Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: xshadow on October 07, 2019, 05:29:12 AM
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HI..I have some doubt about the relative basicity order of H2O and H2S
If H2O and H2S act as a base I'll get:
H3O+
H3S+
Now I think that H3S+ is more stable than H30+ because the positive charge is disperded in a bigger volume
So H3S+ is more stable...so H2S is more reactive than H2O in adding a proton ,H+ ---> H2S is a better base
But is this correct? Because in water H2S never adds a proton while H2O can. But consdering the basicity in gas phase ...maybe...?
Thanks
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[...]H2S is a better base
Incorrect. Think about it again...
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[...]H2S is a better base
Incorrect. Think about it again...
I'll try :
H2S vs H2O basicity:
I have to see which lone pore is more ""basic"", more avaiable??
For two different elements of a group the main difference is the size:
S is bigger than O...so O has a bigger electron density...better base?
Now is it correct?
BUT (a big but) if I think at H3O+ vs H3S+ stabilty I can say that H3S+ is more stable because the positive charge is dispersed on a bigger volume...H3S+ is more stable...so H2S is more reactive than H2O in order to form H3S+ (than H3O+ to form H2O)
In other words why is H3S+ less stable than H3O+??
Because this is the requirement in order to have H2O basicity(reactivity towards H3O+ formation ) > H2S basicity(reactivity towards H3S+ formation)
Thx