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chemistry 12 > REDOX chapter 9/10 > Flashcards

REDOX chapter 9/10 Flashcards

(58 cards)

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1
Q

oxidation

A

loss of electron(s)

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2
Q

reduction

A

gain of electron(s)

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3
Q

oxidizing agent

A

electron acceptor; species is reduced
more negative oxidation state

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4
Q

reducing agent

A

electron donor; species is oxidized
more positive oxidation state

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5
Q

oxidation states rule

A

oxidation state of elements in their standard states is zero

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6
Q

oxidation state rule for monoatomic ions

A

same as their charge

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7
Q

OIL RIG

A

oxidation is loss, reduction is gain

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8
Q

oxidant state of oxygen

A

-2 in its covalent compounds except as peroxide

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9
Q

oxidation state hydrogen

A

with non-metals it is +1

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10
Q

oxidation state fluorine

A

in compounds always -1

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11
Q

oxidation state compound sum rule

A

the sum of oxidation states must be zero in compounds

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12
Q

oxidation state sum rule

A

the sum must be equal the charge of the ion

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13
Q

oxidation state group IA

A

always +1

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14
Q

oxidation state rule hydrogen

A

always +1 with the exception of hydrides

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15
Q

oxidation state rule group IIA

A

always +2

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16
Q

metals have ____ oxidation numbers

A

positive

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17
Q

transition metals have _____ oxidation number

A

more than one

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18
Q

non metals and semi metals have ____ oxidation numbers

A

both positive and negative

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19
Q

no element exists in a compound with an oxidation number greater than __

A

+8

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20
Q

the most negative oxidation number equals ___

A

8 - the group number

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21
Q

in basic solutions balance hydrogen with ___

A

OH to create H2O

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22
Q

in acidic solutions balance oxygen with __

A

H2O

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23
Q

in acidic solutions balance hydrogen using __

A

H+ (proton)

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24
Q

a spontaneous reaction occurs if the redox chart shows a ________

Study These Flashcards
A

downhill direction from left to right

25
half-reaction equation
the part of a redox reaction equations representing either the oxidation or reduction
26
oxidation number
a number used to keep track of electrons in oxidation–reduction reactions according to certain rules; also known as oxidation state
27
half-cell
an electrode and an electrolyte that form half a complete cell
28
electrode
a solid electrical conductor
29
cell
a system in which two connected electrodes are in contact with an electrolyte
30
salt bridge
a tube that contains an electrolyte solution and connects the two half-cells in a galvanic cell
31
galvanic cell
an arrangement of two connected half-cells that spontaneously produces electric current
32
anode
the electrode where oxidation occurs
33
cathode
the electrode where reduction occurs
34
cell potential
the electric potential difference (voltage) between the two half-cells in a galvanic cell (SI unit is V)
35
standard cell
a galvanic cell in which  all the entities involved in the half-cell  reactions are at SATP and the solutions  have a concentration of 1.0 mol/L
36
standard cell potential (∆E°r (cell))
the electric potential difference of a galvanic  cell that is operating under standard  conditions 
37
standard reduction potential (E°r)
the ability of a half-cell to attract electrons  in a cell that is operating under standard  conditions
38
standard hydrogen half-cell
the galvanic cell from which all the half-cell  potentials are determined; E°r 5 0 V (by  definition)
39
SPONTANEOUS REACTION E°r (cell)
> 0
40
REACTION AT EQUILIBRIUM, DE°r (cell) 
= 0
41
NON-SPONTANEOUS REACTION, DE°r (cell)
< 0
42
battery
a group of two or more galvanic cells connected in series
43
primary cell
a cell that cannot be recharged
44
secondary cell
a cell that can be  recharged by being attached to an external  source of electrical energy; recharging  reverses the chemical reaction that  generates the electrical energy
45
fuel cell
a galvanic cell for which the reactants are continuously supplied
46
corrosion
the deterioration of a metal by a redox reaction
47
galvanizing
the process in which steel is coated with a thin layer of zinc to protect the steel from corrosion
48
cathodic protection
a form of corrosion prevention in which electrons are continually supplied to the metal that is being protected, making the metal a cathode
49
sacrificial anode
a form of cathodic  protection in which the oxidation of a more  active metal that is attached to the steel  prevents the iron in the steel from being  oxidized
50
impressed current
a form of cathodic  protection in which electrons from a DC  power source are pumped into the metal  that is being protected
51
electrolytic cell
a cell that uses electrical energy to produce a chemical change that would not occur spontaneously
52
electrolysis
the application of current through a cell to produce a chemical change
53
electrochemical cell
a general term that is used to refer to both a galvanic cell and an electrolytic cell
54
alkaline dry cells
most common types of primary cells tiny lightweight long lasting anode consists of a paste surrounded by solid MnO2 cathode
55
lead storage batteries
used in vehicles lead cathode coated in lead (iv) oxide and a lead anode liquid electrolyte, therefore is a wet cell
56
lithium ion cells and batteries
outside made of metal with pressure sensitive vent holes. inside contains several sheets of material pressed together containing an anode, cathode and seperator
57
electrorefining metals
purification of metal
58
electroplating metals
applying a thin coating of a metal that resists corrosion

chemistry 12 (5 decks)

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