Back to AI Flashcard MakerChemistry /Chemistry: Electrode Potentials Part 1

Chemistry: Electrode Potentials Part 1

Chemistry40 CardsCreated 2 months ago

This deck covers key concepts related to electrode potentials, including oxidation and reduction processes, electrochemical cells, and standard electrode potentials.

What is the process of oxidation and reduction expressed in terms of?

electron transfer
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Key Terms

Term
Definition
What is the process of oxidation and reduction expressed in terms of?
electron transfer
oxidation
loss of electrons
reduction
gain of electrons
oxidation is an increase in
oxidation state
reduction is a decrease in
oxidation state
what can we work out by assigning oxidation states
which species have been oxidised and which have been reduced without writing half equations

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TermDefinition
What is the process of oxidation and reduction expressed in terms of?
electron transfer
oxidation
loss of electrons
reduction
gain of electrons
oxidation is an increase in
oxidation state
reduction is a decrease in
oxidation state
what can we work out by assigning oxidation states
which species have been oxidised and which have been reduced without writing half equations
oxidising agent
species that accepts electrons
reducing agent
species that donates electrons
example of an oxidising agent
halogens
example of a reducing agent
reactive metals
what does an electrochemical cell use the electron transfer which occurs during a redox reaction to do
produce electrochemical energy
what does each electrochemical cell consist of
2 half cells corresponding to the two half equations occurring in the redox reaction
what does a half cell consist of
two species of the same element in different oxidation states
what is the electrode in a copper half cell
solid copper
what is the solution in copper half cell
1 mol dm3 copper 2+ ions
what is the IUPAC convention for writing half equations for electrode reactions
to give them as an equilibrium reaction where the forward reaction is reduction
what must the half cells be connected via in order to make use of the electrical energy produced in a redox reaction
connected via an external circuit and a salt bridge
what is the circuit usually
a conducting wire
what flow through the wire
electrons
what does the salt bridge consist of
a strip of filter paper soaked in saturated potassium nitrate or potassium chloride solution
what flows through the salt bridge
ions
what are the electrodes connected to
a high resistance voltmeter
what does the voltmeter measure
electromotive force (emf) in volts
what is the emf
potential difference
what is the other name for emf
cell potential

what are the standard conditions are there for a half cell

  • 100kPa

  • 298K

  • solution of ions at 1moldm-3

which metal goes on the rhs
the more positive metal
which metal goes on the rhs in the standard copper-zinc cell
copper
why is the copper the positive electrode in the copper-zinc cell
because it is connected to the positive terminal of the voltmeter and so is the positive electrode
what is the IUPAC convention for cell diagrams
to draw the positive electrode as the half cell on the RHS (except when measuring standard electrode potential against hydrogen electrode when hydrogen always on left)
what occurs at the negative electrode
oxidation
what occurs at the positive electrode
reduction
where do electrons flow in cell
from negative electrode to positive electrode
what does the standard electrode potential of a half cell indicate
its tendency to lose/gain electrons
is it possible to measure the standard electrode potential of one half cell alone
no
what is used as a reference to measure standard electrode potential against
a primary standard
what is the primary standard for measuring electrode potentials
the standard hydrogen electrode
what emf does the standard hydrogen electrode have by definition
0.00V

standard hydrogen electrode

  • H2 gas at 1 00kPa

  • 1 moldm-3H+ (aq)

  • 298K

  • Pt electrode

equation for standard hydrogen electrode
2H+ + 2e->< H2(g)