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Princeton Chemistry > Electrochemistry and Nuclear Chemistry > Flashcards

Electrochemistry and Nuclear Chemistry Flashcards

1
Q

oxidation

A
  • increase bonds to O
  • lose electrons
  • lose bonds to hydrogen
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2
Q

reduction

A
  • lose bonds to O
  • gain electrons
  • gain bonds to hydrogen
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3
Q

the oxidation state of any element in its standard state

A

0

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4
Q

ox state of group 1 metals

A

+1

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5
Q

ox state of group 2 metals

A

+2

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6
Q

ox state of fluorine

A

-1

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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
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8
Q

ox state of oxygen

A

-2

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9
Q

ox state of halogens

A

-1

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10
Q

ox state of oxygen family

A
  • 2
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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
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12
Q

oxidizing agents

A
  • compounds that cause others to lose electrons
  • they like to get reduced in the process
  • neutral nonmetals
  • MNO4
  • Cro3
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13
Q

+E

A
  • indicates a spontaneous reaction as written
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14
Q

-E

A
  • indicates a nonspontaneous reaction as written
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15
Q

when you reverse the reaction

A
  • flip the sign of E
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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
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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.
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18
Q

do the coefficients affect the value of E cell?

A

NO!

  • just do Hess’s law except never multiply by coefficients
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19
Q

relationship between free energy and E_cell

A
  • inverse relationship
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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
Q

what occurs at the cathode

A
  • reduction
26
Q

anode of a galvanic cell

A
  • where oxidation occurs
  • (-) terminal
  • nonspontaneous reduction E-
27
Q

cathode of a galvanic cell

A
  • where reduction occurs
  • (+) terminal
  • spontaneous reduction E+
28
Q

conduction wire

A
  • flows from anode to cathode

- current flows opposite

29
Q

salt bridge

A
  • completes circuit by balancing charge
30
Q

cut wire

A
  • instant death
31
Q

cut salt bridge

A
  • slow death

- capacitor

32
Q

run out of stuff

A
  • equilibrium
33
Q

increase temperature

A
  • lose solution to evaporation
34
Q

decrease temperature

A
  • too viscous
35
Q

will you ever see a metal with a negative charge on the MCAT?

A
  • no!
36
Q

what does iron do?

A
  • oxidize

- spontaneous corruption

37
Q

what does copper do?

A
  • reduce

- spontaneous plating

38
Q

where does solid metal form

A
  • always at the cathode
39
Q

where does H2 form

A
  • always at the cathode
40
Q

where does O2 form?

A
  • always at the anode
41
Q

anode in an electrolytic cell

A
  • where oxidation occurs

- (+) terminal

42
Q

cathode in electrolytic cell

A
  • where reduction occurs

- (-) terminal

43
Q

Nernst equation

A
  • 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
Q

Iodometry

A
  • a redox titration where the consumption of iodine indicates the titration end point.
45
Q

alpha decay

A
  • Helium emitted from nucleus

4
2 He

  • Z decreases by 2
  • atoms with very large nuclei
  • least dangerous type
46
Q

beta decay

A
  • electron emitted

0
-1 e-

  • nuclei with high ratio of neutrons to protons
  • more dangerous (have a higher penetrating ability) than alpha particles
47
Q

positron emission

A

0
1 e+ released by nucleus

  • nuclei with high ratios of protons to neutrons
48
Q

electron capture

A

0
-1 e absorbed by nucleus

  • Z decrease by 1
  • nuclei with high proton to neutron ratios
49
Q

gamma decay

A

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

Princeton Chemistry (6 decks)

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