Discuss the types of intermolecular forces acting in the liquid state of each of the following substances. (Select all that apply.)

1. CH3CH2CH2CH2OH

a) dipole-dipole forces
b) London dispersion forces
c) hydrogen bonding

2. CH3OH

a) dipole-dipole forces
b) London dispersion forces
c) hydrogen bonding

You think what? and why?

For #1 I think all three because there's hydrogen bonding between the O-H, there's dipole-dipole between C-H and there's Londond dispersion between the individual H.

If that's the case, then all three would apply for #2 as well.

Am I close?

I agree

Thank you!

the intermolecular force acting on this molecules is hydrogen bonding because if hydrogen in molecule is attached with nitrogen, oxygen and floride it forms a hydrogen bonding

To determine the types of intermolecular forces acting in the liquid state of each substance, we need to examine the chemical structures and identify the key characteristics that contribute to specific types of intermolecular forces.

1. CH3CH2CH2CH2OH (butanol)
a) Dipole-dipole forces: This compound contains an oxygen atom (O) bonded to a hydrogen atom (H). The O-H bond creates a significant electronegativity difference, resulting in a polar covalent bond. As a result, dipole-dipole forces exist due to the partial positive charge on the hydrogen atom and the partial negative charge on the oxygen atom.
b) London dispersion forces: In addition to dipole-dipole forces, butanol also exhibits London dispersion forces. These forces occur between all molecules, regardless of their polarity. London dispersion forces arise due to temporary fluctuations in electron density, resulting in temporary dipoles that induce similar fluctuations in nearby molecules.
c) Hydrogen bonding: Hydrogen bonding occurs when hydrogen is directly bonded to a highly electronegative atom like nitrogen (N), oxygen (O), or fluorine (F). In butanol (CH3CH2CH2CH2OH), the oxygen atom bonded to the hydrogen atom provides this condition. Hence, hydrogen bonding is present.

2. CH3OH (methanol)
a) Dipole-dipole forces: Similar to butanol, methanol contains an oxygen atom bonded to a hydrogen atom. This polar covalent bond produces dipole-dipole forces.
b) London dispersion forces: Like any molecular compound, methanol also exhibits London dispersion forces due to temporary fluctuations in electron density.
c) Hydrogen bonding: Methanol possesses a hydrogen atom bonded directly to an oxygen atom. Since oxygen is highly electronegative, hydrogen bonding is present.

In summary, the intermolecular forces acting in the liquid state of:
1. CH3CH2CH2CH2OH (butanol) are:
a) Dipole-dipole forces
b) London dispersion forces
c) Hydrogen bonding

2. CH3OH (methanol) are:
a) Dipole-dipole forces
b) London dispersion forces
c) Hydrogen bonding