potentials and half-equations.
Standard reduction potential:
A numerical measure of the relative _____________ of a substance to gain one or more
electrons compared to the hydrogen half cell, measured under standard conditions:
_________ , __________, __________ electrolytes.
The higher the E º value, the stronger the ___________ power of a substance.
Redox table

A list of standard reduction potentials ( __), forward reactions are written as
___________ reactions.

The more positive the reduction potential the more easily the species is
______________

Oxidising agents are on the ______________ of the table and they increase in strength
as you move __________ the table.

The strongest oxidising agent is _________________. _________________ is most
likely to accept ______________ from another species, thus causing the oxidation of
that species.

Reducing agents are found on the right hand side of the table, the strongest reducing
agent is __________________ at the top of the table.

Potassium is the most likely to ______ electrons to another species, thus causing it to
be reduced.
oxidising
Eº
25 C,
reduced
1 atm,
1 mol L-1
Tendency
left
reduction
fluorine
down
fluorine
electrons
potassium
lose