The boiling points of ethane (C2H6), methyl amine (CH3NH2), methylfluorine (CH3F), and lithium fluoride (LiF) are (in random order): -89oC, -78oC, -6oC, and +1673oC. Using the attached sheet if needed, answer the following questions. a. Which of the compounds is most likely to have the boiling point of -6oC? ________________________ b. Which of the compounds would have only London forces as possible intermolecular forces between its molecules? ________________________ c. Which of the compounds could have hydrogen bonds as possible intermolecular forces between its molecules? ________________________ d. Which of the compounds is most likely to have the boiling point of -78oC? ________________________
The boiling points of ethane (C2H6), methyl amine (CH3NH2), methylfluorine (CH3F), and lithium fluoride (LiF) are (in random order): -89oC, -78oC, -6oC, and +1673oC. Using the attached sheet if needed, answer the following questions. a. Which of the compounds is most likely to have the boiling point of -6oC? ________________________ b. Which of the compounds would have only London forces as possible intermolecular forces between its molecules? ________________________ c. Which of the compounds could have hydrogen bonds as possible intermolecular forces between its molecules? ________________________ d. Which of the compounds is most likely to have the boiling point of -78oC? ________________________
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Related questions
Water has a higher boiling point than hydrogen fluoride because it can participate in more hydrogen bonding. What is the maximum number of hydrogen bonds in which a water molecule could theoretically participate?
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QUESTION 2
What statement best describes London (also called dispersion) forces?
They are only present in non-polar substances. | ||
They are the most important type of intermolecular force in water. | ||
They are present in every substance, but often become irrelevant in very polar materials. | ||
They are only present in atoms such as Helium or Argon. |