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

Redox Chapter 7 - 10 and 22 Flashcards

(111 cards)

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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
How does Sodium react with oxygen
Vigorous reaction Burns with yellow flame 4Na + O2 --> 2Na2O White solid
26
How does magnesium react with oxygen
Vigorous reaction Burns with white flame 2Mg + O2 --> 2MgO
27
How does aluminium react with oxygen
Vigorous reaction 4Al + 3O2 --> 2Al2O3
28
How does silicon react with oxygen
Low reaction Requires heat Si + O2 --> SiO2
29
How does phosphorous react with oxygen
Red phosphorous must be heated for reaction White phosphorous reacts spontaneously P4 + 5O2 --> P4O10 White flame
30
How does sulphur react with oxygen
Sulphur melts easily Blue flame Pungent choking gas S + O2 --> SO2
31
What are the melting points of Non-Metal oxides
Silicon oxide has a giant covalent structure so high MP Phosphorous oxide and sulfur oxide are simple covalent molecules so low MP's
32
What are the properties of metal oxides
High MP and BP Mp increases across period as the charge is higher and so the forces are higher
33
How does sodium oxide react with water
Bubbles pH 13 Dissolves exothermically Na2O + H2O --> 2NaOH
34
How does magnesium oxide react with water
pH 9 Sparingly soluble MgO + H2O --> Mg(OH)2
35
How does aluminium oxide react with water
Insoluble Bonding is too strong
36
How does Silicon oxide react with water
Insoluble
37
How does phosphorous oxide react with water
Violent reaction pH 1 P4O10 + 6H2O --> 4H3PO4
38
How does sulfur dioxide react with water
pH 3 Soluble SO2 + H2O --> H2SO3 The product is a weak acid
39
How does Sodium and magnesium oxide react with acids and bases
They are both basic oxides and will react with acids Na2O + H2SO4 --> Na2SO4 + H2O MgO + H2SO4 --> MgSO4 + H2O
40
How does aluminium oxide react with acids and bases
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
41
How does Silicon dioxide react with bases
It acts as a weak acid with strong bases SiO2 + 2NaOH --> 2Na2SiO3 + H2O
42
How does phosphorous oxide react with bases
It reacts with bases It becomes phosphoric acid when in water H3PO4 + 3NaOH --> Na3PO4 + 3H2O
43
Does sulphur dioxide react with bases
It reacts SO2 + NaOH --> NaHSO4 NaHSO3 + NaOH --> Na2SO3 + H2O
44
Describe sodium oxide Appearance Structure Solubility with water pH in water Acid/base/amphoteric
White solid Ionic Dissolves exothermically 13 Base
45
Describe Magnesium oxide Appearance Structure Solubility with water pH in water Acid/base/amphoteric
White solid Ionic Sparingly soluble 9 Base
46
Describe aluminium oxide Appearance Structure Solubility with water pH in water Acid/base/amphoteric
White solid Ionic (covalent character) Insoluble 7 Amphoteric
47
Describe Silicon dioxide Appearance Structure Solubility with water pH in water Acid/base/amphoteric
White solid Giant covalent Insoluble 7 Acidic
48
Describe Phosphorous oxide Appearance Structure Solubility with water pH in water Acid/base/amphoteric
White solid Simple molecular Violent reaction 1 Acidic
49
Describe Sulfur dioxide Appearance Structure Solubility with water pH in water Acid/base/amphoteric
Gas Simple molecular Soluble 3 Acidic
50
What is group 2 called and why
The alkaline earth metals Because their oxides and hydroxides are alkaline
51
What is the trend in atomic radius in group 2
Increases down the group More electron shells Bigger atoms
52
What is the trend in melting point in group 2
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
What is the trend in 1st IE in group 2
Decreases down the group e- are further from nucleus More shielding Weaker attraction from nucleus to electron
54
How does group 2 metals react with water
Redox reaction M + 2H20 --> M(OH)2 + H2 React more violently as you go down the group
55
What is the solubility of group 2 hydroxides
They are increasingly soluble down the group Mg - insoluble Ca - Slightly soluble Sr - Soluble Ba - Soluble
56
What is the solubility of group 2 sulphates
Sulphate solubility decreases down the group Mg Soluble Ca Slightly soluble Sr and Ba insoluble
57
What are the uses of Magnesium hydroxide
Treat constipation Extract titanium
58
Uses of Calcium hydroxide
Root canal fillings Sewage treatment
59
Uses of calcium oxide
used to manufacture cement Ingredient for caustic soda
60
Uses of calcium carbonate
Used to relive heartburn
61
Uses of barium sulphate
Used in CAT scans
62
Test for sulphate ions
Solution is acidified Barium chloride is added If sulphate ions are present, a white precipitate is formed Ba2+ + SO4 2- --> BaSO4
63
Why is the fluorine fluorine bond weak
This is due to the small size of the atoms which leads to a repulsion between electrons
64
What is the trend in atomic radius in group 7
