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chem Flashcards

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1
Q

it states that matter is made up of particles that are constantly moving

A

kinetic molecular theory of solids and liquids

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2
Q

the arrangement of particles in solids, liquids, and gases explains the _

A

different properties

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3
Q

held by very strong forces of attraction, particle not free to move, particle vibrate about in fixed positions

A

solid (movement)

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4
Q

held together by strong forces of attraction, particles are able to slide past one another

A

liquid (movement)

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5
Q

very high density

A

solid

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6
Q

high density

A

liquid

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7
Q

extremely slowly infusibility

A

solid

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8
Q

slow infusibility

A

liquid

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9
Q

slighty compressible (solid and liquid)

A

compressibility

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10
Q

has fixed volume and shape

A

solid

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11
Q

assumes the shape of the container it occupies. has fixed volume

A

liquid

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12
Q

matter in the gas state

A

has indefinite shape and volume

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13
Q

matter in the _ state has indefinite shape and volume

A

gas

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14
Q

matter in the liquid state

A

has indefinite shape and definite volume

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15
Q

matter in the _ state has indefinite shape and definite volume

A

liquid

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16
Q

matter in the solid state

A

has definite shape and volume

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17
Q

matter in the _ state has definite shape and volume

A

solid

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18
Q

nobel prize for physics in 1910. norwegian dutch physicist. suggested that there must be a reason why gases condensed when cooled

A

Johannes Diderik van der Waals

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19
Q

sometimes called as noncovalent bonds

A

intermolecular forces

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20
Q

intermolecular forces sometimes called as

A

noncovalent bonds

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21
Q

Named after bonding, and London dispersion forces.
* Also Known as van der waals forces, named after a Dutch chemist, Johannes van der Waal (1837-1923).

A

intermolecular forces

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22
Q

are weak attractions that are used to explain the attraction between nonpolar molecules as it apparent that even nonpolar molecules can have dipoles for short periods of
time.

A

London Dispersion Forces (LDF)

