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Chemistry > Redox Reactions > Flashcards

Redox Reactions Flashcards

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1
Q

oxidation state

A

value assigned to atom of compound, measures electron control or possession. The apparent chage that an atom has in a molecule or ion.

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2
Q

Fluorine Oxidation State

A

-1

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3
Q

Chlorine Oxidation State

A

-1

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4
Q

Hydrogen Oxidation State

A

+1

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5
Q

Oxygen Oxidation State

A

-2

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6
Q

Exceptions to O, H, Cl, F oxidation states

A

when F, Cl, H, O are bonded to each other, the oxidation state stays the same

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7
Q

What is the oxidation number of an element on its own?

A

0

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8
Q

What is the oxidation number of a simple ion?

A

the charge of the ion

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9
Q

What is the sum of oxidation state of a compound?

A

0

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10
Q

What charge do metals have

A

positive

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11
Q

In reduction what happens for ionic and covalent bonds?

A
  • ionic bond- negative ion

- covalent bond- atom has higher electron density around it

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12
Q

In oxidation what happens for ionic and covalent bonds?

A
  • ionic bond- positive ion

- covalent bond- ion has lower electron density around it

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13
Q

What are the exceptions to F having an oxidative state of -1?

A

F is always -1

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14
Q

What are the exceptions of O have an oxidative state of -1?

A
  • combining with H2, where it’s -1

- combining with F2, where it’s +2

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15
Q

Li, Na, K Oxidation State

A

+1

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16
Q

Mg, Ca Oxidation State

A

+2

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17
Q

oxidizing agent

A

reactant that accepts electrons to become reduced, bringing about oxidation of other reactant

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18
Q

reducing agent

A

reactant that supplies the electrons to become oxidized, bringing about reduction of other reactant

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19
Q

Where are the electrons in the equation for oxidation?

A

right side/ product side

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20
Q

Where are the electrons in the equations for reduction?

A

left side/ reactant side

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21
Q

Which metals are stronger reducing agents? And why?

A

reactive metals, they have the tendency to lose electrons and will push their electrons on to other substances to form positive ion
- displace other substance

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22
Q

What is the definition of an activity series?

A

to predict if a particular redox reaction between metal and ions of another metal will be feasible

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23
Q

What are the products of the electrolysis of Brine?

A
  • hydrogen gas
  • chlorine gas
  • sodium hydroxide
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24
Q

What is 2 things hydrogen gas is used for?

A
  • rocket fuel

- tracer isotope

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25
Q

What are two things chlorine gas is used for?

A
  • disinfectant

- treat swimming pool water

26
Q

What are 2 sodium hydroxide is used for?

A
  • drain cleaner

- soaps/ detergent

27
Q

What is a redox reaction?

A

a reaction where 1 substance is reduced and the other is oxidized

28
Q

More reactive non-metals are stronger ______ agents.

A

stronger oxidizing agents, most readily reduced

29
Q

Differences between acid/base titration and redox titration

A
  • AC titr. = neutralization between acid and base
  • RT= between oxidizing and reducing agent
  • AC titr= protons transferred from acid to base
  • RT= electrons transferred from reducing to oxidizing agent
30
Q

State what is oxidized and reduced in analysis of iron with manganate (VII)

A
  • oxidized- Fe2+ to Fe3+

- reduced- MnO4- to Mn2+

31
Q

In analysis of iron with manganate (VII) what is the color change?

A

purple to colourless

32
Q

What are redox titrations used for?

A
  • pharmaceutical industry

- food and beverage industry

33
Q

In iodine-thiosulfate reaction, what is the visible color change?

A

deep blue to colourless

34
Q

In iodine-thiosulfate reaction, what is the indicator and when is it added

A

starch, and it is added during the titration

35
Q

In iodine-thiosulfate reaction, what is the oxidizing and reducing agent?

A
  • oxidizing: iodine

- reducing: thiosulfate ion

36
Q

What is the BOD- biological oxygen demand?

A
  • high BOD- low oxygen content in water

- low BOD- good oxygen content in water

37
Q

What precautions do you take in the Winkler method?

A
  • when pouring water, funnel should touch flask so no extra oxygen in added from air
38
Q

What phosphates cause eutrophication and what does this do to oxygen?

A
  • NO3- and PO43- cause algae blooms

decimating levels of O2

39
Q

How is dissolved oxygen fixed during the winkler method?

A
  • by adding Mn2+ compound
40
Q

What compound is always added to the iodine in the winkler method, making it a titrations?

A
  • iodine thiosulfate
41
Q

What are the two types of electrochemical cells?

A

voltaic (galvanic) and electrolytic

42
Q

How do voltaic cells generate electricity?

A

from spontaneous redox reactions which generate electricity`

43
Q

How do electrolytic cells generate electricity?

A

non-spontaneous redox reactions: drive chemical reactions using electricity

44
Q

What is a half cell?

A

a strip of metal in an electrolytic solution of its own ions

45
Q

What is the oxidation number for copper?

A

Cu2+

46
Q

What is the electrode potential?

A

the charge difference between the strip of metal and the solution of its own ions

47
Q

Term used to describe electrodes when they don’t take part in redox reactions.

A

Inert

48
Q

In an electrolytic cell, where does oxidation take place?

A

anode (+), where anions are oxidized

49
Q

In an electrolytic cell, where does reduction take place?

A

cathode (-), where cations are reduced

50
Q

What is an electrolytic cell?

A

Cell that produces a non-spontaneous redox reaction driven by outside electricity

51
Q

What type of reaction is produced through an electrolytic cell?

A

endothermic reaction

52
Q

What type of reaction is produced through a voltaic cell?

A

exothermic reaction

53
Q

What is a voltaic/galvanic cell?

A

a spontaneous redox reaction that produces electricity

54
Q

What two connections must a voltaic cell have?

A
  • external electronic circuit

- salt bridge to complete the circuit

55
Q

What does a salt bridge contain? Also, what does the salt bridge maintain?

A

an aqueous solution of ions

- maintains the potential difference

56
Q

Without a salt bridge, what happens to the voltage?

A

no voltage is generated

57
Q

How to test for hydrogen

A

squeaky pop

58
Q

How to test for chlorine

A

damp blue litmus paper turns red then white

59
Q

In all cells, electrons flow from ____ to _____.

A

In all cells, electrons flow from anode to cathode.

60
Q

Write equation for iron with manganate (VII)

A

DO IT

61
Q

Write 2 of the equations for the Iodine- thiosulfate reactions.

A

DO IT NOW

Chemistry (11 decks)

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