File:Metals and their hydroxides.JPG

Summary

An assortment of metals and their hydroxides produced by placing them on the anode of a sodium-carbonate-electrolyte electrolysis system in lids. Aluminium does not form its hydroxide well this way. With a longer wait all of the others could have formed more hydroxides. Lithium hydroxide is formed by reacting lithium with water and not by electrolysis. It dissolves in water so it could not be placed in a large amount of water as the others are. The arrows point to where the metal was electrolyzed. Carbon was used as the cathode.

1. Copper produced bluish copper(II) hydroxide, here tainted with a yellow impurity.
2. Tin produced off-white tin(II) oxide hydrate and white tin dioxide. Most remained on the tin piece.
3. Aluminium produced small amounts of aluminium hydroxide. Most remained on the aluminium piece.
4. Zinc produced white zinc hydroxide. Some remained on the zinc piece.
5. Lithium reacted with a small amount of water to make white and corrosive lithium hydroxide. It dissolves in water. Lithium is silvery when pure but very easily blackens in air. The piece on the side is blackened lithium.
6. Cupronickel from a U.S. nickel produced blue copper(II) hydroxide and blue nickel(II) hydroxide.
7. Iron produced dark green-gray iron(II) hydroxide, which oxidizes on exposure to air to brown iron(III) oxide.

For those who cannot read or understand English, chemical symbols are provided on the photo.

Copyright status:

Public Domain

Source:

user:chemicalinterest