Final Exam Review Flashcards
(114 cards)
1
Q
solute
A
what is being dissolved
2
Q
solvent
A
what is doing the dissolving
3
Q
solution
A
solute and solvent combination
4
Q
non-saturated solutions
A
more solute can be dissolved in solvent
5
Q
saturated solution
A
no more solute can be dissolved at a given temperature
6
Q
super saturated solution
A
past saturation point by raising the temperature
7
Q
non miscible
A
no mixing-heterogeneous solution
8
Q
miscible
A
mixing-homogenous solution
9
Q
percent volume
A
volume solute/volume solutionx100
10
Q
percent mass
A
mass solute/mass solutionx100
11
Q
mole fraction (solute)
A
moles solute/total moles (solute and solvent)
12
Q
mole fraction (solvent)
A
moles solvent/total moles (solvent and solute)
13
Q
molarity (M)
A
moles solute/L solution
14
Q
molality (m)
A
moles solute/kg solvent
15
Q
forces of attraction
A
electrostatic network covalent h-bonding dipole-dipole dispersion
16
Q
electrostatic
A
ionic (M/NM)
-greater charge
-smaller size
=stronger force
17
Q
network covalent
A
covalent (NM/NM)
18
Q
H bonding
A
H-O
H-N
H-F
Acids act in H bonding ways
19
Q
dipole dipole
A
has a molecular dipole
20
Q
dispersion
A
has no moleculer dipole
21
Q
energetics of solutions
A
enthalpy
remember heat flows and is ever lost
22
Q
solubility of gas solutes
A
Henry’s Law: Sgas=KhPgas
(Sgas=M=moles gas/L)
(Kh=henry’s constant mol/L*atm)
(Pgas=pressure of gas)
solubility of gas is pressure dependent, higher the gas pressure the greater its solubility
solubility of a gas decreases with increasing temperature
23
Q
solubility of liquid solutes
A
raoult’s law: Psoln=XliqAPliqA+XliqBPliqB
-raoult’s law predicts ideal liquid-liquid mixtures but when predicting non-ideal mixtures the greater Psoln=the weaker the IMF and smaller the Psoln=the stronger the IMF
24
Q
solubility of solid solutes
A
Psoln=XsolventPsolvent
deltaP=XsolutePsolvent
deltaT=iKbm
deltaT=iKfm
osmostic pressure=iMRTionics dissolving separate into ionds
molecular solids dissolving do not separate
25
percent ionization
iactual/ipredictedx100
26
rate of rxn
delta[substace]/deltaT
27
average rates
aA-->bB
| rate=-1/a (deltaA/deltaT)=1/b(deltaB/deltaT)
28
rate expressions are in terms of...
SM (never PROD)
29
zero-order rate expressions
rate=k[A]^0
| horizontal line
30
first-order rate expressions
rate=k[A]^1
| [A] directly proportional to the rate of rxn
31
second-order rate expressions
rate=k[A]^2
| rate of rxn is exponentially related to the [A]
32
multiple SMs rate reaction
rate=k[A]^m[B]^n...
| overall order=sum of individual orders (m+n=overall order)
33
zero-order integrated rate law
rate=[A]t=-kt+[A]0
| t1/2=[A]0/2k
34
first-order integrated rate law
rate=ln[A]t=-kt+ln[A]0
| t1/2=0.693/k
35
second-order integrated rate law
rate=1/[A]=kt+1/[A]0
36
activation energy
ALWAYS POSITIVE
the energy that needs to be overcome to get SM's to react
-catalysts are molecules that lower activation energy
37
reaction mechanisms
tells us how a reaction proceeds from SM to PROD
- when deriving rate expression from a mechanism it is always dependent on the slowest mechanism SM's
- stoichiometry corresponds to order
38
equilibrium is when...
