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GCSE CHEMISTRY > P1- Chemical changes > Flashcards

P1- Chemical changes Flashcards

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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
Q

What do metals + acids make

A

Salt + Hydrogen (MASH)

26
Q

What do Carbonate + Acids make

A

Water + Carbon dioxide + Salt (CAWCS)

27
Q

What are the two components of a salt name

A

The first name comes from the metal/ alkali, the second name comes from the acid

28
Q

What is the ending of Hydrochloric acid

A

Chloride

29
Q

What is the ending of sulfuric acid

A

Sulfate

30
Q

What is the ending of Nitric acid

A

Nitrate

31
Q

What are the two ways of making salts

A

Acid reactions (AAWS) and Reactions between two salts (Soluble salt + Soluble salt -> Insoluble salt (s)

32
Q

Properties of insoluble salts

A

The solid cannot dissolve in solution, forms a precipitate, two soluble salts react to make an insoluble salt

33
Q

What does the strength of an acid depend on

A

The extent to which it ionises in water

34
Q

How ionised in water would a strong acid be

A

100% meaning that the acid will react very quickly as lots of collisions occur

35
Q

How ionised in water would a weak acid be

A

Only partially ionised in water

36
Q

Examples of strong acids

A

Hydrochloric acid, sulfuric acid, nitric acid

37
Q

Examples of weak acids

A

Citric acid, ethanoic acid, carbonic acid

38
Q

Examples of strong alkalis

A

Sodium hydroxide, lithium hydroxide

39
Q

Example of weak alkali

A

Ammonia

40
Q

What do all acids ionised in water to give

A

H+

41
Q

Hydrochloric acid (HCl) ->

A

H+ + Cl-

42
Q

Ethanoic acid (CH3COOH)

A

H+ + CH3COO-

43
Q

What does concentration refer to

A

The moles of acid (amount of acid) in a dm3 of solution (given volume)

44
Q

Example of increasing hydrogen ion concentration

A

10^-12, 10^-11, 10^-10, 10^-9 etc

45
Q

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

A

Concentration has decreased, so pH has increased, changed by x100 or two orders of magnitude so the pH would be 6

46
Q

What are titrations used for

A

Determining an unknown concentration of a solution using a known concentration (standard solution). They are generally neutralisation reactions

47
Q

What does adding an acid to alkali result in

A

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
Q

In the electrolysis of aqueous solutions what are the products at the anode (+)

A

If a hairline ion (group 7) is present, a halogen is formed and if not, oxygen is formed

49
Q

In the electrolysis of aqueous solutions what are the products at the cathode (-)

A

If the metal is more reactive than hydrogen, hydrogen gas is formed. If it less reactive, the metal is formed

50
Q

What are the industrial uses of electrolysis

A

Extracting reactive metals from their compounds, Purifying copper and Extracting brine

51
Q

Explain the effects of extracting reactive metals from their compounds

A

It is expensive due to the large amounts of electrical energy needed

52
Q

Explain the electrolysis of brine

A

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
Q

Explain electrolysis fro purifying copper

A

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
Q

What are the uses of Aluminium

A

Tin foil, planes, cans and electricity pylons

55
Q

Explain the use of cryolite

A

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

56
Q
A
57
Q
A

GCSE CHEMISTRY (9 decks)

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