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IGCSE Chemistry > chemical reactivity, metal extraction, acid base salt > Flashcards

chemical reactivity, metal extraction, acid base salt Flashcards

1
Q

Metal + acid ->

A

Salt + hydrogen

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2
Q

Metal oxide + acid ->

A

Salt + water

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3
Q

Metal hydroxide + acid ->

A

salt + water

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4
Q

Metal carbonate + acid ->

A

salt + carbon dioxide + water

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5
Q

Define saturated solution

A

A solution that can hold no more solute / solid at the specified temperature

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6
Q

What is an acid?

A

A proton donor

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7
Q

What is difference between weak and strong acids?

A

1) Strong acids fully ionise
2) Weak acid partially ionise

The ionisation of a strong acid is shown by using a → in the equation, showing it is non-reversible
The ionisation of a weak acid is shown by using a rightwards harpoon over leftwards harpoonin the equation, showing it is reversible
H2SO3 (reversible arrow sign) HSO3– + H+

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8
Q

Hydorchloric acid

A

HCL

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9
Q

What is a base? in terms of particles

A

Protons acceptors

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10
Q

Define water of crystallisation

A

Water molecules present in hydrated crystals

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11
Q

What are amphoteric oxides?

A

Oxides that react with acids & bases the same.
Both reaction produce salt and water

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12
Q

Are metal oxides base or acidic?

A

Metal oxides are usually basic

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13
Q

Give examples of amphoteric oxides

A

Aluminum oxide Al2O3
Zinc oxide ZnO

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14
Q

When hydrochloric acid dissolves into water the acid compound ionises
give ionic equation

A

HCL(aq) —> H+ (aq) + CL- (aq)

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15
Q

Sulfuric acid formula

A

H2SO4

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16
Q

Ammonia formula

A

NH3

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17
Q

Aqueous solutions of acids contain

A

H+ ions

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18
Q

Aqueous solutiosn of base contain

A

OH- ions

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19
Q

Litmus paper with acid

A

Red

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20
Q

Litmus paper with base

A

Blue

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21
Q

Thymolphthalein with acid

A

Colourless

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22
Q

Methyl Orange with base

A

Red

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23
Q

Methyl orange with acid

A

Yellow

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24
Q

Neutralisation reaction between acid and alkaline to produce water ionic equation

A

H+ (aq) + OH-(aq) -> H2O(L)

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25
Q

Base vs alkali

A

Base are oxides or hydroxides of metals
Alkali are soluble bases

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26
Q

List the reactivity series

A

Please - Potassium
Stop - Sodium
Calling - Calcium
Me - Magnesium
A - Aluminium
Careless - Carbon
Zebra - Zinc
Instead - Iron
Try - Tin
Learning - Lead
How - Hydrogen
Copper - Copper
Saves - Silver
Gold -Gold

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27
Q

Group 1 reactions with cold water

A

More fire and explosives as you go down the group

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28
Q

reaction of magnesium with steam

A

Magnesium burns in steam to produce white magnesium oxide and hydrogen gas

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28
Q

Neutralisation equation

A

acid + alkali = salt + water

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29
Q

define ionise

A

When ions in an ionic solid separate during dissolving

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30
Q

When an alkali like sodium hydroxide dissolves give ionic equation

A

NaOH -> Na+ + OH-

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31
Q

The strength of an acid is also a measure of…

A

How much the acid compound ionises

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32
Q

Strong acid will… [2]

A

Fully ionise
Completely disasscoiate in water

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33
Q

Weak acid will… [2]

A

Partially ionise
partially dissociate in water

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34
Q

Ethanoic acid (Vinegar) & Citric acid weak or strong

A

Weak acid

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35
Q

Good method writing [5]

A

1) Start each step with a command word (Measure, pour etc)
2) Include at least 2 control variables
3) Include measurements
4) Include scientific equippments
5) Include repeats for the same measurements to identify anomalies and calculate a mean

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36
Q

Calculate mass of water from using crystallisation

A

Mass of hydrated salt - mass of anhydrous salt

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37
Q

Define Precipitation

A

2 soluble ionic salts are combined, they can form an insoluble salt, a precipitate

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38
Q

How is Calcium oxide manufactured from limestone

A

By thermal decomposition of calcium carbonate

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39
Q

Slag

A

the substance that is formed when impurities in the ore react with calcium hydroxide (Limewater)

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40
Q

What gas do K, Li, and Na release when reacting with water

41
Q

Non-metal oxides are acidic or alkaline

42
Q

Ammonium chloride + Base =

43
Q

Name of aluminium ore

44
Q

What is another name for iron ore

45
Q

Limestone largely contains…

A

Calcium carbonate

46
Q

Two functions of the coke used in the blast furnace are

A

1) To provide heat
2) To produce carbon dioxide

47
Q

Limewater is another name for..

A

aqueous solution of calcium hydroxide

48
Q

Making salt practical using sulfuric acid and copper oxide [7]

A

1)Measure 20ml of sulfuric acid
2) Add copper oxide in excess and stir
3) Filter the mixture
4) Place filtrate into evaporating basin
5) Heat gently on yellow flame
6) Stop heating when the liquid has reduced by half
7)Leave the mixture to dry on drying rack and crystalise

49
Q

Make salt from sulfuric acid and Copper oxide word equation

A

Sulfuric acid + copper oxide -> copper sulfat + water

50
Q

How to know if gas is sulfur dioxide?

