Exam 2 Flashcards
exam 2 (115 cards)
1
Q
molality
A
moles solute/kg solvent
2
Q
Strong electrolyte
A
disassociate completely into ions
ex: strong base/acids
Ex: SALTS
3
Q
weak electrolyte
A
Only forms few ions
examples: Acetic acid
4
Q
non electrolytes
A
no ions formed in solution
ex: Alcohols -end in ol
5
Q
Sugar
A
non electrolyte
6
Q
ethylene
A
non electrolyte
7
Q
ethanol
A
non electrolyte
8
Q
glycol
A
non electrolyte (no ions formed)
9
Q
urea
A
non electrolyte
10
Q
H2SO4
A
Strong acid
11
Q
KOH
A
STRONG base🍌
12
Q
HCLO4
A
Strong Acid
13
Q
Ba(OH)2
A
Strong Base
14
Q
HBr
A
Strong Acid
15
Q
NaOH
A
Strong Base
16
Q
HNO3
A
Strong Acid
17
Q
HF
A
Weak acid
18
Q
LiOH
A
Strong base (Logan)
19
Q
CH3COOH
A
Weak acid (acetic acid)
20
Q
HClO3
A
Strong Acid
21
Q
Ca(OH)2
A
Strong Base
22
Q
RNH2
A
Weak base (any amine)
23
Q
Sr(OH)2
A
Strong base
24
Q
NH3
A
Weak base (ammonia)
25
H3PO4
Strong Acid
26
HI
Strong Acid (HI!!)
27
HCl
Strong Acid
28
Trend between EN and acid strength
Higher EN, stronger acid
⬆️➡️
29
Trend between EN and base strenght
Higher EN, Weaker Base
30
definition of osmotic pressure
Osmotic pressure is the pressure needed to stop water from flowing across a semipermeable membrane into a solution.
31
Henry's law
C=kP
* C_gas = k_H * P_gas
P is the partial pressure of the gas above the liquid
k changes on teh substance
C is the concentration of the gas dissolved in the liquid
32
How does equilibrium reached above a substance through partial pressure
Equilibrium reached when the
pressure produced by the solvent
height balances the pressure of
solvent molecules moving through
the membrane
33
Deviations from Raoul's law
when the IMF between teh molecules are significantly different
34
Positive deviation from Raolt's law
when IMF are weaker between molecules
35
Negative deviaton from Raoult's law
When IMF are stronger between molecules
36
When Raoul's law is Raolut's law
When the IMF between teh substances are similar
37
Ranking the strengths of IMF
1. Ionic
2.Hydrogen (H attached to NOF interacting with NOF on other molecule)
3. Dipole dipole
4. London dispersion
38
when vapor pressure changes...
The identity of the solute doesn't matter
39
Colligative properties
Colligative properties depend only on the
concentration of solute particles, not their
identity or properties
40
average rate =
∆[]/∆t
41
inst rate
average rate between two time periods
42
Bronstead Lowry acid
Acid: donate Hydrogen
Base: receive hydrogen
43
ph =
ph = -log[H_eq]
44
pH + pOH =?
14
45
arhenius acid
produces H
HCl -> H + Cl
46
Arhenius base
increase OH concentration
NaOH -> Na + OH
47
why do buffers resist changes in pH
buffer: Weak acid+conjugate base or weak base + conjugate acid
This allows the buffer to absorb excess OH or excess H without a change in pH
48
purpose of titration
To determine the concentration of an unknown solution
49
Equivalence point
all of the analyte has reacted with our titrant
50
n type semiconductor
when something is doped with extra electrons, like phosphorous, so there are more electrons
51
p type semiconductor
doping something that has more electrons with something that has less electrons. doping Si with B.
52
30.0% w/v
30g/100mL
53
rate of appearance and rate of disappearance are always +
big facts
however rate of change CAN and WILL be negative for prdocur going away
54
how to do rate law
Find the slowest rate
rate = k[reactants]^coefficient[reactants]^coefficient...
*once we find the slowest rate, this is our rate, but we can't have intermediates in our equation
55
β decay
We are adding one proton, misusing a neutron
beta
211, 82Pb -> 211, 83Bi + 0, -1 e
56
Positron emission
We are minussing a proton, but adding a neutron
50, 25Mn->50,24Cr + 0, 1 e
57
Electron capture
minus a proton, keep total count the same(adding a neutron)
179,74,W + 0, -1 e-> 179,73Ta
58
⍺ decay
230, 90 Th -> 286, 88 Ra +4,2 He
59
how do we find the change of mass in breaking up a nucleus
Find the initial mass in Kg (change the total amu of the nucleus given, put into kg. Then find the mass of each proton and neutron in kg. Then minus the two
60
the order of alpha decay, beta decay, and electron capture
1st order
61
the order of positron emission
second order
62
can we put grams in for the concentrations in decay orders
Oh yes you can!
