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MCAT chem > redox and electrochemistry > Flashcards

redox and electrochemistry Flashcards

1
Q

oxidation

A

lose e-

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2
Q

reduction

A

gain e-

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3
Q

redox reactions

A

e- are transfrered and one molecule gains e- while one loses e-
- oxidation state of compounds changes

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4
Q

oxidation state

A

measured using oxidation numbers
- keep track of how e- are shared in a molecule
- model of electron distribution where e- is given to most eneg atom

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5
Q

oxidation state rule for pure atoms

A

pure elements in natural form like diatomics have an oxidation state of 0
ex: o2

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6
Q

what is oxidation state of monoatomic ion

A

its charge
ex: mg is 2+

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7
Q

what is true about the sum of oxidation states among atoms in a molecule

A

they add up to the overall charge of the molecule

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8
Q

oxidation state of F

A

-1, oxidizing agent

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9
Q

oxidation state of most halonges

A

-1

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10
Q

what is oxidation state of cholrine in HClO4

A

+7

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11
Q

oxidation state of hydrogen

A

usualyl 1+ unless bonded to a more electropositive atom like NAH and LIAlH

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12
Q

oxidation state of oxygen

A

usually -2 unless peroxide, then its -1

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13
Q

oxidation state of alkali metals

A

1+

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14
Q

oxidation state of alkali earth metals

A

2+

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15
Q

nonredox reactions

A

overall, the distribution of e- does not change
acid base, subsitution reactions, precipitation reactions , double displacement reactions

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15
Q

nonredox reactions

A

overall, the distribution of e- does not change
acid base, subsitution reactions, precipitation reactions , double displacement reactions

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15
Q

nonredox reactions

A

overall, the distribution of e- does not change
acid base, subsitution reactions, precipitation reactions , double displacement reactions

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15
Q

nonredox reactions

A

overall, the distribution of e- does not change
acid base, subsitution reactions, precipitation reactions , double displacement reactions

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16
Q

classic redox

A

single displacement

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17
Q

is combustion a type of redox

A

yes
something + 02 –> co2 + h2o

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18
Q

are combination reactions redox

A

yes
free elements –> compound

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19
Q

how to balance redox reactions

A
  1. split into half reactions
  2. balence non O and non H atoms
  3. balence ox
  4. balence H
  5. balence e-
  6. multiply so both half rxn has same amount of e-
  7. add/ cancel like terms
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19
Q

how to balance redox reactions

A
  1. split into half reactions
  2. balence non O and non H atoms
  3. balence ox
  4. balence H
  5. balence e-
  6. multiply so both half rxn has same amount of e-
  7. add/ cancel like terms
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20
Q

