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Beryllium chloride is an inorganic compound with the formula BeCl2.
Beryllium chloride is a colourless, hygroscopic solid that dissolves well in many polar solvents.
Beryllium chloride's properties are similar to those of aluminium chloride, due to beryllium's diagonal relationship with aluminium.
CAS Number: 7787-47-5
EC Number: 232-116-4
IUPAC Name: beryllium dichloride
Chemical formula: BeCl2
Other names: Beryllium dichloride, 7787-47-5, BeCl2, Beryllium chloride (BeCl2), CHEBI:62843, NSC84263, NSC-84263, 58B7024067, dichloroberyllium, DTXCID30809487, 232-116-4, DTXSID10858756, beryllium;dichloride, Beryllium chloride(BeCl2), CCRIS 4490, HSDB 357, EINECS 232-116-4, NSC 84263, Berylliumchlorid, UNII-58B7024067, WLN: BE G2, SCHEMBL3695807, Beryllium chloride, purified by sublimation, 99%
Structure and synthesis
Beryllium chloride is prepared by reaction of the metal with chlorine at high temperatures:
Be + Cl2 → BeCl2
BeCl2 can also be prepared by carbothermal reduction of beryllium oxide in the presence of chlorine.
BeCl2 can be prepared by treating beryllium with hydrogen chloride.
Two forms (polymorphs) of BeCl2 are known. Both structures consist tetrahedral Be2+ centers interconnected by doubly bridging chloride ligands. One form consist of edge-sharing polytetrahedra. The other form resembles zinc iodide with interconnected adamantane-like cages.
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.
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.
Beryllium chloride dissolves to give tetrahedral [Be(OH2)4]2+ ion in aqueous solutions as confirmed by vibrational spectroscopy.
Properties:
Chemical formula: BeCl2
Molar mass: 79.9182 g/mol
Color and Appearance: Colorless/white, whitish-yellow, green crystalline mass
Odor: Sharp, pungent
Taste: Sweetish taste
Vapor Pressure: 1 mm Hg at 291 °C (sublimes)
Density: 1.899 g/mL at 25 °C (lit.)
Melting point: 399 °C (750 °F; 672 K)
Boiling point: 482 °C (900 °F; 755 K)
Hydrogen Bond Acceptor Count: 2
Exact Mass: 78.949888
Monoisotopic Mass: 78.949888
Heavy Atom Count: 3
Complexity: 2.8
Covalently-Bonded Unit Count: 3
Compound Is Canonicalized: Yes
Reactions
When treated with water, beryllium chloride forms a tetrahydrate, BeCl2•4H2O ([Be(H2O)4]Cl2). BeCl2 is also soluble in some ethers.
When suspended in diethyl ether, beryllium chloride converts to the colorless dietherate:
BeCl2 2 O(C2H5)2 → BeCl2(O(C2H5)2)2
This ether ligand can be displaced by other Lewis bases.
Beryllium chloride forms complexes with phosphines.
Applications
Beryllium chloride is used as a raw material for the electrolysis of beryllium, and as a catalyst for Friedel-Crafts reactions.
Thermochemistry
Heat capacity: 7.808 J/K or 71.1 J/mol K
Std molar entropy (So298): 63 J/mol K
Std enthalpy of formation (ΔfH⦵298): −6.136 kJ/g or -494 kJ/mol
Gibbs free energy (ΔfG˚): -468 kJ/mol
Std enthalpy of combustion (ΔcH⦵298): 16 kJ/mol
Description:
A colourless, hygroscopic solid with the formula BeCl2.
Beryllium chloride is an inorganic compound with the formula BeCl2.
Beryllium chloride is a white to faintly yellow powder with a sharp odor.
Beryllium chloride is used in refining Beryllium ores and as a chemical reagent.
Beryllium chloride, also known as beryllium dichloride in IUPAC nomenclature, is an inorganic compound of beryllium and chloride.
Beryllium chloride can attract and hold water from the surrounding environment (hygroscopic compound) and dissolves well in several polar solvents.
Beryllium chloride is a white to faintly yellow powder with a sharp odor.
Beryllium chloride is used in refining Beryllium ores and as a chemical reagent.
Beryllium chloride is a colourless, hygroscopic solid that dissolves well in many polar solvents.
