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Boron, the first member of group 13 (p-block) is a typical non-metal. It exists in two allotropic forms. The compounds of boron are mainly electron deficient as well as Lewis acids. For example, all the trihalides of boron \( \left(\mathrm{BX}_{3}\right) \) are Lewis acids. The expected order of acidic strength based on the electronegativity of halogen atoms is: \( \mathrm{BF}_{3}\mathrm{BCl}_{3}\mathrm{BBr}_{3}\mathrm{Bl}_{3} \). But the actual order is the reverse. This is explained with the help of the concept of back bonding \( (p \pi-p \pi) \). Among the hydrides of boron, diborane has a bridged structure.

Which of the statements is wrong about \( \mathrm{BCl}_{3} \) ?
(A) \( \mathrm{BCl}_{3} \) is a covalent compound
(B) \( \mathrm{BCl}_{3} \) acts as a Lewis acid
(C) \( \mathrm{BCl}_{3} \) does not form a dimer
(D) In \( \mathrm{BCl}_{3} \), the \( \mathrm{B}-\mathrm{Cl} \) bond length is greater than the bond length of single covalent bond.
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