Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

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

Chapter 11 Liquids, Solids & Intermolecular Forces Flashcards

1
Q

What are the 3 phases?

A

Solid, liquid & gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

T/F High degree of freedom = more unstable

A

True

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

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

A

False ; more stable

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What type of molecules are not easily compressible?

A

Molecules closely spaced

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What type of molecules are highly compressible?

A

Molecules widely spaced

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Define Thermal Expansion

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

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

A

Weak

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

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

A

Moderate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

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

A

Strong

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is the process from solid to liquid phase?

A

Melting

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is the process from liquid to gas phase?

A

Vaporization

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is the process from gas to liquid phase?

A

Condensation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is the process from liquid to solid phase?

A

Freezing

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Define Intermolecular Forces?

A

Forces that hold condensed states together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

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

A

Structure ; strength

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is the equation for Coulomb’s Law?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What does Coulomb’s Law state?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

List the following Intermolecular Forces in order from weakest to strongest

A

London Dispersion
Dipole - Dipole
Hydrogen Bonding
Ion - Dipole

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Which Intermolecular Force exists among all particles and molecules

A

London Dispersion Force

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Define London Dispersion Force

A

When there are fluctuations in electron distributions within molecules or atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Define Polarizability

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Strong force = ________ polarized, ________ mass and __________ boiling point
Easily ; larger ; larger
26
Weak force = ________ polarized, ________ mass and _________ boiling point
Not easily ; smaller ; smaller
27
If a particle has the same mass what factor can be used to determine a difference in force?
Shape
28
Which halogen has the highest boiling point? F2, Cl2, Br2, I2
I2 ; because it has the largest mass
29
Define Dipole - Dipole Force
Force that is present between polar molecules
30
More polar = ________ dipole, _________ melting/boiling point
Stronger ; higher
31
Less polar = ________ dipole, __________ melting/boiling point
Weaker ; lower
32
Define Miscibility
The ability to mix without separating into 2 states
33
The _________ of a molecule affects the Miscibility
Polarity
34
Which has the higher melting/boiling point? A) CH2O B) C2H6
CH2O ; because it is more polar, which automatically means that it has a higher melting/boiling point
35
Which molecules have Dipole - Dipole Forces? A) CO2 B) CH2Cl2 C) CH4
A and B
36
Define Hydrogen Bonding
Intermolecular forces that occur when polar molecules with H atoms are bonded directly to small/highly electronegative F, O and N atoms
37
T/F Hydrogen Bonding pairs include H-O, H-N and H-F
True
38
Define Ion Dipole Force
When ions from an ionic compound is mixed with a polar compound
39
Which Intermolecular Force is the strongest?
Ion Dipole Force
40
Determine what Intermolecular Force PH3 has
Dispersion, Dipole - Dipole
41
Determine what Intermolecular Force HBr has
Dispersion, Dipole - Dipole
42
Determine what Intermolecular Force CH3OH has
Dispersion, Dipole - Dipole, Hydrogen Bonding
43
Determine what Intermolecular Force He2 has
Dispersion
44
``` Arrange the following in order of increasing boiling point A) CH4 B) CH3CH3 C) CH3CH2Cl D) CH3CH2OH ```
A --> B --> C --> D
45
What are the Intermolecular Forces in action in liquids?
Tension, Viscosity and Capillary Action
46
Define Surface Tension
When a molecule on the interior can experience more Intermolecular Forces than a molecule on the surface
47
T/F Interior molecules are less stable
False; more stable
48
Surface tension _________ when Intermolecular Force __________
Decreases ; decreases
49
Define Viscosity
The resistance of a liquid to flow
50
Intermolecular Force _________ when viscosity ___________
Increases ; increases
51
Do longer molecules have higher or lower viscosity?
Higher
52
Higher temperature results in __________ viscosity
Lower
53
Why do longer molecules have higher viscosity?
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
What is a good example of viscosity?
Honey (syrup)
55
Define Capillary Action
The ability of a liquid to flow against gravity up a narrow tube
56
What 2 actions work together to create capillary action?
Cohesive and adhesive forces
57
What does cohesive forces hold together?
Liquid molecules
58
What does adhesive forces hold together?
Outer liquid molecules to the tube's surface
59
What is the liquid to gas phase called? What kind of process is occurring during this phase?
Vaporization ; endothermic (heat absorbed)
60
Define Heat of Vaporization
Amount of heat (enthalpy) required to vaporize 1 mole liquid to gas
61
T/F Heat of Vaporization will always be a positive value
True
62
What is the gas to liquid phase called? What kind of process is occurring during this phase?
Condensation ; exothermic (heat released)
63
Define Dynamic Equilibrium
When 2 opposite processes reach the same rate so there is no gain or loss of material
64
Weaker Intermolecular Forces results in _________ vapor pressure
Higher
65
Higher temperature results in __________ vapor pressure
Higher
66
T/F The stronger the Intermolecular Force the lower the boiling point
False ; higher
67
Pick the higher vapor pressure compound from each pair A) Br2 or I2 B) CH4 or CH3Cl C) NH3 or PH3
A) Br2 B) CH4 C) PH3
68
Place the following substances in order of increasing vapor pressure A) NF3 B) NH3 C) BCl3
NH3 --> NF3 --> BCl3
69
``` Arrange the following compounds in order of increasing boiling points A) CH4 B) CH3CH3 C) CH3CH2Cl D) CH3CH2OH ```
A) Dispersion B) Dispersion w/ larger mass C) Dispersion, Dipole -Dipole D) Dispersion, Dipole - Dipole, Hydrogen Bonding
70
What does the Clausius - Clapeyron equation state?
States that vapor pressure of a liquid increases with increasing temperature
71
Define Sublimation
The amount of heat required to sublime 1 mole of a solid to gas
72
Define Fusion
Phase transition from solid to liquid
73
Define Freezing
Phase transition from liquid to solid
74
T/F Heat of Fusion values are always negative
False ; positive
75
Define Phase Diagram
A map of the states of a substance as a function of pressure (y-axis) and temperature (x-axis)
76
What are the 3 main regions of Phase Diagrams?
Solid, liquid and gas
77
What do the regions of a Phase Diagram represent?
Represent the conditions where that particular state is stable
78
What do lines in Phase Diagrams represent?
Represent the substance when it is in equilibrium between the 2 states on either side of the line
79
T/F If a point lands on the line than it is coexisting between 2 states
True
80
What does Triple Point represent?
When the 3 states are equally states (coexist) and are in equilibrium
81
Define Supercritical Fluid
When the temperature and pressure in a Phase Diagram is ABOVE its critical point
82
T/F Liquid and gas states still exist in the supercritical fluid point
False ; do not exist
83
What is the equation for Clausius Clapeyron?
ln P2/P1 = -DeltaHvap / R (1/T2 - 1/T1)

Chemistry 2 (10 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions