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phases gases and solutions Flashcards

1
Q

basic phases of matter

A

solid liquids and gases

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2
Q

what forces determine which phase a substance will be in?

A

intermolecular forcers

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3
Q

solid

A

phase with rigid and tighly packed atoms
- fixed volume and noncompressible
- crystalline or amorphous

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4
Q

lattice energy

A

amount of energy required to disrput the crystalline structure of a salt into cations and anions

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5
Q

amorphous solids

A

solids without a crystalline structure (glass and silcone)

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6
Q

liquid

A

phase with fixed volume and are not compressible but do not have a fixed shape

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7
Q

viscocity

A

property of liquids: resistance to flow

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8
Q

gas

A

phase with no fixed volume or shape
- compressible

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9
Q

compressibility

A

lack of fixed volume (only a property of gases)

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10
Q

phase change

A

when substance transitions from one phase to another

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11
Q

melting/fusion

A

solid to liquid

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12
Q

freezing

A

liquid to solid

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13
Q

evaporation/boiling

A

liquid to gas

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14
Q

condensation

A

gas to liquid

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15
Q

sublimation

A

solid to gas

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16
Q

deposition

A

gas to solid

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17
Q

endothermic phase changes

A

melting, evaporating, sublimation
require heat input
breaking bonds

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18
Q

exothermic reactions

A

freezing, condensation, deposition
release heat
forming bonds

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19
Q

is bond formation exothermic or endothermic

A

exothermic

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20
Q

heat of fusion

A

point in phase change where the added heat is no longer increasing the temperature and is focused on breaking the intermolecular forces

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21
Q

heat of vaporization

A

heat required to convert liquid to gas where temperature is no longer rising and heat is focused on breaking intermolecular forces of liquid

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22
Q

specific heat capacity

A

amount of heat required to raise the temperature of one unit mass of a substance by 1 degree

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23
Q

specific heat equation

A

Q = mc ∆T
q is heat, m is mass, c is specific heat capacity

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24
Q

heat at phase changes

A

typically a ratio because temperature remains constant

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25
heat between phase changes
q= mc ∆T
26
how can a gas be converted into solid
increase in pressure or decrease in temperature
27
what phase changes are promoted by a decrease in pressure and an increase in temperature
solid to liquid liquid to gas solid to gas
28
triple point
point at which solids liquid and gases are at equillibrium
29
critical point
end of the liquid-gas interface - above this point the substance exsist as a supercritical liquid
30
high tempertaure and low pressure promotes which phase
gas
31
low temp and high pressure favors which phase
solid
32
vapor pressure
gas is in equillibrium with liquid
33
gas @ STP
volume 22.4L
34
ideal gas
1. average KE of gas molecules is proportional to temperature 2. gas particle has no volume 3. gas particles do not exert attractive forces on one another , although they do exert forces on the container they are in --> all collisions are elastic
35
when do gases deviate from ideal gas law?
at high pressure and low temperature
36
when do gases behave most ideal?
low pressures and high temperatures
37
boyle's law
pressure and volume of a gas are inversely proportional at constant temperature V1P1=V2P2
38
what happens to the pressure of a gas if the volume increases
pressure decreases
39
charles law
volume and temperature of a gas are directly proportional under constant pressure V1/T1 = V2/T2
40
what happens to the volume of a gas if the temperature is increased at constant pressure
volume with increase with temperature
41
ideal gas law
PV=nRT n is number of moles of gas R is gas constant
42
mole fraction
Ngas/Ntotal
43
partial pressure
pgas/Ptotal
44
Dalton's Law
Pgas = Xgas*Ptotal partial pressure of gas = total p * moles of gas
45
solution
homogenous mixture
46
dissolutions
solutes dissolved in solvent
47
supersaturated
excess solute not dissolved
48
crystallization
supersaturated solute creates nucleation site for solute to parcipitate out and form a cyrstal
49
molarity
mols solute/ L solution
50
molality
moles of solute/ Kg solvent
51
normality (N)
number of equivilent reactive species per liter of solution N= equivelent solute/ L solution
52
normality for acids
N = molarity * (# of H+ in acid)
53
colligative properties
vapor pressure reduction boiling point elevation freezing pt reduction osmotic pressure
54
Raoult's Law
P=XaPa p is vaport pressure of solution Pa is vapor pressure of pure solvent Xa is mole fraction of solvent
55
boiling point elevation
∆T= iKb*m - t is change in boiling point elevation - i is ionization factor - kb is boiling point constant - m is molal solute conc
56
reducing vapor pressure does what to boiling point
increases
57
what does added solute do to the freezing point
decreases
58
freezing point depression eqn
∆Tf= iKf*m
59
osmotic pressure
Π= iMRT pressure required to prevent osmosis M= n solute/ L solution
60
solubility
equillibrium process between nondissolved and dissolved forms of substance
61
equillibrium constant (Ksp)
solubility product constant [p][p]
62
high ksp
substance readily dissolves into solution
63
low ksp
largely insoluble
64
common ion effect
decrease in solubility of an ionic compound by adding a solute compound with an ion in the precipitate
65
are alkali metals soluble
yes
66
are nitrates soluble
yes
67
are chlorates soluble
yes
68
are halides soluble
yes
69
is AgCl soluble
no
70
is PbAg soluble
no
71
is HgI soluble
no
72
are carbonates (CO3 2-) soluble
no
73
PO4 2- soluble?
no
74
OH- compounds soluble?
no
75
is caoh2 soluble?
soluble
76
is baoh soluble
yes, exception to rule

MCAT chem (11 decks)

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