Question
Explain the change in bonding when $\mathrm{Al}_2 \mathrm{Cl}_6$ dissociates to form $\mathrm{AlCl}_3$ in the gas phase.
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Explain the change in bonding when $\mathrm{Al}_{2} \mathrm{Cl}_{6}$ dissociates to form $\mathrm{AlCl}_{3}$ in the gas phase.
(a) Write the Lewis formula for $\mathrm{AlCl}_{3}$, a molecular compound. Note that in $\mathrm{AlCl}_{3}$, the aluminum atom is an exception to the octet rule. (b) In the gaseous phase, two molecules of $\mathrm{AlCl}_{3}$ join together (dimerize) to form $\mathrm{Al}_{2} \mathrm{Cl}_{0}$. (The two molecules are joined by two "bridging" Al-Cl-Al bonds.) Write the Lewis formula for the resulting molecule.
Aluminium chloride exists as dimer $\mathrm{Al}_{2} \mathrm{Cl}_{6}$ in solid state as well as in solution of non-polar solvents such as benzene. When dissolved in water, it gives (a) $\mathrm{Al}_{2} \mathrm{O}_{3}+6 \mathrm{HCl}$ (b) $\mathrm{Al}^{3+}+3 \mathrm{Cl}$ (c) $[\mathrm{Al}(\mathrm{OH})]^{3-}+3 \mathrm{HCl}$ (d) $\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}+3 \mathrm{Cl}^{-}$
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