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Chem > Ch 10 Section 3 > Flashcards

Ch 10 Section 3 Flashcards

1
Q

the particles of a solid are more closely packed than those of a

A

liquid or gas

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2
Q

intermolecular forces between particles are therefore much more

A

effective in solids

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3
Q

all interparticle attractions exert stronger effects in solids than in the corresponding

A

liquids or gases

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4
Q

attractive forces tend to hold the particles of a solid in

A

relatively fixed points, with only vibrational movement around fixed points

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5
Q

because the motions of the particles are restricted in this way, solids are more ordered than

A

liquids and are much more ordered than gases

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6
Q

there are two types of solids:

A

crystalline solids and amorphous solids

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7
Q

Most solids are crystalline solids→they

A

consist of crystals

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8
Q

a crystal is a substance in which the particles are arranged in an

A

orderly, geometric, repeating pattern

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9
Q

noncrystalline solids, including glass and particles, are called

A

amorphous solids

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10
Q

an amorphous solid is one in which the particles are arranged

A

randomly

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11
Q

unlike liquids and gases, solids can maintain a definite

A

shape without a container

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12
Q

crystalline solids are

A

geometrically regular

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13
Q

even the fragments of a shattered crystalline solid have distinct

A

geometric shapes that reflect their internal structure

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14
Q

amorphous solids maintain a definite shape, but they do not have the

A

distinct geometric shapes of crystalline solids

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15
Q

the volume of a solid changes only slightly with a change in

A

temperature or pressure

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16
Q

solids have definite volume because their particles are

A

packed closely together

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17
Q

there is very little empty space into which the particles can be

A

compressed

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18
Q

crystalline solids generally do not flow because their particles are held in

A

relatively fixed positions

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19
Q

melting is the physical change of a solid to a liquid by the addition of

A

energy as heat

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20
Q

the temperature at which a solid becomes a liquid is its

A

melting point

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21
Q

at this temperature, the kinetic energies of the particles within the solid overcome the a

A

attractive forces holding them together

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22
Q

the particles can then break out of their positions in

A

crystalline solids, which have definite melting points

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23
Q

amorphous solids have no definite

A

melting point

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24
Q

amorphous solids have the ability to flow over a

A

range of temperatures

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25
amorphous solids are sometimes classified as supercooled liquids, which are substances that retain certain liquid properties even at
temperatures at which they appear to be solid
26
these properties exist because the particles in amorphous solids are arranged
randomly, much like the particles in a liquid
27
unlike the particles in a true liquid, however, the particles in amorphous solids are not
constantly changing their positions
28
substances are most dense in the
solid state
29
solids tend to be slightly denser than
liquids and much denser than gases
30
the higher density results from the fact that the particles of a solid are more
closely packed than those of a liquid or a gas
31
solid hydrogen is the least dense solid; it has a density of about
1/320 the densest element, osmium
32
solids are generally less compressible than
liquids
33
some solids, such as wood and cork, may seem compressible, but they are
not
34
diffusion does occur in
solids
35
the rate of diffusion in solids is millions of times slower than in
liquids
36
crystalline solids exist either as single crystals or as
groups of crystals fused together
37
the total 3d arrangement of particles of a crystal is called a
crystal structure
38
the arrangement of particles in the crystal can be represented by a coordinate system called a
lattice
39
the smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice is called a
unit cell
40
each crystal lattice contains many
unit cells packed together
41
a crystal and its unit cells can have any one of
seven types of symmetry which enables scientists to classify crystals by their shape
42
crystal structures can also be described in terms of the types of particles in them and the types of
chemical bonding between the particles
43
(types of crystals) ionic crystals: ionic crystal structure consists of positive and
negative ions arranged in a regular pattern
44
(types of crystals) ionic crystals: the ions can be monatomic or
polyatomic
45
(types of crystals) ionic crystals: ionic crystals form when group 1 or group 2 metals combine with group 16 or group 17
nonmetals or nonmetallic polyatomic ions
46
(types of crystals) ionic crystals: the strong binding forces between the positive and negative ions in the crystal structure give the ionic crystals
certain properties→hardness, brittleness, high melting pts., good insulators
47
(types of crystals) covalent network crystals: each atom is covalently bonded to its
nearest neighboring atoms
48
(types of crystals) covalent network crystals: the covalent bonding extends throughout a network that includes a
very large number of atoms
49
(types of crystals) covalent network crystals: three-dimensional covalent network solids include
diamond, quartz, silicon carbide, and many oxides of transition metals
50
(types of crystals) covalent network crystals: the subscript x in these formulas (e.g. (SiO2)x ) indicates that the component within the parentheses
extends indefinitely
51
(types of crystals) covalent network crystals: the network solids are nearly always very
hard and brittle
52
(types of crystals) covalent network crystals: they have rather high melting points and are usually
nonconductors or semiconductors
53
(types of crystals) metallic crystals: the metallic crystal structure consists of
metal cations surrounded by a sea of delocalized valence electrons
54
(types of crystals) metallic crystals: the electrons come from the metal atoms and belong to the
crystal as a whole
55
(types of crystals) metallic crystals: the freedom of these delocalized electrons to move throughout the crystal explains the
high electric conductivity of metals
56
(types of crystals) covalent molecular crystals: the crystal structure of a covalent molecular substance consists of covalently bonded
molecules held together by intermolecular forces
57
(types of crystals) covalent molecular crystals: if the molecules are nonpolar then there are only weak
London dispersion forces between molecules (e.g. hydrogen, methane, benzene C6H6)
58
(types of crystals) covalent molecular crystals: in a polar covalent molecular crystal molecules are
held together by dispersion forces, somewhat stronger dipole-dipole forces, and sometimes by even stronger hydrogen bonding (e.g. H20, ammonia NH3)
59
(types of crystals) covalent molecular crystals: the forces that hold polar/nonpolar molecules together in the structure are much weaker than the
covalent chemical bonds between the atoms within each molecule
60
(types of crystals) covalent molecular crystals: covalent molecular crystals thus have
low melting points
61
(types of crystals) covalent molecular crystals: easily..., are relatively..., and are good...
vaporized; soft; insulators
62
amorphous comes from greek word for
without shape
63
the atoms that make up amorphous solids are not arranged in
a regular pattern
64
glasses are made by cooling certain molten materials in a way that
prevents them from crystallizing
65
plastics (amorphous solid) are easily molded at high
temperatures and pressures and are used in many structural materials
66
amorphous semiconductors are used in
electronic devices

Chem (54 decks)

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