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Chemistry A Level > Redox Chapter 7 - 10 and 22 > Flashcards

Redox Chapter 7 - 10 and 22 Flashcards

1
Q

In terms of oxygen
What is oxidation and reduction

A

Oxidation is gain of oxygen
Reduction is loss of oxygen

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2
Q

In terms of oxygen
What is the oxidising and reducing agent

A

Oxidising agent is oxygen donor
Reducing agent is oxygen acceptor

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3
Q

In terms of hydrogen
What is oxidation and reduction

A

Oxidation is loss of hydrogen
reduction is gain of hydrogen

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4
Q

In terms of hydrogen
What is the oxidising and reducing agent

A

Oxidising agent is hydrogen acceptor
Reducing agent is hydrogen donor

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5
Q

What is oxidation and reduction in terms of electrons

A

Oxidation is loss
Reduction is gain

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6
Q

What is the oxidising and reducing agent in terms of electrons

A

Oxidising agent is electron acceptor
Reducing agent is electron donor

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7
Q

What is oxidation state

A

It is another way to work out what is going on in a redox reaction
The oxidation state of any element shows the number of electrons over which it has lost or gained

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8
Q

What does the sign show for oxidation state

A

Positive - loss of electrons
negative - gain of electrons

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9
Q

What rules are there for oxidation numbers

A

All elements are 0
The number of ions is the charge of the ion
In compounds the sum of numbers is zero
Group 1 are +1
Group 2 are +2
Aluminium is +3
Fluorine is -1

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10
Q

What elements are special for oxidation numbers

A

Oxygen is -2 - except in peroxides -1 and in OF2 when its +2
Hydrogen is +1 - except in metal hydrides -1
Chlorine is -1 - except in compounds with O or F where its positive

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11
Q

What are the rules for half equations

A

Only one element changes oxidation state
Balance oxygen atoms with water
Balance hydrogen atoms with H+
Balance the charges with electrons

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12
Q

Rules for adding half equations

A

One must be oxidation and the other reduction
The number of electrons must be the same
The equation must balance for electrons and atoms

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13
Q

What structure are sodium, magnesium and aluminium

A

Giant Metallic

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14
Q

What structure is silicon

A

Macromolecular

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15
Q

What structure is P, S and Cl

A

Simple molecular

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16
Q

What structure is Argon

A

Simple atomic

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17
Q

What is the trend in melting point for period 3 and why

A

Increases from Na to Si as bond strength increases
Decreases from P to Ar as Van der Waal forces decreases as molecular size decreases

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18
Q

What is the trend with BP across period 3

A

Increases from Na to Al as metallic bond gets stronger
Decreases from Si to Ar VDW get weaker as size decreases

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19
Q

Trend of atomic radius across period 3

A

Decreases across period as nuclear charge increases

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20
Q

Trend in first ionisation energy across period 3

A

Increases across period as nuclear charge increases and shielding remains constant

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21
Q

Why is there a decrease in 1st IE from Mg to Al

A

Al’s outer electron is in a less shielded 3p orbital

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22
Q

Why is there a decrease in 1st IE energy from P to S

A

S has a pair of electrons in orbital causing repulsion

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23
Q

How does Sodium react with water
Equation

A

Fizzing
Turns alkaline
Gives off heat
2Na + 2H2O –> 2NaOH + H2

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24
Q

How does magnesium react with water

A

Reacts slowly
Forms weak alkali
Mg + 2H2O –> MgO + H2 Steam
Mg + 2H20 –> Mg(OH)2 + H2

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25
Q

How does Sodium react with oxygen

A

Vigorous reaction
Burns with yellow flame
4Na + O2 –> 2Na2O
White solid

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26
Q

How does magnesium react with oxygen

A

Vigorous reaction
Burns with white flame
2Mg + O2 –> 2MgO

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27
Q

How does aluminium react with oxygen

A

Vigorous reaction
4Al + 3O2 –> 2Al2O3

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28
Q

How does silicon react with oxygen

A

Low reaction
Requires heat
Si + O2 –> SiO2

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29
Q

How does phosphorous react with oxygen

A

Red phosphorous must be heated for reaction
White phosphorous reacts spontaneously
P4 + 5O2 –> P4O10
White flame

