Ap Chem - Ch 10 & 11

Front 1

intramolecular bonding

Back 1

within the molecule

Front 2

intermolecular forces

Back 2

between molecules

Front 3

dipole-dipole attraction

Back 3

molecules with dipole moments (polar bonds, center for + and - charge) attract

Front 4

hydrogen bonding

Back 4

dipole-dipole attractions which are found in molecules with hydrogen bond to highly electronegative atoms (HN, HO, HF)

Front 5

London dispersion force

Back 5

weak forces existing among noble gas atoms & non-polar molecules; caused by an instantaneous dipole, which in triggers others

Front 6

polarizability

Back 6

ease with which the e- cloud of an atom can be distorted to give a dipolar charge distribution (large atoms with more e- have a higher polarizability than smaller)

Front 7

surface tension

Back 7

resistance of a liquid to an increase in SA (have to break IMFs to move further away and increase SA)

Front 8

capillary action

Back 8

spontaneous rising of a liquid in a narrow tube, exhibited by polar liquids

Front 9

cohesive forces

Back 9

IMFs among the molecules of a liquid

Front 10

adhesive forces

Back 10

forces b/n the liquid molecules and their container

Front 11

viscosity

Back 11

a measure of a liquid's resistance to flow (large IMFS - highly viscous)

Front 12

crystalline solids

Back 12

regular arrangements of components

Front 13

amorphous solids

Back 13

solids with considerable disorder in their structure

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lattice

Back 14

3D system of pts designating the centers of the components of a solid

Front 15

unit cell

Back 15

smallest repeating unit of a lattice

Front 16

x-ray diffraction

Back 16

shooting of single x-rays at a crystalline solid to determine their structure from the x-rays' diffraction (scattering of beams of light from a regular array of points)

Front 17

bragg equation

Back 17

n lambda = 2 d sin theta

Front 18

ionic solid

Back 18

solid containing cations and anions that dissolves in water to give a solution containing free-floating ions

Front 19

molecular solid

Back 19

a solid composed of neutral molecules at the lattice points

Front 20

atomic solid

Back 20

a solid that contains atoms at the lattice points. 3 subgroups: metallic solids, network solids, and Group VIIIA solids.

Front 21

closest packing

Back 21

modeling a metallic crystal by packing uniform, hard spheres in a manner that most efficiently uses the space available; abc or aba

Front 22

hexagonal closest packed

Back 22

structure composed of closest packed spheres with an ababab arrangement of layers, the unit cell is hexagonal

Front 23

cubic closest packed structure

Back 23

solid modeled by the closest packing of spheres with an abcabc arrangement of layers; unit cell is face-centered cubic. Some metals assume structures that are not closest packed: these have a simple cubic or body-centered cubic unit cell.

Front 24

e- sea model

Back 24

simpler bonding model for metals; regular array of metal cations in a sea of valence e-

Front 25

band model/molecular orbital (MO) model

Back 25

more complex bonding model for metals; e- travel around the metal crystal in molecular orbitals formed from te valence atomic orbitals of the metal atoms. As more and more metal atoms interact the large # of molecular orbitals become closely spaced and finally a continuum of levels, which are partially occupied

Front 26

bands

Back 26

continuum of molecular orbitals formed when many metals interact, where the valence e- can travel

Front 27

conduction bands

Back 27

molecular orbitals occupied by conducting e-

Front 28

alloy

Back 28

a substance that contians a mixture of elements and has metallic properties

Front 29

substitutional alloy

Back 29

host metal atoms are replaced by other metal atoms of similar size

Front 30

interstitial alloy

Back 30

interstices in the ccp metal structure are occupied by small atoms

Front 31

network solid

Back 31

atomic solid containing strong directional covalent bonds that form a giant molecules

Front 32

silica

Back 32

fundamental silicon-oxygen compound; has the empirical formula of SiO2

Front 33

silicate

Back 33

O/Si ratios higher than 2:1 and contain Si-O anions

Front 34

glass

Back 34

amorphous solid formed when silica is heated above its melting point

Front 35

aluminosilicate

Back 35

aluminum as well as silicon atoms are part of the polyanion

Front 36

semiconductor

Back 36

substance conducting only slight electrical current at room rmperature but showing increased conductivity at higher T's

Front 37

doping

Back 37

replacing atoms of one element with the atoms of another element to increase conductivity

Front 38

n-type semiconductor

Back 38

substance whose conductivity is increased by doping it with atoms with one more v e- than the host atom

Front 39

p-type semiconductor

Back 39

semiconductor whose conductivity is increased by doping it with atoms having one fewer valence e- than the host atoms

Front 40

p-n junction

Back 40

connection of a p-type and an n-type semiconductor; e- travel from n-type to p-type, giving the p-type a (-) charge and the n-type a (+) charge

