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Beryllium chloride molecule

In the beryllium chloride molecule (BeCl2(g)), the beryllium atom has only four electrons in its valence shell (Figure 4-31). The molecule is described as electron deficient. The boron trichloride molecule is also electron deficient the central boron atom has only six electrons in its valence shell (Figure 4-32). A related example of an electron-deficient molecule is aluminium trichloride, AICI3. The aluminium atom has only six electrons in its valence shell. All these molecules have incomplete octets. [Pg.132]

Consider the gaseous beryllium chloride molecule, BeCl2(g) The Lewis structure of the molecule shows there are only two electron pairs (two electron domains) in the valence shell of the beryllium atom (Figure 4-44). These two pairs of electrons try to separate as far as possible from each other so as to minimize electron repulsion. Thus, the beryllium chloride molecule adopts a linear shape with a bond angle of 180°, because the electron pairs are ferthest apart when they are on opposite sides of the beryllium atom. [Pg.137]

Thus the carbon dioxide molecule, COj, has a linear structure like the beryllium chloride molecule (Figure 4 50), and the ethene molecule, C2H4, is trigonal planar around each of the two carbon atoms (Figure 4 51). It is a planar molecule. [Pg.139]

In solvents that have donor properties, solubility leads to complex formation to give species such as S A1C13 (where S is a solvent molecule). Beryllium chloride is soluble in solvents such as alcohols, ether, and pyridine, but slightly soluble in benzene. [Pg.372]

Beryllium is in Group 2 and so has two outer electrons. The two Cl atoms contribute one electron each. This gives four electrons in two electron pairs. As beryllium chloride has two Be-Cl bonds, the two electron pairs are two bonding pairs there are two bonds around the central beryllium atom. Thus beryllium chloride will be a linear molecule, Cl-Be-Cl, with bond angles equal to 180°. [Pg.20]

A coordination number of 6 is common for a metal ion. Small, highly charged cations, such as Be + and Al +, have low coordination numbers, although these coordination numbers are usually higher in crystals than in gases or liquids. For example, beryllium chloride, BeCU, in the gas phase, exists as an isolated linear molecule," with coordination number 2 (not truly ionic) in crystals, however, it exists as a polymeric, bridged structure in which the beryllium has the preferable coordination number of 4 (Figure 15.5). Ionic radii vary somewhat with coordination number, and are shorter if the coordination number is smaller. For example, a cation with a tetrahedral coordination of 4 anions has 93-95% the radius... [Pg.636]

Boron Trichloride, BCI3. Here the molecule is planar, with the boron atom at the centre of an equilateral triangle of chlorine atoms (Fig. 46). The valence state must be described in terms of three similar hybrid AO s pointing towards the comers of the triangle. Such orbitals can be formed by mixing 2s and two 2p AO s, 2p and 2p say they lie in the plane of the latter and are precisely equivalent (Fig. 47). If the so-called trigonal hybrids are denoted by h, hg and hg, the appropriate boron valence state must be B(ls2 h h2 hg ). The hybrid AO s overlap chlorine 3p AO s, directed towards the boron atom, to form localised MO s similar to those in beryllium chloride. [Pg.101]

In the vapor phase, beryllium chloride consists of discrete BeCl2 molecules. Is the octet rule satisfied for Be in this compound If not, can you form an octet around Be by drawing another resonance stmcture How plausible is this structure ... [Pg.362]

The beryllium chloride (BeCl2) molecule is predicted to be linear by VSEPR. The orbital diagram for the valence electrons in Be is... [Pg.386]

Beryllium chloride is a substance of low melting point, is non-conducting when in the molten state, and is soluble in many organic solvents. All these characteristics point to a covalent compound, but it is difficult to see how this is to result from a beryllium atom with a fully filled outer s orbital. X-ray studies have established that the molecule contains two linear Be—Cl bonds, of equal strength. The problem is solved with the introduction of a concept of hybrid orbitals. [Pg.35]

Gaseous beryllium chloride (BeCl2) is a linear molecule (AX2). Gaseous beryllium compounds are electron deficient, with only two electron pairs around the central Be atom ... [Pg.308]

