The small size and high charge of \( \mathrm{Al}^{3+} \) ion gives it a high charge density whic....

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The small size and high charge of \( \mathrm{Al}^{3+} \) ion gives it a high charge density which is responsible for its tendency to show (a) covalency in its compounds in the gaseous state (b) high hydration energy which stabilizes its compounds in solution, and (c) high lattice energy of its compounds in the solid state. Thus, aluminium can forms both covalent and ionic Which one of the following statements is correct? bond.
Like halides of boron, halides of aluminium do not show back bonding because of increase in size of aluminium. Actually, aluminium atoms complete their octets by forming dimers. Thus, chloride and (1) All boron trihalides are hydrolysed to boric acid.
(2) Anhydrous aluminium chloride is an ionic compound bromide of aluminium exist as dimers, both in the vapour state and in polar-solvents like benzene while the corresponding boron halides exists as monomer. In boron trihalides the extent of back bonding decreases with increase in size of halogens and thus Lewis acid character increases. All \( \mathrm{BX}_{3} \) are hydrolysed by water but \( \mathrm{BF}_{3} \) shows a different behaviour.


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