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Potassium, 19K
Potassium-2.jpg
Potassium pearls (in paraffin oil, ~5 mm each)
Potassium
Pronunciation /pəˈtæsiəm/ (pə-TAS-ee-əm)
Appearance silvery gray
Standard atomic weight Ar, std(K) 39.0983(1)
Potassium in the periodic table
Hydrogen Helium
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton
Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon
Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon
Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson
Na

K

Rb
argonpotassiumcalcium
Atomic number (Z) 19
Group group 1: hydrogen and alkali metals
Period period 4
Block   s
Electron configuration [Ar] 4s1
Electrons per shell 2, 8, 8, 1
Physical properties
Phase at STP solid
Melting point 336.53 K ​(63.38 °C, ​146.08 °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
Triple point 336.35 K, ​ kPa
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
  • (more)
Atomic radius empirical: 227 pm
Covalent radius 203±12 pm
Van der Waals radius 275 pm
Color lines in a spectral range
Spectral lines of potassium
Other properties
Natural occurrence primordial
Crystal structure body-centered cubic (bcc)
Body-centered cubic crystal structure for potassium
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 n Ω⋅m (at 20 °C)
Magnetic ordering paramagnetic
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 Humphry Davy (1807)
First isolation Humphry Davy (1807)
Symbol "K": from New Latin kalium
Main isotopes of potassium
Iso­tope Abun­dance Half-life (t1/2) Decay mode Pro­duct
39K 93.26% 39K is stable with 20 neutrons
40K 0.012% 1.248(3)×109 y β 1.311 40Ca
ε 1.505 40Ar
β+ 1.505 40Ar
41K 6.73% 41K is stable with 22 neutrons
Potassium
Potassium metal

Potassium is a special chemical element you can find on the periodic table. Its symbol is K, which comes from the Latin word kalium. Potassium has an atomic number of 19. This means it has 19 protons and 19 electrons. You won't find pure potassium metal in nature because it reacts very easily with other things.

Potassium has different forms called isotopes. Two of its stable isotopes have 20 or 22 neutrons. Its atomic mass is about 39.098. There's also an unstable isotope with 21 neutrons. This one is a common radioactive material.

What is Potassium Like?

Physical Features

Potassium is a soft, silvery-gray metal. It's so soft you can easily cut it with a knife! It melts at a very low temperature, around 63 degrees Celsius (145.4 degrees Fahrenheit). This makes it one of the metals that melts easily. It belongs to a group of elements called alkali metals. After lithium, it's the second lightest metal.

How Potassium Reacts

Potassium reacts in many ways, similar to sodium and other alkali metals. When it touches air, it quickly gets a whitish layer on its surface. This is called oxidation or tarnishing. Because it reacts so fast with air and water, potassium is usually stored in oil.

If you put a large piece of potassium in water, it reacts very strongly. This reaction creates hydrogen gas, which can catch fire! It also forms a substance called potassium hydroxide. Potassium also burns easily in the air, forming other compounds like peroxides or superoxides.

Potassium Compounds

Flame Test K
Potassium chloride in a flame

Potassium always forms compounds where it has a +1 oxidation state. This means it loses one electron when it forms a chemical bond. Potassium ions are clear and look a lot like sodium ions.

Many potassium compounds are safe to use. If a potassium compound is harmful, it's usually because of the other part of the compound, not the potassium itself. For example, potassium chromate is yellow and harmful because of the chromate part, not the potassium.

Here are some common potassium compounds:

Where Does the Name "Potassium" Come From?

The name "potassium" comes from the word "potash." Potash is a mix of potassium carbonate and potassium hydroxide. People have used potash for a very long time. In the past, it was made by burning ashes in pots. Today, potash is used to make fertilizer, soap, and glass.

Where is Potassium Found?

You won't find pure potassium metal in nature because it's too reactive. Instead, it's found in different minerals. We get potassium from these minerals using a process called electrolysis. This involves melting potassium hydroxide or potassium chloride at very high temperatures and then using electricity to separate the potassium.

How is Potassium Used?

Pure potassium metal is used in science to remove water from certain liquids called solvents. It's also used in some scientific tools.

Potassium compounds are used in many everyday items:

Potassium ions are super important for living things, including you! That's why fertilizers contain potassium compounds. These ions help send messages between cells in your body. They help biological membranes change their electric charge, which is needed for muscles to contract (get shorter and move things). This is also vital for your heart to beat and pump blood. If the amount of potassium in your blood is too high or too low, it can be very dangerous and even stop your heart. Foods like bananas, apricots, and raisins are good sources of potassium.

Is Potassium Safe?

Pure potassium metal is very dangerous. If it's left in the air, it can form a coating that might explode. It also reacts very strongly with water, creating a harmful liquid.

However, most potassium compounds are not dangerous on their own. They are only harmful if they contain a toxic anion, which is the other part of the compound, like chromate or chlorate.

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