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Chemistry I > Chapter 13 > Flashcards

Chapter 13 Flashcards

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1
Q

describes the behavior of gases in terms of particles in motion

A

kinetic-molecular theory

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2
Q

one in which no kinetic energy is lost

A

elastic collision

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3
Q

measure of average kinetic energy of the particles in a sample of matter

A

temperature

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4
Q

describes movement of one material through another

A

diffusion

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5
Q

rate of effusion for a gas Is inversely proportional to the square root of its molar mass

A

Graham’s law of effusion

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6
Q

force per unit area

A

pressure

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7
Q

used to measure atmospheric pressure

A

barometer

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8
Q

equal to a force of one newton per square meter: 1 Pa = 1 N/m squared

A

pascal

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9
Q

total pressure of a mixture of gases is equal to the sum of all the gases in a mixture

A

Dalton’s law of partial pressures

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10
Q

equal to 760 mm Hg or 770 torr or 101.3 kilopascals (KPa)

A

atmosphere

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11
Q

weak forces resulting from temporary shifts in the density of electrons in electron clouds

A

dispersion forces

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12
Q

attractions between oppositely charged regions of polar molecules

A

dipole-dipole forces

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13
Q

a dipole-dipole attraction that occurs between molecules containing a H atm bonded to a small, highly EN atm with at least 1 lone electron pair

A

hydrogen bond

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14
Q

the kinetic molecular theory describes the behavior of gases in terms of particles in

A

motion

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15
Q

in a sample of gas, the volume of the gas particles themselves is very _____ compared to the volume of the sample

A

small

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16
Q

because gas particles are far apart, there are no significant attractive or repulsive ______ between gas particles

A

forces

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17
Q

gas particles are in constant and ______ motion

A

random

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18
Q

the collisions between gas particles are _______; that is, no _______ energy is lost

A

elastic, kinetic

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19
Q

the kinetic energy of a particle is represented by the equation

A

KE = 1/2mv squared

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20
Q

___________ is a measure of the average kinetic energy of the particles in a sample of matter

A

temperature

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21
Q

gases are less dense than solids because there is a lot of space between particles of a gas

A

true

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22
Q

the random motion of gas particles causes a gas to expand until it fills its container

