Draw The Structure Of Beryllium Chloride Molecule

Beryllium chloride

Names

IUPAC name

Beryllium chloride

Identifiers

CAS Number

7787-47-5 ^N

3D model (JSmol)

ionic depiction: Interactive image
covalent monomer: Interactive image
polymer: Interactive image

ChemSpider

22991 ^Y

ECHA InfoCard

100.029.197

PubChem CID

24588

RTECS number

DS2625000

CompTox Dashboard (EPA)

DTXSID10858756

InChI

InChI=1S/Be.2ClH/h;2*1H/q+2;;/p-2^Y

Key: LWBPNIJBHRISSS-UHFFFAOYSA-L^Y
InChI=1/Be.2ClH/h;2*1H/q+2;;/p-2

Key: LWBPNIJBHRISSS-NUQVWONBAX

SMILES

ionic depiction: [Be+2].[Cl-].[Cl-]
covalent monomer: Cl[Be]Cl
polymer: Cl[Be-2](Cl)([Cl+]1)[Cl+][Be-2]1([Cl+]1)[Cl+][Be-2]1([Cl+]1)[Cl+][Be-2]1([Cl+]1)[Cl+][Be-2]1([Cl+]1)[Cl+][Be-2]1([Cl+]1)[Cl+][Be-2]1([Cl+]1)[Cl+][Be-2]1([Cl+]1)[Cl+][Be-2]1([Cl+]1)[Cl+][Be-2]1([Cl+]1)[Cl+][Be-2]1([Cl+]1)[Cl+][Be-2]1([Cl+]1)[Cl+][Be-2]1(Cl)Cl

Properties

Chemical formula

BeCl₂

Molar mass

79.9182 g/mol

Appearance

White or yellow crystals

Density

1.899 g/cm³, solid

Melting point

399 °C (750 °F; 672 K)

Boiling point

482 °C (900 °F; 755 K)

Solubility in water

15.1 g/100 mL (20 °C)

Solubility

soluble in alcohol, ether, benzene, and pyridine
slightly soluble in chloroform and sulfur dioxide

Structure

Crystal structure

hexagonal

Molecular shape

polymer

Thermochemistry

Heat capacity (C)

7.808 J/K or 71.1 J/mol K

Std molar
entropy (S ^o ₂₉₈)

63 J/mol K

Std enthalpy of
formation (Δ_f H ^⦵ ₂₉₈)

−6.136 kJ/g or -494 kJ/mol

Gibbs free energy (Δ_f G˚)

-468 kJ/mol

Std enthalpy of
combustion (Δ_c H ^⦵ ₂₉₈)

16 kJ/mol

Hazards

Lethal dose or concentration (LD, LC):

LD₅₀ (median dose)

86 mg/kg (rat, oral)

NIOSH (US health exposure limits):

PEL (Permissible)

TWA 0.002 mg/m³
C 0.005 mg/m³ (30 minutes), with a maximum peak of 0.025 mg/m³ (as Be)^[1]

REL (Recommended)

Ca C 0.0005 mg/m³ (as Be)^[1]

IDLH (Immediate danger)

Ca [4 mg/m³ (as Be)]^[1]

Related compounds

Other anions

Beryllium fluoride
Beryllium bromide
Beryllium iodide

Other cations

Magnesium chloride
Calcium chloride
Strontium chloride
Barium chloride
Radium chloride

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

Nverify (what is^{Y N} ?)

Infobox references

Chemical compound

Beryllium chloride is an inorganic compound with the formula BeCl₂. It is a colourless, hygroscopic solid that dissolves well in many polar solvents. Its properties are similar to those of aluminium chloride, due to beryllium's diagonal relationship with aluminium.

Structure and synthesis [edit]

Beryllium chloride is prepared by reaction of the metal with chlorine at high temperatures:^[2]

Be + Cl₂ → BeCl₂

BeCl₂ can also be prepared by carbothermal reduction of beryllium oxide in the presence of chlorine.^[3] BeCl₂ can be prepared by treating beryllium with hydrogen chloride.

The solid is a 1-dimensional polymer consisting of edge-shared tetrahedra.^[4] In contrast, BeF₂ is a 3-dimensional polymer, with a structure akin to that of quartz. In the gas phase, BeCl₂ exists both as a linear monomer and a bridged dimer with two bridging chlorine atoms where the beryllium atom is 3-coordinate.^[5] The linear shape of the monomeric form is as predicted by VSEPR theory. The linear shape contrasts with the monomeric forms of some of the dihalides of the heavier members of group 2, e.g. CaF₂, SrF₂, BaF₂, SrCl₂, BaCl₂, BaBr₂, and BaI₂, which are all non-linear.^[5] Beryllium chloride dissolves to give tetrahedral [Be(OH₂)₄]²⁺ ion in aqueous solutions as confirmed by vibrational spectroscopy.^[6]

Reactions [edit]

Beryllium chloride forms a tetrahydrate, BeCl₂•4H₂O ([Be(H₂O)₄]Cl₂). BeCl₂ is also soluble in some ethers.^[7] ^[8]

Applications [edit]

Beryllium chloride is used as a raw material for the electrolysis of beryllium, and as a catalyst for Friedel-Crafts reactions.

References [edit]

^ ^a ^b ^c NIOSH Pocket Guide to Chemical Hazards. "#0054". National Institute for Occupational Safety and Health (NIOSH).
^ Irving R. Tannenbaum "Beryllium Chloride" Inorganic Syntheses, 1957, vol. 5, p. 22. doi:10.1002/9780470132364.ch7
^ Cotton, F. A.; Wilkinson, G. (1980) Advanced Inorganic Chemistry John Wiley and Sons, Inc: New York, ISBN 0-471-02775-8.
^ Wells, A. F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
^ ^a ^b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN978-0-08-037941-8.
^ Rudolph, Wolfram W.; Fischer, Dieter; Irmer, Gert; Pye, Cory C. (2009). "Hydration of Beryllium(II) in Aqueous Solutions of Common Inorganic Salts. A Combined Vibrational Spectroscopic and ab initio Molecular Orbital Study". Dalton Transactions (33): 6513. doi:10.1039/B902481F. PMID 19672497.
^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN0-8493-0487-3.
^ Holleman, A. F.; Wiberg, E. (2001) Inorganic Chemistry Academic Press: San Diego, ISBN 0-12-352651-5