How can you explain higher stability of BCl3 as compared to TlCl3?
Harshit Singh , 4 Years ago
Grade 12th pass
Physical Chemistry> How can you explain higher stability of B...
1 AnswersPawan Prajapati
Last Activity: 4 Years ago
Answer: BCl3 is quite stable. Because there is absence of d- and f-electrons in boron three valence electrons (2s2 2p) are there for bonding with chlorine atom. In Tl the valence s-electron (6s2) are experiencing maximum inert pair effect. Thus, only 6p1 electron is available for bonding. Therefore, BCl3 is stable but TlCl3 is comparatively unstable.
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