Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

chemistry > unit 11 - redox > Flashcards

unit 11 - redox Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

what are redox reactions caused by

A

caused by competition of atoms for electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

redox is an abbreviation for

A

Reduction/Oxidation Reactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

oxidation

A
  • The LOSS of electrons.
  • Charge becomes more positive
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

reduction

A
  • The GAIN of electrons.
  • Charge becomes more negative
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

ATOMS are neutral but in a bond there is

A

shuffling of electrons (sharing, transferring) which ultimately gives them an “apparent” charge.

  • this apparent charge is the Oxidation Number
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Oxidation Number

A

The ”apparent charge” on an atom in a compound, due to difference in electronegativity and bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Ion

A

Charge an atom becomes when it gains or loses electron(s).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Redox: Rule 1

A

all neutral compounds must sum to the total charge of ZERO

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Redox: Rule 2

A

polyatomic ions have a sum of charges equal to the ion’s charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Redox: Rule 3

A

Any atom uncombined has an oxidation of zero, because atoms are neutral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Redox: Rule 4

A

Charge on a mono-atomic ion equals the charge of the ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Redox: Rule 5

A

In Binary Compounds the MORE electronegative element is assigned FIRST (it’s the oxidation number is the name charge as an ion)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Redox: Rule 6

A

Elements in groups 1, 2, & aluminum have oxidation states ALWAYS +1, +2, and +3 respectively

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Redox: Rule 8

A

oxygen is always -2 unless its combined with fluorine (OF2), then its +2, or in a peroxide (H2O2) then its -1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Redox: Rule 7

A
  • Fluorine is the MOST ELECTRONEGATIVE ELEMENT so it takes precedence over ANY
  • fluorine will always have a -1 oxidation #
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Redox: Rule 9

A

hydrogen is +1; unless it combines with a metal then its -1 because thats a hydride

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

redox is a reaction defined by

A

the transfer of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

LEO the Lion says GER

A

Lose Electrons Oxidize
Gain Electrons Reduction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

redox reaction can be broken into two parts that happen…

A

simultaneously!!
- oxidation and reduction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what typa reaction is never redox?

A

double replacement

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

hint to identify redox!!

A
  • if theres a free guy and hes a compound on the otherside, yk it’s a redox
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

oxidizing agent

A

The substance that makes
something else undergo oxidation.

  • Takes away the electrons (it gains electrons)
  • Oxidizing Agent is also Reduced
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

reducing agent

A

Any substance that makes
something else gain electrons.

  • Supplies Electrons (it loses electrons)
  • Reducing Agent is also Oxidized
23
Q

what gets oxidized is the ____ agent

A

reducing agent

24
Q

what gets reduced is the ____ agent

A

oxidizing agent

25
Q

in redox reactions, electrons shift from

A

one atom/species to another SIMULTANEOUSLY!!

26
Q

half reaction

A

an equation which shows only a reduction OR oxidation

27
Q

half reactions show conservations of what? exceptions?

A

**show conservation of Mass, Charge, and Energy

  • except for Nuclear Reactions
28
Q

Redox reactions like all chemical reactions MUST be balanced to show conservation of

A

mass, charge, and energy

29
Q

shortcut for balancing redox

A

the difference in charge is the coefficient of the opposite
- does not work if you have diatomics

30
Q

when a redox reaction takes place in an acidic solution,

A

it has excess H+ ion concentration as opposed to neutral conditions

31
Q

redox in acidic: what are we adding

A

We will now add Water molecules and H+ ions to balance the Oxygens & Hydrogens under acidic conditions.

32
Q

voltaic cells

A
  • are electrochemical cells (batteries)
  • involve a spontaneous redox reaction
  • chemical energy is converted into electrical energy
33
Q

voltaic cells setup: two electrodes

A

are the site of oxidation/reduction

34
Q

voltaic cells setup: salt bridge

A

connects the two containers and produces the path for a flow of ions

35
Q

voltaic cells setup: the wires of voltmeter

A

connect the 2 half cells and electrons travel through them

36
Q

voltaic cell: table j

A
  • most active metals lose electrons easily
  • top: atom oxidized
  • bottom: ion reduced
37
Q

voltaic cell: anode

A

Anode is the site of oxidation

38
Q

voltaic cell: cathode

A

cathode is site of reduction

39
Q

voltaic cell: electrons move from…

A

anode to cathode through the wire

40
Q

voltaic cell: anode mass/size

A

anode decreases in mass/size

41
Q

voltaic cell: cathode mass/size

A

cathode increases in mass/size

42
Q

voltaic cell: ions move through

A

Ions (+/-) move through salt bridge in the direction of electrode with same charge to maintain neutrality.

43
Q

voltaic cell: battery

A

battery will die and voltage will read zero (state of equilibrium)

44
Q

maximum battery voltage or cell potential

A
  • based reduction potential chart
  • cell potential (v) = reduction potential (v) - oxidation potential (v)
45
Q

if cell potential (+)

A

reaction is spontaneous

46
Q

if cell potential (-)

A

reaction is nonspontaneous

47
Q

predicting spontaneous reactions

A
  • one metal must be neutral ex. Mg (s) or Al (s) these can be oxidized (lose electrons)
  • the other must be an ion ex. Mg^+2 or Al^+3 these can be reduced (gain electrons)
48
Q

predicting spontaneous reactions: table j

A

the metal atom being oxidized (the neutral one) must be higher on the table J than the ion being reduced

49
Q

electrolysis

A
  • is a non spontaneous reaction
  • requires electricity (battery)
50
Q

electrolytic cells:

A
  • electrolysis
  • requires electricity
  • need an electric generator (battery) placed into the circuit to force electrons to flow from the anode (+) to the cathode (-)
  • electrical energy drives a chemical (redox rxn)
51
Q

electroplating

A

used to plate expensive metal on top of cheaper metals

52
Q

electrolytic: anode

A

● (+)
● always the expensive metal
● site of oxidation

53
Q

electrolytic: cathode

A

● (-)
● site of reduction

54
Q

electrolytic cells are used to

A

retrieve very active metals (group 1 & 2) from salts that contain them

chemistry (11 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions