Polarity and IMFs

Predict the STRONGEST IMF

• London Dispersion

• Dipole-dipole

• Hydrogen Bond

Which of the following does NOT contain hydrogen bonding?

• NH₃

• H₂O

• CF₄

• HOF

Which of the following can result in a London dispersion force?

• When a non-polar molecule becomes slightly polar for an instant

• When the oppositely charged ends of a polar molecule attract each other.

• When there is very strong dipole-dipole attraction between a hydrogen atom and a polar molecule

• When an ion comes close enough to a non-polar molecule to change its electron density.

Which one of the following substances will have hydrogen bonding as one of its intermolecular forces?

• IV only

• II and V

• I and III

• IV and II

Tags

NGSS.HS-PS1-5

Consider the following structures. If the A-B bonds are polar, which of the following molecules are polar?

• I and III

• II and V

•  I, II, and IV

• II and IV

For a container of liquid propylamine, what intermolecular forces would be present?

• London dispersion forces

• London dispersion forces, dipole-dipole forces

• London dispersion forces, dipole-dipole forces, hydrogen bonding

• London dispersion forces, dipole-dipole forces, covalent bonding

In liquid sulfur dioxide, which of the following types of intermolecular force(s) would be present?

• London dispersion forces 

• London dispersion forces, dipole-dipole forces

• London dispersion forces, dipole-dipole forces, hydrogen bonding 

• London dispersion forces, dipole-dipole forces, hydrogen bonding, covalent bonds

Tags

NGSS.HS-PS1-3

Which phrase best completes the following statement: “The electrons in a bond between two iodine atoms (I2)  are shared…”? 

• Equally, and the resulting bond is polar. 

• Equally, and the resulting bond is nonpolar.

• Unequally, and the resulting bond is polar.

• Unequally, and the resulting bond is nonpolar

Which number represents the hydrogen that is capable of hydrogen bonding in acetic acid?

• (i)

• (ii)

• (iii)

•  (iv)

Tags

NGSS.HS-PS1-3

Water (H2O) and dihydrogen monosulfide (H2S) have similar chemical formulas and structures. At room temperature, H2O is a liquid and H2S is a gas. Which of the following best explains this difference?

• H2S molecules are larger and exhibit stronger London dispersion forces and require a greater amount of energy to break.

• H2S molecules are larger and thus the electrons are not attracted as strongly, which makes the  covalent bonds in H2S molecules easier to break.

•  H2O molecules exhibit hydrogen bonding, and thus the attractive forces between water  molecules are stronger than the attractive forces between H2S molecules.

• H2O molecules are smaller and thus exhibit weaker London dispersion forces and require a lesser amount of energy to break