rate foreward is equal to rate backwards
| constant k
39
Q>K
too much product, more starting material needs to form
40
Q
too much starting material, more product needs to form
41
Q=K
in equilibrium:)
42
K>1
product is favored, more products
43
K<1
starting material is favored, more starting material
44
K=1
neither is favored, same stability
45
when writing K expressions phase is important
solids and pure liquids DO NOT appear
| gases and solutes DO appear
46
Kc
concentration (in terms of molarity)
47
Kp
pressure (in terms of pressure)
48
Ka
acid equilibria
49
Kb
base equilibria
50
Ksp
solubility equilibria (precipitation)
51
la chatlier's principle
describes how an application of stress affects an equilibrium reaction
52
pressure and volume (la chatlier's principle)
increase in pressure/decrease in volume-shift to side with less moles
decrease in pressure/increase in volume-shift to side with more moles
53
concentration of SM/PROD (la chatlier's principle)
increase SM equilibrium will shift to PROD (right)
increase PROD equilibrium will shift to SM (left)
decrease SM equilibrium will shift to SM (left)
decrease in PROd equilibrium will shift to PROD (right)
54
temperature (exothermic/endothermic) (la chatlier's principle)
Endothermic:
-decrease in temp is like a decrease in SM (shift left)
-increase in temp is like an increase in SM (shift right)
Exothermic:
-decrease in temp is a decrease in prod (shifts right)
-increase in temp is an increase in prod (shifts left)1
55
3 ways to define acid/base
arrhenius definition
bronstead-lowry definition
lewis definition
56
arrhenius definition
an acid is a source of an H+ (protons)
| a base is a source of OH- (hydroxide)
57
bronsted-lowry definition
all protons
an acid is a source of protons (H+) in solution or source of hydronium ions (H3O+)
a base is a proton acceptor, accepts H+ from solution
both need to react with water
58
lewis definition
a lewis acid accepts electrons
| a lewis base donates electrons
59
autoionization of water
water reacts with water
60
acid-base equilibria
conjugates
| acid form and base form
61
strong acids
HCl, HBr, HI, HNO3, H2SO4, HClO4
| dissociate into water (inorganic acids)
62
weak acids
CH3CO2H, H2CO3, ClCH3CO2H (R-CO2H)
do not 100% dissociate into water (organic acids)
greater # of oxygens=stronger the acid
if same # of oxygens compare electronegativity of central element...more electronegative=stronger
63
inductive effect
the more electronegative groups=stronger
| the closer the electronegative groups=stronger
64
metal hydroxides
very strong bases (inorganic bases)
[MOH] *complete dissociation*
*all are based on dissocation, so no way to qualitively rank the strong base strength*
65
amine bases
```
weak bases (organic bases)
R3N
*greater inductive/electronegativity=weaker the base*
```
66
buffer
a mixture of a parent and its conjugate initially. since both parent and conjugate are present, buffers keep constant pH
67
buffer capacity
is how much the buffer can neutralize before a pH change>1 is observed
68
buffer equilibria is written in terms of the...
parent
69
titrations
determination of an unknown [conc] of an acid or base
determination of an unkown Ka or Kb
determine molar mass of an acid or a base
70
titration curve
represents a titration where you plot pH vs volume of titrant
71
titrant
a strong acid (if titrating a base) or strong base (if titrating an acid). The strong nature ensures a quantitative instantaneous neutralization rxn
72
equivalence point
when moles of the strong titrant are equal to moles of what is being titrated
73
indicator
a molecule thats color is pH dependent. Helps in visualizing the equivalence point when doing a titration
74
slightly soluble solids
precipitation reactions
-all ionics do dissolve into water to a certain degree. If that molar solubility is greater than 0.1M, it is a very soluble salt. If less than 0.1M slightly soluble salt
Ksp=solubility product
75
predicting precipitate
will solid fall out of solution?
| Q vs Ksp
76
Q>Ksp
equilibrium shifting to SM, yes a solid will precipitate
77
Q
equilibrium shifting to PROD, no a solid will not precipitate (unsaturated solution)
78
Q=Ksp
at equilibrium, no precipitate forms (saturated solutions)
79
common ion effect
a slightly soluble solid is less soluble in an aqueous solution that already contains one of its ions (common ion) compared to that of an aqueous solution without common ion
80
fractional precipitation
precipitate one ion out selectively when two possible solids can be generated
81
entropy
the amount of randomners, or chaos in a system, surrounding, or universe
82
first law of thermodynamics
energy in the universe is constant
83
second law of thermodynamics
for a spontaneous process the entropy of the universe must be positive
84
entropy and phase change
for phase change deltaH and deltaS are related to one another via temperature
85
third law of thermodynamics
the entropy of a perfect crystal at absolute zero is equal to zero
- everything has entropy
- -gas having the highest entropy
- -liquid having a lot of entropy but less than gas
- -solid having the least entropy
- all molecules regardless of phase have entropy inherent to their structure, phase, and quantity
86
entropy rules
phase is most important
-g>l>s
solution>liquid
if all the same phase the one with more moles means greater entropy
if all the same phase and moles the more complex molecule has more entropy
87
deltaG is a temperature dependent process, spontaneity increases with increasing temperature when...
