Brainscape's Knowledge GenomeTM

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


See full index

Z A Level Chemistry > Redox > Flashcards

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 is oxidation?

A
  1. The loss of electrons
  2. The gain of electrons
    - Increase in oxidation number
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is reduction?

A
  1. The gain of electrons
  2. The loss of oxygen
    - Decrease in oxidation number
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is an oxidation number?

A

Oxidation numbers are assigned to elements to show the extent to which they have been oxidised or reduced

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

What is the oxidation number for an uncombined element?

A

0 e.g. Fe

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

What is the oxidation number for a group 1 metal?

A

+1 e.g. Na

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

What is the oxidation number for a group 2 metal?

A

+2 e.g. Mg

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

What is the oxidation number for aluminium?

A

+3

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

How do you figure out the oxidation number for other metals?

A
  1. Look to the group number for the theoretical maximum

- E.G Mn is Group 7 so the maximum it could be is +7

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

When is the oxidation number for oxygen not -2?

A
  1. In peroxides

2. In compounds with fluorine

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

When is the oxidation number for chlorine not -1?

A
  1. In compounds with fluorine or oxygen
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

How do you figure out the oxidation number for other non-metals?

A
  1. As with metals, look at the group number for the theoretical maximum
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What does the sum of the oxidation states in a neutral molecule always add up to?

A
  1. Zero
    - One element must have a positive oxidation states and the other must be negative
    - If neither atom has a fixed oxidation number, the more electronegative species will have the negative value
    - Plug in numbers you know are fixed
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What does the sum of the oxidation states in a compound ion always add up to?

A
  1. The overall charge on the ion e.g. negative one or positive 2
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is the role of oxidation numbers in naming compounds?

A
  1. If a compound contains an element that does not always have the same oxidation number (e.g. a transition metal), the oxidation number of this element is shown as a Roman numeral in brackets as part of the name of the compound e.g. iron (III) hydroxide
    - Roman numeral’s after the negative compound ion e.g. sulphate (VI)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is the first ionisation energy down group 2 like?

A

Decreases

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

What is the reactivity down group 2 like?

A

Increases

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

What is the atomic radius down group 2 like?

A

Increases

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

What is the alkalinity down group 2 like?

A

Increases

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

What is the solubility down group 2 like?

A

Increases

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

What is the electronegativity down group 2 like?

A

Decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is the melting point down group 2 like?

A

Decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What does group 2 metal and oxygen form?

A
  1. Metal oxide
    - Redox Reaction
    - Increasing reactivity down the group
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is the flame colour of magnesium?

A

Bright white

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is the flame colour of calcium?

A

Brick red

25
Q

What is the flame colour of strontium?

A

Crimson red

26
Q

What is the flame colour of barium?

A

Apple green

27
Q

What does group 2 metal and water form?

A
  1. Metal hydroxide and hydrogen gas
    - Redox Reaction
    - Reaction becomes more vigorous (remember for observe you don’t see hydrogen you see bubbles!) and no more hydrogen is produced it is just more vigorous!
28
Q

What does group 2 metal oxides and water form?

A
  1. Metal hydroxides (this reaction does not result in the formation of hydrogen gas!)
    - NOT Redox Reaction
    - Better to go through two steps of make metal oxide and then react with water then straight with water as it is safer as no hydrogen is produced
29
Q

How does magnesium reaction with steam?

A

1, Magnesium only reacts very slowly with cold water, hot water is required to make magnesium hydroxide and hydrogen
2. In contrast magnesium will react violent with steam ti takes magnesium oxide and hydrogen

30
Q

Why does the solubility of group 2 hydroxides increase down the group?

A
  1. The IONIC RADIUS of M2+ increase
  2. Charge density of M2+ increases
  3. The attraction between the M2+ and OH- decreases
  4. The lattice will break up and solvate? more easily
31
Q

How is calcium hydroxide used?

A
  1. Neutralises acidic soils

2. Used as lime water

32
Q

How is magnesium hydroxide used? (and CaCO3)

A
  1. ‘anti acids’, intreating indigestion as they neutralise stomach acid
33
Q

What does group 2 and acids form?

A
  1. Salts and hydrogen
    - Redox Reaction
    - metal and HCL, metal chloride and hydrogen
34
Q

How does the reactivity change down group 7?

