Boron is unable to form $BF_{6}^{3-}$ ion. Explain.
(N/A) Boron belongs to the second period and has an electronic configuration of $1s^2 2s^2 2p^1$.
Due to the absence of $d$-orbitals in its valence shell,boron cannot expand its octet beyond $8$ electrons.
Consequently,the maximum covalency of boron is limited to $4$.
Therefore,it cannot form the $BF_{6}^{3-}$ ion,which would require a covalency of $6$.
Due to the absence of $d$-orbitals in its valence shell,boron cannot expand its octet beyond $8$ electrons.
Consequently,the maximum covalency of boron is limited to $4$.
Therefore,it cannot form the $BF_{6}^{3-}$ ion,which would require a covalency of $6$.
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Similar Questions
The correct statements from the following are:
$(A)$ The decreasing order of atomic radii of group $13$ elements is $Tl > In > Ga > Al > B$.
$(B)$ Down the group $13$ electronegativity decreases from top to bottom.
$(C)$ $Al$ dissolves in dil. $HCl$ and liberates $H_2$,but conc. $HNO_3$ renders $Al$ passive by forming a protective oxide layer on the surface.
$(D)$ All elements of group $13$ exhibit a highly stable $+1$ oxidation state.
$(E)$ Hybridisation of $Al$ in $[Al(H_2O)_6]^{3+}$ ion is $sp^3d^2$.
Choose the correct answer from the options given below:
$(A)$ The decreasing order of atomic radii of group $13$ elements is $Tl > In > Ga > Al > B$.
$(B)$ Down the group $13$ electronegativity decreases from top to bottom.
$(C)$ $Al$ dissolves in dil. $HCl$ and liberates $H_2$,but conc. $HNO_3$ renders $Al$ passive by forming a protective oxide layer on the surface.
$(D)$ All elements of group $13$ exhibit a highly stable $+1$ oxidation state.
$(E)$ Hybridisation of $Al$ in $[Al(H_2O)_6]^{3+}$ ion is $sp^3d^2$.
Choose the correct answer from the options given below:
Which of the following oxides is amphoteric in nature?
Diborane reacts with $HCl$ in the presence of $AlCl_3$ and liberates:
DifficultAP EAMCET 2013
View SolutionThe structure of diborane contains:
Medium
View SolutionThe correct statements among $I$ to $III$ regarding group $13$ element oxides are,
$I$. Boron trioxide is acidic
$II$. Oxides of aluminium and gallium are amphoteric
$III$. Oxides of indium and thallium are basic
$I$. Boron trioxide is acidic
$II$. Oxides of aluminium and gallium are amphoteric
$III$. Oxides of indium and thallium are basic
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