Science, Tech, Math › Science Platinum Element Facts You Need to Know Platinum Chemical & Physical Properties Share Flipboard Email Print Douglas Sacha / Getty Images Science Chemistry Periodic Table Basics Chemical Laws Molecules Projects & Experiments Scientific Method Biochemistry Physical Chemistry Medical Chemistry Chemistry In Everyday Life Famous Chemists Activities for Kids Abbreviations & Acronyms Biology Physics Geology Astronomy Weather & Climate By Anne Marie Helmenstine, Ph.D. Chemistry Expert Ph.D., Biomedical Sciences, University of Tennessee at Knoxville B.A., Physics and Mathematics, Hastings College Dr. Helmenstine holds a Ph.D. in biomedical sciences and is a science writer, educator, and consultant. She has taught science courses at the high school, college, and graduate levels. our editorial process Facebook Facebook Twitter Twitter Anne Marie Helmenstine, Ph.D. Updated November 16, 2019 Platinum is a transition metal that is highly valued for jewelry and alloys. There are many interesting facts about this element. Platinum Basic Facts Atomic number: 78Symbol: PtAtomic weight: 195.08 Discovery It's difficult to assign credit for the discovery. Ulloa 1735 (in South America), Wood in 1741, Julius Scaliger in 1735 (Italy) can all make claims to this honor. Platinum was used in relatively pure form by the pre-Columbian Native Americans. Electron configuration: [Xe] 4f14 5d9 6s1 Word Origin "Platinum" comes from the Spanish word platina, meaning "little silver." Isotopes Six stable isotopes of platinum occur in nature (190, 192, 194, 195, 196, 198). Information on three additional radioisotopes is available (191, 193, 197). Properties Platinum has a melting point of 1772 degrees C, the boiling point of 3827 +/- 100 degrees C, the specific gravity of 21.45 (20 degrees C), with a valence of 1, 2, 3, or 4. Platinum is a ductile and malleable silvery-white metal. It does not oxidize in air at any temperature, although it is corroded by cyanides, halogens, sulfur, and caustic alkalis. Platinum does not dissolve in hydrochloric or nitric acid but will dissolve when the two acids are mixed to form aqua regia. Uses Platinum is used in jewelry, wire, to make crucibles and vessels for laboratory work, electrical contacts, thermocouples, for coating items that must be exposed to high temperatures for long periods of time or must resist corrosion, and in dentistry. Platinum-cobalt alloys have interesting magnetic properties. Platinum absorbs large amounts of hydrogen at room temperature, yielding it at red heat. The metal is often used as a catalyst. The platinum wire will glow red-hot in the vapor of methanol, where it acts as a catalyst, converting it to formaldehyde. Hydrogen and oxygen will explode in the presence of platinum. Where to Find It Platinum occurs in native form, usually with small amounts of other metals belonging to the same group (osmium, iridium, ruthenium, palladium, and rhodium). Another source of the metal is sperrylite (PtAs2). Element Classification Transition metal Platinum Physical Data Density (g/cc): 21.45Melting point (K): 2045Boiling point (K): 4100Appearance: Very heavy, soft, silvery-white metalAtomic radius (pm): 139Atomic volume (cc/mol): 9.10Covalent radius (pm): 130Ionic radius: 65 (+4e) 80 (+2e)Specific heat (@20 degrees C J/g mol): 0.133Fusion heat (kJ/mol): 21.76Evaporation heat (kJ/mol): ~470Debye temperature (K): 230.00Pauling negativity number: 2.28First ionizing energy (kJ/mol): 868.1Oxidation states: 4, 2, 0Lattice structure: Face-Centered CubicLattice constant (Å): 3.920 Sources Dean, John A. "Lange's Handbook of Chemistry." 15th Edition, McGraw-Hill Professional, October 30, 1998. "Platinum." Periodic Table of Elements, Los Alamos National Laboratory, U.S. Department of Energy's NNSA, 2016. Rumble, John. "CRC Handbook of Chemistry and Physics, 100th Edition." CRC Press, June 7, 2019.