IMF's and Physical Properties

Relative Strength's of IMF's and Physical Properties

Be able to identify all IMF's exhibited by a molecule and determine relative strength's of physical properties based on IMF's present

Categorize

Options (6)

only IMF between nonpolar molecules

exist between both polar and nonpolar molecules

generally the weakest of the forces

exist between polar molecules

exist between molecules that have hydrogen bonded to N, O, or F

generally the strongest of the IMF's

Organize these options into the right categories

London Dispersion Forces Only

Dipole Dipole

Hydrogen Bonding

Match

Match the following

• Nonpolar, therefore London Dispersion Forces Only

• Polar therefore London Dispersion Forces and Dipole Dipole forces

• Special case of a polar molecule therefore London Dispersion Force

  Dipole Dipole and Hydrogen Bonding

CBr₄

NO₂ ^--

NH₃

• CBr₄

• NO₂ ^--

• NH₃

Multiple Select

SiO₂ has what kind of intermolecular force? (list all that apply)

• dipole dipole

• London Dispersion Force

• H-bond

• covalent bonds

Multiple Select

List all Intermolecular force(s) exhibited by HCl?

• dipole dipole

• London dispersion forces

• H-bond

• ionic

Reorder

Arrange the following molecules from predicted lowest boiling point to highest boiling point:

• Cl₂

• SO₂

• H₂O

1

2

3

• 1
• 2
• 3

• when comparing nonpolar molecules

• the larger the electron cloud (size) of the molecule the more polarizable

• the more polarizable the stronger s the IMF's

​

How to determine the relative strength of London Dispersion Forces

Drag and Drop

When determining the relative strength of IMF's between nonpolar molecules, the ​

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the more ​

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As the polarizablity increases the strength of the IMF's ​

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. Thus, CH₄ would have ​

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London Dispersion Forces than ​ CCl₄ and would be predicted to have a​

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.

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larger the electron cloud

smaller the electron cloud

polarizable.

increases

decreases

weaker

higher vapor pressure

lower vapor pressure 

magnetizable

Reorder

All of the following molecules are non-polar. Place them f in order of weakest to strongest IMF's

• CH₄

• C₂H₆

• C₃H₈

• C₄H₁₀

• C₅H₁₂

1

2

3

4

5

• 1
• 2
• 3
• 4
• 5

Multiple Choice

Which statement explains why Br₂ is a liquid and I₂ is a solid?

• Molecules of Br₂ are polar, and molecules of I₂ are nonpolar

• Molecules of Br₂ are nonpolar, and molecules of I₂ are polar

• Molecules of Br₂ have stronger intermolecular forces than molecules of I₂.

• Molecules of I₂ have stronger intermolecular forces than molecules of Br₂.

Drag and Drop

Ammonia, NH₃, is a polar molecule as is phosphine, PH_3. However, ammonia exhibits ​

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whereas phosphine does not. This explains why ammonia has such a ​

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and ​

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vapor pressure and ​ ​

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surface tension. ​Between the two,

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would be expected to be more volatile.

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hydrogen bonding

higher boiling point

lower boiling point

lower

higher

Phosphine

Ammonia 

Reorder

Arrange the following from predicted lowest vapor pressure to predicted highest vapor pressure:

• NH₃

• H₂S

• CCl₄

1

2

3

• 1
• 2
• 3

Reorder

Arrange the following from lowest vapor pressure to highet

• HF

• HCN

• CO₂

• H₂

1

2

3

4

• 1
• 2
• 3
• 4

Drag and Drop

Ammonia, NH₃ is a ​

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and exhibits all types of IMF's. The strongest IMF exhibited by ammonia is ​

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. One would predict ammonia to have a ​

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vapor pressure, a ​

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boiling point, and a ​

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.

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polar molecule

nonpolar molecule

hydrogen bonding

London dispersion Forces 

dipole dipole

low

high

high surface tension

low surface tension 

Drag and Drop

When looking at the picture to the left, one can see that container A has ​

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and therefore a ​

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. Based on this observation, one can assume that substance A has ​

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than substance B. This is because as the strength of IMF's increase the volatility ​

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. If the two substances were known to be Cl₂ and HCl then one would predict that substance B would be​

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.

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less vapor particles

lower vapor pressure

stronger IMF's

decreases

Cl2

HCl

higher vapor pressure 

increases

weaker IMF's

more vapor particles

Drag and Drop

The molecule to the left is a ​

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because the dipoles ​

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. Therefore, the strongest IMFs exhibited by the molecules are ​

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and the weakest are ​

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. When compared to a molecule of CCl₄ , one would predict the boiling point of NCl to be ​

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that of CCl_4.

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Hydrogen Bonds

Covalent Bond

polar molecule

do not cancel

do cancel

dipole-dipole attractions

London Dispersion Forces

hydrogen bonding

greater than

less than

Dropdown

The molecule to the left ​

Select answer

and water ​

Select answer

. One would expect the substance to the left to have a ​

Select answer

and ​

Select answer

boiling point than that of H₂O because the IMF's of water are ​

Select answer

of the molecule to the left.

Drag and Drop

The molecule carbon dioxide, CO_2, has a linear geometry as does the carbon monoxide, CO, molecule. The bond dipoles in carbon dioxide ​

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whereas the bond dipoles in carbon monoxide ​​

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. Carbon dioxide is a ​

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and carbon monoxide is a​

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. Thus, one would predict ​

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to be most volatile.

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have a high surface tension

have high boiling points

cancel

do not cancel

non polar compound

polar compound

carbon dioxide

carbon monoxide

Multiple Choice

Which compound has the strongest IMF

• HOH

• CH4

• C2H6

• CH3OH

Multiple Choice

Which container has the strongest IMF's?

• red

• yellow

• blue

Multiple Choice

Which of the following molecules would dissolve in oil (oil is non-polar)?

• CHCl₃

• NH₃

• CCl₄

• HBr

Multiple Select

Based on IMF's, which would you predict to be soluble in water? (check all that apply)

• CH₄

• BeCl₂

• CO₂

• NH₃

• HF

Multiple Choice

Which of the following has the lowest boiling point?

• CaCl₂
• PH₃
• Cl₂
• N₂

Multiple Choice

Which substance would you predict to have the highest vapor pressure?

• C₃H₈

• H2O

• CH4

• CH3F