Explain structures of diborane and boric acid.
Explain structures of diborane and boric acid.
$(a)$ Diborane is an electron deficient compound in which only $12$ valence electrons are present. $2 B$ atoms and $4$ terminal $H$ atoms are co-planar whereas two bridging hydrogen are present in perpendicular plane. One bridging hydrogen is above the plane and other bridging $H$ atom is below the plane. Terminal $B - H$ bonds are $2 c -2 e$ bonds and bridging $B - H - B$ bonds are $3 c$ $-2 e$ bonds.
$(b)$ Boric acid has layered structure. Planar $BO _3$ unit is linked to another unit through $H$ atoms. The $H$ atoms form covalent bond with $BO _3$ unit and hydrogen bond with other $BO _3$ unit.
Similar Questions
$N{a_2}{B_4}{O_7}\xrightarrow{x}{H_3}B{O_3}\xrightarrow{\Delta }{B_2}{O_3}\xrightarrow{y}B$
Here $X, Y$ are respectively
$N{a_2}{B_4}{O_7}\xrightarrow{x}{H_3}B{O_3}\xrightarrow{\Delta }{B_2}{O_3}\xrightarrow{y}B$
Here $X, Y$ are respectively
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Assertion : Atomic radius of gallium is higher than that of aluminium
Reason : The presence of additional $d-$ electron offer poor screening effect for the outer electrons from increased nuclear charge.
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Reason : The presence of additional $d-$ electron offer poor screening effect for the outer electrons from increased nuclear charge.
- [AIIMS 2017]
The $+1 -$ oxidation state in group $-13$ and $+2$ oxidation state in group $-14$ becomes more and more stable with increasing atomic number. Explain.
The $+1 -$ oxidation state in group $-13$ and $+2$ oxidation state in group $-14$ becomes more and more stable with increasing atomic number. Explain.