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Loong
Loong
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Butan-1-ol has a boiling point of approx. 117.7 celsiusdegrees Celsius, and Butanbutan-2-ol has a boiling point of approx. 99.5 celsiusdegrees Celsius. What causes this difference in boiling points?

My initial idea would be that Butanbutan-2-ol essentially has a side-branch (the OH-group), whereas Butanbutan-1-ol does not. This should disrupt the London dispersion forces and thereby reduce the strength. Another idea would be that the position of the OH-group being in the middle for Butanbutan-2-ol creates fewer Hydrogenhydrogen bonds than Butanbutan-1-ol does. My third idea is that the position reduces the strength of the regular dipole-dipole bonds (when I mean regular I mean not hydrogen bonds), because the polarisation is weakened.

Am I correct in any of my assumptions? Is there something else to it?

Butan-1-ol has a boiling point of approx. 117.7 celsius, and Butan-2-ol has a boiling point of approx. 99.5 celsius. What causes this difference in boiling points?

My initial idea would be that Butan-2-ol essentially has a side-branch (the OH-group), whereas Butan-1-ol does not. This should disrupt the London dispersion forces and thereby reduce the strength. Another idea would be that the position of the OH-group being in the middle for Butan-2-ol creates fewer Hydrogen bonds than Butan-1-ol does. My third idea is that the position reduces the strength of the regular dipole-dipole bonds (when I mean regular I mean not hydrogen bonds), because the polarisation is weakened.

Am I correct in any of my assumptions? Is there something else to it?

Butan-1-ol has a boiling point of approx. 117.7 degrees Celsius, and butan-2-ol has a boiling point of approx. 99.5 degrees Celsius. What causes this difference in boiling points?

My initial idea would be that butan-2-ol essentially has a side-branch (the OH-group), whereas butan-1-ol does not. This should disrupt the London dispersion forces and thereby reduce the strength. Another idea would be that the position of the OH-group being in the middle for butan-2-ol creates fewer hydrogen bonds than butan-1-ol does. My third idea is that the position reduces the strength of the regular dipole-dipole bonds (when I mean regular I mean not hydrogen bonds), because the polarisation is weakened.

Am I correct in any of my assumptions? Is there something else to it?

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javanewbie
javanewbie
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Boiling points of Butan-2-ol and Butan-1-ol

Butan-1-ol has a boiling point of approx. 117.7 celsius, and Butan-2-ol has a boiling point of approx. 99.5 celsius. What causes this difference in boiling points?

My initial idea would be that Butan-2-ol essentially has a side-branch (the OH-group), whereas Butan-1-ol does not. This should disrupt the London dispersion forces and thereby reduce the strength. Another idea would be that the position of the OH-group being in the middle for Butan-2-ol creates fewer Hydrogen bonds than Butan-1-ol does. My third idea is that the position reduces the strength of the regular dipole-dipole bonds (when I mean regular I mean not hydrogen bonds), because the polarisation is weakened.

Am I correct in any of my assumptions? Is there something else to it?