The properties of beryllium chloride are similar to those of aluminium chloride, due to beryllium's diagonal relationship with aluminium.
Beryllium chloride is isomorphous with dimethylberyllium and silicon disulfide.
The orthorhombic unit, a0=9.86, b0=5.36, c0=5.26A contains four beryllium chloride molecules.
The Cl-Be-Cl bond angle within the four membered rings is 98.2°.
The bond angles indicate that all bonds in beryllium chloride contain an electron pair, so that chlorine uses an unshared pair in forming bridge bonds.
Beryllium chloride, BeCl2, has played an important part in the history of beryllium.
Beryllium chloride was the first source of the metal, and the discovery that the vapour density of beryllium chloride between 490° and 1520° C.
The formula has been confirmed by the molecular weight of beryllium chloride in pyridine.
Beryllium chloride is a white to green solid with a sharp odor.
Beryllium dichloride is a compound of beryllium (+2 oxidation state) and chloride in the ratio 1:2.
Beryllium chloride has a role as a carcinogenic agent and a genotoxin.
Beryllium chloride is a beryllium molecular entity and an inorganic chloride.
Beryllium Chloride is an excellent water soluble crystalline.
Beryllium source for uses compatible with chlorides.
Chloride compounds such as beryllium chloride can conduct electricity when fused or dissolved in water and, can be decomposed by electrolysis to chlorine gas and the metal.
Chlorine compounds such as beryllium chloride are formed through various chlorination processes whereby at least one chlorine anion (Cl-) is covalently bonded to the relevant metal or cation.
The chloride ion of beryllium chloride controls fluid equilibrium and pH levels in metabolic systems.
Using X-ray diffraction study it is shown that complexing of BeCl2 with 15-crown-5 in the medium of diethyl ether results in the preparation of molecular complex with tetrahedral metal atom.
In solid-state, beryllium chloride forms continuous coordinate bonds with surrounding chlorine atoms which is analogous to the structure of aluminium chloride.
While beryllium chloride is in gaseous state, atoms are joined through a bridge of chlorine atoms.
The bond formation of beryllium chloride takes place to complete the octet of atoms.
Beryllium chloride is an inorganic compound.
Beryllium chloride is a colorless solid which can be dissolved in many polar solvents.
Beryllium has 2 valence electrons and according to Valence Bond Theory, beryllium chloride has linear geometry in which the Be atom is sp-hybridized.
Beryllium chloride is hygroscopic in nature that means it readily absorbs moisture through adsorption and thus it exists as a tetrahydrate - BeCl2.4H20.
Beryllium tends to form different structures of beryllium chloride in the solid and vapor phase to fulfill the number of electrons required to complete its octet.
Beryllium chloride can exist in both monomeric and 1-D polymeric forms.
The properties of beryllium chloride are similar to aluminum chloride owing to the diagonal relationship of beryllium with aluminum.
Beryllium chloride dissolves well in many polar solvents.
Beryllium chloride is known as an electron-deficient compound because it has the two empty orbitals at the bonding level.
Beryllium chloride is prepared by reaction of the metal with chlorine at high temperatures.
Beryllium chloride can also be prepared by carbothermal reduction of beryllium oxide in the presence of chlorine.
Beryllium chloride can be prepared by treating be metal with hydrogen chloride.
Beryllium chloride reacts vigorously and exothermically with water with the evolution of acidic, steamy hydrogen chloride gas.
Beryllium chloride has played an important part in the history of beryllium.
Beryllium chloride was the first source of the metal, and the discovery that its vapour density between 490° and 1520° C.
Beryllium chloride was fundamental for the discussion over the valency and atomic weight of the element.
The formula of beryllium chloride has been confirmed by the molecular weight of beryllium chloride in pyridine.
Anhydrous beryllium chloride is a white crystalline solid, of density 1.8995 at 25° C., which melts at about 440° C and boils at about 520° C.
Beryllium chloride dissolves violently in water with loss of hydrogen chloride.
With ether, beryllium chloride forms a compound, BeCl2.2H2O, and dissolves readily in alcohol but not in chloroform, carbon tetrachloride, benzene, or sulphur dichloride.
The tetrahydrate can be obtained by treatment with hydrogen chloride and ether: alcohol can replace the ether in preparing it.
Anhydrous beryllium chloride forms compounds with many organic bases.