A

true

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23
Q

the density of a gas decreases as it is compressed

A

false

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24
Q

a gas can flow into a space occupied by another gas

A

true

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25
the diffusion of a gas is caused by the random motion of the particles of a gas
true
26
lighter gas particles diffuse less rapidly than do heavier gas particles
false
27
during effusion, a gas escapes through a tiny opening into a vacuum
true
28
Graham's law of effusion states that the rate of effusion for a gas is directly related to the square root of its molar mass
false
29
pressure is defined as force per unit
area
30
what is an instrument designed to measure atmospheric pressure?
barometer
31
the height of the liquid in a barometer is affected by all of the following EXCEPT the
diameter of the column tube
32
the pressure of the gas in a manometer is directly related to which of the following quantities?
a - b
33
one atmosphere is equal to a pressure of
101.3 kPa
34
the partial pressure of a gas depends on all of the following EXCEPT the
identity of the gas
35
the pressure of a sample of air in a manometer is 102.3 kPa. What is the partial pressure of nitrogen (N2) in the sample if the compound partial pressures of the other gases is 22.4 kPa?
79.9 kPa
36
what instrument is illustrated in the figure?
barometer
37
who invented the barometer?
Torrecelli
38
what are the two opposing forces that control the height of the mercury in the column?
gravity and air pressure
39
what does it mean when the level of mercury rises in the column?
air pressure has risen
40
is it possible to measure temperature directly?
no, not directly
41
what is necessary to measure temperature effectively?
an accepted scale, C or F
42
what is pressure?
force per unit area exerted
43
heating a gas increases the ____________ of molecules
kinetic energy
44
how does the pressure of a gas relate to its volume?
pressure in a gas is inversely proportional to the volume
45
state Boyle's law:
pv = constant, constant = 2/3 nk, pv = 2/3 nk
46
define "absolute zero"
lowest possible temperature
47
where does ice melt on the kelvin scale?
273 K
48
what is the temperature at the core of the sun?
15,000,000 K
49
what mechanical property of a gas does temperature depend on?
kinetic energy for the molecules of a gas
50
describe how Fahrenheit came up with his temperature scale?
based on body temperature, made an adjustment to make numbers better, other adjustments. Boiled water, weather temperatures.
51
measure of the resistance of a liquid to flow
viscosity
52
energy required to increase surface area of a liquid by a given amount
surface tension
53
compounds that lower surface tension of water
surfactants
54
a solid whose atoms, ions, or molecules are arranged in an orderly, geometric three-dimensional structure
crystalline solid
55
smallest arrangement of connected points that can be repeated in three directions to form the lattice
unit cell
56
particles are not arranged in a regular, repeating pattern
amorphous solid
57
ionic, metallic, and covalent bonds are examples of what type of forces?
intramolecular forces
58
dispersion forces, dipole-dipole forces, and hydrogen bonds are examples of what type of forces?
intermolecular forces
59
describe dispersion forces
weak forces resulting from temporary shifts in the density of electrons in electron clouds
60
dispersion forces are greatest between what type of molecules?
identical nonpolar molecules
61
describe a permanent dipole
contains regions that always have a slightly negative charge and regions that have a slightly positive charge
62
describe dipole-dipole forces
attractions between oppositely charged regions of polar molecules
63
describe a hydrogen bond
a dipole-dipole attraction occurring between molecules, each containing a hydrogen atom bonded to a small, highly electronegative atom with at least one lone electron pair
64
triangle like
hydrogen bonds
65
straight like
dispersion forces
66
angled line
dipole-dipole forces
67
rank dipole-dipole forces dispersion forces, and hydrogen bonds in order of increasing strength
dispersion forces, dipole-dipole forces, hydrogen bonds
68
of a crystalline solid is the temperature at which the forces holding its crystal lattice together are broken and it becomes a liquid
melting point
69
process by which a liquid changes to a gas or vapor
vaporization
70
when vaporization occurs only at the surface of a liquid
evaporation
71
pressure exerted by a vapor over a liquid
vapor pressure
72
temperature at which the vapor pressure of a liquid equals the external or atmospheric pressure
boiling point
73
process by which a solid changes directly to a gas without first becoming a liquid
sublimation
74
because liquids are more dense than vapors, process by which a gas or a vapor becomes a liquid
condensation
75
process by which a substance changes from a gas or vapor to a solid without first becoming a liquid
doposition
76
temperature at which a liquid is converted into a crystalline solid
freezing point
77
a graph of pressure versus temperature that shows in which phase a substance exists under different conditions of temperature and pressure
phase diagram
78
point on a phase diagram that represent the temperature and pressure at which three phases of a substance can coexist
triple point
79
the constant MOTION of the particles in a liquid causes the liquid to take the shape of its container
true
80
at room temperature and one atmosphere of pressure, the density of a liquid is much GREATER than that of its vapor
true
81
liquids are not easily compressed because their particles are LOOSELY packed
false; tightly
82
a liquid is less fluid than a gas because INTRAMOLECULAR attractions interfere with the ability of particles to flow past one another
false; intermolecular
83
liquids that have stronger intermolecular forces have HIGHER viscosities than do liquids with weaker intermolecular forces
true
84
the viscosity of a liquid INCREASES with temperature because the increased average kinetic energy of the particles makes it easier for the liquids to flow
false; decreases
85
liquids that can form hydrogen bonds generally have a HIGH surface tension
true
86
a liquid that rises in a narrow glass tube shows that the adhesive forces between the particles of the liquid and glass are GREATER than the cohesive forces between the particles of the liquid
true
87
solids have a definite shape and volume because the motion of their particles is limited to VIBRATIONS around fixed locations
true
88
most solids are LESS dense than liquids because the particles in a solid are more closely packed than those in a liquid
false; more
89
rubber is a CRYSTALLINE solid because its particles are not arranged in a regular, repeating pattern
false; amorphous
90
temperature at which a liquid is converted into a crystalline solid
freezing point
91
temperature at which the forces holding a crystalline lattice together are broken
melting point
92
temperature at which the vapor pressure of a liquid equals the external or atmospheric pressure
boiling point
93
what variables are plotted on a phase diagram?
temperature and pressure

Chemistry I (8 decks)

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