Doubt about flourine and bromine

  • Thread starter nithin
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  • #1
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hey guys , as i was reading some chemistry , i came to know about this weird thing :"iodine" (I3)- ion exists but "flourine "(F3)- does not exist... it seems that there are 2reasons for this ... i searched the internet and it seems tohave nothing ans my textbook do not also have anything on it ... pls help . intially i thought that the electronegativity of flourine might have to do smth with it........
 

Answers and Replies

  • #2
well that's because of the relatively smaller size of fluoride ion F 1- that does not allow the addition of another electron .
 
  • #3
well thats because the relatively smaller size of fluoride 1- ion does not allow the addition of another electron.
 
  • #4
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Part of the reason that I3- exists because iodine is a much larger atom than fluorine and thus the central iodine atom has more "room" than a fluorine atom would. (Edit: as deepakalways points out...but it's not that simple)

Secondly, if 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.

I have read that the Br3- and I3- exist but I have never heard of the Cl3- ion. This is probably similar to F3- in regards to the size of the atom. I think that the chlorine atom is too small for Cl3- to exist. I am not entirely sure though- you'll have to look that one up for me.

Both Br3- and I3- only can exist in solution as they are fairly unstable. They exist in equilibirum when Br2/I2 and Br-/I- are mixed. For example:

I2 (purple) + I- (colorless) <--> I3- (brown)

That is why tincture of iodine is brown because it is a mixture of I2 and KI.
 
Last edited:

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