Increases down the group More shells Bigger atoms
65
What is the trend in electronegativity in group 7
decreases down the group bigger atoms more shielding
66
What is the trend in boiling points down group 7
increases Stronger van der waal forces
67
Trend in 1st IE down group 7
Decreasing Atoms get bigger More shielding
68
What is the trend in oxidising ability down group 7
Decreasing They gain electrons Harder to gain electrons as atoms are larger and more shielding
69
How strong of reducing agents are fluorine and chlorides
They aren't very strong so a displacement reaction occurs instead
70
How strong of a reducing agent is bromide
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
How strong a reducing agent is iodine
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
What are the products from sodium fluoride with sulphuric acid
HF Displacement reaction
73
What are the products of NaCl reacting with H2SO4
HCl Displacement reaction
74
What are the products of NaBr reacting with H2SO4
HBr - displacement SO2 - H2SO4 reduction Br2 - Br- oxidation
75
What are the products from NaI reacting with H2SO4
HI - displacement SO2 and S and H2S - H2SO4 reduction I2 - I- oxidation
76
What are chlorine's uses
Water treatment as its soluble in water Cl2 + H2O --> HCl + HClO This is a disporoportionation
77
What is a disporoportionation
A reaction in which the same species is both oxidised and reduced
78
What reaction does chlorine have with water in sunlight
2Cl2 + 2H2O --> 4HCl + O2
79
What else can be used to chlorinate pools
Sodium chlorate Cl2 + 2NaOH --> NaCl + NaClO + H2O NaClO + H2O --> Na+ + OH- + HCLO
80
Why are pools kept slightly acidic
in an alkaline solution the equilibrium would shift to the left
81
What is the test for group 2 ions
Add sodium hydroxide Add dilute sulphuric acid
82
What are the results for the group 2 ions when sodium hydroxide is added
Magnesium - White precipitate Calcium - White precipitate Strontium - colourless solution Barium - Colourless solution
83
What are the results for the group 2 ions when sulphuric acid is added
Magnesium - Colourless solution Calcium - Colourless solution Strontium - slight white precipitate Barium - White precipitate
84
test for sulphate ions
HCl and barium chloride Solution turns white, white precipitate formed
85
What is the tests for chloride.bromide and iodide ions
Silver Nitrate Chloride - White precipitate Ag+ + Cl- --> AgCl Bromide - Cream Insoluble Ag+ + Cl- --> AgBr Iodide - Yellow Ag+ + I- --> AgI
86
How does dilute ammonia react with silver chloride, bromide and Iodide
Dilute NH3 Chlorine - Colourless solution AgCl + 2NH3 --> [Ag(NH3)2]+ + Cl- Bromine - Precipitate Iodine - Precipitate
87
What are the tests for halide ions when in solid form
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
Test for carbonate ions
Add HCl Lime water turns cloudy, Fizzy and colourless solution
89
Test for hydroxide ions
Universal indicator turns purple
90
Test for ammonia ions
Red litmus paper turns dark blue
91
Test for ammonium ions
NaOH Gas formed turns Red litmus paper blue
92
How does concentrated ammonia react with silver chloride, bromide and Iodide
Chlorine - Colourless solution AgCl + 2NH3 --> [Ag(NH3)2]+ + Cl- Bromine - Colourless solution AgBr + 2NH3 --> [Ag(NH3)2]+ + Br- Iodine - Precipitate
93
What does a brown precipitate mean when reacted with NaOH
Iron 3
94
What is the observation of HCl
Steamy fumes
95
What is the observation of HBr
Steamy Fumes
96
What is the observation of Br2
Brown fumes
97
What is the observation of SO2
Colourless Gas
98
What is the observation of HI
Steamy Fumes
99
What is the observation of I2
Purple Fumes
100
What is the observation of SO2
Colourless gas
101
What is the observation of S
Yellow Solid
102
What is the observation H2S
Gas Bad egg smell
103
What is the reaction of chlorine with cold dilute sodium hydroxide
Cl2 + 2NaOH-> NaCl + NaClO + H2O Sodium chlorate is an active ingredient in household bleach
104
How does aluminium react with sodium hydroxide
White precipitate which dissolves in excess NaOH
105
Who has a greater first ionisation energy, magnesium or Aluminium
Magnesium Aluminium has covalent character
106
What is the definition of periodicity
Repeating pattern/trends of physical or chemical properties/reactions
107
What is a Lewis acid
a species that accepts an electron pair
108
What is a Lewis base
a species that donates an electron pair
109
What is a Bronsted Lowry base
It is any species that is capable of accepting a proton
110
What is a Bronsted Lowry Acid
It is any species that is capable of donating a proton
111
How do you differentiate sulfur dioxide and sulfur trioxide
Universal Indicator SO2 - orange red SO3 - Red

Chemistry A Level (20 decks)

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