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Chemistry 1045 > Final Exam- 9,10,11,16 > Flashcards

Final Exam- 9,10,11,16 Flashcards

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1
Q

Solids with highly ordered structures are said to be ___________

A

Crystalline

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2
Q

Physical properties of liquids and solids are due to _____________ _______.
These are ______ between _______

A

Intermolecular forces
forces
molecules

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3
Q

_______ _______ reflect intermolecular force strength.
_______ _______ also reflect intermolecular fore strength.
A high ___ ___ or ___ ___ indicates strong attractive forces.

A

Boiling Point

Melting Point

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4
Q

Collectively _________ forces are intermolecular forces that exist between natural molecules

A

van-der-waals

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5
Q

Van der waals forces include
______
______
______

A

Dispersion forces
dipole-dipole forces
hydrogen forces

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6
Q

For an instant, the electron cloud become distorted. In that instant a dipole i formed.
it is called an ___________ or momentary _____.

A

Instantaneous or momentary dipole

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7
Q

One instantaneous dipole can induce another instantaneous dipole in an adjacent molecule (or atom). These two ________ ____ attract each other.

A

Temporary dipoles

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8
Q

___________ is the ease with which an electron distribution can be deformed

A

Polarizability

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9
Q

Dispersion force ______ as molecular weight ______.

A

Increases

Increases

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10
Q

The _____ _____ ____ reflects the dipole-dipole forces present.

A

Higher boiling point

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11
Q

Polar molecules _______ ____ ____

A

Attract each other

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12
Q

The partially _____ end of one molecule attracts the partially _____ end of another.

A

Positive

Negative

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13
Q

Polar molecular need to be ____ ______ to form strong ____- ___ interactions

A

close together

dipole-dipole

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14
Q

If two molecules have similar mass and size, then dipole- dipole forces ______ with ______ _______.

A

Increase with increasing polarity.

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15
Q

_______ _______ is a special type of ________ _______. This is a special case of dipole-dipole interactions.

A

Hydrogen bonding

intermolecular attraction

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16
Q

H bonding require:
H Bonded to a small _______ ______.
Most important for compounds of _, _, and _.

A

electronegative element

F, O, & N

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17
Q

Bond energies of Hydrogen bonds vary from about 4kj/mol to 25kj/mol. They are much _____ than ______ ______ _____.

A

weaker than ordinary chemical bonds

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18
Q

An interesting consequence of H-bonding is that for such a low molar mass molecule (Mm = 18g/mol) water has an unusually:
a)____ ____ _____
b)____ ____ of __________
c)water is a liquid under most circumstances
makes life possible.
d)water is a _____ _____
e) The solid has a ____ density than the liquid, causing the ice to ____.

A

a) High surface tension
b) High heat of vaporization (makes possible evaporative cooling)
d) Is a Superior Solvent
e) Lower density, causing Ice to float.

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19
Q

The molecules in solids are usually more closely packed than those in liquids.
Therefore, solids are usually denser than liquids.
But a few molecules have their solids less dense than their liquids, like

A

Ice to water.

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20
Q

An ___-___ force is an interaction between an ion (e.g., Na+) and the partial change on the end of a polar molecule/dipole (e.g. water)

A

Ion-dipoles

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21
Q

H-bonding is the _____ of the intermolecular forces while Dispersion Force is the _______.

A

Strongest

weakest

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22
Q

Ion-Dipole interaction are _____ than H-bonds

A

Stronger

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23
Q

Intermolecular attractive force will generally be ______ in the substance with the ______ ______ _____.

A

greater

higher molecular weight

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24
Q

_______ is the resistance of a liquid to flow.

A

Viscosity

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25
Q

Viscosity depends on…

A

the attractive forces between molecules

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26
Q

________ ______.
Bulk molecules (those in the liquid) are equally attracted to all of their neighbors.
Surface molecules are only attracted inward towards the bulk of the molecules.

A

Surface Tension

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27
Q

______ ____ is the rise of liquids up very narrow tubes. The liquid climbs until adhesive and cohesive forces are balanced by gravity.

A

Capillary Action

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28
Q

______ _____ are intermolecular fores that bind molecules to one another.

A

Cohesive Force

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29
Q

____ _____ are intermolecular forces that bind molecules to a surface.

A

Adhesive Force

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30
Q

An example of Capillary action is the _____ in a tube filled with water.

A

Meniscus

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31
Q

Matter in one state is converted into another state

A

Phase change or change of state

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32
Q

Sublimation

A

Solid –> Gas

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33
Q

Melting or Fusion

A

Solid –>Liquid

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34
Q

Vaporization

A

Liquid –> Gas

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35
Q

Deposition

A

Gas –> Solid

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36
Q

Condensation

A

Gas –> Liquid

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37
Q

Freezing

A

Liquid –> Solid

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38
Q

Is any substance at a temperature and pressure above its critical point, where distinct liquid and gas phases do not exist.

A

Supercritical Fluid

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39
Q

when a liquid is cooled below its freezing point and its still remains a Liquid

A

Supercooling

ex: Glass

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40
Q

https://upload.wikimedia.org/wikipedia/commons/thumb/3/34/Phase-diag2.svg/300px-Phase-diag2.svg.png

A

https://upload.wikimedia.org/wikipedia/commons/thumb/3/34/Phase-diag2.svg/300px-Phase-diag2.svg.png

41
Q

Plot of temperature change versus heat added is a _____ ____

A

Heating Curve

42
Q

_______ _______ is the highest temperature at which a substance can exist as a liquid

A

Critical Temperature

43
Q

_______ _______ is the pressure required for liquefaction at this critical temperature.

A

Critical Pressure

44
Q

Supercritical fluid extraction is used to ______ ______ ______

A

Separate Complex Mixtures

45
Q

Some of the molecules on the surface of a liquid have enough energy to….

