Comparison of boiling points of aldehydes and ketones?
Butanone has a higher boiling point than butanal, even though butanal has one more hydrogen atom. Why? Thank you 🙂
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They both have the same formula, there’s no one H left. Ergo is also not decisive here. Both have a carbonyl group and are not capable of forming hydrogen bridges. Different intermolecular forces are thus also out. The only difference that remains is the steric, i.e. the spatial construction of the molecule. And he’s obviously a little better at Butanon. Probably because it has a more rigid structure. I mean, the molecule is pretty rigid and can’t twist as much as Butanal can. This makes it easier to pack especially in the solid body but also in the liquid. The molecules can stick together better.
Two questions. Why is this written in this funny format and then still wrong?
I was wondering about the format and why is that wrong?
Because you write that the carbonyl group allows the formation of H bridges. But you also need a donor, a positively polarized H. But you don’t. And if the intermolecular forces were actually so different in the two, the boiling point would not only differ by 5° C. These are just packing effects.
The boiling points are practically identical. The tiny difference is due to packing effects. What is important is the isomeric alcohols 2-butanol (melting point -115 °C) and 2-methyl-2-propanol (melting point +26 °C).