Question

place the following substances in order of increasing boiling point. ch3ch2oh ch3och3 ch3ch2ch3 ch3ch2oh < ch3och3 < ch3ch2ch3 ch3och3 < ch3ch2ch3 < ch3ch2oh ch3och3 < ch3ch2oh < ch3ch2ch3 ch3ch2ch3 < ch3och3 < ch3ch2oh question 12 1 pts choose the substance with the lowest boiling point. h2o2 cf2h2 nbr3 f2 h2s

Explanation:

Step1: Analyze intermolecular forces for first - set of substances

$CH_3CH_2CH_3$ is a non - polar molecule with only London dispersion forces. $CH_3OCH_3$ is polar and has dipole - dipole forces in addition to London dispersion forces. $CH_3CH_2OH$ can form hydrogen bonds (in addition to London dispersion and dipole - dipole forces), and hydrogen bonds are stronger than dipole - dipole and London dispersion forces. So, the order of increasing boiling point for $CH_3CH_2OH$, $CH_3OCH_3$, $CH_3CH_2CH_3$ is $CH_3CH_2CH_3

Step2: Analyze intermolecular forces for second - set of substances

$H_2O_2$ can form hydrogen bonds. $CF_2H_2$ is polar and has dipole - dipole forces. $NBr_3$ is polar with dipole - dipole forces. $F_2$ is non - polar and has only London dispersion forces. $H_2S$ is polar with dipole - dipole forces. Among them, $F_2$ has the weakest intermolecular forces (only London dispersion forces) and the lowest molar mass among non - hydrogen - bonding substances in this set, so it has the lowest boiling point.

Answer:

For the first question: $CH_3CH_2CH_3For the second question: $F_2$