How can you explain higher stability of


How can you explain higher stability of $\mathrm{BCl}_{3}$ as compared to $\mathrm{TICl}_{3}$ ?



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. BCl3 is more stable than TlCl3 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.

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