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Chemistry 2 > Chapter 11 Liquids, Solids & Intermolecular Forces > Flashcards

Chapter 11 Liquids, Solids & Intermolecular Forces Flashcards

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1
Q

What are the 3 phases?

A

Solid, liquid & gas

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2
Q 
Which of the following is not true about the solid phase?
A) High density
B) Limited to freedom of motion 
C) Weak intermolecular forces 
D) Short distance between molecules
A

C ; strong intermolecular forces

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3
Q

Which of the following is not true about the liquid phase?
A) Low density
B) Some freedom of motion
C) Moderate intermolecular forces
D) Somewhat short distance between molecules

A

A ; high density

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4
Q 
Which of the following is not true about the gas phase?
A) Low density 
B) Large freedom of motion 
C) Strong intermolecular forces 
D) Long distance between molecules
A

C ; weak intermolecular forces

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5
Q

T/F High degree of freedom = more unstable

A

True

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6
Q

T/F Low degree of freedom = neither stable/unstable

A

False ; more stable

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7
Q

What type of molecules are not easily compressible?

A

Molecules closely spaced

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8
Q

What type of molecules are highly compressible?

A

Molecules widely spaced

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9
Q

Define Thermal Expansion

A

The tendency of matter to change shape, area and volume in response to change in temperature

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10
Q

Does the solid phase have weak/moderate/strong Thermal Expansion?

A

Weak

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11
Q

Does the liquid phase have weak/moderate/strong Thermal Expansion

A

Moderate

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12
Q

Does the gas phase have weak/moderate/strong Thermal Expansion?

A

Strong

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13
Q

What is the process from solid to liquid phase?

A

Melting

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14
Q

What is the process from liquid to gas phase?

A

Vaporization

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15
Q

What is the process from gas to liquid phase?

A

Condensation

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16
Q

What is the process from liquid to solid phase?

A

Freezing

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17
Q

Define Intermolecular Forces?

A

Forces that hold condensed states together

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18
Q

The __________ of particles determines the __________ of Intermolecular Forces that hold the substance together

A

Structure ; strength

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19
Q

What is the equation for Coulomb’s Law?

A

E = 1 / 4(pi)E0 (q1q2 / r)

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20
Q

What does Coulomb’s Law state?

A

States that Intermolecular Forces are due to attractive forces between opposite charges

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21
Q

List the following Intermolecular Forces in order from weakest to strongest

A

London Dispersion
Dipole - Dipole
Hydrogen Bonding
Ion - Dipole

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22
Q

Which Intermolecular Force exists among all particles and molecules

A

London Dispersion Force

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23
Q

Define London Dispersion Force

A

When there are fluctuations in electron distributions within molecules or atoms

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24
Q

Define Polarizability

A

The ease with which the electron distribution around an atom or molecule can be distorted

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25
Q

Strong force = ________ polarized, ________ mass and __________ boiling point

A

Easily ; larger ; larger

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26
Q

Weak force = ________ polarized, ________ mass and _________ boiling point

A

Not easily ; smaller ; smaller

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27
Q

If a particle has the same mass what factor can be used to determine a difference in force?

A

Shape

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28
Q

Which halogen has the highest boiling point? F2, Cl2, Br2, I2

A

I2 ; because it has the largest mass

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29
Q

Define Dipole - Dipole Force

A

Force that is present between polar molecules

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30
Q

More polar = ________ dipole, _________ melting/boiling point

A

Stronger ; higher

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31
Q

Less polar = ________ dipole, __________ melting/boiling point

A

Weaker ; lower

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32
Q

Define Miscibility

A

The ability to mix without separating into 2 states

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33
Q

The _________ of a molecule affects the Miscibility

A

Polarity

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34
Q

Which has the higher melting/boiling point?
A) CH2O
B) C2H6

A

CH2O ; because it is more polar, which automatically means that it has a higher melting/boiling point

35
Q

Which molecules have Dipole - Dipole Forces?
A) CO2
B) CH2Cl2
C) CH4

A

A and B

36
Q

Define Hydrogen Bonding

A

Intermolecular forces that occur when polar molecules with H atoms are bonded directly to small/highly electronegative F, O and N atoms

37
Q

T/F Hydrogen Bonding pairs include H-O, H-N and H-F

A

True

38
Q

Define Ion Dipole Force

A

When ions from an ionic compound is mixed with a polar compound

39
Q

Which Intermolecular Force is the strongest?

