Back to AI Flashcard MakerAnatomy and Physiology /Chemistry: Electrode Potentials Part 2
Chemistry: Electrode Potentials Part 2
This deck covers key concepts related to electrode potentials, including standard electrode potentials, electrochemical cells, and the electrochemical series. It provides a comprehensive review of how these principles are applied in chemistry.
standard electrode potential
emf of a half cell compared with a standard hydrogen half-cell
measured at 298K, all solutions having conc of 1moldm-3 and all gases at a pressure of 100kPa
Tap or swipe ↕ to flip
Swipe ←→Navigate
1/40
Key Terms
Term
Definition
standard electrode potential
emf of a half cell compared with a standard hydrogen half-cell
measured at 298K, all solutions having conc of 1moldm-3 and all gases at a pre...
what is the standard electrode potential found by measuring
the voltage of a cell with the standard hydrogen half cell as one half cell and the half cell under investigation as the other
what gives the sign of the electrode potential
the polarity of the half cell relative to the hydrogen half cell
conventional representation of a cell: what does a vertical solid line indicate
a phase boundary eg between a solid and a solution
conventional representation of a cell: what does a double vertical line show
a salt bridge
conventional representation of a cell: which species for each half cell is written next to the salt bridge
the species with the highest oxidation state
Related Flashcard Decks
Study Tips
- Press F to enter focus mode for distraction-free studying
- Review cards regularly to improve retention
- Try to recall the answer before flipping the card
- Share this deck with friends to study together
| Term | Definition |
|---|---|
standard electrode potential | emf of a half cell compared with a standard hydrogen half-cell measured at 298K, all solutions having conc of 1moldm-3 and all gases at a pressure of 100kPa |
what is the standard electrode potential found by measuring | the voltage of a cell with the standard hydrogen half cell as one half cell and the half cell under investigation as the other |
what gives the sign of the electrode potential | the polarity of the half cell relative to the hydrogen half cell |
conventional representation of a cell: what does a vertical solid line indicate | a phase boundary eg between a solid and a solution |
conventional representation of a cell: what does a double vertical line show | a salt bridge |
conventional representation of a cell: which species for each half cell is written next to the salt bridge | the species with the highest oxidation state |
conventional representation of a cell: where is the standard hydrogen half cell shown when measuring the standard electrode potential of a half cell | LHS |
conventional representation of a cell: where is the positive electrode shown when showing any other electrochemical cell | RHS |
conventional representation of a cell: where is the negative electrode shown when showing any other electrochemical cell | LHS |
what is an ion/ion half cell | half cells in which both species are aqueous ions |
what must an ion/ion half cell contain | both the oxidised and reduced species |
what electrode is used in an ion/ion half cell | platinum |
what are standard electrode potential values determined by | measurement against the standard hydrogen electrode |
what are all reactions shown as in the electrochemical series | reductions |
what can we determine looking at the electrochemical series | the relative reactivity of different species |
metals react by losing what to form positive ions | electrons |
what do reactive metals undergo more readily | oxidation |
the most reactive metals will have the most negative | E0 values |
what are the most reactive metals good at | being reducing agents |
what is the correlation between negativity of E0 value of metal and tendency for species on RHS to lose electrons and be oxidised | more negative E0 value, greater tendency for species on RHS to lose electrons and be oxidised |
how to non metals react | by gaining electrons to form negative ions |
reactive metals undergo what more readily | reduction |
most reactive non metals will have most positive what | E0 values |
most reactive non metals are good at what | being oxidising agents |
correlation between positivity of E0 value of non metal and tendency for species of LHS to gain electrons and be reduced | more positive E0 value, greater tendency for species on LHS to gain electrons and be reduced |
what must a half cell be connected to to determine the electrode potential of it | the standard hydrogen electrode |
what can be connected to generate an emf | any 2 half cells |
what is the cell potential the difference between | the standard electrode potentials of the two half cells |
what is chemical energy converted into in an electrochemical cell | electrical energy |
what does the emf drop to once the chemicals are used up | 0.00v |
which half equation goes forwards | the one with the more positive e0 value- gains electrons |
which half equation goes backwards | the one with the more negative e0 value- loses electrons |
how to determine which reaction will occur in the cell or in a test tube | add the two half equations, making sure that the number of electrons lost equals number of electrons gained |
measuring electrode potential for a metal/metal ion half cell eg copper: equation | Cu2+ +2e- <> Cu(s) |
the conventional representation of a cell: what does a vertical solid line indicate | a phase boundary eg between a solid and a solution |
the conventional representation of a cell: a double vertical line shows the | salt briddge |
the conventional representation of a cell: the species with the highest ? for each half cell is written next to the salt bridge | oxidation state |
the conventional representation of a cell: when measuring the standard electrode potential of a half cell the standard hydrogen half cell is always shown on the | left hand side |
The conventional representation of a cell: on which side is the positive electrode shown | The RHS |
The conventional representation of a cell: on which side is the negative electrode | Left hand side |