ACS final exam ALL topic review Flashcards
1
Q
molarity
A
moles of solute/ Liters of solution
2
Q
molality
A
moles of solute/ Kg solution
3
Q
mass %
A
(mass solute/ mass solution)x100 (solution is solute+solvent)
4
Q
mole fraction (Xa)
A
moles of A/ total moles of solution (mol A+mol B)
5
Q
ppm
A
(moles solute/mass solution) x10^6
6
Q
osmotic pressure
A
iMRT (i=van’t hoff, T=temp in Kelvin, M is molarity, and R is 0.08206)
7
Q
freezing point (∆Tfp)=
A
Kfp x molality x i (∆Tfp is pure freezing point - freezing point of the solution)
8
Q
boiling point (∆Tbp)=
A
Kbp x molality x i (pure Bp + ∆Tbp=kbp)
9
Q
as the amount of particles increase in a solution (relating to bp,vp, osmosis)
A
the bp and osmotic pressure increase
the vp decreases
10
Q
osmosis flows
A
from low solute to high solute concentration
11
Q
Psolution
A
Pressure x mole fraction of the solvent
12
Q
vol %
A
(volume of solute/ vol of solution) x100
13
Q
hydrogen bonds form with
A
-EN atoms usual N,O,F with a lone pair
14
Q
hydrogen bonds and IMF relationship
A
-hydrogen bonds are the strongest IMF
-are a special type of dipole-dipole force
15
Q
when establishing how well a compound will dissolve in a solution (relating to IMFs)
A
-“like dissolves like”
-atoms with similar IMFs will be able to bond and dissolve better with similar IMFs
ex) ethanol (CH3CH2OH), dissolves better in a solution with one hydrogen bond rather than a solution with 2 hydrogen bonds or no hydrogen bonds
16
Q
more carbons in an organic compound
A
-more carbons=more “oil like”
-the more “oil-like” it is, the more is will dissolve better in oil than water
ex) C22H2OH is more oil like than C2H3OH because it has more carbons, thus dissolves better in oil
17
Q
when deciding what is a solute and what is a solvent, the compound in greater excess is the…
A
solvent
18
Q
how is a super saturated solution made?
A
1) heat up solution 2) add more solute 3) let cool 4) supersaturated solution
19
Q
Henrys law
A
C=Kh x P
c=concentration
kh=henrys constant
p=partial pressure
20
Q
osmotic pressure increases with
A
increasing # of particles, increasing bp, higher molar mass, decreasing volume (at constant temp), and a higher van’t hoff factor
21
Q
semipermeable membrane allows
A
only water to pass through, moving to the more concentrated side, diluting it
22
Q
breaking a bond is
A
endothermic
23
Q
making a bond is
A
exothermic
24
Q
non-polar bonds
A
linear, trigonal planar, tetrahedral, trigional biprymidal, octahedral, square planar
-only non polar if all the terminal atoms are the same, if they are different, then they are polar
25
every molecule has this IMF
LDF
26
IMF with a non-polar and polar molecule
dipole-induced dipole
27
IMF with 2 polar moleules
dipole-dipole
28
IMF with and Ion and a polar molecule
ion-dipole
29
IMF with H and N,O,F
hydrogen bond
-type of dipole-dipole
30
Ion-dipoles have the
highest boiling points
31
as IMF increases, the enthalpy of vaporization ____ and the rate of vapor pressure _____
-increases (directly related to IMFs)
-decreases (indirectly related to IMFs)
32
FCC information
-CN is 12
-holds 4 atoms
33
BCC information
-CN is 8
-hold 2 atoms
34
Simple cubic unit information
-CN is 6
-holds 1 atom
35
molecular solids
-low melting points
-weak IMFs
-soft, and poor conductivity
36
covalent network solids
(C, dimond/graphite), SiO2
-high melting point
-hard
-poor conductors
37
ionic solids
-held by ion-ion forces
-non conducting
-hard
-high melting point
38
metallic soilds
-held by a "sea" of e-
-conducting
-variable melting point and hardness
39
rate constant expression
=k[reactants]
40
when finding the rate expression with trails given...
