Thallium: the essentials
Thallium atoms have 81 electrons and the shell structure is 126.96.36.199.18.3. The ground state electronic configuration of neutral thallium is [Xe].4f14.5d10.6s2.6p1 and the term symbol of thallium is 2P1/2.
When freshly exposed to air, thallium exhibits a metallic lustre, but soon develops a bluish-grey tinge, resembling lead in appearance. A heavy oxide builds up on thallium if left in air, and in the presence of water the hydroxide is formed. The metal is very soft and malleable. It can be cut with a knife.
The element and its compounds are toxic and should be handled carefully. Thallium may cause cancer.
Cartoon by Nick D Kim ([Science and Ink], used by permission).
Thallium: physical properties
Thallium: heat properties
- Melting point: 577 [304 °C (579 °F)] K
- Boiling point: 1746 [1473 °C (2683 °F)] K
- Enthalpy of fusion: 20.5 kJ mol-1
Thallium: atom sizes
- Atomic radius (empirical): 190 pm
- Molecular single bond covalent radius: 144 (coordination number 3) ppm
- van der Waals radius: 260 ppm
- Pauling electronegativity: 1.62 (Pauling units)
- Allred Rochow electronegativity: 1.44 (Pauling units)
- Mulliken-Jaffe electronegativity: 1.96 (sp2 orbital)
Thallium: orbital properties
- First ionisation energy: 589.36 kJ mol‑1
- Second ionisation energy: 1971.03 kJ mol‑1
- Third ionisation energy: 2880.28 kJ mol‑1
Thallium: crystal structure
Thallium: biological data
- Human abundance by weight: (no data) ppb by weight
Thallium has no biological role. Thallium compounds are extremely toxic. Their effects are cumulative and they can be absorbed though the skin. Thallium poisoning takes several days to act and it affects the nervous system.
Reactions of thallium as the element with air, water, halogens, acids, and bases where known.
Thallium: binary compounds
Binary compounds with halogens (known as halides), oxygen (known as oxides), hydrogen (known as hydrides), and other compounds of thallium where known.
Thallium: compound properties
Bond strengths; lattice energies of thallium halides, hydrides, oxides (where known); and reduction potentials where known.
Thallium: historyThallium was discovered by Sir William Crookes in 1861 at England. Origin of name: from the Greek word "thallos" meaning "green twig" or green shoot.
Thallium has two stable isotopes and one of these, Tl-203, is used to produce one of the (workhorses( of nuclear medicine: Tl-201. Tl-201 is used extensively for imaging and in particular for perfusion tests of the myocardium. These tests are done to determine the damage to the heart from a heart attack or from heart diseases. Tl205 has been proposed as an alternative target for the production of Tl-201. Tl-205 is also used in nuclear magnetic resonance research.
Isolation: thallium metal would not normally be made in the laboratory as it is available commercially. Crude thallium is present as a component in flue dust along with arsenic, cadmium, indium, germanium, lead, nickel, selenium, tellurium, and zinc. This is done by dissolving in dilute acid, precipitating out lead sulphate, and then adding HCl to precipitate thallium chloride, TlCl. Further purification can be achieve by electrolysis of soluble thallium salts.