Covalent and Dative covalent bonding.
To draw the Lewis structure of aluminum chloride (Al2Cl6) dimer, you would have two aluminum atoms (Al) connected to each other through a single covalent bond, with each aluminum atom bonded to three chlorine atoms (Cl) each through single covalent bonds. There would also be two lone pairs on each of the chlorine atoms to satisfy their octet.
AlCl3 forms a dimer because of the presence of electron-deficient aluminum atom which attracts lone pairs on neighboring AlCl3 molecules, leading to the formation of coordinate bonds. This results in the formation of a stable dimeric structure, Al2Cl6, where two AlCl3 molecules are linked together by coordinate bonds.
yes to produce aluminium chloride AlCl3 vapour which is Al2Cl6 . Aluminium(III) in crystalline AlCl3 are six coordinate, on melting or sublimation (at 150C) the molecule assume the molecular form Al2Cl6
Formula: Al2Cl6
The point group for Al2Cl6 is (D_{3h}). It consists of two Al atoms and six Cl atoms arranged in a symmetric manner with a trigonal prismatic geometry.
Four or eight, depending on the state. It exists as AlCl3 or Al2Cl6.
A coordinate covalent bond is a type of covalent bond where both of the shared electrons come from the same atom. In this bond, one atom donates both electrons to be shared with another atom that lacks electrons. This type of bond is also known as a dative bond.
First, draw an AlCl3 molecule, in dot-structure. You will see that in the molecule, Aluminum has only 6 electrons, 3 of which are shared with the chlorine atoms. It needs 2 more electrons to become more stable (8 electrons in the outer shell is usually stable). Now look at the chlorine atom in the AlCl3 molecule.It has 8 electrons, and thus, it is somewhat "stable". If a Chlorine atom from ANOTHER AlCl3 molecule formed a dative bond with the Aluminum atom(a dative bond is a covalent bond where both shared electrons come from just one species. In this case, both electrons come from the chlorine atom), this Al atom would now have 8 electrons as well. That is why AlCl3 exists as a dimer- as Al2Cl6 . It's structure is shown in this picture.
yes to produce aluminium chloride AlCl3 vapour which is Al2Cl6 . Aluminium(III) in crystalline AlCl3 are six coordinate, on melting or sublimation (at 150C) the molecule assume the molecular form Al2Cl6
The point group for Al2Cl6 is (D_{3h}). It consists of two Al atoms and six Cl atoms arranged in a symmetric manner with a trigonal prismatic geometry.
Formula: Al2Cl6
AlCl3 at high temperatres in the vapor phase is molcular, planar AlCl3. with polar covalent bonds. In the melt and at lower temperatures in the vapor phase it is dimeric, Al2Cl6 with two bridging Cl atoms ( Cl2AlCl2AlCl2), each aluminium atom is approximately surrounded by a tetrahedron of Cl atoms. in the solid the structure has each Al surrounded by 6 Cl atoms and the bonding is more ionic in nature. As the solid is heated just before it melts the electrical conductivity rises due to the presence of ions.
Four or eight, depending on the state. It exists as AlCl3 or Al2Cl6.
The sublimation of a molecule depends on the intermolecular forces. Since Aluminium Chloride exists as a dimer, Al2Cl6. It has weak intermolecular forces (also, Vander Waal Forces) due to which it sublimes at a relatively low temperature of 180 degree Celsius.
Sodium and calcium chlorides are extended ionic solids because they consist of repeating unit cells formed by the attraction between positively charged metal ions and negatively charged chloride ions. In contrast, aluminum trichloride exists as a dimer, Al2Cl6, because it forms covalent bonds between two aluminum atoms and six chlorine atoms in a small cluster rather than a large, repeating lattice structure like the ionic solids.
The ratio in aluminum chloride is 1:3 aluminum to chloride ( AlCl3 or Al2Cl6 )
Solid FeCl3 (ferric chloride or Fe(III) chloride) is indeed ionic. there are two forms the anhydrous and hexahydrate FeCl3.6H2O. In the vapour phase it forms a dimer Fe2Cl6 which has the same chlorine bridged structure, Al2Cl6 ,as aluminium trichloride does in the vapour phase. The bonding in this well its probably best described as polar covalent.
If the difference in electronegativity between the two atoms is greater than 2.0, then the bond is ionic. If one of the elements is a metal the rule is then relaxed a little to a difference of 1.6. Compounds on the "boundary of the rules" such as aluminium chloride Al, 1.61 Cl, 3.16 exhibit ionic and covalent tendencies. Al2Cl6 in the solid is ionic but in the liquid and vapour dimerises to form Al2Cl6 molecules.