chose where the reactants have the same M for one compound and a different for the other compound to find what coefficient the compound is raised to
41
1st order rate law
ln([At]/[A0])=-kt
42
1st order 1/2 life
ln(2)/k
43
1st order graph info and units
- ln[A] vs Time
- negative slope
- seconds inverse
44
second order graph and information
-positive slope
- 1/[A] vs Time
- m^-1 x s^-1
45
zero order graph information and units
-negative slope
- [A] v Time
- M/s
46
rate law equation for zero order
[At]= -kt +[A0]
47
rate law equation for second order
1/[At]= kt + 1/[A0]
48
zero order 1/2 life
[A0]/2k
49
second order 1/2 life
1/ k[A0]
50
exothermic rate graph: way to mem. it
reactants over products is odd so (-)
51
endothermic rate graph: way to mem. it
products over reactants is normal/positive (+)
52
when a catalyst is added
-it changes the rate of mechanism
-speeding up the rate of reaction to follower a faster path
53
is concentration related to K (for kinetics)
no, not really
54
at constant temp, according to the Arrhenius equation, reactions with a lower Ea proceed
-more rapidly
-fewer collisions are needed at low Ea, so with a lower Ea more molecules can hold the potential which can increase the rate of the reaction
55
endothermic K and T for kinetics
-they are directly related
-so if T increases, then K increases, speeding up the reaction
56
as T increases in a kinetic reaction, molecules move ____ and have more ____ which_____ because that is needed to ____ the Ea
as temp increases, more molecules move faster and have more kinetic energy which increases the # molecules w/ energy needed to overcome the Ea
57
Arrhenius equation
ln(k2/k1)= -Ea/R (1/T2 - 1/T1)
58
the slow step in a kinetic reaction is
the rate determining step
(what you make a rate expression for)
59
catalysts START as a ____ and END as a ____
start as a REACTANT and end as a PRODUCT
60
intermediates START as a ____ and END as a ____
start as a PRODUCT and end as a REACTANT
61
for equilibrium
-concentrations are constant
-the rate of the forward and the reverse reaction are equal
-the reaction is still ongoing, it doesn't stop
62
for Kc and Kp, how do you write the expression?
concentration/pressure of the products raised to their coefficient divided by the concentration/pressure of the reactants raised by their coefficient
-only gases and aqueous elements are involved in the K expression
(NOT solids or liquids)
63
the equilibrium constant can tell us
-the extent of the reaction
-the direction of the reaction
-quantity of products/reactants remain at equilibrium
(It does NOT tell us anything about time)
64
when k>>1
-reaction is product favored
-reaction moves to the right
-at equilibrium, products will be in greater concentration
65
for Hesses law dealing with K and equilibrium
-when you want to reverse something you raise it by -1 (inverse it)
-when you multiply something you raise it by what you are multiplying by
-the overall K is all the Ks multiplied together
66
when k << 1
-the reaction moves to the left
-it is reactant favored, meaning reactants will be in greater concentration at equilibrium
67
if a reaction is exothermic, what is the relation between K and T
-inversely related
-the reaction releases heat so Temp decreases as you increase K
application) if you decrease T, you are increasing K which is making the reaction move to the right, making more products
68
if Q>K
odd, so you move to the left, to the reactants
69
if Q
normal, so you move to the right, to the products
70
going from a gas to a liquid is _____ spontaneous than going from a liquid to a gas
LESS
71
endothermic reactions, the K and T have a
direct relationship
72
to move to the products in a endothermic reaction K and T
are both increasing
73
to move to the products in an exothermic reaction K and T
are inverse
T must decrease and K must increase for the equilibrium to shift right
74
at constant volume: changing pressure
shifts equilibrium to the side with fewer moles of gas to counteract the change
75
adding products/reactants to an equation
equilibrium shifts away from the side that is being added to and goes to the side being taken out
76
at constant pressure if volume decreases
pressure increases and shifts to the side with fewer moles of gas
77
Lewis acid definition
a lewis acid will accept e- pairs
78
Lewis base definition
a lewis base will donate e- pairs
-must have a non-bonding lone pair to give away to the acids
79
bronsted lowry acid
donates a H+ ion
80
bronsted lowry base
accepts an H+ ion
81
in pure water Kw=
[H3O+][OH-]
82
Kw (with ka and kb)=
Ka x Kb
83
henderson hasslebach equation is____ and is used when
PH= PKa + log (conj/acid)
-used when there is left over of the acid/base and its conjugate acid/base
84
when the Ka or Kb is small
-the acid/base reaction is most likely reactant favored and equilibrium moves to the left
85
oxyacid trend
-the acidity of an oxyacid increases with the number of oxygens apart of the compound
86
binary acid trend
-binary acids increase in acidity with an EN central atom, a large central atom, and the conj base stability
-the longer the H bond (relating to atomic size), the easier it is to donate the H+ ion, meaning it is more acidic
87
the Keq>1
-reaction is product favored because more reactants are present than products so equilibrium pushes to the right to increase product concentration
88
for acids and bases: equilibrium moves to the side with the
weaker acid/base
89
basic PH is ____ than an acidic PH
higher
90
POH+PH=
14
91
how can you tell what the PKa is looking at a PH curve?
