Dipole-Dipole Hydrogen Bonding

What explains the very high melting and boiling point of water?

• Strong dipole-dipole bonds between water molecules

• Strong hydrogen bonds between water molecules

• London dispersion forces which are present in all molecules

• Asymmetrical shape of the polar bonds.

Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?

• CBr₄
• NO₂
• H₂S
• NH₃

Does H₂O have hydrogen bonding?

• yes
• no

Does H₂S have hydrogen bonding?

• yes
• no

Which is the next strongest intermolecular force, after hydrogen bonding?

• dipole-dipole attraction

• London dispersion forces

• ion-ion attraction

• ion-dipole attraction

All molecules have London dispersion forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces. Which of these has ONLY London dispersion forces?

• I₂

• NH₃

• OCl₂

• SH₂

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

• F₂

• Br₂

• I₂

• Cl₂

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

• F₂

• Br₂

• I₂

• Cl₂

In general, substances with stronger intermolecular forces have ___________  boiling points than those with weaker intermolecular forces

• higher
• lower

How will the following molecule bond with itself?

• London dispersion forces

• Dipole-dipole attraction

• Hydrogen bond

• ion-ion attraction