Explain why the following compounds behave as Lewis acids?
$(A)$ $BCl_3$
$(B)$ $AlCl_3$
$(A)$ $BCl_3$
$(B)$ $AlCl_3$
(N/A) $BCl_3$ and $AlCl_3$ are electron-deficient compounds because the central metal atom has an incomplete octet. Therefore,they act as Lewis acids by accepting a lone pair of electrons.
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In $B_2H_6$:
Medium
View SolutionWrite balanced equations for :
$(i) \, BF_{3} + LiH \to $
$(ii) \, B_{2}H_{6} + H_{2}O \to $
$(iii) \, NaH + B_{2}H_{6} \to $
$(iv) \, H_{3}BO_{3} \xrightarrow{\Delta }$
$(v) \, Al + NaOH \to $
$(vi) \, B_{2}H_{6} + NH_{3} \to $
$(i) \, BF_{3} + LiH \to $
$(ii) \, B_{2}H_{6} + H_{2}O \to $
$(iii) \, NaH + B_{2}H_{6} \to $
$(iv) \, H_{3}BO_{3} \xrightarrow{\Delta }$
$(v) \, Al + NaOH \to $
$(vi) \, B_{2}H_{6} + NH_{3} \to $
Medium
View SolutionIn the reactions $I$ and $II$,the covalencies of $Be$ and $Al$ in $X$ and $Y$ are respectively:
$I$ $Be(OH)_2 + NaOH \text{ (excess)} \rightarrow X$
$II$ $Al(OH)_3 + NaOH \text{ (excess)} \rightarrow Y$
$I$ $Be(OH)_2 + NaOH \text{ (excess)} \rightarrow X$
$II$ $Al(OH)_3 + NaOH \text{ (excess)} \rightarrow Y$
Diborane reacts with ammonia under different conditions to give a variety of products. Which one among the following is not formed in these reactions?
Give the increasing order of group $13$ elements for atomic radius.
Easy
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