Seaborgium

1 · Identity

Symbol, number

Sg, 106

Oxidation states in water

6, 5, 4, 3 and 0 (book entry); never measured in water

Note

Identity from the book entry; nothing measured in water.

Sources

Identity

Name and symbol

Seaborgium, Sg

Atomic number

106 protons

Position

group 6 · period 7 · d-block · transition metal

CAS number

54038-81-2

Atomic structure

Atomic mass

271 u

Electron configuration

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s² 4f¹⁴ 5d¹⁰ 6p⁶ 7s² 5f¹⁴ 6d⁴
[Rn] 7s²⁵f¹⁴⁶d⁴

Electrons per shell

2, 8, 18, 32, 32, 12, 2

Valence electrons

6 ns and (n-1)d

Physical properties

State at room temperature

Solid

Melting point

not in sources

Boiling point

not in sources

Density

not in sources

Appearance

not in sources

Thermal conductivity

not in sources

Electrical resistivity

not in sources

Electrical conductivity

not in sources

Crystal structure

body-centered cubic

Molar heat capacity

not in sources

Chemical properties

Oxidation states

6, (5), (4), (3), 0 ​(parenthesized oxidation states are predictions)

Electronegativity

not in sources

Ionisation energy

7.8 eV

Electron affinity

not in sources

Atomic radius

not in sources

Ionic radius

not in sources

Reactivity

A group 6 transactinide studied a few atoms at a time; gas-phase and ion-exchange experiments confirm a stable +6 state and molybdenum- and tungsten-like chemistry, plus a zero-valent hexacarbonyl Sg(CO)6 made in 2014.

with water

Not known for the element; single atoms oxidized in moist oxygen gave the oxide hydroxide: $\ce{SgO3 + H2O -> SgO2(OH)2}$.

with oxygen, air

Single atoms react with oxygen, the inferred first step of the 2001 gas-phase experiment being the trioxide: $\ce{2 Sg + 3 O2 -> 2 SgO3}$, the species actually detected being its hydrate SgO2(OH)2.

with acids

In nitric and hydrofluoric acid seaborgium elutes from cation-exchange resin most likely as neutral SgO2F2 or the anion SgO2F3^-, while in 0.1 M nitric acid it stays cationic, hydrolyzing less than molybdenum and tungsten.

with halogens

With oxygen and hydrogen chloride single atoms form the volatile oxychloride: $\ce{Sg + O2 + 2 HCl -> SgO2Cl2 + H2}$, the least volatile of the group 6 oxychlorides.

Typical compounds

• SgO₂Cl₂ seaborgium dioxide dichloride volatile oxychloride, first seaborgium compound (1995)
• SgO₂(OH)₂ seaborgium oxide hydroxide formed from the trioxide with water vapor
• Sg(CO)₆ seaborgium hexacarbonyl volatile zero-valent carbonyl, made in 2014

Occurrence, production and use

Crustal abundance

Not Applicable

Oceanic abundance

Not Applicable

Occurrence and sources

• synthetic only californium-249 bombarded with oxygen-18 nuclei

Extraction, production

not in sources

Uses

Since only a few atoms of seaborgium have ever been made, there are currently no uses for seaborgium outside of basic scientific research.

Safety, toxicity

not in sources

Discovery and name

Discovered by

Lawrence Berkeley National Laboratory

Discovered

1974

First isolated

not in sources

Named by

not in sources

Origin of the name

after Glenn T. Seaborg

Seaborgium does not occur naturally in the Earth’s crust. In 1974, seaborgium was first synthesized by Albert Ghiorso and his team at the University of California in Berkeley using the nuclear reaction 249Cf (18O, 4n) 263Sg. The element is named for Glenn T. Seaborg (Fig. IUPAC.106.1), who synthesized a number of trans-uranium elements [634], [648].

Seaborgium has no commercial applications. However, 265Sg was one of the decay products used to confirm the synthesis of copernicium in a particle accelerator experiment.

Seaborgium is named after Glenn Seaborg.