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23
Q

LDF

A

London Dispersion Forces

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24
Q

the attraction of bond dipoles, in different molecules

A

dipole-dipole forces

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25
exist when polar molecules are attracted to ions
ion-dipole forces
26
A weak bond formed when a hydrogen with partial positive charge is close to an atom in a molecule with lone pairs of electrons or with excess electronic charge.
hydrogen bond or hydrogen bridge
27
s the force that causes the molecules on the surface of a liquid to "tighten their hold to one another" creating the effect of a thin membrane on the surface.
surface tension
28
Substances with strong attractive forces between the molecules have high surface tensions.
surface tension
29
It is temperature-dependent; it decreases as temperature increases.
surface tension
30
is a measure of its tendency to resist flowing motion
viscosity
31
Polar molecules and molecules with complex structures tend to have higher viscosity, being less able to slip and slide over one another than those with simple structures and less polarty.
viscosity
32
the spontaneous rising of a liquid in a narrow tube, is also observed
capillary action
33
is much less in a liquid than in a gas, but it takes place at an easily measured rate ( it can slide over one another to effect diffusion)
diffusibility
34
another property of liquids
incompressibility
35
Since the molecules in a liquid are already close, touching one another, they cannot be crowded together anymore unless they are squeezed and deformed, which would require a great amount of energy.
incompressibility
36
is an indication of the escape of molecules from the surface of the liquid. It is an evidence of molecular motion.
evaporation
37
the molecules that escape from the surface of the liquid
cooling effect of evaporation
38
is the temperature at which the vapor pressure of a liquid is equal to the external pressure
boiling point
39
normal boiling point
760 mm Hg at sea level
40
when a liquid vaporizes in a closed container, the space above the liquid becomes saturated with vapor and an equilibrium state exist between the liquid and the vapor.
vapor pressure
41
expressed in cal/g or in kcal/g-atom or in kJ/kg, is the energy required to change exactly one gram of liquid to vapor at its normal boiling point
heat of vaporization
42
is a good solvent
water
43
has a high specific heat
water
44
the specific heat of water
1 calorie/g-˚C (4.18 J/g-˚C)
45
solids are generally classifies into:
amorphous or crystalline solids
46
means that the solid does not always adopt the same form
amorphous
47
its constituent particles are randomly arranged. Do not have sharp melting point that is, melting within a narrow temperature range. They soften first and melt little by little over a wide temperature range.
amorphous solid
48
A solid in which the constituent particles (atoms, ions, or molecules) have an orderly arrangement, that is, it has regularly arranged structure units with characteristics geometric forms. Show regular shapes which reflect the arrangement of the particles within them.
crystalline solid
49
types of crystalline solids (4)
metallic crystals, ionic crystals, molecular crystals, covalent network crystals
50
have atoms arranged in an orderly repeating pattern
crystalline solids
51
lack the order found in crystalline solids
amorphous solids
52
are the simplest type of structure. can be thought of as three dimensional arrays of metal cations
metallic crystals
53
metallic crystals two choices
face centered cubic packing and hexagonal close-packing
54
Have ions as constituent particles. This is exemplitied the sodium chloride crystal. The oppositely charged Na' and CH ions arrange themselves in a regular three-dimensional pattern of a crystal lattice.
ionic crystals
55
is the property shown by substances which have molecules or ions that can assume more than one stable arrangement in the solid state.
polymorphism
56
The diferent molecular forms or various crystal modification of a polymorphous element are known as
allotropes
57
Those which have molecules as constituent particles as well as structure units. Weak van der waals forces of attraction hold them together. Solids like iodine, camphor, menthol and napthalene are recognized readily by their odor, an evidence that they are undergoing sublimation.
molecular crystals
58
Are giant molecules or macromolecules. They consist of very large numbers of atoms linked by a network of covalent bonds. These molecules may build up in one direction as long as chains which form fibrous crystals.
covalent network crystals
59
intermolecular forces of matter and properties of liquids (2)
surface tension and viscosity
60
other properties observed when matter is in the liquid phase (8)
capillary action, diffusibility, incompressibility, evaporation, cooling effect of evaporation, boiling point, vapor pressure, and heat of vaporization
61
is the temperature where vapor pressure equals atmospheric pressure
boiling point
62
intermolecular forces (4)
London Dispersion Forces, Dipole-Dipole Forces, Ion-Dipole Forces, Hydrogen Bond or Hydrogen Bridge
63
classes of solids (2)
amorphous solid and crystalline solid
64
consists of discrete regions that represent the different phases exhibited by a substance
typical phase diagram
65
is favored at low temperature and high pressure
solid phase
66
is favored at high temperature and low pressure
gas phase
67
is for a single pure substance in a closed system, not for a liquid in an open beaker in contact with air at 1 atm pressure.
phase diagram
68
correspond to the combinations of temperature and pressure at which two phases can coexist in equilibrium.
the lines in a phase diagram
69
Sublimation of water at low temperature and pressure can be used to _ foods and beverages.
"freeze-dry"
70
is emerging as a natural refrigerant, making it a low carbon (and thus a more environmentally friendly) solution for domestic heat pumps.
supercritical carbon dioxide
71
the graph of temperature against time is called a _
heating curve
72
show how the temperature changes as a substance is heated up
heating curves
73
they show how the temperature changes as a substance is cooled down. it have the horizontal flat parts where the state changes from gas to liquid
cooling curves
74
the _ ang _ occur at the same temperature
melting and freezing
75
during _, energy is removed and during _, energy is absorbed
freezing, melting
76
is a measure of average kinetic energy
temperature
77
temperature is a measure of _
average kinetic energy
78
any change in temperature is a change in _
kinetic energy
79
all the energy that is absorbed or released is related to changes in _
potential energy
80
3 Ps
plateau, phase change, and potential energy change
81
lesson 2
phase diagrams, heating and cooling curves
82
lesson 1
properties of solids and liquids to the nature of forces between particles

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