63
equilibrium equation
k = products^coeffiecients/reactants^coefficients
don't include pure liquids or solids in the equilibrium equation
64
If Q is bigger than k, reaction proceeds to the ...
left
65
Le Chat when total volume increases
equilibrium will shift towards the side with more moles of gas
66
What is ∆G at equilibrium
ZERO man
67
pX = -log(x)
facts
68
generic reaction at equilibrium for a weak base
B(aq) + H2O(l) -><- BH(aq) + OH-(aq)
69
pKa +pKb = ?
14.0
70
how to find coordination nu per
coordination number equals the number of bonds INSIDE THE BRAKCET
[Pt(NH3)6]Cl4, Coord. number = 6
71
bi dentate atoms
gly C2H5O2
en C2H8N2
CO3
72
Amount of stereoisomers [MA6] [MA5B]
zero
73
[MA4B2] [MA3B3]
2 stereoisomers
can have both cis and trans isomers
74
[MA2B2C2] [M(en)2B2] & [M(en)3]
cis compounds that can have enantiomers
75
Charge of Ammonia
NH3 zero (NH4 is +1)
76
charge of sulfate
-2
77
Strong Field ligand
large ∆_o (splitting energy)
low spin
78
weak field ligand
smaller ∆_o (splitting energy)
higher spin
79
low spin
low wavelength of absorption
80
high spin
high wavelength of absorption
81
If we are putting energy into the system
Potential energy of the cell for the cathode will be more negative, as we are putting in energy and will run in the reverse direction
82
VB and CB overlap
conductor
83
medium band gap
semi conductor
84
high band gap
insulator
85
higher vapor pressure
more volatile
86
Smaller molecule
weaker IMF
87
Relation between IMF and vapor pressure
vapor pressure ⍺ 1/IMF
88
How do we find partial pressure amidst volatile substances
Pttl(including volatile substances in theory) (vapor pressure) = 𝛘_non volatile substance1 * P_non volatile substance
We do not add theχP of the volatile substances
89
change in BP / FP is dependent on
amount of ions in solution, want Hoff factor
90
graph of zero order
linear when y = [A]t
91
graph of 1st order
linear when y = ln[A]t
92
graph of 2nd order
linear when 1/[A]t // x axis is t
93
Collision theory
The order of molecules, or the direction f molecules determines the speed of reactions
94
what is the fastest reaction?
The one with the lowest activation energy, or the one with the lowest activation energy, not dependent on energy starting with
95
What type of decay will happen according to the situation: neutron rich
beta decay
96
What type of decay will happen according to the situation: nuetron poor
positron emission or electron capture
97
What type of decay will happen according to the situation: large nuclei
alpha decay
98
1 Sievert (Sv)
J/kg
99
when ∆Gº >0, keq is
<1
100
when ∆Gº < 0, keq is
>1
101
Strong base + strong acid titration
go to H + OH -> H2O
do ICF to find how many moles will be left over after full reacts
Convert to molarity, use pH = -log[H]
102
non volatile:
can't turn to gas
103
what happens to vapor pressure of a volatile substance when we dilute it with a non volatile substance?
The partial pressure decreases
104
what order are decay problems?
1st order
105
for graph of free energy
products and reactant needs ot be at the same level, the catalase decreases activation energy
106
if we have more oxygen atoms, it will make a stronger acid
acid strength: HBrO < HClO < HClO2
107
What way do you want the reaction to go to increase solubility?
to the right
108
Common Ion effect
When we add an ion to an ionic solution, there solubility goes down
109
weaker field strength
high spin (goes to top level, not paired up)
weak energy
high wavelength
110
simple
atoms = 1
neighbors = 6
l , a = 2r
aaaaa
lattice: simple cubic
111
body centered
atoms = 2
neighbors 8
a = 4r/√3
ababab
lattice: body centered
112
fcc
atoms 4
neighbors 12
c = 4r
abcabc
lattice: cubic closest packed
113
Rock Salt Ionic Crystal lattice structure
atoms: 8
Nearest neighbor: 6
a = 2(r1 + r2)
114
What doesn't change the orientation of the unit cell
if the radius is the same
If the SOLUTE is small enough to fit into the crevices of the SOLVENT's unit cell
115
When titrating weak acid + strong base
The strong base kills the
A + OH -> A- + H2O
do ICF table with this, then flip to RICE table with A- + H2O -> A + OH
Find the concentration of OH