A

Decreases

35
Q

How does the atomic radius change down group 7?

A

Increases

36
Q

How does the electronegativity change down group 7?

A

Decreases

37
Q

How does the melting point change down group 7?

A

Increases

38
Q

How does the ability to be an oxidising agent change down group 7?

A

Decreases

39
Q

Why is there this trend of melting point in group 7?

A
  1. Larger molecules, as atomic radius increases
  2. More electrons
  3. Chance of instantaneous dipoles forming increases
  4. Increased number of induced dipoles
  5. Increased number of London forces
  6. Increase in boiling and emptying point / decreases in volatility
40
Q

Why is there this trend in oxidising power?

A
  1. larger molecules, so atomic radius increases
  2. More electrons
  3. More full inner shells, so shielding is increased
  4. Incoming electron is therefore less attracted to the nuclear charge
  5. Reactivity / oxidising ability decreases
41
Q

What is an oxidising agent?

A

An oxidising agent is a substance that will accept electrons. The ability of halogens to accept an electron to from a halide ion makes them very good oxidising agents

42
Q

What is the rule in displacement reactions?

A
  1. A more reactive halogen will displace a less reactive halogen from a solution of its halide ions
  2. Loose halogens give colour of solution not salts!
43
Q

What colour is chlorine in hexane (non-polar solvent)?

A

colourless

44
Q

What colour is bromine in hexane?

A

orange

45
Q

What colour is iodine in hexane?

A

purple

46
Q

What colour is chlorine in water?

A

colourless

47
Q

What colour is bromine in water?

A

orange

48
Q

What colour is iodine in water?

A

brown

49
Q

What are the three displacement reactions and what is the colour change in each?

A
  1. 2KBr + Cl2 –> 2KCl + Br2
    - Water: colourless to orange
    - Hexane: colourless to orange
  2. 2KI + Cl2 –> 2KCl + I2
    - Water: colourless to brown
    - Hexane: colourless to purple
  3. 2KI + Br2 –> 2KBr + I2
    - Water: orange to brown
    - Hexane: orange to purple
50
Q

What is a disproportionation reaction?

A

A reaction in which the same element is both oxidised and reduced

51
Q

What are some examples of a disproportionation reaction? Where are they used?

A
  1. Chlorine and water, in water purification and is used to STERILISE drinking water
  2. Chlorine and (cold, dilute, aqueous) sodium hydroxide, used to from bleach as active ingredient in bleach is the NaClO
52
Q

How do you test for halide ions? What are the results?

A

-Aqueous halide ions can be tested for using by adding an aqueous solution of silver nitrate
1. Halide: Cl-
Precipitate Colour: Silver chloride, white
2. Halide: Br-
Precipitate Colour: Silver bromide, cream
3. Halide: I-
Precipitate Colour: Silver iodide, yellow

53
Q

How do you test the solubility of a silver halide?

A
  • The relative solubility in ammonia can be used to double check
    1. AgCl : soluble in DILUTE NH3
    2. AgBr: soluble in CONCENTRATED NH3
    3. AgI: insoluble in dilute and concentrated NH3
54
Q

What are the benefits and risks of using chlorine in water treatment?

A
  1. B: Kills bacteria
  2. R: hazards of toxic chlorine gas and possible risks from formation of chlorinated hydrocarbons
    - However, the overall risk to health of not adding chlorine to the water supply is far greater than the risk posed by chlorinated hydrocarbons, as the quality of drinking water would be compromised and sieges such as typhoid and cholera might break out
55
Q

Why does magnesium gave a greater second ionisation energy than strontium?

A
  1. Ionic radius increases
  2. Shielding increases
  3. Attraction between the nucleus and outermost electron decreases
    - Mg+ –> Mg2+ + e-
56
Q

Why is calcium nitrate a salt?

A

The H+ ion in an acid has been replaced by a metal ion

57
Q

Why does the hydroxide ion in aqueous calcium hydroxide acts as a base when it neutralises dilute nitric acid

A

It accepts a proton/H+

58
Q

Explain the decrease in atomic radio acids the period from Na to Cl

A
  1. Nuclear charge increases
  2. Electrons added to the same shell and shielding remains the same
  3. Greater attraction

Z A Level Chemistry (13 decks)

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