"The difference between the boiling point of methane and chloroform

[Science Person]

The difference between the boiling point of methane and chloroform. Methan's boiling point is -164 C and chloroform's boiling point is 62 C. Explain the difference between two boiling points.

 

I do not get this question at all and really need help answering this particular question. Both the CHCL3 and CH4 have the same shape....but how does that affect their boiling points.

[UC]

The difference between the boiling point of methane and chloroform. Methan's boiling point is -164 C and chloroform's boiling point is 62 C. Explain the difference between two boiling points.

 

I do not get this question at all and really need help answering this particular question. Both the CHCL3 and CH4 have the same shape....but how does that affect their boiling points.

 

There are two factors that govern boiling points. The first is the kind of bonds that the molecules can participate in and the second is molecular mass.

 

Different kinds of intermolecular bonds can be formed, and if the liquid wants to boil, these bonds need to be broken, which requires energy. The stronger the intermolecular bonds, the higher the boiling point. Mass is also important, since on a molecular level, temperature is a measure of the kinetic energy of the molecules, and kinetic energy is dependent on mass. Think about it this way: It takes a lot more effort to keep an elephant airborne than it does to keep a balloon floating.

 

Or something like that. I never was very good at anything physicsy.

[hermanntrude]

check your textbook's chapter on intermolecular bonds.

[Kaeroll]

In addition to the above wisdom, two words: dipole moment.

[Kroughfire]

there are several types of intermolecular forces. ion-ion, London Dispersion, dipole-dipole ion-dipole and H-bonds... the more of these forces, the higher the heat of vaporization. LDF relates to the size of the molocule, giving CHCl3 more intermolecular forces than CH4already. there are no ion-ion, ion-dipole, or dipole-dipole forces in CH4 because those rely on the polarity of the molocule and because Cl is polar, CHCl3 has more intermolecular forces and a higher boiling point.

[hermanntrude]

there are several types of intermolecular forces. ion-ion, London Dispersion, dipole-dipole ion-dipole and H-bonds... the more of these forces, the higher the heat of vaporization. LDF relates to the size of the molocule, giving CHCl3 more intermolecular forces than CH4already. there are no ion-ion, ion-dipole, or dipole-dipole forces in CH4 because those rely on the polarity of the molocule and because Cl is polar, CHCl3 has more intermolecular forces and a higher boiling point.

 

Kroughfire, welcome to the forum. Please check our policy on answering homework questions. Please also review our rules and hazmat policy before posting any more.

 

We do not give out the answers to questions but help our posters to find the answers for themselves.

[Kroughfire]

I am extremely sorry for violating this rule, and I will read them again carefully. Thank you for letting me know.

[hermanntrude]

no biggie, kroughfire. Welcome to the forums :0)