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AP Chemistry > Chapter 10: Liquids and Solids > Flashcards

Chapter 10: Liquids and Solids Flashcards

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1
Q

Condensed states

A

Liquids and solids

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2
Q

Intermolecular forces

A

Forces that occur between molecules

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3
Q

Dipole-dipole attraction

A

Molecules with dipole moments can attract each other electrostatically by lining up so that the positive and negative ends are close to each other

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4
Q

Hydrogen bonding

A

Particularly strong dipole-dipole forces where hydrogen is bound to a highly electronegative atom, such as N, O, or F

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5
Q

London dispersion forces

A

The forces, existing among noble gas atoms and nonpolar molecules, that involve an accidental dipole that induces a momentary dipole in a neighbor

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6
Q

Surface tension

A

The resistance of a liquid to an increase in its surface area

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7
Q

Capillary action

A

The spontaneous rising of a liquid in a narrow tube

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8
Q

Cohesive forces

A

The intermolecular forces among the molecules of the liquid

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9
Q

Adhesive forces

A

The forces between the liquid molecules and their container

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10
Q

Viscosity

A

A measure of a liquid’s resistance to flow

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11
Q

Crystalline solids

A

Solids with a highly regular arrangement of their components

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12
Q

Amorphous solids

A

Solids with considerable disorder in their structures

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13
Q

Lattice

A

A three-dimensional system of points designating the positions of the components (atoms, ions, or molecules) that make up the substance

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14
Q

Unit cell

A

The smallest repeating unit of the lattice

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15
Q

Bragg equation

A

nλ = 2d sin θ

n = integer
λ = wavelength of the x rays
d = distance between the atoms
θ = angle of incidence and reflection
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16
Q

Ionic solid

A

A solid containing cations and anions that dissolves in water to give a solution containing the separated ions, which are mobile and thus free to conduct an electric current

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17
Q

Molecular solid

A

A solid composed of neutral molecules at the lattice points

Bonding: Dipole-dipole and/or London dispersion forces

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18
Q

Atomic solid

A

A solid that contains atoms at the lattice points

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19
Q

Three types of atomic solids

A
  1. Metallic - metal, delocalized covalent bonding
  2. Network - nonmetal, directional covalent
  3. Group 8A - group 8A, London dispersion forces
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20
Q

Closest packing

A

Packing uniform, hard spheres in a manner that most efficiently uses the available space

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21
Q

aba Arrangement

A

The third layer occupies positions so that each sphere in the third layer lies directly over a sphere in the first layer (Hexagonal unit cell, hexagonal closest packed structure)

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22
Q

abc Arrangement

A

The third layer occupies positions so that no sphere in the third layer lies over one in the first layer (face-centered cubic unit cell, cubic closest packed structure)

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23
Q

In both hcp and ccp structures, each sphere has __ equivalent nearest neighbors.

A

12

  • 6 in the same layer
  • 3 in the layer above
  • 3 in the layer below (that form the dimples)
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24
Q

How many atoms are in a face-centered cubic unit cell?

A

(8 x 1/8) + (6 x 1/2) = 4

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25
Q

How many atoms are in a simple cubic unit cell?

A

(8 x 1/8) = 1

26
Q

How many atoms are in a body-centered cubic unit cell?

A

(8 x 1/8) + 1 = 2

27
Q

Alloy

A

A substance that contains a mixture of elements and has metallic properties

28
Q

Substitutional alloy

A

Some of the host metal atoms are REPLACED by other metal atoms of similar size.

29
Q

Interstitial alloy

A

When some of the interstices (holes) in the closest packed metal structure are occupied by small atoms

30
Q

Network solids

A

Atomic solids that contain strong directional covalent bonds to form a solid viewed as a “giant molecule”
(e.g.: Two most common forms of carbon: graphite and diamond)

31
Q

Silica

A

The fundamental silicon-oxygen compound, which has the empirical formula SiO2, and forms the basis of quartz and certain types of sand.