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30
Q

How does sulphur react with oxygen

A

Sulphur melts easily
Blue flame
Pungent choking gas
S + O2 –> SO2

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31
Q

What are the melting points of Non-Metal oxides

A

Silicon oxide has a giant covalent structure so high MP
Phosphorous oxide and sulfur oxide are simple covalent molecules so low MP’s

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32
Q

What are the properties of metal oxides

A

High MP and BP
Mp increases across period as the charge is higher and so the forces are higher

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33
Q

How does sodium oxide react with water

A

Bubbles
pH 13
Dissolves exothermically
Na2O + H2O –> 2NaOH

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34
Q

How does magnesium oxide react with water

A

pH 9
Sparingly soluble
MgO + H2O –> Mg(OH)2

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35
Q

How does aluminium oxide react with water

A

Insoluble
Bonding is too strong

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36
Q

How does Silicon oxide react with water

A

Insoluble

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37
Q

How does phosphorous oxide react with water

A

Violent reaction
pH 1
P4O10 + 6H2O –> 4H3PO4

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38
Q

How does sulfur dioxide react with water

A

pH 3
Soluble
SO2 + H2O –> H2SO3
The product is a weak acid

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39
Q

How does Sodium and magnesium oxide react with acids and bases

A

They are both basic oxides and will react with acids
Na2O + H2SO4 –> Na2SO4 + H2O
MgO + H2SO4 –> MgSO4 + H2O

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40
Q

How does aluminium oxide react with acids and bases

A

It is a amphoteric oxide so can be acidic and alkaline so reacts with both acids and bases
Al2O3 + 6HCl –> 2AlCl3 + 3H20
Al2O3 + 2NaOH + 3H2O –> 2NaAl(OH)4

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41
Q

How does Silicon dioxide react with bases

A

It acts as a weak acid with strong bases
SiO2 + 2NaOH –> 2Na2SiO3 + H2O

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42
Q

How does phosphorous oxide react with bases

A

It reacts with bases
It becomes phosphoric acid when in water
H3PO4 + 3NaOH –> Na3PO4 + 3H2O

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43
Q

Does sulphur dioxide react with bases

A

It reacts
SO2 + NaOH –> NaHSO4
NaHSO3 + NaOH –> Na2SO3 + H2O

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44
Q

Describe sodium oxide
Appearance
Structure
Solubility with water
pH in water
Acid/base/amphoteric

A

White solid
Ionic
Dissolves exothermically
13
Base

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45
Q

Describe Magnesium oxide
Appearance
Structure
Solubility with water
pH in water
Acid/base/amphoteric

A

White solid
Ionic
Sparingly soluble
9
Base

46
Q

Describe aluminium oxide
Appearance
Structure
Solubility with water
pH in water
Acid/base/amphoteric

A

White solid
Ionic (covalent character)
Insoluble
7
Amphoteric

47
Q

Describe Silicon dioxide
Appearance
Structure
Solubility with water
pH in water
Acid/base/amphoteric

A

White solid
Giant covalent
Insoluble
7
Acidic

48
Q

Describe Phosphorous oxide
Appearance
Structure
Solubility with water
pH in water
Acid/base/amphoteric

A

White solid
Simple molecular
Violent reaction
1
Acidic

49
Q

Describe Sulfur dioxide
Appearance
Structure
Solubility with water
pH in water
Acid/base/amphoteric

A

Gas
Simple molecular
Soluble
3
Acidic

50
Q

What is group 2 called and why

A

The alkaline earth metals
Because their oxides and hydroxides are alkaline

51
Q

What is the trend in atomic radius in group 2

A

Increases down the group
More electron shells
Bigger atoms

52
Q

What is the trend in melting point in group 2

A

Decreases down the group
Weaker metallic bonding
As metal ions get bigger the sea of delocalised e- are further from nucleus
Mg doesn’t follow trend as it has a different lattice structure

