Question

Experiment 7 The boiling point of the alcohol reactant for Exp. 7 is 163-166 °C, while the hydrocarbon methylcyclohexene products are lower (range from 101-111°C). What could explain the difference in these values? Select all that are correct. The alcohol has higher intermolecular forces (H-bonding), which take more energy to break so that the molecule can evaporate. The products have weaker intermolecular forces (dispersion forces), which makes it easier for each molecule to evaporate. The products have weaker intermolecular forces (H-bonding), which take more energy to break so that the molecule can evaporate. The alcohol has stronger intermolecular forces (dipole-dipole), which makes it easier for each molecule to evaporate.

          Experiment 7
The boiling point of the alcohol reactant for Exp. 7 is 163-166 °C, while the hydrocarbon methylcyclohexene products are lower (range from 101-111°C).
What could explain the difference in these values? Select all that are correct.
The alcohol has higher intermolecular forces (H-bonding), which take more energy to break so that the molecule can evaporate.
The products have weaker intermolecular forces (dispersion forces), which makes it easier for each molecule to evaporate.
The products have weaker intermolecular forces (H-bonding), which take more energy to break so that the molecule can evaporate.
The alcohol has stronger intermolecular forces (dipole-dipole), which makes it easier for each molecule to evaporate.

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Experiment 7
The boiling point of the alcohol reactant for Exp. 7 is 163-166 °C, while the hydrocarbon methylcyclohexene products are lower (range from 101-111°C).
What could explain the difference in these values? Select all that are correct.
The alcohol has higher intermolecular forces (H-bonding), which take more energy to break so that the molecule can evaporate.
The products have weaker intermolecular forces (dispersion forces), which makes it easier for each molecule to evaporate.
The products have weaker intermolecular forces (H-bonding), which take more energy to break so that the molecule can evaporate.
The alcohol has stronger intermolecular forces (dipole-dipole), which makes it easier for each molecule to evaporate.

Added by Suzanne I.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Jital V

01/31/2022

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The stronger the intermolecular forces, the more energy is required to overcome them and cause the substance to boil. Show more…

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Experiment 7 The boiling point of the alcohol reactant for Exp. 7 is 163-166 °C, while the hydrocarbon methylcyclohexene products are lower (range from 101-111°C). What could explain the difference in these values? Select all that are correct. The alcohol has higher intermolecular forces (H-bonding), which take more energy to break so that the molecule can evaporate. The products have weaker intermolecular forces (dispersion forces), which makes it easier for each molecule to evaporate. The products have weaker intermolecular forces (H-bonding), which take more energy to break so that the molecule can evaporate. The alcohol has stronger intermolecular forces (dipole-dipole), which makes it easier for each molecule to evaporate.

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Transcript

00:01 Hello students, welcome.

00:01 Here in this question we have given that the there are four parts in this question.

00:08 So the first part is given that there is a ketone is given hexanone.

00:14 So this is two hexanone and hexanol also given.

00:19 So this is hexanol.

00:21 So the boiling point of hexanol, hexanone is 20 degrees celsius less when compared with alcohol, okay? when compared with hexanol, the ketone having less boiling point.

00:39 What is the reason? so we can see here, there is oxygen which is present here.

00:45 It can make hydrogen bonding.

00:49 Okay.

00:50 So the intermolecular forces are strong intermolecular forces, strong hydrogen bonding, intra -intermolecular forces are present in alcohol but there is no such type of intermolecular forces in ketone so that's why ketone having less boiling point when compared with alcohol so that is the reason both having the same now same molecular formula but different boiling point due to the process of intramolecular forces strong intermolecular forces in alcohol but not in ketone.

01:28 And the second question is, cis dichloroethane and trans dichloroethane.

01:39 So both are having, it is a polar, so cis one is polar, but trans is non -polar.

01:48 That is the reason they are asking.

01:50 So we can see the polarity, electronegativity of chlorine is higher when compared with carbon.

01:58 So it will be electrons are pulled towards chlorine.

02:03 So negative charge will be this side and positive charge will be this side...

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