Electrode Theory Flashcards

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1
Q

Redox Processes

A

1) Oxidation = Electron Release
2) Reduction = Electron uptake/absorption
3) Redox process: Electron Transfer

  • -> Oxidant: Uptake of electrons causing Reduction –> ability to oxidize other substances
  • -> Reductant: Release of electrons causing oxidation –> ability to reduce other substances

Reaction depends on electrochemical potential

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2
Q

Anode & Cathode

A

Anode: (base metal)

  • Current flow Positive –> from metal into electrolyte
  • oxidation at boundary surface: Metal –> Metal+ + e-
  • reduction of electrode

Cathode: (noble metal)

  • Current flow negative –> from electrolyte into metal
  • reduction at boundary surface: Metal+ + e- –> Metal
  • oxidation of electrode
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3
Q

Galvanic Cell

A

!!! Combination of 2 half cells
–> different electrodes and electrolytes

spatial separation of oxidation and reduction and electron flow through an electric conductor

–> use salt bridge for charge exchange without mixing the electrolytes

e.g. Daniell Cell

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4
Q

Helmoltz Double Layer

A
  • forces of attraction between negative and positive charge at interface form a double layer
  • -> between Anode and Cathode
  • due to Nernst equation, an electric potential is formed
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5
Q

Polarization of Electrodes and Overpotentials

A

1) Transfer Overpotential (charge transport processes)
2) Diffusion Overpotential
3) Reaction Overpotential (chemical reactions)

  • Ohmic polarization: resistive voltage drop (no overpotential!)
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6
Q

Transfer Overpotential

A

inhibition of the passage of the charge carriers through the electrolytic double layer requires energy and generates voltage drop

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7
Q

Diffusion Overpotential

A

occurs if the current flow of the advection of the consuming substances or the evacuation of produced substances is inhibited

Ion movements –> due to convection, electric potential, chemical potential (diffusion)

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8
Q

Reaction Overpotential

A

reaction inhibition may lead to different concentrations of the charge carriers near the electrode interface –> leads to charge separation –> reaction overpotential

chemical reactions may be tied to transfer reaction:

  • solvation
  • desolvation
  • complex formation
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9
Q

Ohmic Voltage Drop

–> on what does it depend?

A
  • Voltage Drop Outside the electrolytic double layer
  • no influence over the electrochemical processes at the interface
  • depends only on the conductivity of the electrolyte and geometrical factors
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10
Q

Electrodes - What kind of system?

What types of Electrodes exist?

A

Multiphase systems, where equilibria are formed between two conductive phases (metal, electrolyte)

1) Redox electrode: electrones are used as charge carriers through the interface
2) Ion Electrodes: ions travel through interface

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11
Q

Electrode Type 1

–> Ion Electrode

A

Polarizable Electrodes

  • high R
  • behave rather capacitive

–> potential depends directly on the concentration
of the electrolyte solution surrounding them

  • metal/metal salt solution
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12
Q

Electrode Type 2

–> Ion Electrode

A

Unpolarizable Eletrodes

  • small R
  • behave rather conductive
  • -> convenient for medical engineering
  • 3 Phase system

e.g. Ag/AgCl electrode

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13
Q

Structure of Skin

A

1) Epidermes
2) Dermis
- elastic and collagen fibers
3) Subcutaneous adipose tissue
- thick

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14
Q

Tasks of Skin

A
  • mechanical and chemical protective function

- protects body from drying up, heat and light

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15
Q

Bioimpedance Measurement

A

4 electrode Array –> determination of tissue resistance

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16
Q

Are electrons used as charge carriers through the interface in Electrodes of Type 2?

A

No, they use ions

17
Q

Are common metals oxidants?

A

No

18
Q

Is the capacitance of the Helmoltz Layer dependent on the current flow through the electrode?

A

Yes

19
Q

Of what does the Daniell cell consist?

A

Anode: Zinc electrode (Oxidation)

Cathode: Copper electrode (Reduction)

typically 1 molar solutions

20
Q

What are the advantages of Electrodes of Type 2 in comparsion to Electrodes of Type 1?

A

–> the electrode potential is almost insensitive to concentration fluctuations and is therefore very stable

  • resulting electrode potential only depends on the concentration of chloride ions in the electrolyte solution
  • -> almost independent of the concentration of silver cations
21
Q

How is the advantage of Electrodes of Type 2 in comparsion to Electrodes of Type 1 achieved?

A

–> keep the concentration of the anion constant in order to achieve an almost constant potential

  • electrode is coated with poorly soluble salt, which has the same cation as
    the electrode itself (Ag+)

The electrolyte solution consists of a highly concentrated salt which has the same anion as the poorly soluble salt.

22
Q

What is an overpotential?

A

Deviation of the electrode voltage from the resting potential

23
Q

On what does the Electromotive Force depend?

A

on the concentration of the electrolyte solution