U2AoS1 - Redox Reactions Flashcards

1
Q

What are Redox Reactions?

A

A reaction that involves the transfer of electrons.
Processes of oxidation and reduction

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

What are the types of redox reactions?

A
  • Addition/combination reaction
  • Decomposition reaction
  • Displacement reaction
  • Combustion reaction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is an addition reaction?

A

A + B – C

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

What is a decomposition reaction?

A

c - A + B

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

What is a displacement reaction?

A

A + BC – B + AC

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is oxidation?

A

Loss of electrons

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

What is reduction?

A

Gain of electrons

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

Half equation

A

electrons shown as either a product or reactant depending on oxidation or reduction

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

Reductant

A

Substance that causes another to be reduced and itself oxidised

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

Oxidant

A

Substance which causes another to be oxidised and itself reduced

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

Overall balance equation

A

Shows products/reactants but not electrons

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

Ionic equation

A

Two half equations written together
- no spectator ions
- must be balanced when two added together

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

Conjugate redox pair

A

Pair differ by one or more electrons
Oxidised form written first

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

Are ionic compounds formed through redox reactions?

A

Transfer of electrons hence, yes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Covalent molecular compounds… are they redox?

A
  • can be involved despite shared
  • partial electron transfer, unequal sharing of electrons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Oxidation numbers

A

determines if a redox reaction has occured

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

Oxidation number increases

A

Oxidised

18
Q

Oxidation number decreases

A

Reduced

19
Q

Oxidation number of free elements

A

O

20
Q

Oxidation number of ionic compounds

A

Charge of the ion

21
Q

Polyatomic oxidation numbers

A

Sum is equal to the charge on the ion

22
Q

Oxygen and Hydrogen Numbers

A

usually, -2 and +1

23
Q

UNDER ACIDIC CONDITIONS

A

KOHES
- key elements
- oxygen balanced by water
- hydrogen by H+ ions
- electrons added
- states

24
Q

Overall ionic equations

A
  • balance no.
  • add half equations
  • cancel species on both sides
25
Q

Reactivity of metals

A

A will only replace B if A is more reactive. A is oxidised and B is reduced

26
Q

Forwards Reaction

A

Reduction

27
Q

Backwards Reaction

A

Oxidisation

28
Q

Strong oxidants

A

accept electrons more readily

29
Q

Strong reductants

A

donate protons more readily

30
Q

What is a Galvanic Cell?

A

Converts chemical energy to electrical energy from spontaneous redox reactions taking place in the cell

31
Q

What is a laboratory galvanic cell?

A

Reactants separated into half cells connected with wire and a salt bridge to complete the circuit and allow for movement of electrons

32
Q

Half cells

A

contains a conjugate redox pair, electrodes must conduct electricity

33
Q

Anode

A

negative polarity (oxidation) will decrease mass and increase color intensity

34
Q

Cathode

A

positive polarity will increase in size

35
Q

If conjugate redox pair is metal

A

metal electrode

36
Q

If it does not contain metal

A

inert electrode (graphite or platnum) for fe4+ and sn 2+

37
Q

If it is a gas

A

Gas electrode platinum used

38
Q

Two electrolytes

A

Solution which contains free moving ions

39
Q

Salt bridge

A
  • connects/completes the circuit
  • provides ions to compensate for those lost/gained during a reation
    KNO3
40
Q

Voltmeter

A

records voltage (potential difference) produced by cell

41
Q

External circuit

A

electrodes+ wire

42
Q

Internal circuit

A

salt bridge + electrodes