32
Q

Diamond

A

Each carbon atom is surrounded by a tetrahedral arrangement, stabilized by covalent bonds.

33
Q

Graphite

A

Layers of carbon atoms arranged in fused six-membered rings. Each carbon atom in a particular layer of graphite is surrounded by the three other carbon atoms in a trigonal planar arrangement.

34
Q

Silicates

A

Salts that contain metal cations and polyatomic silicon-oxygen anions that are usually polymeric.

35
Q

Glass

A

An amorphous solid obtained when silica is mixed with other compounds, heated above its melting point, and then cooled rapidly (HOMOGENEOUS)

36
Q

Quartz

A

Based on interconnected SiO4 tetrahedra with shared oxygen atoms, composed of silica

37
Q

Ceramics

A

Made from clays (which contain silicates) and hardened by firing at high temperatures. Nonmetallic materials that are strong, brittle, and resistant to heat and attack by chemicals (HETEROGENEOUS: minutes crystals of silicates that are suspended in a glassy cement)

38
Q

Semiconductor

A

A substance conducting only a slight electric current at room temperature, but showing increased conductivity at higher temperatures

39
Q

n-type semiconductor

A

A substance whose conductivity is increased by doping it with atoms having more valence electrons than the atoms in the host crystal

40
Q

p-type semiconductor

A

A substance whose conductivity is increased by doping it with atoms having fewer valence electrons than the atoms of the host crystal

41
Q

Size of the the three holes in closest packed structures from smallest to largest

A

Trigonal

42
Q

In the closest packed structure, there are _____ as many tetrahedral holes as packed anions

A

Twice

43
Q

Vaporization/evaporation

A

The change in state that occurs when a liquid evaporates to form a gas (ENDOTHERMIC)

44
Q

Heat/enthalpy of vaporization

A

The energy required to vaporize 1 mole of a liquid at a pressure of 1 atm

45
Q

Condensation

A

The process by which vapor molecules re-form a liquid

46
Q

Equilibrium

A

When enough vapor molecules are present above the liquid so that the rate of condensation equals the rate of evaporation, thus the two opposite processes exactly balance each other

47
Q

Vapor pressure

A

The pressure of the vapor present at equilibrium

48
Q

Volatile

A

Describes liquids with high vapor pressures and evaporate rapidly from an open dish

49
Q

Vapor pressure decreases with…

A

Larger intermolecular forces and molar masses

50
Q

Vapor pressure increases with…

A

Higher temperatures

51
Q

Vapor pressure and heat of vaporization equation

A

ln(Pvap) = -(∆Hvap/R)(1/T) + C

T = Kelvin temperature
R = universal gas constant = 8.3145 J/K • mol
C = constant characteristic of a given liquid
52
Q

Change in Vapor Pressures and Temperatures equation

A

ln(Pvap,T1/Pvap,T2) = (∆Hvap/R)(1/T2 - 1/T1)

53
Q

Heating curve

A

A plot of temperature versus time for a process where energy is added at a constant rate

54
Q

Heat/enthalpy of fusion

A

The enthalpy change that occurs at the melting point when a solid melts

55
Q

Normal melting point

A

The temperature at which the solid and liquid states have the same vapor pressure under conditions where the total pressure is 1 atmosphere

56
Q

Normal boiling point

A

The temperature at which the vapor pressure of the liquid is exactly 1 atmosphere

57
Q

Supercooling

A

The process of cooling a liquid below its freezing point without its changing to a solid

58
Q

Superheating

A

The process of heating a liquid above its boiling point without its boiling

59
Q

Triple point

A

The point on a phase diagram at which all three states of a substance are present

60
Q

Critical temperature

A

The temperature above which the vapor cannot be liquefied no matter what pressure is applied

61
Q

Critical pressure

A

The pressure to produce liquefaction at the critical temperature

62
Q

Critical point

A

The point on a phase diagram at which the temperature and pressure have their critical values; the endpoint of the liquid-vapor line

AP Chemistry (10 decks)

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