Halogen Reactions Watch

staywithme
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#1
Report Thread starter 3 years ago
#1
Hey all,

So I'm really confused with something I'm trying to do in a revision question book.

It says this:
Sodium was reacted with bromine vapour and a white solid was formed.
Would this reaction occur faster or slower than a similar reaction between:
a) sodium and iodine vapour?
b) sodium and chlorine vapour?

I thought a) would be slower as iodine is further down in the Halogens so would therefore be less reactive and b) would be faster as Chlorine is higher up and therefore more reactive; however, the revision guide states that it is the opposite way round!
Please could somebody clarify for me?

Thanks x
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CandyKoRn
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That would apply if electronegativity was the only factor. You have to go back to the basic rule of; reactivity increases down a group.
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Kallisto
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Looking at some periodic tables, we can see that chlorine has 3.0 as electronegativity, iodine has 2.5 and bromine 2.0. The reactant is always sodium. Sodium has an electronegativity of 0.9.

The greater the difference between the reactants in terms of their electronegativities, the more reactive are the reactants to each other. Here is the calculation:

chlorine (3.0) - sodium (0.9) = 2.1
iodine (2.5) - sodium (0.9) = 1.6
bromine (2.0) - sodium (0.9) = 1.1

So the order of the reactivity start with the weakest one is:

bromine < iodine < chlorine

So from this point of view the reaction occurs faster by using chlorine vapour and iodine vapour.
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staywithme
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Thankyou !
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