The boiling point of o-nitrophenol is lower than that of p-nitrophenol due to differences in intermolecular hydrogen bonding. In o-nitrophenol, the hydroxyl (-OH) group and the nitro (-NO2) group are positioned ortho to each other, which can lead to steric hindrance and less effective hydrogen bonding compared to the para isomer. In p-nitrophenol, the groups are positioned para to each other, allowing for stronger and more stable hydrogen bonding interactions, which results in a higher boiling point. Thus, the molecular interactions significantly influence their boiling points.
It is lower.
Yes
The boiling point of methanol is lower than the boiling point of ethanol.
the ortho position is the key to the answer of this question. in this case the NO2 and OH group are neighbors and thus can interact via intramolecular bonding this on the other hand decreases the overall polarity of the molecule. when a molecule is less polar it travels faster through a polar adsorbent than a highly polar molecule.
Yes, but-1-ene boiling at −6.47 °C, which is lower than the boiling point of but-1-yne: 8.08 °C
o-nitrophenol forms intramolecular H bond and no association occurs whereas molecules of p-nitrophenol get associated through intermolecular H bonding and boils relatively at higher tem. (above the B.P.of water). Hence,only ortho-nitrophenol is steam volatile.
4-Nitrophenol is more polar than 2-nitrophenol primarily due to the positioning of the nitro group relative to the hydroxyl group. In 4-nitrophenol, the nitro group is located para to the hydroxyl group, allowing for effective resonance and dipole interactions that enhance polarity. In contrast, in 2-nitrophenol, the nitro group is ortho to the hydroxyl group, where steric hindrance and less effective resonance diminish the overall polarity. As a result, the intermolecular forces in 4-nitrophenol are stronger, contributing to its increased polarity.
The dipole moment of para-nitrophenol is greater than ortho-nitrophenol. This is because in para-nitrophenol, the nitro group is positioned opposite to the hydroxyl group, leading to a higher dipole moment due to the greater separation between the polar groups.
At a constant pressure, the freezing point is always going to be lower than the boiling point.
It is lower.
Oxygen has a lower point.
Covalent compounds have a lower melting point.
Covalent compounds have a lower melting point.
It depends what chemical or compound you are comparing the boiling point to. Ethanol has an atmospheric pressure boiling point of 78.1 °C (172.6 °F). This is slightly lower than the boiling point of water at the same pressure, much lower than the boiling point of iron, much higher than the boiling point of bromine.
Yes
Yes
lower.