How you can explain higher stability of BCl3 as compared to TICl3
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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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Answer:
As we go down the Boron family, +1 oxidation state is highly stable,, and not +3 as it is highly oxidising in nature.
In both the above mentioned compounds, the elements have +3 state.Tl which is situated down the group is stable therefore with +1 state.So BCl3 is highly stable than TlCl3.
Explanation:
In BCl3, B is in +3 oxidation state. Since boron is a small atom and it contains 3 electrons in the outer most
shell, it can easily show +3 oxidation state. (It can form 3 B-Cl bonds). Down the group +1 oxidation state becomes
more common due to inert pair effect. It is the reluctance of s-electrons to participate in chemical binding. Thus
only p-electrons take part in chemical reaction and hence Tl mainly shows +1 oxidation state.
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