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1
Q

Electrolysis

A

splitting up of substances using current

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2
Q

anode

reaction =>

A

oxidation
(rac = reduction at cathode)

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3
Q

cathode

reaction =>

A

reduction
(rac = reduction at cathode)

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4
Q

anode

metal/non-metal =>

A

non - metal
(namc = non-metal anode metal cathode)

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5
Q

cathode

metal/non-metal =>

A

metal
(namc = non-metal anode metal cathode)

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6
Q

aluminium ore

A

bauxite

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7
Q

metals that do not conduct

A

graphite

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8
Q

inert

A

doesnt react/ corrode

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9
Q

Substance remaining in solution that is not displaced

A

most reactive

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10
Q

Element that is released at anode

A

family 7 (halogen) / 02

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11
Q

substance released at cathode

A

reactivity series

h2
copper
ag (silver)
gold
platinum

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12
Q

electroplating
cathode is a _

A

conductor

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13
Q

electroplating
cathode is a _

A

conductor

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14
Q

Ammonia FORMULA

A

NH3

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15
Q

Ammonium

A

NH4

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16
Q

Nitrate

A

NO3

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17
Q

Reactivity series phrase

A

Please Send Cats, Monkeys And Zebras In Lovely Cages of Silver, Gold and Platinum

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18
Q

Reactivity series

A

5
Potassium - please
Sodium - send
Calcium - cats
Magnesium - monkeys
Aluminum - and

Carbon

3
Zinc - zebras
Iron - in
Lead - lovely

Hydrogen

3
Copper - cages of
Silver - silver
Goldsliver - gold
Platinum -platinum

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19
Q

Electrolysis
Metals are produced at

A

Non-metal - Anode (+)
Metal - Catode (-)

Anode = + (anions -)
Cathode = - (cations +)

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20
Q

Electrolysis
Metals are produced at

A

Non-metal - Anode (+)
Metal - Catode (-)

Catode = - (cations +)
Anode = + (anions -)

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21
Q

Equation at anode (reduction/oxidation)

A

Oxidation

RAC (Reduction at cation)

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22
Q

Eq at cathode

Reduction/oxidation

A

Reduction

RAC (Reduction at cathode)

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23
Q

Metal + acid

A

metal hydroxide + hydrogen

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24
Q

Metal + steam

A

metal oxide + hydrogen

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25
Aluminium ore
Bauxite
26
Bauxite
Aluminium ore
27
How is aluminium extracted
Electrolysis
28
Transition elements valency
Variable
29
pH of sugar
7
30
Colour of pH 7
Green
31
CH4
Methane
32
CO
Carbon monoxide
33
Methane
CH4
34
Most abundant metal in earth's crust
Aluminium
35
Reactive def
Strong drive to give up electrons and form ions
36
Do salts conduct electricity
Some salts, such as sodium chloride (NaCl), potassium nitrate (KNO3), and calcium chloride (CaCl2), dissolve in water and dissociate into ions, which makes them good conductors of electricity. These salts are called electrolytes. Other salts, such as silver chloride (AgCl) and lead sulfate (PbSO4), do not dissociate in water and do not conduct electricity. These salts are not electrolytes. So, whether or not a salt is an electrolyte depends on its ability to dissociate into ions in water.
37
What is rusting Oxidation or reduction
Oxidation
38
What does rust require
Both water and air
39
Weaker acids dissociate
Less
40
Acidic oxides
Dissolve in water to form acids
41
Amphoteric oxides
React with both acids and alkaline
42
Neutral oxides
React with neither acids not alkaline
43
Eg of amphoteric oxides
Aluminium oxide
44
Eg of neutral oxides
Carbon monoxide
45
Galvanized
Coating iron with zinc Zinc is more reactive so it gets oxidised rather than the iron
46
Brine
Conc NaCl
47
In electrolysis of brine what is the cathode made out of
Titanium
48
In electrolysis of brine what is the anode made out of
Nickel
49
Down a group of metals, elements become more/less reactive
Down a group of metals, elements become morereactive
50
Table moves from metals on the ____ to non-metals on the ____. | left/right
Table moves from metals on the left to non-metals onthe right.
51
With non-metals, going down a group, reactivity increases/decreases
With non-metals, going down a group, reactivitydecreases
52
Alkali metals are what
Group 1
53
In periodic table:- groups vs periods
Groups - columns Periods - rows
54
Alkali metals (chemical properties)
* Readily react with oxygen andwater; stored in oil * React violently with chlorine * Burst into flames when heated with oxygen[red flame for lithium; yellow flame forsodium; lilac flame forpotassium] * Produce soluble white compounds. * React with water to form alkaline metal and hydrogen gas
55
Alkali physical properties
* Good conductors of heat andelectricity * Soft and easy to cut * Shiny when freshly cut * Low melting and boiling pointscompared to most metals. * Low densities for metals
56
Rubidium reacts with water
* Explodes with spark * Produces Rubidium hydroxide
57
Caesium reacts with water
* Violent explosion * Produces caesium hydroxide
58
Francium reacts with water
* Cannot predictive due to radioactive reactivity
59
Test ammonia (NH3)
Damp red litmus paper turns blue
60
Test CO2
Turns lime water milky
61
Chlorine test
Bleaches red/blue litmus paper
62
Hydrogen test
Place lighted splint, squeaky pop
63
Oxygen test
Place glowing splint, splint relights
64
Halogen Properties
* Down the group; size, massand density increase * Poisonous * Down the group, colordarkens * Diatomic; form halide ions indisplacement reaction * Reactivity decreases down thegroup, * because it has to gain anelectron, * so the closer the electron is tothe positive nucleus the moreeasily it will be gained, * so atoms with fewer shells willreact more easily. * Do not conduct electricity * melting point increases downthe group * Brittle and crumbly when solid
65
Halogens are group
Group 17
66
States and Colors, at RTP: * Fluorine- * Chlorine- * Bromine- * Iodine-
States and Colors, at RTP: * Fluorine- Yellow gas * Chlorine- Green gas * Bromine- Red liquid * Iodine- Black solid
67
Transition metals properties
* High melting points (except mercury) * Malleable and ductile * Good conductors of heat & electricity (silver is the best) * High density * Have no trend in reactivity * Used as catalysts * Form colored compounds * Can form complex ions as they have variable valences
68
Nobel gases are group
group 18
69
Halogens properties
* Density increases down thegroup * Monoatomic and colorless * M.P. and B.P. increases down the group * Don’t conduct electricity * Inert due to full outer shell electrons
70
Physical properties of metals
Physical Properties 1.Good conductors of heat and electricity 2.High melting and boiling points 3.Malleable and Ductile 4.High densities 5.Solids at room temperature (except mercury)
71
Chemical properties of metals
* Form positive ions * Form basic oxides that dissolve in water
72
Brass alloy
* Copper and zinc * Stronger and more resistant to corrosion * Used for Electrical fittings, car radiators
73
Bronze alloy
* Copper and tin * Harder,stronger andsonorous * Statues, springs,coins
74
Stainless steel alloy
* Iron, carbon,chromium and nickel * resistant to corrosion * Kitchen sinks,cutlery, surgical instruments
75
Why are alloys stronger than the pure metals
Metal alloys, due to the irregularity in atom sizes andstructure which stop layers from sliding over each other,are stronger | There structure are not like a grid but are more cramped

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