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Chem > Ch 10 Section 3 > Flashcards

Ch 10 Section 3 Flashcards

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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
Q

amorphous solids are sometimes classified as supercooled liquids, which are substances that retain certain liquid properties even at

A

temperatures at which they appear to be solid

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26
Q

these properties exist because the particles in amorphous solids are arranged

A

randomly, much like the particles in a liquid

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27
Q

unlike the particles in a true liquid, however, the particles in amorphous solids are not

A

constantly changing their positions

28
Q

substances are most dense in the

A

solid state

29
Q

solids tend to be slightly denser than

A

liquids and much denser than gases

30
Q

the higher density results from the fact that the particles of a solid are more

A

closely packed than those of a liquid or a gas

31
Q

solid hydrogen is the least dense solid; it has a density of about

A

1/320 the densest element, osmium

32
Q

solids are generally less compressible than

A

liquids

33
Q

some solids, such as wood and cork, may seem compressible, but they are

A

not

34
Q

diffusion does occur in

A

solids

35
Q

the rate of diffusion in solids is millions of times slower than in

A

liquids

36
Q

crystalline solids exist either as single crystals or as

A

groups of crystals fused together

37
Q

the total 3d arrangement of particles of a crystal is called a

A

crystal structure

38
Q

the arrangement of particles in the crystal can be represented by a coordinate system called a

A

lattice

39
Q

the smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice is called a

A

unit cell

40
Q

each crystal lattice contains many

A

unit cells packed together

41
Q

a crystal and its unit cells can have any one of

A

seven types of symmetry which enables scientists to classify crystals by their shape

42
Q

crystal structures can also be described in terms of the types of particles in them and the types of

A

chemical bonding between the particles

43
Q

(types of crystals) ionic crystals: ionic crystal structure consists of positive and

A

negative ions arranged in a regular pattern

44
Q

(types of crystals) ionic crystals: the ions can be monatomic or

A

polyatomic

45
Q

(types of crystals) ionic crystals: ionic crystals form when group 1 or group 2 metals combine with group 16 or group 17

A

nonmetals or nonmetallic polyatomic ions

46
Q

(types of crystals) ionic crystals: the strong binding forces between the positive and negative ions in the crystal structure give the ionic crystals

A

certain properties→hardness, brittleness, high melting pts., good insulators

47
Q

(types of crystals) covalent network crystals: each atom is covalently bonded to its

A

nearest neighboring atoms

48
Q

(types of crystals) covalent network crystals: the covalent bonding extends throughout a network that includes a

A

very large number of atoms

49
Q

(types of crystals) covalent network crystals: three-dimensional covalent network solids include

A

diamond, quartz, silicon carbide, and many oxides of transition metals

50
Q

(types of crystals) covalent network crystals: the subscript x in these formulas (e.g. (SiO2)x ) indicates that the component within the parentheses

A

extends indefinitely

51
Q

(types of crystals) covalent network crystals: the network solids are nearly always very

A

hard and brittle

52
Q

(types of crystals) covalent network crystals: they have rather high melting points and are usually

A

nonconductors or semiconductors

53
Q

(types of crystals) metallic crystals: the metallic crystal structure consists of

A

metal cations surrounded by a sea of delocalized valence electrons

54
Q

(types of crystals) metallic crystals: the electrons come from the metal atoms and belong to the

A

crystal as a whole

55
Q

(types of crystals) metallic crystals: the freedom of these delocalized electrons to move throughout the crystal explains the

A

high electric conductivity of metals

56
Q

(types of crystals) covalent molecular crystals: the crystal structure of a covalent molecular substance consists of covalently bonded

A

molecules held together by intermolecular forces

57
Q

(types of crystals) covalent molecular crystals: if the molecules are nonpolar then there are only weak

A

London dispersion forces between molecules (e.g. hydrogen, methane, benzene C6H6)

58
Q

(types of crystals) covalent molecular crystals: in a polar covalent molecular crystal molecules are

A

held together by dispersion forces, somewhat stronger dipole-dipole forces, and sometimes by even stronger hydrogen bonding (e.g. H20, ammonia NH3)

59
Q

(types of crystals) covalent molecular crystals: the forces that hold polar/nonpolar molecules together in the structure are much weaker than the

A

covalent chemical bonds between the atoms within each molecule

60
Q

(types of crystals) covalent molecular crystals: covalent molecular crystals thus have

A

low melting points

61
Q

(types of crystals) covalent molecular crystals: easily…, are relatively…, and are good…

A

vaporized; soft; insulators

62
Q

amorphous comes from greek word for

A

without shape

63
Q

the atoms that make up amorphous solids are not arranged in

A

a regular pattern

64
Q

glasses are made by cooling certain molten materials in a way that

A

prevents them from crystallizing

65
Q

plastics (amorphous solid) are easily molded at high

A

temperatures and pressures and are used in many structural materials

66
Q

amorphous semiconductors are used in

A

electronic devices

Chem (54 decks)

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