Front 41

contact/junction potential

Back 41

charge buildup in a p-n junction as e- migrate from the n-type to the p-type

Front 42

reverse bias

Back 42

when a (+) and (-) terminal of a battery are applied to the wrong ends of a p-n junction and the junction resists the imposed current flow because it is opposite to its natural flow

Front 43

forward bias

Back 43

low resistance to the current; flows easily

Front 44

rectifier

Back 44

device that produces a pulsating direct (one direction) current from an alternating (both directions) current

Front 45

vaporization

Back 45

change of a substance from liquid to gas state

Front 46

heat of vaporization

Back 46

E required to vaporize 1 mol of a liquid at 1 atm

Front 47

condensation

Back 47

change of a substance from gas to liquid

Front 48

vapor pressure

Back 48

pressure of the vapor present at equilibrium

Front 49

equilibrium

Back 49

pt at which no further net change occurs in the amount of liquid or vapor because the rate of vaporization and condensation balance each other

Front 50

volatile

Back 50

evaporate rapidly; has a high VP

Front 51

sublimation

Back 51

going directly from the solid to the gaseous state without passing through the liquid state

Front 52

heating curve

Back 52

polt of temperature vs. time, where E is added at a constant rate

Front 53

heat of fusion

Back 53

enthalpy change that occurs when a solid melts

Front 54

normal melting point

Back 54

temperature at which the solid and liquid have the same VP; total p=1

Front 55

normal boiling point

Back 55

temperature at which the vapor pressure of the liquid is exactly 1 atm (if the outside p= 1 atm)

Front 56

boiling

Back 56

VP liquid = P environment

Front 57

supercooled

Back 57

a liquid can be cooled below its freezing point at 1 atm and remain in the liquid state if the liquid does not have enough organization to form a solid at that point

Front 58

superheated

Back 58

a liquid can be raised to temperature above its boiling point without boiling because there are not enough high E molecules in the same vicinity

Front 59

phase diagram

Back 59

convenient way of representing the phases of a substance as a function of temperature and P

Front 60

triple point

Back 60

point on a phase diagram where all 3 states of a substance are present

Front 61

critical temperature

Back 61

T above which vapor cannot be liquefied, no matter what P

Front 62

critical pressure

Back 62

P required to produce liquefaction at the critical temperature

Front 63

critical point

Back 63

critical T + critical P; beyond this point the substance exist in an intermediate "fluid-gas" state

Front 64

molarity (M)

Back 64

moles of solute/L solution

Front 65

molality (m)

Back 65

moles of solute/kg of solvent

Front 66

mass percent

Back 66

mass of solute/mass of solution x 100

Front 67

mole fraction

Back 67

# mol A/(# mol A + # mol B)

Front 68

normality

Back 68

# of equivalents per L of solution

Front 69

hydrophobic

Back 69

water-fearing

Front 70

hydrophilic

Back 70

water-loving

Front 71

Henry's Law

Back 71

deals with gas dissolving into a liquid; P = kC (P is the pressure of the gaseous solute, k is particular to the solution and C is the concentration of dissolved gas)

Front 72

thermal pollution

Back 72

water being used for industrial cooling then returned to its natural source at a higher than ambient temperature

Front 73

Raoult's Law

Back 73

deals with solid-liquid solutions; Psoln = XsolventPsolvent

Front 74

Raoult's Law (modified)

Back 74

deals with liquid-liquid solutions; Ptotal = XaPa + XbPb

Front 75

ideal solution

Back 75

liquid-liquid solution that obeys Raoult's law

Front 76

colligative properties

Back 76

frz. pt depression, bpt elevation, osmotic P; depend on the number of solute particles in a solution

Front 77

semipermeable membrane

Back 77

allows solvent but not solute molecules to pass through

Front 78

osmosis

Back 78

flow of solvent into the solution through the semipermeable membrane

Front 79

osmotic pressure

Back 79

P required to stop osmosis

Front 80

dialysis

Back 80

cell version of osmosis (allows small solute molecules and ions through)

Front 81

hypertonic

Back 81

higher osmotic P

Front 82

hypotonic

Back 82

lower osmotic P

Front 83

isotonic solutions

Back 83

solutions with identical osmotic P

Front 84

crenation

Back 84

cells bathed in a hypertonic solution, shrivel because water flows out

Front 85

hemolysis

Back 85

cells bathed in a hypotonic solution, bloat and explode because water flows in

Front 86

desalination

Back 86

removal of dissolved salts

Front 87

ion pairing

Back 87

oppositely charged particles aggregate and behave as a single particle; the i value is lowered because of this; happens less when particles are further away (more dilute)

Front 88

Tyndall effect

Back 88

scattering of light by particles

Front 89

colloid

Back 89

suspension of tiny particles in some medium

Front 90

coagulation

Back 90

destruction of a colloid (adding an electrolyte or heating)