A

Ion Dipole Force

40
Q

Determine what Intermolecular Force PH3 has

A

Dispersion, Dipole - Dipole

41
Q

Determine what Intermolecular Force HBr has

A

Dispersion, Dipole - Dipole

42
Q

Determine what Intermolecular Force CH3OH has

A

Dispersion, Dipole - Dipole, Hydrogen Bonding

43
Q

Determine what Intermolecular Force He2 has

A

Dispersion

44
Q 
Arrange the following in order of increasing boiling point
A) CH4 
B) CH3CH3 
C) CH3CH2Cl
D) CH3CH2OH
A

A –> B –> C –> D

45
Q

What are the Intermolecular Forces in action in liquids?

A

Tension, Viscosity and Capillary Action

46
Q

Define Surface Tension

A

When a molecule on the interior can experience more Intermolecular Forces than a molecule on the surface

47
Q

T/F Interior molecules are less stable

A

False; more stable

48
Q

Surface tension _________ when Intermolecular Force __________

A

Decreases ; decreases

49
Q

Define Viscosity

A

The resistance of a liquid to flow

50
Q

Intermolecular Force _________ when viscosity ___________

A

Increases ; increases

51
Q

Do longer molecules have higher or lower viscosity?

A

Higher

52
Q

Higher temperature results in __________ viscosity

A

Lower

53
Q

Why do longer molecules have higher viscosity?

A

Because think of a long rope, because it is so long it is likely to get tangled and jumbled, making it more difficult to move through

54
Q

What is a good example of viscosity?

A

Honey (syrup)

55
Q

Define Capillary Action

A

The ability of a liquid to flow against gravity up a narrow tube

56
Q

What 2 actions work together to create capillary action?

A

Cohesive and adhesive forces

57
Q

What does cohesive forces hold together?

A

Liquid molecules

58
Q

What does adhesive forces hold together?

A

Outer liquid molecules to the tube’s surface

59
Q

What is the liquid to gas phase called? What kind of process is occurring during this phase?

A

Vaporization ; endothermic (heat absorbed)

60
Q

Define Heat of Vaporization

A

Amount of heat (enthalpy) required to vaporize 1 mole liquid to gas

61
Q

T/F Heat of Vaporization will always be a positive value

A

True

62
Q

What is the gas to liquid phase called? What kind of process is occurring during this phase?

A

Condensation ; exothermic (heat released)

63
Q

Define Dynamic Equilibrium

A

When 2 opposite processes reach the same rate so there is no gain or loss of material

64
Q

Weaker Intermolecular Forces results in _________ vapor pressure

A

Higher

65
Q

Higher temperature results in __________ vapor pressure

A

Higher

66
Q

T/F The stronger the Intermolecular Force the lower the boiling point

A

False ; higher

67
Q

Pick the higher vapor pressure compound from each pair
A) Br2 or I2
B) CH4 or CH3Cl
C) NH3 or PH3

A

A) Br2
B) CH4
C) PH3

68
Q

Place the following substances in order of increasing vapor pressure
A) NF3
B) NH3
C) BCl3

A

NH3 –> NF3 –> BCl3

69
Q 
Arrange the following compounds in order of increasing boiling points 
A) CH4 
B) CH3CH3
C) CH3CH2Cl
D) CH3CH2OH
A

A) Dispersion
B) Dispersion w/ larger mass
C) Dispersion, Dipole -Dipole
D) Dispersion, Dipole - Dipole, Hydrogen Bonding

70
Q

What does the Clausius - Clapeyron equation state?

A

States that vapor pressure of a liquid increases with increasing temperature

71
Q

Define Sublimation

A

The amount of heat required to sublime 1 mole of a solid to gas

72
Q

Define Fusion

A

Phase transition from solid to liquid

73
Q

Define Freezing

A

Phase transition from liquid to solid

74
Q

T/F Heat of Fusion values are always negative

A

False ; positive

75
Q

Define Phase Diagram

A

A map of the states of a substance as a function of pressure (y-axis) and temperature (x-axis)

76
Q

What are the 3 main regions of Phase Diagrams?

A

Solid, liquid and gas

77
Q

What do the regions of a Phase Diagram represent?

A

Represent the conditions where that particular state is stable

78
Q

What do lines in Phase Diagrams represent?

A

Represent the substance when it is in equilibrium between the 2 states on either side of the line

79
Q

T/F If a point lands on the line than it is coexisting between 2 states

A

True

80
Q

What does Triple Point represent?

A

When the 3 states are equally states (coexist) and are in equilibrium

81
Q

Define Supercritical Fluid

A

When the temperature and pressure in a Phase Diagram is ABOVE its critical point

82
Q

T/F Liquid and gas states still exist in the supercritical fluid point

A

False ; do not exist

83
Q

What is the equation for Clausius Clapeyron?

A

ln P2/P1 = -DeltaHvap / R (1/T2 - 1/T1)

Chemistry 2 (10 decks)

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