How can you explain higher stability of $BCl_3$ as compared to $TlCl_3$?
How can you explain higher stability of $BCl_3$ as compared to $TlCl_3$?
Boron and thallium belong to group $13 $ of the periodic table. In this group, the $+1$ oxidation state becomes more stable on moving down the group. $BCl _{3}$ is more stable than $TlCl _{3}$ because the $+3$ oxidation state of $B$ is more stable than the $+3$ oxidation state of $Tl$. In$Tl$, the $+3$ state is highly oxidising and it reverts back to the more stable $+1$ state.
Similar Questions
Which of the following is only acidic in nature
Which of the following is only acidic in nature
- [AIIMS 2004]
What happens when...
$(a)$ Borax is heated strongly,
$(b)$ Boric acid is added to water,
$(c)$ Aluminium is treated with dilute $NaOH,$
$(d) $ $B F_3$ is reacted with ammonia ?
What happens when...
$(a)$ Borax is heated strongly,
$(b)$ Boric acid is added to water,
$(c)$ Aluminium is treated with dilute $NaOH,$
$(d) $ $B F_3$ is reacted with ammonia ?
The crystalline form of borax has
($A$) tetranuclear $\left[\mathrm{B}_4 \mathrm{O}_5(\mathrm{OH})_4\right]^{2-}$ unit
($B$) all boron atoms in the same plane
($C$) equal number of $s p^2$ and $s p^3$ hybridized boron atoms
($D$) one terminal hydroxide per boron atom
The crystalline form of borax has
($A$) tetranuclear $\left[\mathrm{B}_4 \mathrm{O}_5(\mathrm{OH})_4\right]^{2-}$ unit
($B$) all boron atoms in the same plane
($C$) equal number of $s p^2$ and $s p^3$ hybridized boron atoms
($D$) one terminal hydroxide per boron atom
- [IIT 2016]
Explain the nature of boric acid as a Lewis acid in water.
Explain the nature of boric acid as a Lewis acid in water.
The liquefied metal which expands on solidification is
The liquefied metal which expands on solidification is
- [AIIMS 2016]