Polarity and Intermolecular Forces

Does NH₃ or PH₃ have a higher boiling point? (Hint: identify the types of IMF's present for each)

• NH₃ because it has the strongest IMF's

• PH₃ because it has the strongest IMF's

• NH₃ because it has the weakest IMF's

• PH₃ because it has the weakest IMF's

Which substance has the weakest intermolecular forces?

• Substance A, boiling point of 75 °C

• Substance B, boiling point of 105 °C

• Substance C, boiling point of 25 °C

• Substance d, boiling point of 45 °C

The intermolecular force present in all matter is

• Hydrogen Bonding

• Ionic Bonding

• Dipole-Dipole

• London or Dispersion

The strongest IMF is

• London/Dispersion

• Dipole-Dipole

• Hydrogen Bonding

The properties affected by the IMF's are:

• Boiling Point

• Melting Point

• Surface Tension

• all 3 are affected by IMF

Which substance has the weakest intermolecular forces?

• Substance A, boiling point of 75 °C

• Substance B, boiling point of 105 °C

• Substance C, boiling point of 25 °C

• Substance d, boiling point of 45 °C

Tags

NGSS.HS-PS1-3

London forces are stronger in heavier atoms or molecules, and weaker in lighter atoms or molecules.  Which of these has the strongest London forces?

• F₂

• Br₂

• I₂

• Cl₂

Which of the following statements correctly explains why hydrogen bonding is such a strong intermolecular force?

• There is an attraction between a small, weakly electronegative hydrogen atom and a large, strongly electronegative atom of fluorine, nitrogen, or oxygen

• There is an attraction between a small, highly electronegative hydrogen atom and a large, highly electronegative fluorine atom

• There is an attraction between the hydrogen and oxygen atoms, only

• There is an attraction between the hydrogen and nitrogen atoms, only

Water has an unusually high boiling point for a molecular compound because it has

• hydrogen bonding

• ion-ion attractions

• a high density

• a large gram formula mass

Which of the following will NOT have hydrogen bonding?

• 
• 
• 
•