Electrochemistry and Nuclear Chemistry Flashcards
(49 cards)
1
Q
oxidation
A
- increase bonds to O
- lose electrons
- lose bonds to hydrogen
2
Q
reduction
A
- lose bonds to O
- gain electrons
- gain bonds to hydrogen
3
Q
the oxidation state of any element in its standard state
A
0
4
Q
ox state of group 1 metals
A
+1
5
Q
ox state of group 2 metals
A
+2
6
Q
ox state of fluorine
A
-1
7
Q
ox state of hydrogen
A
- +1 when bonded to something more electronegative than carbon
- -1 when bonded to something less electronegative than carbon
- 0 when bonded to carbon
8
Q
ox state of oxygen
A
-2
9
Q
ox state of halogens
A
-1
10
Q
ox state of oxygen family
A
- 2
11
Q
reducing agents
A
- compounds like cause others to gain electrons
- they like to get oxidized in the process
- neutral metals = low EN atoms
- LiAlH4
- NaBH4
12
Q
oxidizing agents
A
- compounds that cause others to lose electrons
- they like to get reduced in the process
- neutral nonmetals
- MNO4
- Cro3
13
Q
+E
A
- indicates a spontaneous reaction as written
14
Q
-E
A
- indicates a nonspontaneous reaction as written
15
Q
when you reverse the reaction
A
- flip the sign of E
16
Q
more negative in the reduction table
A
- means less likely to do the written reaction
- less likely to be reduced
- reducing agents because they want to be oxidized
17
Q
more positive in reduction table
A
- more likely to do the written reaction
- more likely to be reduced
- oxidizing agents because they want to be reduced.
18
Q
do the coefficients affect the value of E cell?
A
NO!
- just do Hess’s law except never multiply by coefficients
19
Q
relationship between free energy and E_cell
A
- inverse relationship
20
Q
formula for free energy and E_cell
A
ΔG = -nFE_cell
F = 96500
21
Q
Faraday’s Law
A
I = nF/t
22
Q
Galvanic cell
A
- spontaneous redox (+Ecell)
- need 2 beakers and a salt bridge
23
Q
Electrolytic cell
A
- non-spontaneous redox (-Ecell)
- has a battery to make it run
- Don’t need two beakers
24
Q
what occurs at the anode
A
- oxidation
25
what occurs at the cathode
- reduction
26
anode of a galvanic cell
- where oxidation occurs
- (-) terminal
- nonspontaneous reduction E-
27
cathode of a galvanic cell
- where reduction occurs
- (+) terminal
- spontaneous reduction E+
28
conduction wire
- flows from anode to cathode
| - current flows opposite
29
salt bridge
- completes circuit by balancing charge
30
cut wire
- instant death
31
cut salt bridge
- slow death
| - capacitor
32
run out of stuff
- equilibrium
33
increase temperature
- lose solution to evaporation
34
decrease temperature
- too viscous
35
will you ever see a metal with a negative charge on the MCAT?
- no!
36
what does iron do?
- oxidize
| - spontaneous corruption
37
what does copper do?
- reduce
| - spontaneous plating
38
where does solid metal form
- always at the cathode
39
where does H2 form
- always at the cathode
40
where does O2 form?
- always at the anode
41
anode in an electrolytic cell
- where oxidation occurs
| - (+) terminal
42
cathode in electrolytic cell
- where reduction occurs
| - (-) terminal
43
Nernst equation
- a cell in equilibrium has a non-zero standard cell potential
E=E^o - RT/nF lnQ
- a cell in equilibrium has an actual cell potential equal to zero
E^o = RT/nF lnQ
44
Iodometry
- a redox titration where the consumption of iodine indicates the titration end point.
45
alpha decay
- Helium emitted from nucleus
4
2 He
- Z decreases by 2
- atoms with very large nuclei
- least dangerous type
46
beta decay
- electron emitted
0
-1 e-
- nuclei with high ratio of neutrons to protons
- more dangerous (have a higher penetrating ability) than alpha particles
47
positron emission
0
1 e+ released by nucleus
- nuclei with high ratios of protons to neutrons
48
electron capture
0
-1 e absorbed by nucleus
- Z decrease by 1
- nuclei with high proton to neutron ratios
49
gamma decay
0
0 y emitted by nucleus
- Z stays the same
- nuclei in an excited state
- accompanies most nuclear reactions
- most dangerous type of radiation with greatest penetrating ability
