Arsenic
Arsenic is a gray, brittle metalloid with a long and infamous history as a poison, even though today its most important role is as a component of high-speed semiconductor materials. It sits in an unusual middle ground chemically, sharing properties with both metals and nonmetals.
- Group · Period
- 15 · 4
- At room temp
- solid
- Melts at
- 1090 K
- Density
- 5.776 g/cm³
- Discovered
- Ancient
Uses
Arsenic’s most significant modern application is in the compound gallium arsenide, a semiconductor that moves electrons faster than silicon and is used in LEDs, laser diodes, solar cells for satellites, and high-frequency components in smartphones and other wireless devices. Lead alloyed with a small amount of arsenic is harder and holds its shape better, which is why it has long been used in things like ammunition and certain bearings.
Historically, arsenic compounds played a much broader role: vivid green pigments like Paris Green colored fabrics, wallpaper and paint for decades before their toxicity became widely understood, and arsenic-based wood preservatives were used to protect lumber from rot and insects, though many of these applications have since been phased out or heavily restricted as their health risks became clear.
History
Unlike most elements, arsenic has no single discoverer — its compounds were recognized and deliberately used by civilizations in Egypt, Greece and China thousands of years ago, both for coloring and, notoriously, for poisoning. The medieval alchemist Albertus Magnus is often credited with being among the first to isolate arsenic in something close to its pure elemental form, around the 13th century, though records from that era are far from precise. Arsenic’s name likely traces back through Latin and Greek to a Persian or Syriac word associated with yellow pigment, reflecting its long use in dyes well before it was understood as a distinct chemical element.
Fun facts
- Arsenic compounds have been used and recognized since antiquity, making it one of the few elements with no single credited discoverer.
- Gallium arsenide, a compound of arsenic, is used in LEDs, solar cells and high-frequency electronics because electrons move through it faster than through silicon.
- Arsenic's toxicity made it a favored poison throughout history, earning it the grim nickname 'inheritance powder' in past centuries.
Frequently asked questions
Who discovered arsenic?
No one person can really claim credit — arsenic compounds were known and used for pigments, poisons and medicines by ancient Egyptian, Greek and Chinese civilizations long before chemistry existed as a science. The medieval scholar Albertus Magnus is sometimes credited with isolating the element itself around the 13th century, but the full history is murky rather than tied to one clean discovery moment.
Is arsenic always dangerous to touch or be near?
Toxicity depends heavily on the amount and chemical form. Solid, elemental arsenic used safely in semiconductors is handled industrially without major risk when contained properly, while certain soluble arsenic compounds are dangerous even in small doses. Naturally occurring arsenic in groundwater is a real public health concern in some parts of the world.
If arsenic is toxic, why is it used in electronics we carry every day?
In compounds like gallium arsenide, arsenic atoms are locked into a stable crystal lattice rather than existing as a free, mobile substance, which is very different from the loose toxic compounds historically associated with poisoning. Manufacturing is tightly controlled specifically because of arsenic's hazards.
Compounds
5 notable compounds containing As
- As2O3oxide
Arsenic trioxide
A white, odorless solid also known as white arsenic, existing as molecular As4O6 units in its common crystalline form. It's the most common commercial arsenic compound and highly toxic even in small doses.
Used for: Historic rodenticide and wood preservative; now a leukemia treatment
- AsH3gas
Arsine
A colorless, extremely toxic gas with a faint garlic-like odor, forming a pyramidal molecule much like ammonia. It decomposes on heated surfaces to deposit elemental arsenic, a reaction once used to detect arsenic poisoning.
Used for: Dopant source gas for gallium arsenide semiconductor manufacturing
- GaAssemiconductor
Gallium arsenide
A crystalline compound semiconductor with the zinc-blende structure common to many III-V materials, prized for its ability to emit and absorb light directly. It underlies much of modern high-speed and optoelectronic device technology.
Used for: LEDs, laser diodes, solar cells, and high-frequency transistors
- As2S3mineral
Orpiment (arsenic trisulfide)
A soft, golden-yellow mineral built from layered As2S3 sheets, long prized for its vivid color. It occurs naturally around hot springs and volcanic vents, often alongside realgar.
Used for: Historic yellow pigment in painting and a natural arsenic ore
- As4S4mineral
Realgar (arsenic sulfide)
A red-orange mineral built from cage-like As4S4 molecules, historically mined as an arsenic ore and pigment. It slowly degrades to a yellow powder called pararealgar when exposed to light.
