Intermolecular Forces

List the following from strongest to weakest.

• ion-dipole bonds

• London Dispersion Forces / Van Der Waals Forces

• Hydrogen bonds

• dipole-dipole interactions

More mass : Stronger gravity :: More mass : ​ ​ (a)   Van Der Waals Forces

• Stronger
• Weaker
• Equal
• Unknown

Potassium is dissolved in an aqueous solution. Click the part of the molecule that will have an affinity to the solute.

Water is liquid at room temperature, but carbon dioxide is not. Why is that?

• CO₂ is straight, while H₂O is bent.

• H₂O has weaker intermolecular forces due to dipole-dipole interactions.

• H₂O has stronger intermolecular forces due to hydrogen bonding.

• CO₂ has less mass than H₂O.

Where in this diagram are the intermolecular forces strongest?

Tags

NGSS.HS-PS1-3

Which of the following characteristics describe the following substance? Select all that apply.

• London dispersion forces (aka Van Der Waals forces)

• dipole-dipole interactions

• Hydrogen bonds

• polar

Tags

NGSS.HS-PS1-5

Which of the following characteristics describe the following substance? Select all that apply.

• London dispersion forces (aka Van Der Waals forces)

• dipole-dipole interactions

• Hydrogen bonds

• polar

Which of the following characteristics describe the following substance? Select all that apply.

• London dispersion forces (aka Van Der Waals forces)

• dipole-dipole interactions

• Hydrogen bonds

• polar

Which of the following characteristics describe the following substance? Select all that apply.

• London dispersion forces (aka Van Der Waals forces)

• dipole-dipole interactions

• Hydrogen bonds

• polar

Tags

NGSS.HS-PS1-3

Stronger bonds:

​ ​ (a)   melting/freezing point.

​ ​ (b)   boiling/condensation point.

​ (c)   viscosity & surface tension.

• increase
• decrease
• don't affect

Tags

NGSS.HS-PS1-3