Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: Studentofhem on August 10, 2019, 07:24:45 AM
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Why are the boiling points of group 16 hydrides higher than that of group 17 hydrides?
Especially H2O and HF I assume that HF would be a stronger Hbonding force than H20. As F is more electronegative. So wouldn’t it therefore have a higher boiling point ?
???
Thanks for answering have a test on intermolecular forces!
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No , what is the boiling point of water and hydrogen fluoride?
Order NH3>PH3<AsH3<SbH3<BiH3
H2O>H2S<H2Se<H2Te<H2Po
HF>HCl<HBr<HI<HAt
And H2O>HF>NH3
The highest values can be seen in the second period. It has to do with the hydrogen bridge bpnding.
Water has the highest value, because Oxygen can coordinate 4 bonds. Ammonia only one so the lowest one. HF can make chains like (HF)2-6
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Thanks for the answer but I don’t understand if it’s answered my question.
Why does H2O have a higher boiling point than HF?
I understand why NH3 is the lowest. But I thought HF would have a higher boiling point than H20 why’s isnt this the case?
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No , what is the boiling point of water and hydrogen fluoride?
Order NH3>PH3<AsH3<SbH3<BiH3
H2O>H2S<H2Se<H2Te<H2Po
HF>HCl<HBr<HI<HAt
And H2O>HF>NH3
The highest values can be seen in the second period. It has to do with the hydrogen bridge bpnding.
Water has the highest value, because Oxygen can coordinate 4 bonds. Ammonia only one so the lowest one. HF can make chains like (HF)2-6
Thanks for the answer but I don’t understand if it’s answered my question.
Why does H2O have a higher boiling point than HF?
I understand why NH3 is the lowest. But I thought HF would have a higher boiling point than H20 why’s isnt this the case?
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As I already told, ammonia and hydrogenflouride get only chains. Water get network structures.
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As I already told, ammonia and hydrogenflouride get only chains. Water get network structures.
is there a general reason why group 16 hydrides have a higher boiling point than 17 hydrides
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It has somethings to do, that the elements in 16 have more metalic charachteristic as the ones in group 17. Halogens all non metallic. Chalcogens after sulfur to selenium and heavier ones are more like a metal. In 15 arsenium already is a half metal. It has an effect also of the bonding that beside kovalent some ionic part is present.
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It has somethings to do, that the elements in 16 have more metalic charachteristic as the ones in group 17. Halogens all non metallic. Chalcogens after sulfur to selenium and heavier ones are more like a metal. In 15 arsenium already is a half metal. It has an effect also of the bonding that beside kovalent some ionic part is present.
thank you