Boron triiodide

Boron triiodide[1] |  |

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Names
IUPAC name

triiodoborane

Identifiers

CAS Number

* 13517-10-7 N

3D model (JSmol)

* Interactive image

ChemSpider |

* 75378 Y

PubChem CID

* 83546

RTECS number |

* ED7400000

InChI

* InChI=1S/BI3/c2-1(3)4 Y

Key: YMEKEHSRPZAOGO-UHFFFAOYSA-N Y

* InChI=1/BI3/c2-1(3)4

Key: YMEKEHSRPZAOGO-UHFFFAOYAR

SMILES

* IB(I)I

Properties

Chemical formula

| BI3
Molar mass | 391.52 g/mol
Appearance  | crystalline solid
Density | 3.35 g/cm3 (50 °C)
Melting point |  49.9 °C (121.8 °F; 323.0 K)
Boiling point |  210 °C (410 °F; 483 K)

Solubility in water

| soluble,hydrolysis
Solubility | soluble in CCl4, CS2, benzene, chloroform

Dipole moment

| 0D
Structure

Crystal structure

| hexagonal
Thermochemistry

Heat capacity (C)

| 71 J/mol K

Std molar
entropy (S ~~o~~ 298)

| 200 J/mol K

Std enthalpy of
formation (ΔfH⦵298)

| -37.2 kJ/mol
Hazards
Safety data sheet | Sigma-Aldrich
NFPA 704 (fire diamond)  |

Flash point |  −18 °C (0 °F; 255 K)
Related compounds

Related compounds

| Boron trifluoride
Boron trichloride
Boron tribromide

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

N verify (what is YN ?)
Infobox references

Boron triiodide is a chemical compound of boron and iodine with chemical formula BI3. It has a trigonal planar molecular geometry.

## Contents

* 1 Preparation
* 2 Properties
* 3 Applications
* 4 References
* 5 External links

## Preparation

Boron triiodide can be prepared by the reaction of boron with iodine at 209.5 °C or 409.1 °F.[citation needed] It can also be prepared by reacting hydroiodic acid with boron trichloride:

3HI + BCl
3 → BI
3 \+ 3HCl (reaction requires high temperature)

Another method is by reacting lithium borohydride with iodine. As well as boron triiodide, this reaction also produces lithium iodide, hydrogen and hydrogen iodide:[2]

3LiBH
4 \+ 8I
2 → 3LiI + 3BI
3 \+ 4H
2 \+ 4HI

## Properties

In its pure state, boron triiodide forms colorless, otherwise reddish, shiny, air and hydrolysis-sensitive[3] crystals, which have a hexagonal crystal structure (a = 699.09 ± 0.02 pm, c = 736.42 ± 0.03 pm, space group P63/m (space group no. 176)).[4] Boron triiodide is a strong Lewis acid and soluble in carbon disulfide.[2]

Boron triiodide reacts with water and decomposes to boric acid and hydriodic acid:

3 \+ 3H
2O ⇌ B(OH)
3 \+ 3HI

Its dielectric constant is 5.38 and its heat of vaporization is 40.5 kJ/mol. At extremely high pressures, BI3 becomes metallic at ~23 GPa and is a superconductor above ~27 GPa.[5]

## Applications

Boron triiodide can be used to produce other chemical compounds and as a catalyst (for example in coal liquefaction).[6]

## References

1. ↑ Lide, D. R., ed (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
2. ↑ 2.0 2.1 Handbuch der präparativen anorganischen Chemie. 2 (3., umgearb. Aufl ed.). Stuttgart: Enke. 1978. ISBN 978-3-432-87813-3.
3. ↑ "Beiträge zur Chemie der Bor-Stickstoff-Verbindungen". http://www-brs.ub.ruhr-uni-bochum.de/netahtml/HSS/Diss/StangeBernd/diss.pdf.
4. ↑ Albert, Barbara; Schmitt, Konny (May 2001). "Die Kristallstruktur von Bortriiodid, BI3" (in de). Zeitschrift für anorganische und allgemeine Chemie 627 (5): 809–810. doi:10.1002/1521-3749(200105)627:5<809::AID-ZAAC809>3.0.CO;2-J. ISSN 0044-2313. https://onlinelibrary.wiley.com/doi/10.1002/1521-3749(200105)627:53.0.CO;2-J.
5. ↑ Hamaya, Nozomu; Ishizuka, Miyuki; Onoda, Suzue; Guishan, Jiang; Ohmura, Ayako; Shimizu, Katsuya (2010). "Pressure-induced phase transition, metallization, and superconductivity in boron triiodide". Physical Review B 82 (9): 094506. doi:10.1103/PhysRevB.82.094506. Bibcode: 2010PhRvB..82i4506H.
6. ↑ "Kohleverflüssigung – Innovations Report". https://www.innovations-report.de/fachgebiete/biowissenschaften-chemie/bericht-53763/.

## External links

* MSDS (link is broken)

* v
* t
* e

Boron compounds

* BAs
* BBr3
* BCl3
* BF
* BF3
* BI3
* BN
* B(NO3)3
* B(OH)3
* BP
* BPO4
* B2F4
* B2Cl4
* B2H6
* BH3NH3
* B2O
* B2O3
* B2S3
* B4C
* B6O
* B5H9
* B5H11
* B6H10
* B6H12
* B10H14

HI |  |  |  | He

|
|
|
|

LiI | BeI2 | BI3 | CI4 | NI3 | I2O4,
I2O5,
I4O9 | IF,
IF3,
IF5,
IF7 | Ne
NaI | MgI2 | AlI3 | SiI4 | PI3,
P2I4 | S  | ICl,
ICl3 | Ar
KI | CaI2 | Sc  | TiI4 | VI3 | CrI3 | MnI2 | FeI2 | CoI2 | NiI2 | CuI | ZnI2 | Ga2I6 | GeI2,
GeI4 | AsI3 | Se  | IBr | Kr
RbI | SrI2 | YI3 | ZrI4 | NbI5 | Mo  | Tc  | Ru  | Rh  | Pd  | AgI | CdI2 | InI3 | SnI4,
SnI2 | SbI3 | TeI4 | I  | Xe
CsI | BaI2 |  | HfI4 | TaI5 | W  | Re  | Os  | Ir  | Pt  | AuI | Hg2I2,
HgI2 | TlI | PbI2 | BiI3 | Po  | AtI | Rn
Fr  | RaI2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
La  | Ce  | Pr  | Nd  | Pm  | SmI2 | Eu  | Gd  | TbI3 | Dy  | Ho  | Er  | Tm  | Yb  | Lu
Ac  | ThI4 | Pa  | UI3,
UI4 | Np  | Pu  | Am  | Cm  | Bk  | Cf  | EsI3 | Fm  | Md  | No  | Lr

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