which compound has the higher boiling point??
1) \/o\
2) \/\OH
a)The compound has a larger dipole moment, resulting in more dipole-dipole interactions
b)The compound is larger in weight and size and thus has more Van der Waals interactions
c)The compound is smaller in weight and size and thus has fewer van der Waals interactions how would this affect van der waals??
d)The compound can form hydrogen bonds with itself what does this have to do with anything??
e)The compound has a less polar functional group, resulting in more van der Waals interactions
f)The compound has a smaller dipole moment, resulting in fewer dipole-dipole interactions
g) The compound has a more polar functional group, resulting in more dipole-dipole interactions
h)The compound cannot form hydrogen bonds with itself
I'm lost with this...Please help me
and the a,b,c,d....is for why it boils at a higher temp...I have to choose 1 but I'm totally at a loss for explanation b/c it's confusing with so many...
Help...
I will be happy to critique your work. In each of these, the higher bp results when some INTERmolecular force exists that makes the INTERmolecular force stronger. For instance, in the first, the OH allows a hydrogen bond to exist between molecules, thus, the bp is higher. In h, that indicates the bp is lower.
To determine which compound has a higher boiling point, we need to consider the intermolecular forces acting between the molecules. The intermolecular forces play a significant role in determining the boiling point as they determine the strength of attraction between molecules.
1) \/o\ and 2) \/\OH refer to the compounds with different functional groups. Let's analyze the given options to understand how each factor affects boiling point:
a) If a compound has a larger dipole moment, it means there is a larger separation of positive and negative charges within the molecule. This results in stronger dipole-dipole interactions, which would increase the boiling point.
b) Larger compounds with more weight and size tend to have more van der Waals (London dispersion) interactions. These are temporary fluctuations in electron density that induce dipoles, resulting in weak attractions between molecules. More van der Waals interactions generally lead to higher boiling points.
c) Smaller compounds with less weight and size would have fewer van der Waals interactions because there are fewer electrons available for temporary fluctuations in electron density. This would generally result in lower boiling points.
d) Hydrogen bonding occurs when a hydrogen atom is bonded to an electronegative atom (such as oxygen or nitrogen) and interacts with another electronegative atom through electrostatic attraction. Hydrogen bonds are stronger than other intermolecular forces and result in higher boiling points.
e) A less polar functional group would have weaker dipole-dipole interactions, resulting in fewer intermolecular forces and lower boiling points.
f) A smaller dipole moment indicates a smaller separation of positive and negative charges in a molecule. This would result in weaker dipole-dipole interactions and lower boiling points.
g) A more polar functional group would have stronger dipole-dipole interactions, leading to higher boiling points.
h) If a compound cannot form hydrogen bonds with itself, it will not have the additional intermolecular force of hydrogen bonding, resulting in lower boiling points.
Given these explanations, options a), b), d), and g) suggest factors that would increase boiling points. Options c), e), f), and h) suggest factors that would decrease boiling points.
By considering the explanations above, you can compare the given factors for compounds 1) \/o\ and 2) \/\OH and determine which compound is likely to have the higher boiling point.