Statement II: Boron has the highest melting and boiling point compared to its other group members. In the light of the above statements, choose the most appropriate answer from the options given below.

Both Statement I and Statement II are incorrect

Correct Answer

Wrong Answer

Statement I is incorrect but Statement II is correct

Correct Answer

Wrong Answer

Statement I is correct but Statement II is incorrect

Correct Answer

Wrong Answer

Both statement I and Statement II are correct

Correct Answer

Wrong Answer

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The incorrect statement from the following for borazine is:

It is a cyclic compound.

Correct Answer

Wrong Answer

It has electronic delocalization.

Correct Answer

Wrong Answer

It can react with water.

Correct Answer

Wrong Answer

It contains banana bonds.

Correct Answer

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What will be the $\mathrm{B.F}$ distance in $\mathrm{\mathrm{BF}_3}$ molecule if you are given with $\mathrm{B-F}$ distance as $\mathrm{139 \mathrm{pm}}$ in $\mathrm{\left(\mathrm{CH}_3\right)_3 \mathrm{~N}-\mathrm{BF}_3}$ molecule?

Because of $\mathrm{p \pi-p \pi }$ back bonding in $\mathrm{ B F_3}$ , it will be less.

Correct Answer

Wrong Answer

because of $\mathrm{p \pi-p \pi}$ back bonding, it will be more in $\mathrm{\mathrm{BF}_3.}$

Correct Answer

Wrong Answer

same as in $\mathrm{\left(\mathrm{CH}_3\right)_3 \mathrm{~N}-\mathrm{BF}_3}$

Correct Answer

Wrong Answer

Because $\mathrm{BF}_3$ exists as dimer, it will be more.

Correct Answer

Wrong Answer

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$\mathrm{BCl}_3$ can act as

Lewis acid

Correct Answer

Wrong Answer

Lewis Base

Correct Answer

Wrong Answer

Bronsted Acid

Correct Answer

Wrong Answer

Bronsted Base

Correct Answer

Wrong Answer

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Which of the following complex doesn't exist?

$B F_4^{-}$

Correct Answer

Wrong Answer

$B F_6^{-3}$

Correct Answer

Wrong Answer

$\mathrm{B}(\mathrm{OH})_4^{-}$

Correct Answer

Wrong Answer

None of these

Correct Answer

Wrong Answer

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Boron has more tendency to form complex than Lithium or any alkali metal. It is due to

less electropositive character of Boron

Correct Answer

Wrong Answer

High electronegativity of Boron

Correct Answer

Wrong Answer

The smaller size of Boron

Correct Answer

Wrong Answer

High electron affinity of Boron

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Diborane acts as

Lewis acid

Correct Answer

Wrong Answer

Lewis base

Correct Answer

Wrong Answer

Nucleophile

Correct Answer

Wrong Answer

Brownsted acid

Correct Answer

Wrong Answer

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Concepts Covered - 1

Anomalous Behaviour of Boron

Certain important trends can be observed in the chemical behaviour of group 13 elements. The tri-chlorides, bromides and iodides of all these elements being covalent in nature are hydrolysed in water. Species like tetrahedral [M(OH)₄]^- and octahedral [M(H₂O)₆]³⁺, except in boron, exist in an aqueous medium.
The monomeric trihalides, being electron-deficient, are strong Lewis acids. Boron trifluoride easily reacts with Lewis bases such as NH₃ to complete octet around boron.

$\mathrm{F}_{3} \mathrm{B}+: \mathrm{NH}_{3} \rightarrow \mathrm{F}_{3} \mathrm{B} \leftarrow \mathrm{NH}_{3}$

It is due to the absence of d orbitals that the maximum covalence of B is 4. Since the d orbitals are available with Al and other elements, the maximum covalence can be expected beyond 4. Most of the other metal halides (e.g., AlCl₃) are dimerised through halogen bridging (e.g., Al₂Cl₆). The metal species completes its octet by accepting electrons from halogen in these halogen bridged molecules.