Redox Chemistry Flashcards by Leigh Tucker

What are the major elements for life?

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

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7 Common elements in life functions
(other than SPONCH)

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

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What happens in Redox?

Flow of electrons from one defined center to another

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What is oxidation?

Loss of electrons

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What is reduction?

Gain of electrons

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Oxidation state of neutral molecules and elemental atoms

Zero

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Oxidation state of monoatomic ion

charge of that ion

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Oxidation state of oxygen in compounds

-2

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

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

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Oxidation state of Group 2 (Mg, Ca)

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Oxidation state of Halogens (Cl)

-1

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Oxidation state of Hydrogen when in compounds with more electronegativity

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What is electronegativity

ability of an element to draw an electron towards it

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H2
name
oxidation state
reduced or oxidized

Hydrogen gas
0
reduced

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H+
name
oxidation state
reduced or oxidized

proton/hydrogen ion
+1
oxidized

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O in H2O
name
oxidation state
reduced or oxidized

water
-2
reduced

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O2
name
oxidation state
reduced or oxidized

molecular oxygen
0
oxidized

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UO2(s)
name
oxidation state
reduced or oxidized

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

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

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

H2S or HS-
name
oxidation state
reduced or oxidized

Sulfide (formula depends on pH)
-2
reduced

S
name
oxidation state
reduced or oxidized

elemental sulfur
0
depends on reaction

(S2O3)2-
name
oxidation state
reduced or oxidized

Thiosulfate
+2
depends on reaction

(SO3)2-
name
oxidation state
reduced or oxidized

Sulfite
+4
depends on reaction

(SO4)2- name oxidation state reduced or oxidized

Sulfate +6 oxidized

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

Ammonia, Ammonium (depends on pH) -3 reduced

N2 name oxidation state reduced or oxidized

molecular Nitrogen 0 depends on reaction

N2O name oxidation state reduced or oxidized

Nitrous oxide +1 depends on reaction

(NO2)- name oxidation state reduced or oxidized

Nitrite +3 depends on reaction

(NO3)- name oxidation state reduced or oxidized

Nitrate +5 oxidized

Fe2+ name oxidation state reduced or oxidized

Iron (II) or ferrous ion 2+ reduced

Fe3+ name oxidation state reduced or oxidized

Iron (III) or ferric ion 3+ oxidized

C name oxidation state reduced or oxidized

graphite 0 depends on reaction

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

organic carbon always has electrons it can give away reduced

CO name oxidation state reduced or oxidized

Carbon monoxide +2 depends on reaction

CO2 name oxidation state reduced or oxidized

Carbon dioxide +4 oxidized

(CO3)- name oxidation state reduced or oxidized

Carbonate +4 oxidized

(HCO3)- name oxidation state reduced or oxidized

Bicarbonate +4 oxidized

H2CO3 name oxidation state reduced or oxidized

Carbonic Acid +4 oxidized

FeS2 name oxidation state reduced or oxidized

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

what bond is in organic carbon? inorganic carbon?

organic carbon = covalent bonds inorganic = ionic bonds

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

Methane organic carbon (anaerobic, reducing environment)

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

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

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

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

oxidizing agent

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

reducing agent

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**

Disproportionation Reaction (example)

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