Platinum

Not to be confused with Palladium.

Platinum is a chemical element. It has symbol Pt and atomic number 78. Platinum is a soft, heavy, white metal. It is a precious metal and a transition metal. Its name comes from the Spanish word platina meaning "little silver".^[4][5]

Platinum, ₇₈Pt

Platinum
Pronunciation	/ˈplætənəm/ ​(PLAT-ən-əm)
Appearance	silvery white
Standard atomic weight Ar°(Pt)
	195.084(9)[1]
Platinum 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 Pd ↑ Pt ↓ Ds iridium ← platinum → gold
Atomic number (Z)	78
Group	group 10
Period	period 6
Block	d-block
Electron configuration	[Xe] 4f14 5d9 6s1
Electrons per shell	2, 8, 18, 32, 17, 1
Physical properties
Phase at STP	solid
Melting point	2041.4 K ​(1768.3 °C, ​3214.9 °F)
Boiling point	4098 K ​(3825 °C, ​6917 °F)
Density (near r.t.)	21.45 g/cm3
when liquid (at m.p.)	19.77 g/cm3
Heat of fusion	22.17 kJ/mol
Heat of vaporization	510 kJ/mol
Molar heat capacity	25.86 J/(mol·K)
Vapor pressure P (Pa) 1 10 100 1 k 10 k 100 k at T (K) 2330 (2550) 2815 3143 3556 4094
Atomic properties
Oxidation states	−3, −2, −1, 0, +1, +2, +3, +4, +5, +6 (a mildly basic oxide)
Electronegativity	Pauling scale: 2.28
Ionization energies	1st: 870 kJ/mol 2nd: 1791 kJ/mol
Atomic radius	empirical: 139 pm
Covalent radius	136±5 pm
Van der Waals radius	175 pm
Spectral lines of platinum
Other properties
Natural occurrence	primordial
Crystal structure	​face-centered cubic (fcc)
Speed of sound thin rod	2800 m/s (at r.t.)
Thermal expansion	8.8 µm/(m⋅K) (at 25 °C)
Thermal conductivity	71.6 W/(m⋅K)
Electrical resistivity	105 nΩ⋅m (at 20 °C)
Magnetic ordering	paramagnetic
Molar magnetic susceptibility	+201.9 × 10−6 cm3/mol (290 K)[2]
Tensile strength	125–240 MPa
Young's modulus	168 GPa
Shear modulus	61 GPa
Bulk modulus	230 GPa
Poisson ratio	0.38
Mohs hardness	3.5
Vickers hardness	400–550 MPa
Brinell hardness	300–500 MPa
CAS Number	7440-06-4
History
Discovery	Antonio de Ulloa (1735)
Isotopes of platinum v e
Main isotopes[3] Decay abun­dance half-life (t1/2) mode pro­duct 190Pt 0.0120% 4.83×1011 y α 186Os 192Pt 0.782% stable 193Pt synth 50 y ε 193Ir 194Pt 32.9% stable 195Pt 33.8% stable 196Pt 25.2% stable 198Pt 7.36% stable
Category: Platinum view talk edit | references

Platinum is part of the platinum group of elements. It is on group 10 in the periodic table of elements. Its atoms have an atomic weight of 195 atomic mass units. It has 6 isotopes that is found in nature. Platinum can be found in some nickel and copper ores. 90% of platinum is found in the Ural Mountains, Colombia, the Sudbury basin of Canada, and a large reserve in South Africa.^[6]: 779

Some platinum nuggets from nature.

In the past, it was worth more than gold. Since the late 2010s, gold cost more. The element is hard to find in the Earth's crust. It has an average abundance of about 5 μg/kg.^[6] Since it is so rare, only a few hundred tonnes of Platinum are made every year.

Platinum is very dense; almost twice as dense as lead. It is malleable and ductile. This means it can be made thin sheets and it can be pulled into wire. Platinum is very stable. Acids do not change platinum.

Platinum has many uses. The most common use of Platinum is in a vehicle's catalytic converter. It is also used in laboratory equipment, electrical contacts and electrodes, platinum resistance thermometers, dentistry equipment, and jewelry. Platinum is also used in the glass industry.^[7] There, it is used to change molten glass. Elemental platinum is not found to be dangerous to human health. Compounds that have platinum, such as cisplatin, oxaliplatin and carboplatin, are used in chemotherapy against some types of cancer.^[8]

Related pages

Platinum group