how to balance redox reactions

A
  1. split into half reactions
  2. balence non O and non H atoms
  3. balence ox
  4. balence H
  5. balence e-
  6. multiply so both half rxn has same amount of e-
  7. add/ cancel like terms
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21
oxidation agent
is reduced and promotes oxidation of other reagnet typically contain oxygen or other electronegative atoms
22
reducing agent
is oxidized and promotes reduction of other reagent tend to have hydrogen
23
PCC
common oxidizing agent (weak)
24
NaBH4
common reducing agent
25
LiAlH4
common reducing agent
26
reduction potential
how likely something is to be reduced, higher value = more likely to be reduced
27
oxidation potential
reduction potential = - oxidation potential
28
standard potential of a cell
measured as reduction potential
29
what do all electrochemical cells have
a cathode and an anode
30
anode
electrode where oxidation happens -surplus of e- generated that travel to the cathode
31
cathode
Electrode where reduction happens
32
galvanic cell
spontaneous redox reaction that generates a positive V difference
33
cell potential eqn
E cell = Ecathode - E anode
34
which electrode possesses the reduction potential in a galvanic cell
cathode (spontaneous rxn )
35
cell potential eqn for a galvanic cell
E cell = E cathode - E anode
36
another way of establishing the cell potential formula
E cell = reduction potential of cathode + oxidation potential of anode
37
Nerst Eqn
how electrical potential of a cell is effected by temperature and concentration of reactants E'cell = E cell - RT/zf * lnQ
38
E' cell
actual electrical potential of cell under given conditions
39
z in nertz eqn
moles of e- transfered
40
F in nertz eqn
faraday constant
41
q
reaction quotient [products]/[reactants]
42
physiology nertz eqn
E'cell = standard potential - .05916/ z(logq)
43
Daniell cell
typical set up of a galvanic cell - half reactions are carried out in two separated half cells - electrodes are connected by a wire and a salt bridge (does not interfere with redox rxns -
43
purpose of salt bridge
to prevent strong charge gradient buildup and hindering progress of rxn
44
Daniell cell
typical set up of a galvanic cell - half reactions are carried out in two separated half cells - electrodes are connected by a wire and a salt bridge (does not interfere with redox rxns -
45
what happens to the zinc electrode (anode)
it becomes smaller as oxidation continues and e- are being stripped
46
what happens to the sulfur electrode (cathode)
will grow because of increased e-
47
galvanic cell notation
anode is on right || cathode is on left
48
charge of galvanic anode
- because it is the source of electrons
49
charge of galvanic cathode
positive because it has greater potential to be reduced
50
concentration cells
galvanice cells where the two half reations occur in the same cell 1. electrodes must be made out of same material 2. must be a concentration difference between the two regions of the cell
51
biological example of concentration cells
cell membrane with concentration difference between inside and outside of cell
52
electrolytic cells
apply energy to system and produce reaction in nonspontaneous direction break down into components
53
which electrode is location of reduction in electrolytic cells
cathode, marked with a negative charge
54
anode of electrolytic cell
positive and where oxidation takes palce
55
portion of battery that provides charge
galvanic
56
portion of battery that allows for recharge
electrolytic
57
benedicts reagent
reduce cu2+ to cu , dark blue color change
58
connection between standard gibbs free energy and electric potential
ΔG= -nFEcell n = moles of electrons moved f is faradays constant
59
how does standard potential relate to Keq
nFEcell = RTlnkeq
60
if the standard redox potential of a cell is positive what happens to gibbes free enrgy
negative so spontaneous
61
trade off in galvanic cell
using spontaneous chemical reaction to provide electrical energy
62
half reactions of galvanic cell
zinc and copper Zu --> Z 2+ + 2 e- Cu 2+ + 2e- --> cu
63
half cell
seperated containers with metal electrodes either cathode or anode
64
electrode on left of galvanic cell
zn
65
electrode on right of galvanic cell
cu
66
what allows e- to flow from zinc to copper in galvanic cell
the current carrying wire
67
zn electrode in galvanic cell
anode negative oxidation
68
cu electrode in galvanic cell
cathode positive (e- move toward positive) reduction
69
galvanic electrodes mnuemonic
An Ox and Red Cat - anode, oxidation - cathode, reduciton
70
electrolysis
uses external energy to power nonspontaneous (electrolytic ) reaction - often used to split molecules --> make pure metals requires voltage source
71
half reactions of electrolytic cells
2 na+ + 2 e- --> 2 Na (s) red 2 cl- --> cl2 + 2 e- (g) ox
72
does electrolytic reaction happen in 2 containers (like galvanic) or one?
only one, and there is no aqueous solution. only the ions na + and Cl-
73
anode of electrolytic cell
on left is positive still oxidation 2 cl - --> cl2 + 2 e- ELECTRONS FLOW FROM ANODE TO BATTERY
74
cathode of electrolytic cell
Na+ +2 e- --> na is negative reduction ELECTRONS ARE FLOWING FROM BATTERY TO CATHODE
75
what side of the battery is the electrolytic cathode attatched to
negative

MCAT chem (11 decks)

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