PKa= 1/2 equilivance point
92
strong acids and bases...
-dissociate completely
-are strong electrolytes
-have neutral anions/cations when in water
ex) HCl + H2O---> H3O+ +Cl- (the Cl- is neutral and plays no extra part in the PH)
93
Qsp
-the reaction moves to the right, making more products = no precipitate
-solution is unsaturated
94
Qsp>Ksp
-the reaction moved to the left, making more reactants = precipitate
-solution is saturated (can be unsaturated?)
95
Qsp=Ksp
-solution is at equilibrium=no precipitate
-solution is saturated
96
Ksp expression
-the ions raised to their coefficents
ex) the ksp= [X^m]^n[Y^m]^n
97
for Keq hesses law
-same as K
-if needing to be reversed, inverse K
-if needing to multiply, raise K to the value you want to multiply with
-Ks are multiplied together
98
larger Ksp=
more M or solubility
99
when comparing different compounds Ksps
you need to have the same number of ions
100
common ion effect
decreases solubility of the ion you are adding, can cause ion to be precipitated out
101
K is usually impacted or changed with
change in temperature
102
enthalpy
∆H
103
entropy
∆S
-the measure of randomness or disorder
104
Gibbs free energy ∆G with ∆S and ∆H equation
∆G= ∆H-T∆S
105
∆G relating with K
∆G = ∆G degree +RTlnK
OR (without ∆G degree)
∆G= -RTlnK
106
∆S will more positive if
-gases are more present (solids and liquids have less entropy in this order g>l>s)
-more product than reactant
107
∆S will be negative if
-there are fewer gases or if gases condense or disappear from equation
-more reactant than product
108
When ∆H and ∆S are (+)
spontaneous at high temperatures
109
when ∆H and ∆S are (-)
spontaneous at low temperatures
110
when ∆H is (+) and ∆S is (-)
the reaction is nonspontaneous
111
when ∆H is (-) and ∆S is (+)
the reaction is spontaneous
112
molar entropy increases with
increase number of gases from reactant to product
-so product has more gases than the reactants
113
entropy increases with temperature b/c
there is more energy states available at higher temperatures
114
dissolving something is a ____ process
spontaneous
115
deposition (g-->s)
nonspontaneous
116
evaporating/vaporization (l-->g)
spontaneous
117
condensation (g-->l)
nonspontaneous
118
largest entropy change in states of matter is
solid to a gas (deposition)
119
freezing water is
nonspontaneous
120
when more molecules are breaking apart, or dissolving, the entropy
increases
121
combustion is usually
nonspontaneous
122
since O2 gas is naturally occurring ∆Gf is
0
123
spontaneous processes always have
∆G<0 (-)
124
as K increases (w/ ∆G)
∆G is more (-)
-more spontaneous
125
as K decreases (w/∆G)
∆G is more (+)
-less spontaneous, more nonspontaneous
126
reduction is the ____ of electrons
GAINING of e-
the oxidation number DECREASES
127
oxidation is the ____ of electrons
LOSS of e-
the oxidation number INCREASES
128
the cathode happens at the
reduction site
-pushes e- out
129
the anode happens at the
oxidation side
-pulls e- in
130
in a galvanic cell the electrons flow
from the anode to the cathode
131
the mass of the anode____ and the mass of the cathode ___
anode: decreases
cathode: increases
132
negative ions go to the ____ and positive ions go to the____
negative ions go to the ANODE
positive ions go to the CATHODE
133
Ecell
Ecathode - Eanode
134
Nerst equation for Ecell
Ecell - 0.0591/n xlogQ
n=number of e-
135
for oxidation the e- are on the
right (anode)
136
for reduction the e- are on the
left (cathode)
137
a higher E is associated with
reduction/cathode
138
a lower E is associated with
oxidation/anode
139
∆G and Ecell are related how?
When ∆G is more (-) Ecell is more (+)
when ∆G is more (+) Ecell is more(-)
140
if Ecell is 0 then
Q=K
141
E =
Ecell degree - 0.0592/n logQ (prod/reactants or cathode/anode)
142
alpha decay
4/2He
-most ionizing, least penetrating
-atomic number decreases by 2 and mass number decreases by 4
143
beta decay
0/1B
-more penetrating but less ionizing than alpha decay
-atomic number increases by one but atomic mass remains the same
144
gamma emission
-lease ionizing, most penetrating
-no change in mass number or mass weight, usually causes no change to a different element
145
poistron
0/+1e
-plus one charge but does not change the atomic mass
-atomic number decreases by one but the atomic mass remains the same
146
electron capture
0/-1e
-electron in outer orbital is pulled into nucleus
-atomic mass stays the same but atomic number decreases by one
-
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