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In a pure solution, potassium slowly reacts with ammonia to form Potassium oxidizes faster than most metals and often forms oxides containing oxygen-oxygen bonds, as do all alkali metals except lithium.

There are three possible oxides of potassium: potassium oxide (K).

With oxygen it forms potassium peroxide, and with water potassium forms potassium hydroxide.

The latter two species, especially the superoxide, are rare and are formed only in reaction of very electropositive metals (Na, K, Rb, Cs, etc.) with oxygen; these species contain oxygen-oxygen bonds.

All potassium-oxygen binary compounds are known to react with water violently, forming potassium hydroxide.

It is found dissolved in sea water (which is 0.04% potassium by weight), and is part of many minerals.

Potassium is chemically very similar to sodium, the previous element in group 1 of the periodic table.

Fresh fruits and vegetables are good dietary sources of potassium.

The body responds to the influx of dietary potassium, which raises serum potassium levels, with a shift of potassium from outside to inside cells and an increase in potassium excretion by the kidneys.

Hydrogen reacts again with atmospheric oxygen, producing water, which reacts with the remaining potassium.

This reaction requires only traces of water; because of this, potassium and the liquid sodium-potassium (Na K) alloy are potent desiccants that can be used to dry solvents prior to distillation.

Potassium is a chemical element with symbol K (from Neo-Latin kalium) and atomic number 19.

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