Beryllium chloride readily sublimes at high temperatures ( 750°) it consists of essentially all monomeric, linear BeCl2 molecules, but at lower temperatures there are appreciable amounts ( 20% at 560°) of the dimer, in which Be is three-coordinate. [Pg.209]

AB2, Ns = 2 beryllium chloride (BeCl2). The Lewis structure of the molecule beryllium chloride is... [Pg.224]

Consider the triatomic molecule beryllium chloride (BeCl2). Experimental evidence shows that the BeCl2 molecule in the gas phase is linear with two equivalent Be—Cl bonds, consistent with the VSEPR model prediction. The construction of a valence bond picture of bonding in linear BeCl2 requires the existence of unpaired electrons in Be atomic orbitals that overlap with the half-filled 3p orbital on each Cl to form two equivalent bonds that are 180° apart. However, the ground state electron configuration for Be is ls 2s, which contains no unpaired electrons. [Pg.240]

The structure of beryllium chloride is linear with a bond angle 180°. The central atom beryllium undergoes sp hybridization and determines the shape of the molecule formed. [Pg.17]

Molecules with Electron-Deficient Atoms Gaseous molecules containing either beryllium or boron as the central atom are often electron deficient they have fewer than eight electrons around the central atom. The Lewis structures, with formal charges, of gaseous beryllium chloride and boron trifluoride are... [Pg.309]

Draw dot-and-cross diagrams for the following covalently bonded molecules. Show only the outer electron shells. Note that in part d the beryllium atom is electron deficient and in part e the phosphorus atom has an expanded octet, a Tetrachloromethane, CCl b Phosphorus(lll) chloride c Bromine, Brj d Beryllium chloride, BeClj e Phosphorus(V) chloride, PCI5... [Pg.62]

Magnesium salts, like those of beryllium, can absorb ammonia gas, forming additive products distinct from the ammonium double salts. Thus, magnesium chloride forms double salts with ammonium chloride and absorbs ammonia gas, forming ammines containing four or six molecules of ammonia. [Pg.45]

Beryllium is normally divalent in its compounds and, because of its high ionic potential, has a tendency to form covalent bonds. In free BeX2 molecules, the Be atom is promoted to a state in which the valence electrons occupy two equivalent sp hybrid orbitals and so a linear X—Be—X system is found. However, such a system is coordinatively unsaturated and there is a strong tendency for the Be to attain its maximum coordination of four. This may be done through polymerization, as in solid BeCk, via bridging chloride ligands, or by the Be acting as an acceptor for suitable donor molecules. The concept of coordinative saturation can be applied to the other M"+ cations, and attempts to achieve it have led to attempts to deliberately synthesize new compounds. [Pg.3]

The crystal structure of cyclopentadienylberyllium chloride has been determined by X-ray diffraction (280). As portrayed in CIII, the molecule has the same structure in the solid state as in the gas phase. These results rule out the possibility suggested by the mass spectrum (281) that H5C5BeCl is associated. Although not precisely located, the hydrogen atoms of the cyclopentadienyl ring show a slight tendency to bend toward the beryllium atom, in agreement with theoretical predictions (63). [Pg.287]

The structures of beryllium bromide, BeBr2, and beryllium iodide, Bel2, are similar to that of BeCl2. The chlorides, bromides, and iodides of cadmium, CdX2, and mercury, HgX2, are also linear, covalent molecules (where X = Cl, Br, or I). [Pg.316]


See other pages where Beryllium chloride molecule is mentioned: [Pg.362]    [Pg.362]    [Pg.99]    [Pg.260]    [Pg.47]    [Pg.25]    [Pg.21]    [Pg.563]    [Pg.459]    [Pg.327]    [Pg.388]    [Pg.354]    [Pg.119]    [Pg.797]    [Pg.65]    [Pg.235]    [Pg.89]    [Pg.322]    [Pg.262]    [Pg.119]    [Pg.42]   
See also in sourсe #XX -- [ Pg.99 ]




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