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Chemistry R120 > Chapter 11: Liquids and Intermolecular Forces > Flashcards

Chapter 11: Liquids and Intermolecular Forces Flashcards

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1
Q

What does the state of a substance depend on?

A

the balance between the KE of particles and the attraction energies between particles

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2
Q

Which one is weaker: intermolecular forces or intramolecular forces?

A

intermolecular forces

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3
Q

What are the 4 types of intermolecular forces?

A

dispersion forces | dipole-dipole interactions | ion-dipole | hydrogen bonding

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4
Q

What are van der Waals forces?

A

dispersion forces and dipole-dipole interactions

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5
Q

Who discovered dispersion forces?

A

Fritz London

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6
Q

What are (London) dispersion forces?

A

one atom’s movement of electrons influence that of its neighbor atoms SO = an INSTANTANEOUS dipole on one atom can induce an instantaneous dipole on an adjacent atom

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7
Q

What does the strength of the dispersion force depend on?

A

the polarizability of a molecule

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8
Q

What is the polarizability of a molecule?

A

how charge distribution is manipulated to induce the instantaneous dipole

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9
Q

What does an increase in the polarizability of a molecule indicate?

A

easier the electron cloud could be manipulated to give an instantaneous dipole

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10
Q

What is the relationship between dispersion forces and molecular weight and its affect on boiling point?

A

dispersion forces are stronger as MW increases = increases boiling point

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11
Q

What are dipole-dipole interactions due to?

A

permanent dipole moments in polar molecules

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12
Q

When are dipole-dipole and dispersion interactions effective?

A

when the molecules are very close to each other

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13
Q

What is hydrogen bonding?

A

an attraction between the H (of an -OH, -NH, or -FH) and a nearby electronegative atom in another molecule/compound

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14
Q

What are ion-dipole forces?

A

exists between an ion and a polar molecule (ie: NaCl in H2O)

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15
Q

In what substances are dispersion forces found?

A

ALL substances

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16
Q

Order the 4 intermolecular forces from strongest to weakest.

A

ion-dipole > H-bonding > dipole-dipole > dispersion

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17
Q

What is viscosity?

A

resistance of a liquid to flow | how easily do molecules flow past each other

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18
Q

What does an increase in viscosity indicate?

A

slow flow

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19
Q

What does a decrease in viscosity indicate?

A

fast flow (like water)

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20
Q

What does viscosity depend on?

A

attractive forces between the molecules

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21
Q

What is the SI unit for viscosity?

A

kg/ms

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22
Q

How does a increase in temperature affect viscosity?

A

decrease in viscosity

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23
Q

What is surface tension?

A

molecules at the surface experience a net inward force that pulls them closer to the middle = decrease in surface area

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24
Q

What is surface tension due to?

A

the imbalance of intermolecular forces at the surface of the liquid

25
Q

What is the unit for surface tension?

A

J/m^2

26
Q

What is capillary action?

A

crawl of liquids up a very narrow tube

27
Q

What is cohesive forces?

A

intermolecular forces that bind similar molecules to one another

28
Q

What is adhesive forces?

A

intermolecular forces that bind a substance to a surface

29
Q

What causes the convex meniscus of water? (cohesion adhesion relationship)

A

cohesion forces H2O < adhesion forces H2O

30
Q

What causes the concave meniscus of Hg? (cohesion adhesion relationship)

A

cohesion forces Hg > adhesion forces Hg

31
Q

What are phase changes?

A

state changes of a substance | transformations

32
Q

What is sublimation?

A

solid changes directly to gas

33
Q

What is fusion?

A

melting

34
Q

What is heat of fusion?

A

(∆Hfus) energy that allows increased freedom of motion particles

35
Q

What is vapor pressure?

A

pressure exerted by the vapor of a liquid when the liquid and vapor are in dynamic equilibrium

36
Q

How does an increase in temperature affect vapor pressure of a gas in solution?

A

increases vapor pressure until vapor pressure equals the external pressure above the liquid

37
Q

What is heat of vaporization?

A

(∆Hvap) energy needed for a quantity of liquid to change into vapor (gas)

38
Q

What is heat of sublimation?

A

(∆Hsub) energy needed for solid to directly change into gas

39
Q

What is the relationship between the heat of sublimation, heat of vaporization and heat of fusion?

A

∆Hsub = ∆Hvap + ∆Hfus

40
Q

What is the opposite of sublimation?

A

deposition

41
Q

What is the opposite of vaporization?

A

condensation

42
Q

What is the opposite of fusion?

A

freezing

43
Q

What is critical temperature?

A

highest temperature at which a distinct liquid phase can form and liquid can exist at

44
Q

What is critical pressure?

A

pressure needed to bring about the liquefaction at the critical temperature

45
Q

How does an increase in intermolecular forces strength affect critical temp/pressure?

A

increases critical temp/pressure

46
Q

What is supercritical fluid?

A

when temperature > critical temp and pressure > critical pressure BUT liquid and gas phases are indistinguishable from each other

47
Q

What state is supercritical fluid in?

A

gas/liquid = can expand to fill container but molecules are still close to each other

48
Q

What is dynamic equilibrium?

A

condition where 2 opposing processes occur at the same time at equal rates

49
Q

What is volatile?

A

describes liquids that readily evaporate

50
Q

How does intermolecular forces and vapor pressure affect how volatile a liquid can be?

A

liquid with weak intermolecular forces and high vapor pressure = highly volatile (compare with strong IMForces and low vapor pressure)

51
Q

What is a boiling point?

A

temperature at which its vapor pressure equals the external pressure acting on the liquid’s surface

52
Q

What is a normal boiling point?

A

boiling point of a liquid at 1 atm

53
Q

What are the 3 curves on a phase diagram (temp vs pressure)?

A

vapor pressure curve | sublimation curve | melting curve

54
Q

What does the vapor pressure curve represent?

A

equilibrium between liquid and gas phases

55
Q

What is the critical point?

A

critical temperature and critical pressure

56
Q

What does the sublimation curve represent?

A

change in vapor pressure of the solid as it sublimes at different temperature | curve is the equilibrium between solid and gas phases

57
Q

What does the melting curve represent?

A

change in melting point of a solid as pressure changes | curve is the equilibrium between solid and liquid phases

58
Q

What is the normal melting point?

A

melting point at 1 atm

59
Q

What is the triple point?

A

where all 3 phases are in equilibrium as their curves all intersect at this point

Chemistry R120 (18 decks)

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