A

1) Add permenganate paper
2) Turn purple to colourless

51
Q

How to know if gas is ammonia?

A

1) Add damp red litmus paper
2) Turns blue (Ammonia is an alkali/base)

52
Q

Sulfite vs sulfate

A

sulfite ion is SO32- and a sulfate ion is SO42-

53
Q

How to know if gas is carbon dioxide?

A

1) Bubble gas through limewater
2) White precipitate of calcium carbonate forms and turns lime water cloudy white

54
Q

How to know if gas is chlorine?

A

1) Add damp blue litmus paper
2) Turns bleach

55
Q

How to know if gas is oxygen?

A

1) Add a glowing splint
2) Relights

56
Q

Flame test barium

A

Light green

57
Q

Flame test calcium

A

Orange-red

58
Q

Flame test copper(II)

A

Blue - green

58
Q

Flame test sodium

59
Q

Flame test potassium

59
Q

Flame test lithium

60
Q

How to test for metal ions? [2]

A

1) Add sodium hydroxide solution
2) Add ammonium NH3

61
Q

How to test for negative ion (Anion) [4]

A

1) Carbonates test
2) Halides test
3) Sulphate test
4) Nitrate test

62
Q

Describe carbonates test

A

1) Add dilute acid to a carbonate
2) It should fizz and produce carbon dioxde

63
Q

Describe halides (Group 7) test

A

1) Add nitric acid then add silver nitrate
2) Chlorides = white precipitate
3) Bromides = Cream precipitate
4) Iodides (Anion with valency of -1) = Pale yellow precipitate

64
Q

Describe sulphate test

A

1) Add dilute hydrochloric acid then barium chloride solution
2) White precipitate to show sulphate ions presence

65
Q

Describe nitrates test

A

1) Aluminium foil + Sodium hydroxide
2) Ammonia gas

66
Q

Define displacement

A

When a more reactive element swaps places with a less reactive element in a compound

67
Q

What is released when acid dissoaciates in water?

A

protons are released when an acid dissociates in water

68
Q

All sodium, potassium and ammonium salts are soluble or insoluble

69
Q

All nitrates are soluble or insoluble

70
Q

Most chlorides, bromides, and iodies (Halides) are soluble or insoluble

71
Q

Most sulphates, except lead, barium, and calcium are soluble or insoluble

72
Q

Sodium, potassium, and ammonium carbonates are soluble or insoluble

73
Q

Sodium, potassium, ammonium, and calcium hydroxide are soluble or insoluble

74
Q

Silver and lead halides are soluble or insoluble

75
Q

lead, barium, and calcium sulphate are soluble or insoluble

76
Q

Most carbonates, except sodium, potassium, and ammonium are soluble or insoluble

77
Q

Most hydroxides, except sodium, potassium, and ammonium are soluble or insoluble

78
Q

Gas test hydrogen

A

ignites easily and will burn with a ‘squeaky pop’

79
Q

Iron(II) and Iron(III) colours and acid used

A

Iron(II) forms green precipitate
Iron(III) forms brown precipitate
uses sodium hydroxide

80
Q

How many different salts could be made from a supply of dilute sulfuric acid, dilute hydrochloric
acid, copper, magnesium oxide and zinc carbonate?

A

4 because copper doesnt really react with dilute acids

81
Q

A pungent smelling gas is produced when ammonium carbonate is added. base or acid

82
Q

Reaction of metal oxide with carbon makes a metal more or less reactive

A

Less reactive because its being replaced in displacement reaction

83
Q

How is carbon dioxide converted into carbon monoxide in the blast furnace?

A

Carbon dioxide reacts with coke

84
Q

Write the chemical equation of calcium oxide with silicon(IV) oxide and state the type of reaction

A

CaO + SiO2 -> CaSiO3
Acid-base reaction

85
Q

Why must the high levels of carbon be lowered before the iron becomes a useful material?

A

Iron becomes too brittle

86
Q

How is carbon removed from the iron?

A

By oxygen blowing in

87
Q

Equvilance point definition
include graph

A

point in titration at which the amount of titrant added is just enough to completely neutralize the solution.
(Graph will show sharp increase at one point)

88
Q

Ore definition

A

Rock containing enough metal to make it worthwhile extracting

89
Q

Word equation of the extraction of iron from iron oxide include which gets oxidised and reduced

A

Iron oxide + carbon -> Iron + carbon dioxide
Carbon gains oxygen oxidation
Iron loses oxygen reduction

90
Q

Define thermal decomposition

A

Chemical decompisiton by heat

91
Q

Tin nitrate thermal decompose to? Sn(NO3)4

A

SnO2 + NO2

92
Q

Name an acidic and alkaline oxide

A

`1) CO2 is acidic
2) NaO alkaline

93
Q

Are non metal oxides acidic or basic

A

Usually acidic

94
Q

Copper (II) colour

95
Q

How are metals above carbon in reactivity series extracted

A

Electrolysis

96
Q

How are metals below carbon in reactivity series extracted

A

Displacement

97
Q

1 use of slaked lime

98
Q

How to get hydrogen gas from metals in the reactivity series and hydrochloric acid?

A

All metals more reactive than hydrogen will release hydrogen when reacting with hydrochloric acid

99
Q

How to test anhydrous copper (II) sulphate with water

A

White (dry) to blue (water)

IGCSE Chemistry (10 decks)

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