53
Q

What is the trend in 1st IE in group 2

A

Decreases down the group
e- are further from nucleus
More shielding
Weaker attraction from nucleus to electron

54
Q

How does group 2 metals react with water

A

Redox reaction
M + 2H20 –> M(OH)2 + H2
React more violently as you go down the group

55
Q

What is the solubility of group 2 hydroxides

A

They are increasingly soluble down the group
Mg - insoluble
Ca - Slightly soluble
Sr - Soluble
Ba - Soluble

56
Q

What is the solubility of group 2 sulphates

A

Sulphate solubility decreases down the group
Mg Soluble
Ca Slightly soluble
Sr and Ba insoluble

57
Q

What are the uses of Magnesium hydroxide

A

Treat constipation
Extract titanium

58
Q

Uses of Calcium hydroxide

A

Root canal fillings
Sewage treatment

59
Q

Uses of calcium oxide

A

used to manufacture cement
Ingredient for caustic soda

60
Q

Uses of calcium carbonate

A

Used to relive heartburn

61
Q

Uses of barium sulphate

A

Used in CAT scans

62
Q

Test for sulphate ions

A

Solution is acidified
Barium chloride is added
If sulphate ions are present, a white precipitate is formed
Ba2+ + SO4 2- –> BaSO4

63
Q

Why is the fluorine fluorine bond weak

A

This is due to the small size of the atoms which leads to a repulsion between electrons

64
Q

What is the trend in atomic radius in group 7

A

Increases down the group
More shells
Bigger atoms

65
Q

What is the trend in electronegativity in group 7

A

decreases down the group
bigger atoms
more shielding

66
Q

What is the trend in boiling points down group 7

A

increases
Stronger van der waal forces

67
Q

Trend in 1st IE down group 7

A

Decreasing
Atoms get bigger
More shielding

68
Q

What is the trend in oxidising ability down group 7

A

Decreasing
They gain electrons
Harder to gain electrons as atoms are larger and more shielding

69
Q

How strong of reducing agents are fluorine and chlorides

A

They aren’t very strong so a displacement reaction occurs instead

70
Q

How strong of a reducing agent is bromide

A

Bromide ion can reduce sulphuric acid
First is a displacement type reaction
NaBr + H2SO4 –> NaHSO4 + HBr
The HBr is oxidised in a redox reaction
2Br- +H2SO4 + 2H+ –> SO2 + 2H2O + Br2

71
Q

How strong a reducing agent is iodine

A

It is powerful enough to reduce sulphuric acid to sulphur dioxide then sulphur and then hydrogen sulphide
NaI + H2SO4 –> NaHSO4 + HI
2I- + H2SO4 + 2H+ –> I2 + SO2 + 2H2O
6I- + H2SO4 + 6H+ –> 3I2 + S + 4H2O
8I- + H2SO4 + 8H+ –> 4I2 + H2S + 4H2O

72
Q

What are the products from sodium fluoride with sulphuric acid

A

HF
Displacement reaction

73
Q

What are the products of NaCl reacting with H2SO4

A

HCl
Displacement reaction

74
Q

What are the products of NaBr reacting with H2SO4

A

HBr - displacement
SO2 - H2SO4 reduction
Br2 - Br- oxidation

75
Q

What are the products from NaI reacting with H2SO4

A

HI - displacement
SO2 and S and H2S - H2SO4 reduction
I2 - I- oxidation

76
Q

What are chlorine’s uses

A

Water treatment as its soluble in water
Cl2 + H2O –> HCl + HClO
This is a disporoportionation

