Potassium

Potassium, ₀₀K
	Potassium pearls (in paraffin oil, ~5 mm each)
Potassium
Appearance	silvery gray
Standard atomic weight Ar°(K)
	39.0983(1)
Potassium in the periodic table
	argon ← potassium → calcium
Group	group 1: hydrogen and alkali metals
Period	period 4
Block	s-block
Electron configuration	[Ar] 4s1
Electrons per shell	2, 8, 8, 1
Physical properties
Phase at STP	solid
Melting point	336.7 K (63.5 °C, 146.3 °F)
Boiling point	1032 K (759 °C, 1398 °F)
Density (near r.t.)	0.862 g/cm3
when liquid (at m.p.)	0.828 g/cm3
Critical point	2223 K, 16 MPa
Heat of fusion	2.33 kJ/mol
Heat of vaporization	76.9 kJ/mol
Molar heat capacity	29.6 J/(mol·K)
Atomic properties
Oxidation states	−1, +1 (a strongly basic oxide)
Electronegativity	Pauling scale: 0.82
Ionization energies	1st: 418.8 kJ/mol ; 2nd: 3052 kJ/mol ; 3rd: 4420 kJ/mol ; (more) ;
Atomic radius	empirical: 227 pm
Covalent radius	203±12 pm
Van der Waals radius	275 pm
	Spectral lines of potassium
Other properties
Natural occurrence	primordial
Crystal structure	body-centered cubic (bcc)
Speed of sound thin rod	2000 m/s (at 20 °C)
Thermal expansion	83.3 µm/(m⋅K) (at 25 °C)
Thermal conductivity	102.5 W/(m⋅K)
Electrical resistivity	72 nΩ⋅m (at 20 °C)
Magnetic ordering	paramagnetic
Molar magnetic susceptibility	+20.8·10−6 cm3/mol (298 K)
Young's modulus	3.53 GPa
Shear modulus	1.3 GPa
Bulk modulus	3.1 GPa
Mohs hardness	0.4
Brinell hardness	0.363 MPa
CAS Number	7440-09-7
History
Discovery and first isolation	Humphry Davy (1807)
Symbol	"K": from New Latin kalium
Isotopes of potassium v; e;
ε	40Ar
β+	40Ar
	Category: Potassium; view; talk; edit; \| references

Potassium is a chemical element in the periodic table. It has the symbol K. This symbol is taken from the Latin word kalium. Potassium's atomic number is 19. It has 19 protons and electrons. Potassium is not found as an element in nature, because it is so reactive.

Potassium has two stable isotopes, with 20 or 22 neutrons. Its atomic mass is 39.098. The unstable isotope with 21 neutrons is one of the most common radioactive materials.

Properties

Physical properties

Potassium is a soft gray metal. It can be cut easily with a knife. Its melting point is 63 degrees Celsius (145.4 degrees Fahrenheit). It melts at a very low temperature. It is an alkali metal. It is the second lightest metal, after lithium.

Chemical properties

A reaction of potassium metal with water. Hydrogen is liberated. The pink or lilac flame comes from burning potassium vapor. Strongly alkaline potassium hydroxide is formed in solution.^[5]

Potassium reacts in many chemical reactions similar to sodium and other alkali metals. It tarnishes in air to produce a whitish oxidized layer on the surface. This is why it is stored in oil. It also reacts very fast with water, which is another reason for its storage in oil. The hydrogen produced during its reaction with water can burst into flames when a large amount of potassium is added to water. Potassium hydroxide is also produced. Potassium also burns in air easily, to make the peroxide or the superoxide.

Chemical compounds

Potassium compounds are only in one oxidation state: +1. Potassium ions are colorless and similar to sodium ions. Potassium chloride can be used as a substitute for table salt. Potassium hydroxide is used in the electrolyte of alkaline cells. Most potassium compounds are nontoxic. If they are toxic, it is because of the anion. Potassium chromate is colored because of the chromate, not the potassium. Potassium chromate is toxic because of the chromate, not the potassium.

Chrome alum
Potash alum
Potassium arsenate, oxidizing agent, toxic
Potassium arsenite, colorless solid, toxic
Potassium bromate, colorless, oxidizing agent, used in flour
Potassium bromide, colorless, used as sedative
Potassium carbonate, colorless, reacts with acids
Potassium chlorate, used in matches and explosives
Potassium chloride, salt substitute
Potassium chromate, yellow solid, oxidizing agent, toxic
Potassium dichromate, red solid, oxidizing agent, toxic
Potassium fluoride, used to make fluorine, corrosive
Potassium hydroxide, also known as potash, caustic, strong base, white solid
Potassium hypomanganate, bright blue hypomanganate, rare
Potassium iodate, used to supply iodine
Potassium iodide, used to supply iodine
Potassium manganate, used to make potassium permanganate
Potassium nitrate, used in gunpowder
Potassium perchlorate, used in some rockets
Potassium periodate
Potassium permanganate, purple, disinfectant, oxidizing agent
Potassium sulfide, reacts with water
Potassium sulfite, used in food preservation
Potassium sulfate, colorless, used in fertilizers

Potassium hydroxide
Potassium chlorate
Potassium chloride
Potassium chromate

Name

The word potassium comes from the word "potash". Potash is a mixture of potassium carbonate and potassium hydroxide that has been used for a very long time. In past centuries potash was made from ashes in pots. It is used to make fertilizer, soap, and glass.

