AP CHEM: CH 11 (IMF)

What explains the very high melting and boiling point of water

• Strong dipole-dipole bonds between water molecules
• Strong hydrogen bonds between water molecules
• Dispersion forces which are present in all molecules
• Asymmetrical shape of the polar bonds.

Tags

NGSS.MS-PS1-4

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

• CBr₄
• NO₂
• H₂S
• NH₃

Does HF have hydrogen bonding?

• yes
• no

Does HCl have hydrogen bonding?

• yes
• no

All molecules have London 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 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 dispersion forces?

• F₂

• Br₂

• I₂

• Cl₂

Rank these in order of strength:

covalent bond

dispersion forces

hydrogen bond

dipole-dipole attraction

• dipole-dipole > covalent bond > hydrogen bond > dispersion forces

• dispersion forces > dipole-dipole > hydrogen bond > covalent bond

• covalent bond > hydrogen bond > dipole-dipole > dispersion forces

• hydrogen bond > dipole-dipole > dispersions forces >covalent bond

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

• higher
• lower

Tags

NGSS.HS-PS1-3

What intermolecular bond forms between dipoles when the partially positive end of one polar molecule is attracted to the partially negative end of another polar molecule?

• dipole-dipole force

• dispersion forces

• London forces

• dipole-induced dipole forces

How will the following molecule bond with itself?

• London dispersion forces

• Dipole- dipole forces

• Hydrogen bond

• Ionic bonding