77
Q

What is a disporoportionation

A

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

78
Q

What reaction does chlorine have with water in sunlight

A

2Cl2 + 2H2O –> 4HCl + O2

79
Q

What else can be used to chlorinate pools

A

Sodium chlorate
Cl2 + 2NaOH –> NaCl + NaClO + H2O

NaClO + H2O –> Na+ + OH- + HCLO

80
Q

Why are pools kept slightly acidic

A

in an alkaline solution the equilibrium would shift to the left

81
Q

What is the test for group 2 ions

A

Add sodium hydroxide
Add dilute sulphuric acid

82
Q

What are the results for the group 2 ions when sodium hydroxide is added

A

Magnesium - White precipitate
Calcium - White precipitate
Strontium - colourless solution
Barium - Colourless solution

83
Q

What are the results for the group 2 ions when sulphuric acid is added

A

Magnesium - Colourless solution
Calcium - Colourless solution
Strontium - slight white precipitate
Barium - White precipitate

84
Q

test for sulphate ions

A

HCl and barium chloride
Solution turns white, white precipitate formed

85
Q

What is the tests for chloride.bromide and iodide ions

A

Silver Nitrate
Chloride - White precipitate
Ag+ + Cl- –> AgCl
Bromide - Cream Insoluble
Ag+ + Cl- –> AgBr
Iodide - Yellow
Ag+ + I- –> AgI

86
Q

How does dilute ammonia react with silver chloride, bromide and Iodide

A

Dilute NH3
Chlorine - Colourless solution
AgCl + 2NH3 –> [Ag(NH3)2]+ + Cl-
Bromine - Precipitate
Iodine - Precipitate

87
Q

What are the tests for halide ions when in solid form

A

Add concentrated sulphuric acid
Chloride - Acid formed and misty gas formed
Bromide - Misty gas, orange vapour
Iodide - Turns acidic, Black solid bad egg smell, gas

88
Q

Test for carbonate ions

A

Add HCl
Lime water turns cloudy, Fizzy and colourless solution

89
Q

Test for hydroxide ions

A

Universal indicator turns purple

90
Q

Test for ammonia ions

A

Red litmus paper turns dark blue

91
Q

Test for ammonium ions

A

NaOH
Gas formed turns Red litmus paper blue

92
Q

How does concentrated ammonia react with silver chloride, bromide and Iodide

A

Chlorine - Colourless solution
AgCl + 2NH3 –> [Ag(NH3)2]+ + Cl-
Bromine - Colourless solution
AgBr + 2NH3 –> [Ag(NH3)2]+ + Br-
Iodine - Precipitate

93
Q

What does a brown precipitate mean when reacted with NaOH

94
Q

What is the observation of HCl

A

Steamy fumes

95
Q

What is the observation of HBr

A

Steamy Fumes

96
Q

What is the observation of Br2

A

Brown fumes

97
Q

What is the observation of SO2

A

Colourless Gas

98
Q

What is the observation of HI

A

Steamy Fumes

99
Q

What is the observation of I2

A

Purple Fumes

100
Q

What is the observation of SO2

A

Colourless gas

101
Q

What is the observation of S

A

Yellow Solid

102
Q

What is the observation H2S

A

Gas
Bad egg smell

103
Q

What is the reaction of chlorine with cold dilute sodium hydroxide

A

Cl2 + 2NaOH-> NaCl + NaClO + H2O
Sodium chlorate is an active ingredient in household bleach

104
Q

How does aluminium react with sodium hydroxide

A

White precipitate which dissolves in excess NaOH

105
Q

Who has a greater first ionisation energy, magnesium or Aluminium

A

Magnesium
Aluminium has covalent character

106
Q

What is the definition of periodicity

A

Repeating pattern/trends of physical or chemical properties/reactions

107
Q

What is a Lewis acid

A

a species that accepts an electron pair

108
Q

What is a Lewis base

A

a species that donates an electron pair

109
Q

What is a Bronsted Lowry base

A

It is any species that is capable of accepting a proton

110
Q

What is a Bronsted Lowry Acid

A

It is any species that is capable of donating a proton

111
Q

How do you differentiate sulfur dioxide and sulfur trioxide

A

Universal Indicator
SO2 - orange red
SO3 - Red

Chemistry A Level (20 decks)

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