Occurrence

Potassium does not occur in nature because it is too reactive. It is found in minerals, though. It is extracted from them by electrolysis of potassium hydroxide or potassium chloride. The potassium hydroxide or potassium chloride has to be melted at a very high temperature.

Uses

Potassium metal is used to absorb water from solvents. It is also used in some scientific instruments.

Potassium compounds are used in soap, fertilizer, explosives, and matches.

Nutrition

Potassium ions are very important to organisms. That is why fertilizers have potassium compounds in them. The ions send messages from cells to other cells. It helps biological membranes depolarize. This means go from a negative to a positive electrical charge. This is needed for muscles to contract (get shorter and move things.) It is needed for the heart to beat (push blood through blood vessels.) If the potassium level in the blood is too high or too low it can cause death because the heart stops.^[6] A few good sources of potassium are bananas, apricots and raisins.

Safety

Potassium metal is very dangerous and can form an explosive coating if it is kept in air. It also reacts violently with water, spewing corrosive liquid. Potassium compounds are not normally dangerous, unless they contain a toxic anion like chromate or chlorate.

Related pages

Other websites

Potassium -Citizendium

References

↑ "Standard Atomic Weights: Potassium". CIAAW. 1979.
↑ Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.122. ISBN 1439855110.
↑ Magnetic susceptibility of the elements and inorganic compounds, in Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
↑ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
↑ "Potassium". Retrieved 13 October 2010.^{[permanent dead link]}
↑ Whelton, P.; He, J.; Cutler, J.; Brancati, F.; Appel, L.; Follmann, D.; Klag, M. (1997). "Effects of oral potassium on blood pressure. Meta-analysis of randomized controlled clinical trials". JAMA. 277 (20): 1624–1632. doi:10.1001/JAMA.1997.03540440058033. PMID 9168293. S2CID 25937399.

This short article about chemistry can be made longer. You can help Wikipedia by adding to it.

[1] "Standard Atomic Weights: Potassium". CIAAW. 1979.

[2] Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.122. ISBN 1439855110.

[3] Magnetic susceptibility of the elements and inorganic compounds, in Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.

[4] Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.

[5] "Potassium". Retrieved 13 October 2010.^{[permanent dead link]}

[6] Whelton, P.; He, J.; Cutler, J.; Brancati, F.; Appel, L.; Follmann, D.; Klag, M. (1997). "Effects of oral potassium on blood pressure. Meta-analysis of randomized controlled clinical trials". JAMA. 277 (20): 1624–1632. doi:10.1001/JAMA.1997.03540440058033. PMID 9168293. S2CID 25937399.

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v t e Potassium compounds
H, (pseudo)halogens	KF KHF₂ KH KCl KClO KClO₃ KClO₄ KBr KBrO₃ KI KIO₃ KIO₄ KAt KCN KCNO KOCN KSCN
chalcogens	K₂O KOH K₂O₂ KO₂ KO₃ K₂S KHS K₂SO₃ KHSO₃ K₂SO₄ KHSO₄ KHSO₅ K₂S₂O₃ K₂S₂O₅ K₂S₂O₇ K₂S₂O₈ K₂Se K₂SeO₃ K₂SeO₄ K₂Te K₂TeO₃ K₂TeO₄ K₂Po
pnictogens	K₃N KNH₂ KN₃ KNO₂ KNO₃ K₃P KH₂PO₃ K₃PO₄ K₂HPO₄ KH₂PO₄ KPF₆ KAsO₂ K₃AsO₄ K₂HAsO₄ KH₂AsO₄
B, C group	B₄K₂O₇ K₂CO₃ KHCO₃ K₂SiO₃ K₂SiF₆ K₂Al₂O₄ K₂Al₂B₂O₇
transition metals	K₂PtCl₄ K₂Pt(CN)₄ K 2TiF 6 K₂PtCl₆ K₂ReCl₆ K ₂ReF ₆ KAsF 6 K 2ReBr 6 K ₂ReI ₆ K 2ZrF 6 K₄Fe(CN)₆ K₃Fe(CN)₆ K₃Fe(C₂O₄)₃ K₂FeO₄ K₂MnO₄ KMnO₄ K₃CrO₄ K₂CrO₄ K₃CrO₈ KCrO₃Cl K₂Cr₂O₇ K₂Cr₃O₁₀ K₂Cr₄O₁₃ K₄Mo₂Cl₈
organic	KHCO₂ KCH₃CO₂ KCF₃CO₂ K₂C₂O₄ KHC₂O₄ KC₁₂H₂₃O₂ KC₁₈H₃₅O₂ C₃H₂K₂O₄ C₄H₆KO₄ C₅H₇KO₄