Used for: Historic red pigment and traditional pesticide
Isotopes
30 known isotopes
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| Isotope | Natural abundance | Half-life | Decay mode | Mass excess | Binding energy / nucleon | Decay width |
|---|---|---|---|---|---|---|
| As-75 stable | 100% | Stable | — | -73,034.2 keV | 8,700.87 keV | — |
Show all 30 isotopes
| As-63 | — | 43 ns | Proton emission | -33,500 keV | 8,193 keV | 1.06 × 10-8 eV |
| As-64 | — | 69.0 ms | Electron capture / beta-plus decay (100%), ECP | -39,532 keV | 8,286 keV | 6.61 × 10-15 eV |
| As-65 | — | 128 ms | Electron capture / beta-plus decay (100%) | -46,937.06 keV | 8,396.24 keV | 3.56 × 10-15 eV |
| As-66 | — | 95.77 ms | Electron capture / beta-plus decay (100%) | -52,025.08 keV | 8,468.4 keV | 4.76 × 10-15 eV |
| As-67 | — | 42.5 s | Electron capture / beta-plus decay (100%) | -56,587.23 keV | 8,530.57 keV | 1.07 × 10-17 eV |
| As-68 | — | 151.6 s | Electron capture / beta-plus decay (100%) | -58,894.53 keV | 8,557.75 keV | 3.01 × 10-18 eV |
| As-69 | — | 15.2 m | Electron capture / beta-plus decay (100%) | -63,112.18 keV | 8,611.82 keV | 5.00 × 10-19 eV |
| As-70 | — | 52.6 m | Electron capture / beta-plus decay (100%) | -64,333.97 keV | 8,621.55 keV | 1.45 × 10-19 eV |
| As-71 | — | 65.30 h | Electron capture / beta-plus decay (100%) | -67,893.26 keV | 8,663.94 keV | 1.94 × 10-21 eV |
| As-72 | — | 26.0 h | Electron capture / beta-plus decay (100%) | -68,229.81 keV | 8,660.38 keV | 4.87 × 10-21 eV |
| As-73 | — | 80.30 d | Electron capture (100%) | -70,952.76 keV | 8,689.61 keV | 6.58 × 10-23 eV |
| As-74 | — | 17.77 d | Electron capture / beta-plus decay (66%), Beta-minus decay (34%) | -70,860.06 keV | 8,680 keV | 2.97 × 10-22 eV |
| As-76 | — | 26.24 h | Beta-minus decay (100%) | -72,291.38 keV | 8,682.82 keV | 4.83 × 10-21 eV |
| As-77 | — | 38.79 h | Beta-minus decay (100%) | -73,916.33 keV | 8,695.98 keV | 3.27 × 10-21 eV |
| As-78 | — | 90.7 m | Beta-minus decay (100%) | -72,816.97 keV | 8,673.88 keV | 8.38 × 10-20 eV |
| As-79 | — | 9.01 m | Beta-minus decay (100%) | -73,636.08 keV | 8,676.62 keV | 8.44 × 10-19 eV |
| As-80 | — | 15.2 s | Beta-minus decay (100%) | -72,214.6 keV | 8,651.28 keV | 3.00 × 10-17 eV |
| As-81 | — | 33.3 s | Beta-minus decay (100%) | -72,533.31 keV | 8,648.06 keV | 1.37 × 10-17 eV |
| As-82 | — | 19.1 s | Beta-minus decay (100%) | -70,105.43 keV | 8,611.42 keV | 2.39 × 10-17 eV |
| As-83 | — | 13.4 s | Beta-minus decay (100%) | -69,669.33 keV | 8,599.65 keV | 3.40 × 10-17 eV |
| As-84 | — | 4.2 s | Beta-minus decay (100%), Beta-minus, neutron emission (0.18%) | -65,853.57 keV | 8,547.94 keV | 1.09 × 10-16 eV |
| As-85 | — | 2.021 s | Beta-minus decay (100%), Beta-minus, neutron emission (62.9%) | -63,189.15 keV | 8,510.99 keV | 2.26 × 10-16 eV |
| As-86 | — | 0.945 s | Beta-minus decay (100%), Beta-minus, neutron emission (35.5%), B-2N | -58,962.15 keV | 8,456.72 keV | 4.83 × 10-16 eV |
| As-87 | — | 484 ms | Beta-minus decay (100%), Beta-minus, neutron emission (15.4%) | -55,617.91 keV | 8,413.85 keV | 9.43 × 10-16 eV |
| As-88 | — | 0.20 s | Beta-minus decay (100%), Beta-minus, neutron emission | -50,450 keV | 8,351 keV | 2.28 × 10-15 eV |
| As-89 | — | — | Beta-minus decay (100%), Beta-minus, neutron emission, B-2N | -46,530 keV | 8,304 keV | — |
| As-90 | — | — | Beta-minus decay (100%), Beta-minus, neutron emission | -40,990 keV | 8,240 keV | — |
| As-91 | — | — | Beta-minus decay (100%), Beta-minus, neutron emission | -36,500 keV | 8,189 keV | — |
| As-92 | — | — | Beta-minus decay (100%) | -30,380 keV | 8,121 keV | — |