Beryllium chloride is easily prepared in solution by dissolving the oxide or hydroxide in hydrochloric acid.
Friedrich Wölhler of Germany and A. Bussy of France, independently produced beryllium by reducing beryllium chloride (BeCl2) with potassium in a platinum crucible.
Physical Properties of Beryllium Chloride:
Beryllium chloride, BeCl2, melts at 405°C and boils at 520°C. That compares with 714°C and 1412°C for magnesium chloride.
Notice how much dramatically lower the boiling point of beryllium chloride is compared with magnesium chloride.
The much higher boiling point of magnesium chloride is what you might expect from the strong forces between the positive and negative ions present.
Because the boiling point of magnesium chloride is much lower, it follows that beryllium chloride can't contain ions, and beryllium chloride must be covalent.
Color and Form of Beryllium Chloride:
Beryllium chloride has white-yellow orthorhombic crystals.
Beryllium chloride has white to faintly yellow, orthorhombic crystals or crystalline mass.
Beryllium chloride is colourless, and has deliquescent needles or orthorhombic crystals.
Beryllium chloride crystallizes in asbestos-like matted needles.
Lewis Structure of Beryllium Chloride:
The electrons present in the outermost shell of an atom are shown in the Lewis structure of any molecule.
These electrons will be both bonding as well as non-bonding electrons.
The electronic configuration of beryllium is [He] 2s2 and chlorine is [Ne] 3s23p5.
The number of electrons on the valence shell of Be and Cl is 2 and 7 electrons, respectively.
As there are two chlorine atoms in beryllium chloride, the total number of valence electrons would be 2 + (7 X 2) =16 electrons.
There are 16 valence electrons in the Lewis structure of beryllium chloride.
The beryllium will be surrounded by the two electrons and, the chlorine atom would like to have eight electrons around it to complete its octet.
Beryllium will act as the central atom and chlorine atoms will surround it.
Each chlorine atom completes its octet by sharing its one electron with the beryllium atom and therefore, there is a single bond between beryllium and chlorine atom.
The octet of beryllium is incomplete and, beryllium chloride is electron-deficient and acts as Lewis acid.
Molecular Geometry of Beryllium Chloride:
Beryllium Chloride has a linear shape, the molecular geometry of beryllium chloride is linear.
The linear geometry of beryllium chloride leads to the bond angle (Cl-Be-Cl) of 180° to minimize bond pair-bond pair repulsions.
If the bond angle is either greater than or lower than 180°, then bond pair-bond pair repulsion will not be minimum.
Polarity of Beryllium Chloride:
Beryllium chloride molecule is considered a nonpolar molecule.
The shape of beryllium chloride is symmetric ie; linear due to which the net dipole of the entire molecule becomes zero leaving behind no partial charge.
The electronegativity of both chlorine atoms of beryllium chlorine is the same and thus has equal influence on the shared electrons.
Hybridization of Beryllium Chloride:
The electron configuration of Be in its ground state is 1s2 2s2.
In beryllium chloride, beryllium shares both the valence electrons in its outer shell with chlorine atoms.
The electrons in 2s get unpaired in its excited state, and one electron moves to the 2p orbital.
As a result, there are two hybrid orbitals formed: one s orbital and one p orbital.
For beryllium chloride, hybridization of Be is sp in its monomeric form.
Bond Angles of Beryllium Chloride:
All the atoms of beryllium chloride are arranged in a single plane.
Beryllium chloride has a symmetric arrangement as both the chlorine atoms are on either side of the central atom.
And both these atoms share one valence electron of beryllium to complete their octet.
The bond angle of beryllium chloride is 180° as there are no lone pairs in the molecule.
Why is Beryllium Chloride Linear?
Beryllium chloride has no lone pairs on the beryllium.
Thus, the electrons on the chlorides will try to stay far apart from each other, since their corresponding electrons repel each other (while experiencing no deflection from electrons on a central atom).
Thus the molecule of beryllium chloride is linear in shape.
Solubility of Beryllium Chloride:
Beryllium chloride is very soluble in water with evolution of heat.
Beryllium chloride soluble in ethanol, ethyl ether, pyridene; insoluble in benzene, toluene.
Beryllium chloride is soluble in carbon disulfide.
