Thallium
Thallium is a soft, bluish-gray post-transition metal that's highly toxic to humans and most other animals, a property that has shaped almost everything about how it's used and regulated. It was first identified not by isolating the metal itself but by spotting a distinctive bright green line in its light spectrum, a then-new technique that was transforming how chemists found new elements.
- Group · Period
- 13 · 6
- At room temp
- solid
- Melts at
- 577 K
- Density
- 11.8 g/cm³
- Discovered
- 1861
Uses
Thallium’s toxicity has limited most of its historical uses, but a few specialized applications remain. Thallium compounds are used in certain optical glasses and infrared-transmitting lenses because they bend light in useful ways that ordinary glass doesn’t. Thallium-doped crystals are also used inside radiation detectors, where they help convert incoming radiation into flashes of light that instruments can measure, a technique used in some medical and scientific equipment. In medicine, a radioactive isotope, thallium-201, is used in small, controlled doses for nuclear imaging tests that assess blood flow to the heart muscle.
Thallium’s older use as an ingredient in rodent and insect poisons has largely been discontinued in most countries, precisely because it proved too dangerous to handle safely and too easy to misuse.
History
Thallium was discovered in 1861 by English chemist William Crookes, who noticed an unfamiliar bright green line while examining the spectrum of residue from sulfuric acid production — a striking signature that pointed to a previously unknown element. He named it thallium after the Greek word for a green shoot, describing that distinctive spectral line. Around the same period, French chemist Claude-Auguste Lamy worked out how to isolate enough of the actual metal to study its properties directly, and the two scientists’ overlapping work helped firmly establish thallium as a new element in the years that followed.
Fun facts
- Thallium is odorless and tasteless, which made it a favored poison in the 20th century before its sale became tightly restricted — it's sometimes nicknamed 'the poisoner's poison.'
- Thallium's name comes from the Greek word thallos, meaning 'green shoot' or 'green twig,' describing the bright green line it produces when its spectrum is examined.
- Despite its toxicity, thallium compounds are used in specialized medical imaging to help doctors assess blood flow to the heart.
Frequently asked questions
Why was thallium used in rat poison?
Thallium sulfate is odorless, tasteless, and highly toxic in small doses, which once made it an effective poison for rodents. Those same properties made it dangerously easy to misuse against people, and concerns over accidental and deliberate poisonings led most countries to ban its use in household pest control.
How was thallium discovered if it's so toxic?
British scientist William Crookes identified thallium in 1861 using spectroscopy, a technique that reveals an element's presence from the specific colors of light it emits, without needing to isolate and handle a pure sample first. Around the same time, French chemist Claude-Auguste Lamy independently worked out how to isolate the metal itself.
Does thallium have any medical use today?
Yes, in a controlled way — a radioactive form called thallium-201 is injected in tiny, carefully measured amounts during certain heart stress tests, since it collects in healthy heart muscle in a pattern doctors can image. This is very different from bulk thallium exposure, which remains dangerous.
Compounds
5 notable compounds containing Tl
- TlClsalt
Thallium(I) chloride
A white, light-sensitive solid whose low solubility and crystal structure closely parallel silver chloride, a reflection of how similarly thallium(I) and silver(I) ions behave in solution.
Used for: Laboratory reagent for preparing other thallium compounds
- TlIsalt
Thallium(I) iodide
A yellow crystalline solid that, unlike most thallium(I) halides, adopts a distorted layered structure rather than the simple rock-salt packing seen in TlCl and TlBr.
Used for: Additive in metal-halide lamps to enhance green light output
- Tl2Ooxide
Thallium(I) oxide
A black, water-reactive solid that readily absorbs moisture from air to form thallium hydroxide, reflecting how thallium's +1 state behaves more like an alkali metal oxide than a typical post-transition-metal oxide.
Used for: Precursor in the manufacture of specialty optical glass
- Tl2SO4salt
Thallium(I) sulfate
A colorless, odorless, water-soluble salt whose lack of taste or smell made it dangerously easy to misuse before its restriction, since thallium(I) mimics potassium closely enough to be absorbed by the body.
Used for: Formerly a widely used rodenticide and ant killer, now banned in most countries
- Tl2O3oxide
Thallium(III) oxide
A black, brittle solid in which thallium sits in its less stable +3 state, making the compound a mild oxidizer that can decompose to thallium(I) oxide on heating.
Used for: Transparent conducting films and component of some thallium-based superconducting ceramics
Isotopes
42 known isotopes
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| Isotope | Natural abundance | Half-life | Decay mode | Mass excess | Binding energy / nucleon | Decay width |
|---|---|---|---|---|---|---|
| Tl-203 stable | 29.515% | Stable | — | -25,761.31 keV | 7,886.05 keV | — |
| Tl-205 stable | 70.485% | Stable | — | -23,820.8 keV | 7,878.39 keV | — |
Show all 42 isotopes
| Tl-176 | — | 5.2 ms | Proton emission (100%) | 584.73 keV | 7,707.94 keV | 8.77 × 10-14 eV |
| Tl-177 | — | 18 ms | Alpha decay (73%), Proton emission (27%) | -3,340.1 keV | 7,732.17 keV | 2.53 × 10-14 eV |
| Tl-178 | — | 254 ms | Alpha decay (53%), Electron capture / beta-plus decay (47%) | -4,613 keV | 7,741 keV | 1.80 × 10-15 eV |
| Tl-179 | — | 0.23 s | Alpha decay (100%), Electron capture / beta-plus decay, Proton emission | -8,269.63 keV | 7,763.49 keV | 1.98 × 10-15 eV |
| Tl-180 | — | 1.09 s | Electron capture / beta-plus decay (94%), Alpha decay (6%), ECSF (0.0032%) | -9,390.44 keV | 7,771.43 keV | 4.19 × 10-16 eV |
| Tl-181 | — | 3.2 s | Alpha decay (10%) | -12,798.75 keV | 7,791.92 keV | 1.43 × 10-16 eV |
| Tl-182 | — | 3.1 s | Electron capture / beta-plus decay (97.5%), Alpha decay (5%) | -13,327.21 keV | 7,796.36 keV | 1.47 × 10-16 eV |
| Tl-183 | — | 6.9 s | Electron capture / beta-plus decay (0%), Alpha decay | -16,587.26 keV | 7,815.67 keV | 6.61 × 10-17 eV |
| Tl-184 | — | 10.1 s | Electron capture / beta-plus decay (97.9%), Alpha decay (2.1%) | -16,883.36 keV | 7,818.67 keV | 4.52 × 10-17 eV |
| Tl-185 | — | 19.5 s | Electron capture / beta-plus decay | -19,757.75 keV | 7,835.58 keV | 2.34 × 10-17 eV |
| Tl-186 | — | 3.4 s | Alpha decay | -19,882.94 keV | 7,837.52 keV | 1.34 × 10-16 eV |
| Tl-187 | — | 51 s | Electron capture / beta-plus decay (100%), Alpha decay (0.03%) | -22,444.59 keV | 7,852.47 keV | 8.95 × 10-18 eV |
| Tl-188 | — | 71 s | Electron capture / beta-plus decay (100%) | -22,336.4 keV | 7,853.05 keV | 6.43 × 10-18 eV |
| Tl-189 | — | 2.3 m | Electron capture / beta-plus decay (100%) | -24,616.11 keV | 7,866.27 keV | 3.31 × 10-18 eV |
| Tl-190 | — | 2.6 m | Electron capture / beta-plus decay (100%) | -24,366.24 keV | 7,866.03 keV | 2.92 × 10-18 eV |
| Tl-191 | — | — | Unknown | -26,282.95 keV | 7,877.14 keV | — |
| Tl-192 | — | 9.6 m | Electron capture / beta-plus decay (100%) | -25,872.25 keV | 7,876.02 keV | 7.92 × 10-19 eV |
