P1- Chemical changes Flashcards

1
Q

Reactivity series from highest to lowest

A

Potassium, Sodium, Lithium, Calcium, Magnesium, Aluminium, Carbon, Zinc, Iron, Tin, Lead, Hydrogen, Copper, Silver, Gold

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2
Q

What are ionic equations

A

Equations that show only the atoms and ions that change in a reaction

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3
Q

How to create an ionic equation

A

Write a balanced equation, fill in state symbols, split all aqueous substances, cancel spectator ions (ions that remain unchanged on the LHS and RHS of the chemical equation

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4
Q

What is oxidation

A

Loss of electrons, gain of oxygen

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5
Q

What is an ore

A

An ore is a rock containing enough metal to make it economically worth extracting. Some unreactive metals like gold can be found as the metal itself and chemical separation is not needed

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6
Q

What is reduction

A

Gain of electrons, removal of oxygen

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7
Q

Compound for Bauxite

A

Aluminium Oxide (Al2O3)

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8
Q

Compound for Haematite

A

Iron oxide (Fe2O3)

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9
Q

Compound for Malachite

A

Copper carbonate (CuCO3)

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10
Q

Examples of unreactive metals

A

Copper, Silver, Gold, Plantinum

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11
Q

How are unreactive metals extracted

A

Little or no extraction is needed

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12
Q

Examples of more reactive metals

A

Zinc, Iron, Tin, Lead

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13
Q

How are more reactive metals extracted

A

Usually extracted by reduction, displacement reaction by heating with carbon to remove oxygen

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14
Q

Examples of very reactive metals

A

Potassium, Sodium, Calcium, Magnesium, Aluminium

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15
Q

How are very reactive metals extracted

A

Extracted using electrolysis

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16
Q

What does carbon + metal oxide make

A

Carbon dioxide + metal, displacement reaction

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17
Q

What is an alkali

A

A hydroxide that can be dissolved in water (soluble) e.g sodium hydroxide solution

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18
Q

What are bases

A

Substances that neutralise acids e.g metal oxides and metal hydroxides

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19
Q

What are acids (examples)

A

Hydrochloric acid (HCl), Sulfuric acid (H2SO4) and Nitric acid (HNO3)

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20
Q

What do all acids from when they are dissolved in water

A

H+ ions

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21
Q

What ions are responsible for making a solution alkaline

A

OH- ions

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22
Q

How to measure pH

A

Using litmus paper and universal indicator

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23
Q

What do Alkalis + Acids make

A

Water + Salt (AAWS)

24
Q

What do Bases + Acids make

A

Water + Salt (BAWS)

25
What do metals + acids make
Salt + Hydrogen (MASH)
26
What do Carbonate + Acids make
Water + Carbon dioxide + Salt (CAWCS)
27
What are the two components of a salt name
The first name comes from the metal/ alkali, the second name comes from the acid
28
What is the ending of Hydrochloric acid
Chloride
29
What is the ending of sulfuric acid
Sulfate
30
What is the ending of Nitric acid
Nitrate
31
What are the two ways of making salts
Acid reactions (AAWS) and Reactions between two salts (Soluble salt + Soluble salt -> Insoluble salt (s)
32
Properties of insoluble salts
The solid cannot dissolve in solution, forms a precipitate, two soluble salts react to make an insoluble salt
33
What does the strength of an acid depend on
The extent to which it ionises in water
34
How ionised in water would a strong acid be
100% meaning that the acid will react very quickly as lots of collisions occur
35
How ionised in water would a weak acid be
Only partially ionised in water
36
Examples of strong acids
Hydrochloric acid, sulfuric acid, nitric acid
37
Examples of weak acids
Citric acid, ethanoic acid, carbonic acid
38
Examples of strong alkalis
Sodium hydroxide, lithium hydroxide
39
Example of weak alkali
Ammonia
40
What do all acids ionised in water to give
H+
41
Hydrochloric acid (HCl) ->
H+ + Cl-
42
Ethanoic acid (CH3COOH)
H+ + CH3COO-
43
What does concentration refer to
The moles of acid (amount of acid) in a dm3 of solution (given volume)
44
Example of increasing hydrogen ion concentration
10^-12, 10^-11, 10^-10, 10^-9 etc
45
If an acid has a concentration if 1.0 x10^-4 mol/dm3 and a pH if 4, what would the pH be of the acid if it’s concentration was 1.0 x 10^-6
Concentration has decreased, so pH has increased, changed by x100 or two orders of magnitude so the pH would be 6
46
What are titrations used for
Determining an unknown concentration of a solution using a known concentration (standard solution). They are generally neutralisation reactions
47
What does adding an acid to alkali result in
A neutralisation reaction. The point at which enough acid has been added to completely react with the alkali is called the end point showing using a chemical called an indicator
48
In the electrolysis of aqueous solutions what are the products at the anode (+)
If a hairline ion (group 7) is present, a halogen is formed and if not, oxygen is formed
49
In the electrolysis of aqueous solutions what are the products at the cathode (-)
If the metal is more reactive than hydrogen, hydrogen gas is formed. If it less reactive, the metal is formed
50
What are the industrial uses of electrolysis
Extracting reactive metals from their compounds, Purifying copper and Extracting brine
51
Explain the effects of extracting reactive metals from their compounds
It is expensive due to the large amounts of electrical energy needed
52
Explain the electrolysis of brine
The salt solution brine produces chlorine (for disinfectants and plastics), hydrogen (for ammonia, fertilisers and margarine) and sodium hydroxide (for soap and cleaning agents)
53
Explain electrolysis fro purifying copper
The copper for wiring etc needs to be more pure than that produced in a blast furnace. Electrolysis is used to convert impure copper to pure copper
54
What are the uses of Aluminium
Tin foil, planes, cans and electricity pylons
55
Explain the use of cryolite
Aluminium oxide has a high melting point which is a problem as it needs a lot of energy and is expensive, To help with this, it is mixed with cryolite which lowers the melting point
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