Cell, voltaic structure

To summarize our discussion of the structure of voltaic cells, note that—... 

The non situ experiment pioneered by Sass uses a preparation of an electrode in an ultrahigh vacuum through cryogenic coadsorption of known quantities of electrolyte species (i.e., solvent, ions, and neutral molecules) on a metal surface. " Such experiments serve as a simulation, or better, as a synthetic model of electrodes. The use of surface spectroscopic techniques makes it possible to determine the coverage and structure of a synthesized electrolyte. The interfacial potential (i.e., the electrode work function) is measured using the voltaic cell technique. Of course, there are reasonable objections to the UHV technique, such as too little water, too low a temperature, too small interfacial potentials, and lack of control of ionic activities. ... 

The batteries used in everyday appliances (Figure 13-10) produce electricity through chemical reactions. The basic structure of converting chemical energy to electricity takes places in a voltaic cell, which is a simple structure consisting of an anode, a cathode, and an electrolyte. These parts are shown in Figure 13-11. 

Corrosion is a natural, spontaneous, electrochemical process with similarities to the operation of a voltaic cell. It is a major economic problem because the anode is typically a metal tool or structure. (Section 21.6)... 

We can use Figures 19.1(b) and 19.6 as a starting point to help you form your mental movie about how electron-transfer reactions occur at the particulate level. Look back and refamiliarize yourself with this figure, a Zn/Zn " and Cu VCu voltaic cell. Now recall the electron-sea model of metallic bonding (Section 12.8), by which a metal is pictured as a crystal structure of metal ions immersed in a sea of electrons. Imagine the metallic zinc electrode in this way zinc ions in a sea of electrons. 

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