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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
Q

exist when polar molecules are attracted to ions

A

ion-dipole forces

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26
Q

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.

A

hydrogen bond or hydrogen bridge

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27
Q

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.

A

surface tension

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28
Q

Substances with strong attractive forces between the molecules have high surface tensions.

A

surface tension

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29
Q

It is temperature-dependent; it decreases as temperature increases.

A

surface tension

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30
Q

is a measure of its tendency to resist flowing motion

A

viscosity

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31
Q

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.

A

viscosity

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32
Q

the spontaneous rising of a liquid in a narrow tube, is also observed

A

capillary action

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33
Q

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)

A

diffusibility

34
Q

another property of liquids

A

incompressibility

35
Q

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.

A

incompressibility

36
Q

is an indication of the escape of molecules from the surface of the liquid. It is an evidence of molecular motion.

A

evaporation

37
Q

the molecules that escape from the surface of the liquid

A

cooling effect of evaporation

38
Q

is the temperature at which the vapor pressure of a liquid is equal to the external pressure

A

boiling point

39
Q

normal boiling point

A

760 mm Hg at sea level

40
Q

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.

A

vapor pressure

41
Q

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

A

heat of vaporization

42
Q

is a good solvent

43
Q

has a high specific heat

44
Q

the specific heat of water

A

1 calorie/g-˚C (4.18 J/g-˚C)

45
Q

solids are generally classifies into:

A

amorphous or crystalline solids

46
Q

means that the solid does not always adopt the same form

47
Q

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.

A

amorphous solid

48
Q

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.

A

crystalline solid

49
Q

types of crystalline solids (4)

A

metallic crystals, ionic crystals, molecular crystals, covalent network crystals

50
Q

have atoms arranged in an orderly repeating pattern

A

crystalline solids

51
Q

lack the order found in crystalline solids

A

amorphous solids

52
Q

are the simplest type of structure. can be thought of as three dimensional arrays of metal cations

A

metallic crystals

53
Q

metallic crystals two choices

A

face centered cubic packing and hexagonal close-packing

54
Q

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.

A

ionic crystals

55
Q

is the property shown by substances which have molecules or ions that
can assume more than one stable arrangement in the solid state.

A

polymorphism

56
Q

The diferent molecular forms or various crystal modification of a polymorphous element are known as

A

allotropes

57
Q

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.

A

molecular crystals

58
Q

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.

A

covalent network crystals

59
Q

intermolecular forces of matter and properties of liquids (2)

A

surface tension and viscosity

60
Q

other properties observed when matter is in the liquid phase (8)

A

capillary action, diffusibility, incompressibility, evaporation, cooling effect of evaporation, boiling point, vapor pressure, and heat of vaporization

61
Q

is the temperature where vapor pressure equals atmospheric pressure

A

boiling point

62
Q

intermolecular forces (4)

A

London Dispersion Forces, Dipole-Dipole Forces, Ion-Dipole Forces, Hydrogen Bond or Hydrogen Bridge

63
Q

classes of solids (2)

A

amorphous solid and crystalline solid

64
Q

consists of discrete regions that represent the different phases exhibited by a substance

A

typical phase diagram

65
Q

is favored at low temperature and high pressure

A

solid phase

66
Q

is favored at high temperature and low pressure

67
Q

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.

A

phase diagram

68
Q

correspond to the combinations of temperature and pressure at which two phases can coexist in equilibrium.

A

the lines in a phase diagram

69
Q

Sublimation of water at low temperature and pressure can be used to _ foods and beverages.

A

“freeze-dry”

70
Q

is emerging as a natural refrigerant, making it a low carbon (and thus a more environmentally friendly) solution for domestic heat pumps.

A

supercritical carbon dioxide

71
Q

the graph of temperature against time is called a _

A

heating curve

72
Q

show how the temperature changes as a substance is heated up

A

heating curves

73
Q

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

A

cooling curves

74
Q

the _ ang _ occur at the same temperature

A

melting and freezing

75
Q

during _, energy is removed and during _, energy is absorbed

A

freezing, melting

76
Q

is a measure of average kinetic energy

A

temperature

77
Q

temperature is a measure of _

A

average kinetic energy

78
Q

any change in temperature is a change in _

A

kinetic energy

79
Q

all the energy that is absorbed or released is related to changes in _

A

potential energy

80
Q

3 Ps

A

plateau, phase change, and potential energy change

81
Q

lesson 2

A

phase diagrams, heating and cooling curves

82
Q

lesson 1

A

properties of solids and liquids to the nature of forces between particles

quizzes (35 decks)

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