Consider the compounds,$BCl_3$ and $CCl_4$. How will they behave with water? Justify.
(N/A) $BCl_3$ acts as a Lewis acid and readily undergoes hydrolysis to form boric acid:
$BCl_3 + 3H_2O \longrightarrow 3HCl + B(OH)_3$
$CCl_4$ resists hydrolysis completely because carbon lacks vacant $d$-orbitals to accept electrons from water molecules to form an intermediate. Thus,when mixed,they form separate layers:
$CCl_4 + H_2O \longrightarrow \text{No reaction}$
$BCl_3 + 3H_2O \longrightarrow 3HCl + B(OH)_3$
$CCl_4$ resists hydrolysis completely because carbon lacks vacant $d$-orbitals to accept electrons from water molecules to form an intermediate. Thus,when mixed,they form separate layers:
$CCl_4 + H_2O \longrightarrow \text{No reaction}$
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Consider the following reactions.
$Na_{2}B_{4}O_{7} \xrightarrow{\Delta} 2 X + Y$
$CuSO_{4} + Y \xrightarrow{\text{Non-Luminous flame}} Z + SO_{3}$
$2Z + 2X + \text{Carbon} \xrightarrow{\text{Luminous flame}} 2Q + Na_{2}B_{4}O_{7} + CO$
The oxidation states of $Cu$ in $Z$ and $Q$,respectively are:
$Na_{2}B_{4}O_{7} \xrightarrow{\Delta} 2 X + Y$
$CuSO_{4} + Y \xrightarrow{\text{Non-Luminous flame}} Z + SO_{3}$
$2Z + 2X + \text{Carbon} \xrightarrow{\text{Luminous flame}} 2Q + Na_{2}B_{4}O_{7} + CO$
The oxidation states of $Cu$ in $Z$ and $Q$,respectively are:
DifficultJEE MAIN 2026
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View SolutionSelect the correct statements from the following:
$A$) Aluminium liberates $H_2$ gas with dil. $HCl$ but not with aqueous $NaOH$.
$B$) Formula of sodium metaborate is $Na_3BO_3$.
$C$) Boric acid is a weak monobasic acid.
$D$) For thallium,$+1$ state is more stable than $+3$ state.
$A$) Aluminium liberates $H_2$ gas with dil. $HCl$ but not with aqueous $NaOH$.
$B$) Formula of sodium metaborate is $Na_3BO_3$.
$C$) Boric acid is a weak monobasic acid.
$D$) For thallium,$+1$ state is more stable than $+3$ state.
In diborane $(B_2H_6)$,the two $H-B-H$ bond angles are nearly
MediumAIIMS 2005
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