1if you draw the lewis structure for I3-, you'll see that the central iodine atom does not obey the octect rule. It has 5 electron domains (10 electrons). This means that its d orbitals are participating in its bonding. Fluroine is only in the second period and since there are no "2d" orbitals, it cannot form the F3- ion.
If we use this same logic than both Cl3- and Br3- should exist because the central atoms in those ions would utilize their 3d and 4d orbitals, respectively.
but Cl3- does not exist.This is probably similar to F3- in regards to the size of the atom. chlorine atom is too small for Cl3- to exist
1But cl3- must first enter the 4s orbital and thn only 3d naaa?
11Well, though Br3- ion is less stable and less common than I3-
A few unstable Cl3- compounds are known, and the ion is formed in concentrated solution. This means Cl3- exist.
No F3- compounds are known
@ Shubham, Chlorine is in 3rd period usme 4th shell kyun dal rahe ho.
1
Shubh
·2010-10-12 03:04:16
@khyati the_myth na bola naa ki Cl3- will use its 3d orbital? how? if chlorine has to uce its 3d orbital as myth told thn it has to first enter 4s orbital......im a lil unclear? Khyati plzz clear? and myth also :)
11
Khyati
·2010-10-12 08:22:09
Well, actually when these kinds of situation arises, the atoms directly use their 3d subshells
without using 4s. (Its a guess, but I think this is what exactly happens), that 3d
and 4s we have to take in sequence when we do electronic configuration, but here I think
electrons have enough energy to jump and get into 3d orbitals for the formation of
molecules.
71Well I think 4s --> then 3d from inside out.
But when electrons comes from outside or any other atom then 3d-->4s (Outside In) orbitals are filled up..