A

escape the attraction of a bulk liquid.

46
Q

_______ _____ of a liquid is the pressure exerted by its vapor when the liquid and vapor are in dynamic equilibrium.

A

Vapor Pressure

47
Q

Liquids that evaporate easily are said to be ______.

A

Volatile

48
Q

The _____ _____ of a liquid is the temperature at which the external pressure at the liquid surface equals the vapor pressure

A

Boiling Point

49
Q

A ______ ______ is a plot of pressure vs temperature summarizing all equilibria between phases

A

Phase Diagram

50
Q

Vapor-pressure curve

A

As temperature increases, vapor pressure increases.

51
Q

Critical Point

A

critical temperature and pressure for the gas

52
Q

Sublimation curve

A

Separates the solid and gas phases

53
Q

Melting Curve

A

Separates the Solid and Liquid phases

54
Q

Normal melting Point

A

1 atm

55
Q

Triple Point

A

temperature and pressure at which all three phases are in equilibrium

56
Q

Any temperature and pressure combination not on a curve represents a ______ _____

A

Single Phase

57
Q

_______ _____Held together by delocalied “sea” of shared valence electrons

A

Metallic solids

58
Q

______ _____Held together by mutual attraction between cations and anions.
Tend to be _____
_____ melting & boiling points

A

Ionic Solids
Brittle
High

59
Q

______ _____Held together by relatively weak intermolecular forces
Tend to be ____
_____ melting & boiling points

A

Molecular Solids
Soft
Low

60
Q

______ _____Have atoms and ions arranged in an orderly repeating pattern.

A

Crystalline Solids

ex: NaCl, quartz, Diamonds

61
Q

_____ _____Lack the order of crystalline solids

A

Amorphous Solids

ex: Rubber, Glass

62
Q

A ________ is a homogeneous mixture of solute and solvent.

A

Solution

63
Q

Each substance present is a ________ of the solution

A

Component

64
Q

The ______ is the component present in the largest amount

A

Solvent

65
Q

The mixing of gases is a ___________ process

A

Spontaneous

66
Q

________ is the thermodynamic quantity that measures the extent of the spreading of the molecules and their associated kinetic energies.

A

Entropy

67
Q

_____ _____ of intermolecular interactions are involved in solution formation

A

Three kinds

68
Q

______ _____ interactions between solute particles

Must be overcome in order to disperse the particles through the solvent.

A

Solute-solute

69
Q

______ _____ interactions between solvent particles

Must be overcome to make room for the solute particle in the solvent

A

Solvent-solvent

70
Q

______ _____ interactions between solvent and solute particles. Occur as particles mix

A

Solvent-solute

71
Q

The opposite process of a solution is _________

A

Crystallization

72
Q

If crystallization and dissolution are in equilibrium with undissolved solute, the solution is ______.

A

Saturated

73
Q

_______ is the amount of the solute required to form a saturated solution.

A

Solubility

74
Q

A solution is said to be _____________ if more solute is dissolve than in a saturated solution.

A

Supersaturated

75
Q 
The tendency of a substance to dissolve in another depends on:
\_\_\_\_\_\_\_\_
\_\_\_\_\_\_\_\_
\_\_\_\_\_\_\_\_
\_\_\_\_\_\_\_\_
A

The nature of the Solute
& Solvent
The temperature
The Pressure (for gases)

76
Q

Pairs of liquids that mix in any proportions are said to be ______

A

Miscible

77
Q

In contrast, ________ liquids do not mix significantly

A

Immiscible

ex: Gas & water

78
Q

____________: like dissolve like

A

Generalization

79
Q

The solubility of most solids solutes in water ________ as the solution temperature increase

A

increases

80
Q

The solubility of gas in water with increasing temperature

A

decreases

81
Q

________ _______If lakes get to warm, CO2 and O2 become less soluble and are not available for plants or animals.

A

Thermal pollution

82
Q

The terms _____ and _________ are qualitative ways to concentration.

A

Dilute

Concentrated

83
Q

A _____ solution has relatively small concentration of solute

A

Dilute

84
Q

A _________ solution has a relatively high concentration of solute

A

Concentrated

85
Q 
The most commonly used expressions for concentration are:
\_\_\_\_\_\_\_\_\_
\_\_\_\_\_\_\_\_
\_\_\_\_\_\_\_\_
\_\_\_\_\_\_\_\_
A

Mass percentage (mass%)
Mole fraction (X)
Molarity (M)
Molality (m)

86
Q

Acids taste ____ and cause certain dyes to change color

A

Sour

87
Q

Bases taste _____ and feel soapy.

A

Bitter

88
Q

In water, cluster of hydrated H+(aq) ions form.

the simplest cluster is ____, we call this a ___________ ___

A

H3O+

Hydronium Ion

89
Q

In bronsted-Lowry, Acids ______ H+

& Bases _____ H+

A

Donates

Accepts

90
Q

An _________ substance can behave either as an acid or as a base

A

Amphiprotic

91
Q

whatever is left of the acid after the proton is donated is called its __________ base

A

Conjugate

92
Q

X- is called the _________ base

A

Conjugate

93
Q

Do strong or weak acids completely transfer their protons to water

A

Strong

94
Q

Do strong or weak acids only partially dissociate in aqueous solution

A

weak

95
Q

Substances with __________ acidity do not transfer a proton to water

A

Negligible

96
Q

In pure water the following equilibrium is established, this process is called

A

Autoionization

97
Q

__ is called the ion-product constant

A

Kw

98
Q

Most ph levels fall between “#” & “#”

A

0 - 14

Chemistry 1045 (2 decks)

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