| Tl-193 | — | 21.6 m | Electron capture / beta-plus decay (100%) | -27,477.22 keV | 7,885.34 keV | 3.52 × 10-19 eV |
| Tl-194 | — | 33.0 m | Electron capture / beta-plus decay (100%), Alpha decay (1e-7%) | -26,937.5 keV | 7,883.52 keV | 2.30 × 10-19 eV |
| Tl-195 | — | 1.16 h | Electron capture / beta-plus decay (100%) | -28,155.29 keV | 7,890.73 keV | 1.09 × 10-19 eV |
| Tl-196 | — | 1.84 h | Electron capture / beta-plus decay (100%) | -27,496.6 keV | 7,888.29 keV | 6.89 × 10-20 eV |
| Tl-197 | — | 2.84 h | Electron capture / beta-plus decay (100%) | -28,354.22 keV | 7,893.57 keV | 4.46 × 10-20 eV |
| Tl-198 | — | 5.3 h | Electron capture / beta-plus decay (100%) | -27,528.75 keV | 7,890.3 keV | 2.39 × 10-20 eV |
| Tl-199 | — | 7.42 h | Electron capture / beta-plus decay (100%) | -28,059.4 keV | 7,893.88 keV | 1.71 × 10-20 eV |
| Tl-200 | — | 26.1 h | Electron capture / beta-plus decay (100%) | -27,047.23 keV | 7,889.7 keV | 4.86 × 10-21 eV |
| Tl-201 | — | 3.0420 d | Electron capture (100%) | -27,180.78 keV | 7,891.27 keV | 1.74 × 10-21 eV |
| Tl-202 | — | 12.31 d | Electron capture / beta-plus decay (100%) | -25,980.42 keV | 7,886.22 keV | 4.29 × 10-22 eV |
| Tl-204 | — | 3.783 Y | Beta-minus decay (97.08%), Electron capture / beta-plus decay (2.92%) | -24,346.07 keV | 7,880.02 keV | 3.82 × 10-24 eV |
| Tl-206 | — | 4.202 m | Beta-minus decay (100%) | -22,253.29 keV | 7,871.72 keV | 1.81 × 10-18 eV |
| Tl-207 | — | 4.77 m | Beta-minus decay (100%) | -21,034.44 keV | 7,866.8 keV | 1.59 × 10-18 eV |
| Tl-208 | — | 3.053 m | Beta-minus decay (100%) | -16,750.12 keV | 7,847.18 keV | 2.49 × 10-18 eV |
| Tl-209 | — | 2.162 m | Beta-minus decay (100%) | -13,644.79 keV | 7,833.4 keV | 3.52 × 10-18 eV |
| Tl-210 | — | 1.30 m | Beta-minus decay (100%), Beta-minus, neutron emission (0.007%) | -9,247 keV | 7,813.59 keV | 5.85 × 10-18 eV |
| Tl-211 | — | 88 s | Beta-minus decay (100%), Beta-minus, neutron emission | -6,078 keV | 7,799.79 keV | 5.18 × 10-18 eV |
| Tl-212 | — | 30.9 s | Beta-minus decay (100%), Beta-minus, neutron emission (1.8%) | -1,551 keV | 7,780 keV | 1.48 × 10-17 eV |
| Tl-213 | — | 23.8 s | Beta-minus decay (100%), Beta-minus, neutron emission (7.6%) | 1,783.81 keV | 7,765.43 keV | 1.92 × 10-17 eV |
| Tl-214 | — | 11.0 s | Beta-minus decay (100%), Beta-minus, neutron emission (34%) | 6,465 keV | 7,745 keV | 4.15 × 10-17 eV |
| Tl-215 | — | 9.7 s | Beta-minus decay (100%), Beta-minus, neutron emission (4.6%) | 10,030 keV | 7,730 keV | 4.70 × 10-17 eV |
| Tl-216 | — | 300 ns | Beta-minus decay, Beta-minus, neutron emission | 14,870 keV | 7,709 keV | 1.52 × 10-9 eV |
| Tl-217 | — | — | Beta-minus decay (100%), Beta-minus, neutron emission | 18,660 keV | 7,693 keV | — |