Chemical elements
  Silver
    Isotopes
    Energy
    Production
    Application
    Physical Properties
    Chemical Properties
      Silver fluoride
      Silver subfluoride
      Silver chloride
      Silver subchloride
      Photohalides
      Silver bromide
      Silver oxybromide
      Silver subbromide
      Silver iodide
      Silver hypochlorite
      Silver chlorite
      Silver chlorate
      Silver perchlorate
      Silver bromate
      Silver perbromate
      Silver iodate
      Silver periodates
      Silver suboxide
      Silver monoxide
      Higher oxides
      Silver subsulphide
      Silver sulphide
      Silver sulphite
      Silver sulphate
      Silver selenide
      Silver telluride
      Silver thiosulphate
      Silver dithionate
      Silver azide
      Silver hyponitrite
      Silver nitrite
      Silver nitrate
      Silver phosphides
      Silver hypophosphate
      Silver orthophosphate
      Silver pyrophosphate
      Silver metaphosphate
      Silver arsenite
      Silver arsenate
      Silver carbide
      Silver carbonate
      Silver cyanide
      Silver thiocyanate
      Silver borate
    PDB 1aoo-3kso

Chemical Properties of Silver






At the ordinary temperature silver is stable towards moisture and atmospheric oxygen, but at 200° C. an invisible, superficial layer of oxide is produced, detected by its power of reacting with ozone at ordinary temperature. It reacts with sulphur and compounds of sulphur to form silver sulphide. In absence of air, hydrogen sulphide and the sulphides of the alkali-metals do not affect silver, but addition of oxygen or hydrogen peroxide induces instantaneous blackening.

Pure silver is dissolved by pure sulphuric acid at the boiling-point, provided the concentration of the acid is not less than 77.5 per cent., and in presence of impurities the metal is attacked also by the dilute acid:

2Ag + 2H2SO4 = Ag2SO4 + SO2 + 2H2O.

Nitric acid reacts energetically at ordinary temperatures, with formation of the nitrate and of the oxides of nitrogen. The behaviour of the metal with hydrochloric acid is similar to that of lead. The action of concentrated sulphuric acid and of nitric acid finds application in the separation of alloys of gold and silver. The corrosive effect of acids is accelerated by the presence of an oxidizer.

The metal is scarcely attacked by fused alkalies, and only slowly by the halogens. In contact with air or hydrogen peroxide it is readily dissolved by potassium cyanide. It is converted by mercury into an amalgam.

At ordinary temperatures and 200 atmospheres hydrogen expels the metal from solutions of its salts. It is precipitated.from its salts by the action of phosphorous acid and of sodium hypophosphite.


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