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GeoBiology > Redox Chemistry > Flashcards

Redox Chemistry Flashcards

1
Q

What are the major elements for life?

A

S ulfur
P hosphorus
O xygen
N itrogen
C arbon
H ydrogen

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2
Q

7 Common elements in life functions
(other than SPONCH)

A

Sodium (Na)
Magnesium ()Mg)
Potassium (K)
Calcium (Ca)
Iron (Fe)
Copper (Cu)
Uranium (U)

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3
Q

What happens in Redox?

A

Flow of electrons from one defined center to another

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4
Q

What is oxidation?

A

Loss of electrons

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5
Q

What is reduction?

A

Gain of electrons

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6
Q

Oxidation state of neutral molecules and elemental atoms

A

Zero

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7
Q

Oxidation state of monoatomic ion

A

charge of that ion

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8
Q

Oxidation state of oxygen in compounds

A

-2

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9
Q

Oxidation state of elements of a polyatomic ion ex: sulfate (SO4)2-

A

sum of oxidation states equals charge of the ion
Oxygen -2 x 4 = -8
ion charge = -2
-8- (-2) = 6 = Sulfur oxidation state

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10
Q

Oxidation state of Group I elements (H, Na, K)

A

+1

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11
Q

Oxidation state of Group 2 (Mg, Ca)

A

+2

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12
Q

Oxidation state of Halogens (Cl)

A

-1

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13
Q

Oxidation state of Hydrogen when in compounds with more electronegativity

A

+1

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14
Q

What is electronegativity

A

ability of an element to draw an electron towards it

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15
Q

H2
name
oxidation state
reduced or oxidized

A

Hydrogen gas
0
reduced

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16
Q

H+
name
oxidation state
reduced or oxidized

A

proton/hydrogen ion
+1
oxidized

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17
Q

O in H2O
name
oxidation state
reduced or oxidized

A

water
-2
reduced

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18
Q

O2
name
oxidation state
reduced or oxidized

A

molecular oxygen
0
oxidized

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19
Q

UO2(s)
name
oxidation state
reduced or oxidized

A

Uraninite
+4
(O2 = 2-*2 = -4, U = +4)
reduced

20
Q

(UO2)2+ (aq)
name
oxidation state
reduced or oxidized

A

Uranyl
+6
(O2 = -2*2 = -4, U = +4 +2 ion charge = +6)
Oxidized

21
Q

H2S or HS-
name
oxidation state
reduced or oxidized

A

Sulfide (formula depends on pH)
-2
reduced

22
Q

S
name
oxidation state
reduced or oxidized

A

elemental sulfur
0
depends on reaction

23
Q

(S2O3)2-
name
oxidation state
reduced or oxidized

A

Thiosulfate
+2
depends on reaction

24
Q

(SO3)2-
name
oxidation state
reduced or oxidized

A

Sulfite
+4
depends on reaction

25
Q

(SO4)2-
name
oxidation state
reduced or oxidized

A

Sulfate
+6
oxidized

26
Q

NH3, (NH4)+
names
oxidation state
reduced or oxidized

A

Ammonia, Ammonium (depends on pH)
-3
reduced

27
Q

N2
name
oxidation state
reduced or oxidized

A

molecular Nitrogen
0
depends on reaction

28
Q

N2O
name
oxidation state
reduced or oxidized

A

Nitrous oxide
+1
depends on reaction

29
Q

(NO2)-
name
oxidation state
reduced or oxidized

A

Nitrite
+3
depends on reaction

30
Q

(NO3)-
name
oxidation state
reduced or oxidized

A

Nitrate
+5
oxidized

31
Q

Fe2+
name
oxidation state
reduced or oxidized

A

Iron (II) or ferrous ion
2+
reduced

32
Q

Fe3+
name
oxidation state
reduced or oxidized

A

Iron (III) or ferric ion
3+
oxidized

33
Q

C
name
oxidation state
reduced or oxidized

A

graphite
0
depends on reaction

34
Q

CH compounds (not HC)
name
oxidation state
reduced or oxidized

A

organic carbon
always has electrons it can give away
reduced

35
Q

CO
name
oxidation state
reduced or oxidized

A

Carbon monoxide
+2
depends on reaction

36
Q

CO2
name
oxidation state
reduced or oxidized

A

Carbon dioxide
+4
oxidized

37
Q

(CO3)-
name
oxidation state
reduced or oxidized

A

Carbonate
+4
oxidized

38
Q

(HCO3)-
name
oxidation state
reduced or oxidized

A

Bicarbonate
+4
oxidized

39
Q

H2CO3
name
oxidation state
reduced or oxidized

A

Carbonic Acid
+4
oxidized

40
Q

FeS2
name
oxidation state
reduced or oxidized

A

Pyrite
S-S bond here has oxidation state of -2
Fe oxidation state +2
both elements are reduced

41
Q

what bond is in organic carbon?
inorganic carbon?

A

organic carbon = covalent bonds
inorganic = ionic bonds

42
Q

/sizeCH4
(name, type of carbon,
environment, conditions)

A

Methane
organic carbon
(anaerobic, reducing environment)

43
Q

C6H12O6
(name, type/size of carbon,
environment, conditions)

A

glucose
organic carbon, large compound
aerobic environment
(reducing or oxidizing conditions)

44
Q

CH3COO-
(name, type/size of carbon,
environment, conditions)

A

Acetate
organic carbon, small compound
aerobic or anaerobic environment
(reducing or oxidizing conditions)

45
Q

oxidizing agent

A

reactant element that decreased oxidation state (has gained electrons) as a product -
it took electrons from the other element, causing it to become reduced

46
Q

reducing agent

A

reactant element that has increased its oxidation state (lost electrons) as a product - it gave electrons to the other element, causing it to become oxidized

47
Q

Disproportionation Reaction
(example)

A

A reaction in which one substance is both oxidized and reduced
thiosulfate (S203^2-) can produce both sulfide (S^2-, or HS-, or H2S), reduced, and sulfate (SO4^2-), oxidized

GeoBiology (15 decks)

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