your turn 1: which imf/bp is greater
based on the guidelines to the right, let’s determine which of the following substances below would have the higher boiling point. molar masses are given in parenthesis.
ch₃ - o - ch₃ (46.1 g/mol) or
ch₃nh₂ (31.1 g/mol)
remember to start by looking at which forces are the most important.
can either substance hydrogen bond?
yes, and because of hydrogen bonding, ch₃nh₂ has intermolecular forces that are stronger than ch₃ - o - ch₃
no, neither can form hydrogen bonds, so you’ll need to look at the other types of intermolecular forces
which substance has the stronger total intermolecular forces/the higher boiling point?
1. first look to see if the substance can hydrogen bond. if so, it likely has the strongest intermolecular forces (e.g., hf hcl).
2. if you are comparing two molecules of very different molar masses, london dispersion forces are more important (e.g., hbr hcl).
3. if you are comparing two molecules of very similar molar mass, dipole - dipole forces are more important. the molecule with the greater dipole - dipole forces (the greatest electronegativity difference between the atoms within the molecule) will have the greatest boiling point.

Question

your turn 1: which imf/bp is greater
based on the guidelines to the right, let’s determine which of the following substances below would have the higher boiling point. molar masses are given in parenthesis.
ch₃ - o - ch₃ (46.1 g/mol) or
ch₃nh₂ (31.1 g/mol)
remember to start by looking at which forces are the most important.
can either substance hydrogen bond?
yes, and because of hydrogen bonding, ch₃nh₂ has intermolecular forces that are stronger than ch₃ - o - ch₃
no, neither can form hydrogen bonds, so you’ll need to look at the other types of intermolecular forces
which substance has the stronger total intermolecular forces/the higher boiling point?
1. first look to see if the substance can hydrogen bond. if so, it likely has the strongest intermolecular forces (e.g., hf > hcl).
2. if you are comparing two molecules of very different molar masses, london dispersion forces are more important (e.g., hbr > hcl).
3. if you are comparing two molecules of very similar molar mass, dipole - dipole forces are more important. the molecule with the greater dipole - dipole forces (the greatest electronegativity difference between the atoms within the molecule) will have the greatest boiling point.

Accepted Answer

# Explanation:
## Step1: Analyze hydrogen bonding capability
Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom (N, O, F). In $CH_{3}NH_{2}$, the hydrogen is bonded to nitrogen, so it can form hydrogen bonds. In $CH_{3}-O - CH_{3}$, there is no hydrogen bonded to a highly electronegative atom (the hydrogens are bonded to carbon), so it cannot form hydrogen bonds.
## Step2: Compare intermolecular forces
Since $CH_{3}NH_{2}$ can form hydrogen bonds (a strong type of intermolecular force) and $CH_{3}-O - CH_{3}$ cannot, $CH_{3}NH_{2}$ will have stronger intermolecular forces. Stronger intermolecular forces lead to a higher boiling point as more energy is required to overcome these forces to convert the liquid to a gas.

# Answer:
Yes, and because of hydrogen bonding, $CH_{3}NH_{2}$ has intermolecular forces that are stronger than $CH_{3}-O - CH_{3}$

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QUESTION IMAGE

Question

Explanation:

Step1: Analyze hydrogen bonding capability

Step2: Compare intermolecular forces

Answer: