Interhalogen compounds
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πŸ‘€︎ u/charlieverma60
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Interhalogens

Do you think it's possible to make chlorine pentafluoride oxide? (ClF5O)? Theoretically, it should be reasonably stable, not to mention a fantastic oxidizer. They made ClF3O and ClF3O2, so I don't see why the pentafluoride variant would be so much harder to manufacture. (that being said, I don't have anywhere near the lab chops and pure guts necessary to make any of the aforementioned substances)

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πŸ‘€︎ u/ksr15
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Inorganic Chemistry: Chemistry of the Halogens and Interhalogens

... is the title of my lab. Anyways, hello! I looked over my laboratory notebook for over 5 times and still couldn't figure out these questions, so I'm turning to you guys.

> The reaction of chlorine and aqueous iodine trichloride with NaBr(aq) and NaI(aq) (four separate reactions to consider). State the important observations that support your conclusions

I made a balanced equation (or I think I did) of

  • Cl2(aq) + 2NaBr(aq) ↔ 2NaCl(aq) + Br2(aq)
  • ICl3(aq) + 3NaBr(aq) ↔ 3NaCl(aq) + IBr3(aq)
  • Cl2(aq) + 2NaI(aq) ↔ 2NaCl(aq) + I2(aq)
  • ICl3(aq) + 3NaI(aq) ↔ 3NaCl(aq) + 2I2(aq)

I am assuming that the above equations are correct (if they are not, please let me know) but I don't know why or how my observations could support them.

For the first equation, I observed clear colorless solution to clear light yellow solution.

For the second equation, I observed clear colorless solution to clear light yellow solution also.

For the third equation, I observed clear colorless solution to clear, reddish-brown solution.

For the fourth equation, I observed clear colorless solution to clear, light yellow solution (lighter than the second).


> The immediate dissolution and decolouration of leftover iodine in the mortar when treated with 6M NaOH(aq) (third equation I'm referring to is X2(aq)+2)H-(aq) ↔ X-(aq) + XO-(aq) + H2O, where X= Cl, Br, or ).

The lab manual states "In neutral or acidic water, the solubility of the elements follows the trend Br2 >> Cl2 > I2 and the following equilibria apply" X2(g,l,s) <=> X2(aq)

However the solid iodine in this case is reacting with a base, NaOH and therefore wouldn't there be no change made from I2(s) and therefore do not turn into I2(aq)? If we pretend it does happen, how does XO- in the third equation work, because as far as I know there's no such molecule as iodine monoxide.


> The imediate decolouration of leftover ICl3(aq) when treated with 6M HaOH(aq). (Hint: this reaction is best thought of as a sequence of steps which should be written out individually and then combined into an overall balanced chemical equation).

I thought I could use equation number 3 for this but this is not I2(aq), but ICl3(aq). I don't know how to reform the equation so that ICl3(aq) would work in place of X2(aq).

--

Sorry for such a lengthy question and thanks.

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[University Inorganic Chemistry] Chemistry of the Halogens and Interhalogens.

... is the title of my lab. Anyways, hello! I looked over my laboratory notebook for over 5 times and still couldn't figure out these questions, so I'm turning to you guys.

> The reaction of chlorine and aqueous iodine trichloride with NaBr(aq) and NaI(aq) (four separate reactions to consider). State the important observations that support your conclusions

I made a balanced equation (or I think I did) of

  • Cl2(aq) + 2NaBr(aq) ↔ 2NaCl(aq) + Br2(aq)
  • ICl3(aq) + 3NaBr(aq) ↔ 3NaCl(aq) + IBr3(aq)
  • Cl2(aq) + 2NaI(aq) ↔ 2NaCl(aq) + I2(aq)
  • ICl3(aq) + 3NaI(aq) ↔ 3NaCl(aq) + 2I2(aq)

I am assuming that the above equations are correct (if they are not, please let me know) but I don't know why or how my observations could support them.

For the first equation, I observed clear colorless solution to clear light yellow solution.

For the second equation, I observed clear colorless solution to clear light yellow solution also.

For the third equation, I observed clear colorless solution to clear, reddish-brown solution.

For the fourth equation, I observed clear colorless solution to clear, light yellow solution (lighter than the second).


> The immediate dissolution and decolouration of leftover iodine in the mortar when treated with 6M NaOH(aq) (third equation I'm referring to is X2(aq)+2)H-(aq) ↔ X-(aq) + XO-(aq) + H2O, where X= Cl, Br, or ).

The lab manual states "In neutral or acidic water, the solubility of the elements follows the trend Br2 >> Cl2 > I2 and the following equilibria apply" X2(g,l,s) <=> X2(aq)

However the solid iodine in this case is reacting with a base, NaOH and therefore wouldn't there be no change made from I2(s) and therefore do not turn into I2(aq)? If we pretend it does happen, how does XO- in the third equation work, because as far as I know there's no such molecule as iodine monoxide.


> The imediate decolouration of leftover ICl3(aq) when treated with 6M HaOH(aq). (Hint: this reaction is best thought of as a sequence of steps which should be written out individually and then combined into an overall balanced chemical equation).

I thought I could use equation number 3 for this but this is not I2(aq), but ICl3(aq). I don't know how to reform the equation so that ICl3(aq) would work in place of X2(aq).

--

Sorry for such a lengthy question and thanks.

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πŸ‘€︎ u/rongrang
πŸ“…︎ Oct 04 2015
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