The solubility of beryllium chloride in water, g/100ml at 25 °C: 71,5.
Corrosivity of Beryllium Chloride:
Beryllium chloride corrodes most metals in the presence of moisture.
Experimental Properties of Beryllium Chloride:
Beryllium chloride is hygroscopic.
Beryllium chloride is very deliquescent; sublimes in vacuo at 300 °C.
Beryllium chloride undergoes transition to high temperature orthorhombic polymorph at 4 °C.
Heat of solution of beryllium chloride is -557 cal/g.
Thermochemical Data of Beryllium Chloride:
[Be] + (2HCl) = [BeCl2] + (H2)+121.1 Cal.
[Be] + (Cl2) = [BeCl2] + 155 Cal.
[BeCl2]+Aq. = BeCl2.Aq.+44.5 Cal.
3D Status of Beryllium Chloride:
Conformer generation is disallowed since MMFF94s unsupported element, MMFF94s unsupported atom valence, mixture or salt.
Reaction of Beryllium Chloride with Water
Beryllium chloride reacts vigorously and exothermically with water with the evolution of acidic, steamy hydrogen chloride gas.
In the first instance, beryllium chloride reacts to give hydrated beryllium ions, [Be(H2O)4]2+, and chloride ions.
But the hydrated beryllium ions are quite strongly acidic.
The small beryllium ion at the centre attracts the electrons in the bonds towards itself, and that makes the hydrogen atoms in the water even more positive than they usually are.
If the solution is hot and concentrated (as it is likely to be if you add water to solid beryllium chloride, chloride ions can remove one or more of these hydrogen ions to produce hydrogen chloride gas.
The Structure of Beryllium Chloride
The shape of beryllium chloride is linear, with the central beryllium bonded on either side to a chlorine atom.
The electronegativities of the chlorine atoms therefore cancel, leaving a nonpolar molecule.
Beryllium chloride is an example of an electron-deficient molecule because the beryllium atom only shares a total of four electrons, whereas atoms in most covalent molecules share eight.
Normally, atoms such as beryllium located in the first or second groups on the periodic table form ionic bonds, which allows them to reach a noble gas configuration without sharing electrons.
However, beryllium is significantly more electronegative than most atoms in these groups, which is why beryllium chlorine has covalent bonds.
As a gas: Beryllium chloride, is a linear molecule with all three atoms in a straight line.
Beryllium chloride is known as an electron-deficient compound because it has the two empty orbitals at the bonding level.
As a solid: Beryllium chloride is a very small molecule, and so the intermolecular attractions would be expected to be fairly weak.
In the solid, beryllium chloride molecules polymerise to make long chains.
Beryllium chloride do this by forming coordinate bonds between lone pairs on chlorine atoms and adjacent beryllium atoms.
Thermodynamical investigations of beryllium chloride give evidence for the existence of two modifications.
A room-temp. stable phase T-BeCl2 = . beta.-BeCl2 undergoes phase transformation at 405 ◦ C to the high-temp. phase, α-BeCl2 of the SiS2 structure type previously described.
According to solution calorimetric measurements, transition enthalpy and entropy values of 2.9 kJ/mol and 9.7 JK-1mol-1, resp., are determined.
Single crystals of β-BeCl2, obtained by recrystallization of the gas phase, crystallize in the tetragonal space group I41/acd with Z = 32 of the Mg(NH2)2 structure type.
The structure consists of (Be4Cl6Cl4/2) supertetrahedral units which are connected by their terminal Cl- ions.
Why Isn't Beryllium Chloride Ionic?
Beryllium has quite a high electronegativity compared with the rest of the group.
Beryllium chloride attracts a bonding pair of electrons towards itself more strongly than magnesium and the rest do.
In order for an ionic bond to form, the beryllium has to let go of its electrons but the beryllium is too electronegative to do that.
Why Is Beryllium Chloride a Covalent Bond?
Due to small size and high charge density Be, its polarizing power is maximum, since Be+2 ion essentially pull the electrons cloud from Cl- , such that the electrons pair are effectively shared.
This give covalent character to beryllium chloride.
Is Beryllium Chloride Polar or Nonpolar?
Although the bonds of beryllium chloride are polar, the entire molecule of beryllium chloride does not have one side that is more or less negative than another.
Beryllium chloride is nonpolar.
