Back to AI Flashcard MakerChemistry /Chemistry: Electrode Potentials Part 1
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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| 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 |
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 |
|
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 |
|
equation for standard hydrogen electrode | 2H+ + 2e->< H2(g) |