deltaH is endothermic/+ (NOT a driving force)
| TdeltaS (IS a driving force when T is + and TdeltaS is -)
88
deltaG is always negative, so this scenerio is ALWAYS spontaneous
deltaH is exothermic/- (IS a driving force)
| TdeltaS (IS a driving force when T is + and TdeltaS is -)
89
deltaG is a temperature dependent process, spontaneity increases with decreasing temperature
deltaH is exothermic/- (IS a driving force)
| TdeltaS (is NOT a driving force when T is - and TdeltaS is +)
90
deltaG is always positive, this process is ALWAYS non-spontaneous
deltaH is endothermic/+ (NOT a driving force)
| TdeltaS (is NOT a driving force T is - and TdeltaS is +)
91
Keq>1
PROD favored deltaG equilibrium is negative
92
Keq<1
SM favored deltaG equilibrium is positive
93
deltaG standard state
25*C, 1 atm, 1m,
94
reduction
gaining of e- by an element
95
oxidation
loss of e- by an element
96
OILRIG
Oxidation Involves Loss/
| Reduction Involved Gain
97
balancing redox reactions
balance out elements besides H and O first
balance out oxygen atoms by adding H2O
balance out hydrogen atoms by adding H+
if under basic conditions add the sam # of OH- as H+ to both sides
balance charge by adding electrons
98
standard hydrogen electrode
this is the potential for H+ to be reduced. this is the standard for all other reduction potentials
99
inert electrodes
they do not influence Ecell, only supply a surface for e- to flow...common use is when reduction or oxidation is occuring completely in solution
Pt or Pd are perfect examples of inert electrodes
100
Ksp and redox
a redox process that produces a slightly soluble solid. use redox E*cell or Ecell to help in determining a Ksp...or vice versa
101
electrolysis
this is a redox process that is non-spontaneous, e- or charge needs to be applied to allow for chemistry to occur. the amount a substance can be reduced is directly related to current flow and the amount of time the current is applied for
102
becquerel
discovered radioactivity but coied it as "uranic rays"
103
curie
postdoc of becquerel and started to look for other sources of "uranic rays" she discovered polonium and also radium
104
beta particles
results from a neutron turning into a proton and an electron
lower ionization then alpha particle
greater penetration power than alpha particle
105
alpha particle
results from highly unstable nuclides
tough to predict
highest ionization power
lowest penetration power
106
gamma particles
usually emitted with other forms of radioactivity
no mass/charge=hard to know how they are produced
lowest ionization power
highest penetration power
107
positron particles
results when a proton turns into a neutron and a positron particle is emmitted
same ionization and penetration power as beta particles
108
k capture
an electron is absorbed into nucleus and reacts with a proton producing a neutron
109
predicting stability and decay process
1) alpha particles are difficult to predict, often result from a large deviation in the stable neutron/proton ratio
2) beta particles are produced when the neutron/proton ratio is too large (too many neutrons)
3) positron emmissions (particles ) are produced when the neutron/proton ratio is too small (too few neutrons)
110
transmutation
is the nuclear reaction of more than one SM nuclide to produce more than one PROD nuclide
111
stepwise decay processes
decay processes that can produce more then one type of particle...same rules of balancing with atomic mass and atomic charge
radioactive decay=always first order process
112
fission
occurs from splitting apart of large unstable nuclides (atomic #>80). not all nuclides are fissionable, often a fissionable nuclide is generated via neutron bombardment. fission splits a large nucleus into smaller nuclei as well as generating massive amounts of energy, as well as other small particles
113
binding energy
converting mass into energy
| very small=in amu
114
fusion
the combining of two small nuclei to create slightly larger nuclides. this is what is occuring in the sun
