Test 4 Flashcards
1
Q
Heterogeneous mixtures
A
- not uniform
- properties vary with sample
2
Q
homogeneous mixtures
A
- uniform
- every sample is the same
3
Q
solute
A
- substance being dissolved
- present in smallest amount
4
Q
solvent
A
- substance doing the dissolving
- present in largest amount
5
Q
molarity
A
mol/L
6
Q
moles
A
volume * concentration
7
Q
▲Hsoln=
A
▲Hsolute+▲Hsolvent+▲Hmixture
8
Q
hydrophilic
A
polar molecules
9
Q
hydrophobic
A
non-polar molecules
10
Q
polar solution
A
polar molecule will dissolve
11
Q
nonpolar solution
A
nonpolar molecule will dissolve
12
Q
cations (+)
A
migrate to the negative electrode
13
Q
anions (-)
A
migrate to the positive electrode
14
Q
electrolytes
A
substances whose aqueous solutions conduct electricity: ions, ionic and SA
15
Q
nonelectrolytes
A
substances whose aqueous solutions do NOT conduct electricity: Molecules
16
Q
K=
A
products over reactants
17
Q
coulomb’s law
A
F= kq1q2/er^2
18
Q
when q1 and q2 > 1
A
ionic solids with ions have a high charge, insoluble
19
Q
when q1 and q2 = 1
A
ionic solids with ions have a low charge, soluble
20
Q
Ions 0.01-0.10 M
A
moderately soluble
21
Q
ions > 0.10 M
A
soluble-no precipitate
22
Q
Ions < 0.01 M
A
insoluble, forms precipitate
23
Q
oxidizing agent
A
gaining electrons, oxidation # decreases, reduction half rxn
24
Q
reducing agent
A
losing electrons, oxidation # increases, oxidizing half reaction
25
reduction 1/2 rxn
electrons on reactant side
26
oxidation 1/2 rxn
electrons on product side
27
spontaneous redox reactions
electrons fall downward
28
nonspontaneous redox reactions
electrons go up
29
best oxidizing agent
lowest energy empty orbital
30
best reducing agent
highest energy full orbital
31
▲G=
-n*F*Ecell
32
n=
moles of electrons transferred in a redox reaction
33
E=
Ecathode-Eanode
34
▲Ecell=
Efinal-Einitial
35
reduction compartment
the one with the cathode
36
oxidizing compartment
the one with anode
37
electrode with metal
should be the same element and charge
38
electrons should transfer
from anode to electrode
39
compartments matter
on where the anode and cathodes are
40
Erxn =
Either Ered-Eox or Efinal-Einitial
41
highest voltage
cathode, on bottom
42
lowest voltage
anode, on the top
43
LEO says GER
```
Losing
Electrons
Oxiding
Gaining
Electrons
Reducing
```
44
salt bridge cations
migrate to the cathode
45
salt bridge anions
migrate to the anode
46
cathode electrode
grows
47
anode electrode
shrinks
48
cathode compartment
decreases
49
anode compartment
increases
50
building redox reactions
only use molecules in reactants
51
if you can hold the metal
the oxidation state is zero
52
ines are
an oxidation state of zero
53
ides are
an oxidation state of one
54
galvanic cell
spontaneous, chemical energy to electrical energy
55
electrolytic cell
non-spontaneous, electrical energy to chemical energy
56
wanted redox chem
batteries, rechargeable batteries, electrolytic cells
57
unwanted redox chem
corrosion
58
unwanted redox chem
corrosion
59
alkaline batteries
Zn, OH, MnO2, H2O
60
Button Battery
Zn, OH, Ag2O, H2O
61
Car Battery
Pb, SO4, PbO2, H
62
galvanic cell when discharging
positive voltage
63
electrolytic cell when recharging
negative voltage
64
lithium-ion battery
holds the most watt-hours per kg
65
nickel-metal hydride
medium watt-hours per kg
66
lead-acid battery
lowest watt-hours per kg
67
corrosion
O2, H+, Fe,
68
corrosion passivation
H+,O2, Al,
69
Copper Passivation
H2O, CO2, H2CO3
70
Galvanization
Protecting metal by using a more reactive one, instead of Fe-O2, main rxn is Zn-O2
71
gold plated metal
Au+Sn
72
electrolysis (used to extract many metal from their ores)
Ca+Cl
73
hydrogen powered vehicles
H2+O2=H2O
74
Arrhenius acid
produce OH^- in water
75
Arrhenius Base
produce H^+ in water
76
Lewis acid
electron pair acceptor, normally has less than 4 regions
77
Lewis base
electron pair donor, normally has base pairs
78
Bronsted acid
proton donor
79
Bronsted base
proton acceptor
80
deprotonation
remove an H and make the charge -1
81
protonation
addition of an H and make the charge 1+
82
amphiprotic
both an acid and a base
83
ide ion
hydro_ic acid
84
ate ion
_ic acid
85
ite ion
_ous acid
86
for all acid names
dont forget per or hypo
87
K>1
dangerous, should leave room
88
K<1
we're going to be fine
89
Strong acids
donates proton easily, smaller amount of electron density holding proton on
90
Weak acid
holds on to proton, has larger amount of electron density holds on to proton
91
Strong Base
has larger amount of electron density to grab proton
92
Weak base
has smaller amount of electron density to hold on to proton
93
weaker the bond
stronger the acid
94
stronger the bond
weaker the acid
95
lower bond energy, bigger element
stronger the acid
96
more polar the bond
stronger the acid
97
thicker bond line is
more electron density there is
98
more oxygens
stronger the acid
99
less oxygens
weaker the acid
100
more electronegative center acid
stronger acid
101
less electronegative atom
weaker acid
102
more electronegative
weaker base
103
less electronegative
stronger base
104
more electron density
stronger base
105
less electron density
weaker base
106
anything above H3O+ on acid/base table
is a strong acid and strong electrolyte
107
Strong acids
large products over small reactants, K>1
108
weak acids
small products over large reactants, K<1
109
anything below H3O+ and above H2O on acid/base table
weak acid and weak electrolyte
110
anything under H2O on acid/base table
not really an acid, conjugates are strong bases
111
no bubbles
very negative exponent
112
some bubbles
medium negative exponent
113
lots of bubbles
positive exponent
114
Krxn
Ka(reacting)/Ka(produced)
115
1A (Ionic Salt)
Cation and Anion
116
1A (Strong Acid)
H3O+ and conjugate base
117
1A (Weak Acid)
write weak acid
118
1B (Strong Base)
OH1 and conjugate acid
119
1B (Weak Base)
weak base and counter ion
120
2
Decide if species can act as acids and bases, eliminate spectator ions
121
3
Strongest acid and base on reactant side
122
4
Conjugate base and acid on product side
123
double arrow
K<10^3
124
single arrow
K>10^3
