Periodic Table

Astatine

Halogen

Quick Facts about Astatine

Po
  • solid- state of matter at room temperature
  • Radioactive- no stable isotopes exist
  • 7, 5, 3, 1, -1- common oxidation states in compounds
Rn

Astatine (At) is element 85 on the periodic table. Atomic mass of At: 210.0000 u. At is in period 6, group 17. Melting point of At: 575.00 K.Density of At: 7.00 g/cm³.

Why Astatine Matters

The rarest naturally occurring element—only ~25 grams exist on Earth

Industry Uses

Medical ResearchAt-211 targeted alpha therapy for cancer (especially thyroid cancer)
Nuclear ResearchProduced by bombarding bismuth with alpha particles

In Your Body

✗ Not essential

No biological role. At-211 shows promise for cancer treatment—it concentrates in the thyroid like iodine. Too little has been produced to fully study biological effects. Alpha particles are effective at killing cancer cells.

Safety: Too rare for toxicity studies. Presumed highly radioactive toxic like other alpha emitters.

Discovery of Astatine

Discovered by D.R.Corson, K.R.MacKenzie, E.Segré in United States, 1940

Name origin: Greek: astatos (unstable).

History & Events

1940
Named from Greek 'astatos' meaning unstable
1940
First synthesized in 1940 at UC Berkeley
1940
Rarest naturally occurring element - only ~25 grams exist on Earth at any time
1940
Dale Corson, Kenneth MacKenzie, and Emilio Segrè created it

About Astatine

Radioactive halogen element. Occurs naturally from uranium and thorium decay. At least 20 known isotopes. At-210, the most stable, has a half-life of 8.3 hours. Synthesized by nuclear bombardment in 1940 by D.R. Corson, K.R. MacKenzie and E. Segre at the University of California.

Atomic Properties of At

Atomic Number of At
85
Atomic Mass of At
210.0000 u
Electron Configuration
[Xe] 4f14 5d10 6s2 6p5
Electronegativity
2.20
Block
p-block
Group
17
Period
6

Physical Properties of At

Phase (STP)
solid
Melting Point of At
575.00 K
Boiling Point of At
610.00 K
Density of At
7.0000 g/cm3

Atomic Radii

Covalent
147 pm
Van der Waals
202 pm

Common Misconceptions

Wrong:Astatine is completely artificial and doesn't occur naturally.
Correct:About 25 grams of astatine exist on Earth at any moment, continuously formed from uranium and thorium decay. It just decays away faster than it accumulates.
Wrong:We know what astatine looks like.
Correct:No one has ever seen astatine. Too little has ever been isolated to be visible. Its color is predicted to be black or dark based on halogen trends.
Wrong:Astatine's chemistry is well understood like other halogens.
Correct:Most of astatine's chemistry is theoretical. Its short half-life (hours) means experiments must be done with tiny trace amounts, making bulk properties unmeasurable.

Isotopes of Astatine

Astatine has 0 naturally occurring isotopes, plus 2 notable radioactive isotopes.

IsotopeAtomic Mass (u)AbundanceHalf-LifeDecay Mode
21085At (At-210)Astatine-210 isotope209.98714798.1 hoursEC, α
21185At (At-211)Astatine-211 isotope210.98749667.2 hoursEC, α

Data source: NIH PubChem (aggregated from IUPAC, NIST)

Isotope Applications

Isotopes of Astatine have important real-world applications in science and industry.

Medical Applications

211At (with a half-life of 7.2 h) is known to accumulate in the thyroid and occasionally is the preferred treatment for hyperthyroidism and thyroid cancer because the particles emitted from 211At provide more energy than radiolabeled iodine, the other treatment method (Fig. IUPAC.85.1). However, astatine has shown a tendency to induce tumors, so its use is limited [565]. The 211At-labeled di-carborane (cluster of boron, carbon, and hydrogen atoms) ligand known as the Venus Flytrap Cluster (VFC) has been used as a robust pharmaceutical in radiotherapy treatment [566].

Uses

Since its isotopes have such short half-lives there are no commercially significant compounds of astatine.

Sources

Does not occur in nature. Similar to iodine. Produced by bombarding bismuth with alpha particles.

Geochemistry

Goldschmidt
synthetic
Geochemical Class
U/Th decay series

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