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In the gas phase, some AlCl3 molecules join in pairs to form this dimer: (i) Identify the hybridization of the aluminium atom in the dimer, Al2Cl6. (ii) Describe, in terms of Lewis acids and bases, how two AlCl3 molecules bond together to…
Manganese, unlike aluminium, is a transition element. (i) Deduce, from the electron configuration of the Mn2+ ion, why manganese is classified as a transition element. (ii) The first four ionization energies of aluminium and manganese are shown. One…
The standard electrode potential, E⊖, of the half-cell Al3+(aq) + 3 e− ⇌ Al(s) is −1.66 V. (i) Calculate the standard cell potential for the reaction 2 Al(s) + 6 H2O(l) → 2 Al3+(aq) + 6 OH−(aq) + 3 H2(g) Use section 19 of the data…
Using nuclear charge, electron sub-levels and the shielding by filled inner shells, explain why the first ionization energy rises from sodium to magnesium but falls from magnesium to aluminium.
Outline how the atomic emission spectrum of aluminium could be used to find its first ionization energy.
The first three ionization energies of two elements, X and Y, are shown in the table. Which two elements are X and Y, in that order? A. Sodium and magnesium B. Magnesium and sodium C. Magnesium and silicon D. Silicon and magnesium
Outline the electrostatic attraction that holds a crystal of aluminium together.
Aluminium is produced by the electrolysis of molten aluminium oxide (in industry dissolved in molten cryolite to lower the operating temperature). A simplified cell is shown in the diagram. (i) Outline why the molten mixture is classified as an electrolyte.…
Aluminium reacts with chlorine to form the chloride AlCl3. (i) Draw a Lewis (electron dot) structure for AlCl3. (ii) Outline in what respect this Lewis structure is unusual.
In the gas phase some aluminium chloride exists as the dimer Al2Cl6, the structure of which is shown below. (i) Identify the hybridization of the aluminium atom in the dimer, Al2Cl6. (ii) Describe, in terms of Lewis acid–base behaviour, the…