Chapter 1.13, Problem 30PTS

For each pair, which has the lowest boiling point? Is the selection correct?

Which compound in each pair has the higher boiling point? Which compound in each pair has the higher melting point? a. CH 4 or C 2H 6 b. C 2H 6 or CH 3OH c. HBr or HCl d. C 2H 6 or CH 3Br

Which molecule will have a higher boiling point and why a.   molecule ‘b’ will have a higher boiling point as the molecule is more compact and therefore will pack better.   b. molecule ‘b’ will have the higher boiling point as the methyl groups are tetrahedrally arranged around the central carbon, giving it higher symmetry. c. molecule ‘a’ will have a higher boiling point as it has a greater surface for London dispersion forces. d. molecule ‘a’ will have a higher boiling point as it has a higher molecular weight than molecule ‘b’.

And pls explain why the boiling points of each compound increase

Arrange the compounds of each group in order of increasing boiling point. a. ethanol, 1-propanol, methanol b. butane, ethylene glycol, 1-propanol

Which of these compounds have the higher boiling point? Why? a) top two compounds b) bottom two compounds

What is the melting point, boiling point and molecular formula  for the compound  on the pic

Q.3. Circle the compound with the highest boiling point and cross out the compound with the lowest boiling point. CI OH HO HO OH

Compare the following two compounds. Which is more soluble in water? Why?   A) Compound 1 is more soluble because it has more ability to hydrogen bond with water.   B) Compound 2 is more soluble because it has more ability to hydrogen bond with water   C) Neither of these compounds is water soluble.   D) Compound 1 is more soluble because it will have more dipole-dipole interactions with water.   E) Compound 2 is more soluble because it will have more dipole-dipole interactions with water.