Explain the following:
$(1)$ Aluminum forms $[AlF_6]^{3-}$ ion but boron does not form $[BF_6]^{3-}$ ion.
$(2)$ $PbX_2$ is more stable than $PbX_4$.
$(1)$ Aluminum forms $[AlF_6]^{3-}$ ion but boron does not form $[BF_6]^{3-}$ ion.
$(2)$ $PbX_2$ is more stable than $PbX_4$.
(N/A) $Al$ has vacant '$d$' orbitals and can expand its coordination number to form $[AlF_6]^{3-}$.
On the other hand,Boron does not have '$d$' orbitals and cannot expand its covalence beyond $4$,thus it forms $[BF_4]^{-}$ instead of $[BF_6]^{3-}$.
Due to the inert pair effect,the $+2$ oxidation state is more stable than the $+4$ oxidation state for lead $(Pb)$.
On the other hand,Boron does not have '$d$' orbitals and cannot expand its covalence beyond $4$,thus it forms $[BF_4]^{-}$ instead of $[BF_6]^{3-}$.
Due to the inert pair effect,the $+2$ oxidation state is more stable than the $+4$ oxidation state for lead $(Pb)$.
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The correct statement$(s)$ for orthoboric acid $(H_3BO_3)$ is/are:
$(A)$ It behaves as a weak acid in water due to self-ionization.
$(B)$ Acidity of its aqueous solution increases upon addition of ethylene glycol.
$(C)$ It has a three-dimensional structure due to hydrogen bonding.
$(D)$ It is a weak electrolyte in water.
$(A)$ It behaves as a weak acid in water due to self-ionization.
$(B)$ Acidity of its aqueous solution increases upon addition of ethylene glycol.
$(C)$ It has a three-dimensional structure due to hydrogen bonding.
$(D)$ It is a weak electrolyte in water.
Which of the following substances is the strongest acid?
Easy
View Solution$Na_2B_4O_7 \cdot 10H_2O \xrightarrow{\Delta} X + NaBO_2 + H_2O$
$X + Cr_2O_3 \xrightarrow{\Delta} Y$ (Green coloured)
$X$ and $Y$ are
$X + Cr_2O_3 \xrightarrow{\Delta} Y$ (Green coloured)
$X$ and $Y$ are
Difficult
View SolutionConsider the following statements for diborane $(B_2H_6)$:
$1.$ Boron is approximately $sp^3$ hybridized.
$2.$ $B-H-B$ angle is $180^{\circ}$.
$3.$ There are two terminal $B-H$ bonds for each boron atom.
$4.$ There are only $12$ bonding electrons available.
Which of these statements are correct?
$1.$ Boron is approximately $sp^3$ hybridized.
$2.$ $B-H-B$ angle is $180^{\circ}$.
$3.$ There are two terminal $B-H$ bonds for each boron atom.
$4.$ There are only $12$ bonding electrons available.
Which of these statements are correct?
Give reasons: Aluminium alloys are used to make aircraft bodies.
Easy
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