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CHEM 1000 > Intermolecular Forces > Flashcards

Intermolecular Forces Flashcards

1
Q

What is the difference between inter and intramolecular force?

A

Inter is between molecules and intra is within molecules

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2
Q

Where do intermolecular forces originate?

A

Interactions between charges, partial charges, and temporary charges

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3
Q

What is stronger intermolecular forces or bonding forces?

A

Bonding forces

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4
Q

What is an ion-induced dipole force?

A

When an ion approaches a non polar molecule it creates a small induced dipole

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5
Q

What does the magnitude of ion-induced dipole depend on?

A

Charge of ion and the polarizability of the atom (how easy electrons move), polarizabilty also depends on size of electron cloud

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6
Q

What intermolecular force is present in all neutral atoms?

A

Dispersion force (LDF)

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7
Q

What is a dispersion force?

A

Electrons are not always uniformly distributed, sometimes creates small positive and negative end

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8
Q

What does an instantaneous dipole on atom atom do?

A

Induces dipoles on neighboring atoms which attract each other

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9
Q

What types of molecules have stronger dispersion forces?

A

Molecules with a lot of electrons and ones that are elongated (more space for interaction)

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10
Q

What force exists in all polar molecules?

A

Dipole-dipole

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11
Q

What are dipole dipole forces?

A

Permanent dipole caused by difference in EN

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12
Q

What is the effect on the boiling point as the dipole moment increase?

A

Boiling point increases

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13
Q

Will a polar liquid mix with another polar liquid? What about non polar!

A

Yes

No

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14
Q

What are hydrogen bonds?

A

Hydrogens bound directly to a highly electronegative atom can form weak bonds with the atom in a adjacent molecule

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15
Q

What atoms does hydrogen bonding occur with?

A

Hydrogen and fluorine, oxygen, and nitrogen

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16
Q

What is dipole induced dipole force?

A

The force between molecules with a permanent dipole and a non polar one

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17
Q

What is ion dipole force?

A

Occur when an ionic compound is mixed with a polar compound, important for aqueous solutions of ionic compounds

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18
Q

What is the strongest intermolecular force?

A

Ion dipole force

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19
Q

Where is dipole induced dipole forces present?

A

Non polar molecules mixed with polar ones

20
Q

Where is ion induced dipole force found?

A

Dilute mixture of ionic compound and non polar substance

21
Q

How do you solve a problem when you are given the mass of a liquid and a solid block and the initial temperature, when the energy released during condensation only warms the block and you need to find final temperature?

A

Find the heat of liquid in joules using mass, molar mass, and energy of vaporization

Then make the heat of block equal to negative heat of liquid

Solve for final temperature

22
Q

Why do liquids tend to minimize surface area?

A

Molecules at surface are less stable and it takes energy to move a molecule from interior to surface

23
Q

What is surface tension?

A

Energy required to increase the surface area

24
Q

What happens to surface tension as intermolecular forces decrease?

A

It decreases

25
Q

What is viscosity? What is the SI unit?

A

Resistance of a liquid to flow

Pa s

26
Q

What are viscosity trends?

A

Increases with increasing intermolecular forces, increased with a longer molecule shape, decreases with temperature

27
Q

What is capillary action? What is it the result of?

A

Ability of a liquid to flow against gravity up a narrow tube

Cohesive and adhesive forces

28
Q

How does temperature affect vaporization?

A

At a lower temperature less molecules have the minimum KE to escape into gas phase

At a higher temperature more molecules have a high enough energy to evaporate

29
Q

What happens in a closed container in terms of condensation and evaporation?

A

Reaches equilibrium

30
Q

What does the rate of vaporization increase with?

A

Temperature, surface area, and decreasing inter molecular forces

31
Q

What is the enthalpy of vaporization? Is it endo or exothermic?

A

Amount of heat required to vaporize one mole of a liquid to gas

Endothermic (always positive)

32
Q

What is the enthalpy of condensation equal to?

A

Negative enthalpy of vapourization

33
Q

How can you find the mass of something that can be vaporized at its boiling point when given heat?

A

Rearrange enthalpy=q/mol and then convert to grams

34
Q

What is dynamic equilibrium? What happens when system is disturbed?

A

Rate of vaporization equals rate of condensation

Systems try’s to minimize the disturbance and return to equilibrium

35
Q

What is the normal boiling point? What is the standard boiling point?

A

The temperature when the vapor pressure is equal to one atmosphere

The temperature where the vapor pressure equals one bar

36
Q

If you are given the heat of vaporization and the temperature of the normal boiling point and are asked to find the vapor pressure at a given temperature what can you use?

A

In(P2/P1)=-deltaHvap/R (1/T2-1/T2)

37
Q

How can you get rid of a natural log?

A

Raise to e^In

38
Q

What is the critical point?

A

When the distinction between liquid and vapor disappears

39
Q

What is the enthalpy of sublimation?

A

Enthalpy of fusion + enthalpy of vaporization

40
Q

What is sublimation vs deposition?

A

Solid to gas

Gas to solid

41
Q

What is fusion? What is the enthalpy of fusion equal to? What is the opposite?

A

Solid to liquid(Melting), heat of fusion, liquid to solid (freezing)

42
Q

Is enthalpy of fusion positive or negative? What about enthalpy of freezing?

A

Positive, opposite sign of fusion but same magnitude

43
Q

How can you calculate a heating curve for water?

A
  1. Heating solid ice (use q=mcdeltaT)
  2. Going from solid to liquid (use q=n x enthalpy of fusion)
  3. Heating liquid water (use q=mcdeltaT)
  4. Going from liquid gas (use q=n x enthalpy of vaporization)
  5. Heating steam (use q=mcdeltaT)
44
Q

What are molecular solids?

A

Crystalline solids composed of molecules, held together by intermolecular forces (dispersion, dipole dipole, hydrogen), low melting points

45
Q

What are ionic solids?

A

Solids made up of ions, held together by interactions between cations and anions

46
Q

What are atomic solids?

A

Made up of individual atoms

Non bonding, held together by weak dispersion forces, noble gases in solid form

Metallic, held together by metallic bonds and de localized molecular orbitals

Network covalent, held together by covalent bonds, sort of like giant molecules

CHEM 1000 (8 decks)

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