How can you explain higher stability of $B C l_{3}$ as compared to $T l C l_{3}$ ?

Open in App

Solution

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. $B C l_{3}$ 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.

Suggest Corrections

Similar questions

How would you explain the lower atomic radius of Ga as compared to Al?

B C l_{3},

- A l C l_{3}

- G a C l_{3}

- T l C l_{3} .

Natural selection lead to directional change ,stabilization or disruption...... Can you explain this line

Join BYJU'S Learning Program

Explore more

Join BYJU'S Learning Program