chemical reactivity, metal extraction, acid base salt Flashcards
1
Q
Metal + acid ->
A
Salt + hydrogen
2
Q
Metal oxide + acid ->
A
Salt + water
3
Q
Metal hydroxide + acid ->
A
salt + water
4
Q
Metal carbonate + acid ->
A
salt + carbon dioxide + water
5
Q
Define saturated solution
A
A solution that can hold no more solute / solid at the specified temperature
6
Q
What is an acid?
A
A proton donor
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+
8
Q
Hydorchloric acid
A
HCL
9
Q
What is a base? in terms of particles
A
Protons acceptors
10
Q
Define water of crystallisation
A
Water molecules present in hydrated crystals
11
Q
What are amphoteric oxides?
A
Oxides that react with acids & bases the same.
Both reaction produce salt and water
12
Q
Are metal oxides base or acidic?
A
Metal oxides are usually basic
13
Q
Give examples of amphoteric oxides
A
Aluminum oxide Al2O3
Zinc oxide ZnO
14
Q
When hydrochloric acid dissolves into water the acid compound ionises
give ionic equation
A
HCL(aq) —> H+ (aq) + CL- (aq)
15
Q
Sulfuric acid formula
A
H2SO4
16
Q
Ammonia formula
A
NH3
17
Q
Aqueous solutions of acids contain
A
H+ ions
18
Q
Aqueous solutiosn of base contain
A
OH- ions
19
Q
Litmus paper with acid
A
Red
20
Q
Litmus paper with base
A
Blue
21
Q
Thymolphthalein with acid
A
Colourless
22
Q
Methyl Orange with base
A
Red
23
Q
Methyl orange with acid
A
Yellow
24
Q
Neutralisation reaction between acid and alkaline to produce water ionic equation
A
H+ (aq) + OH-(aq) -> H2O(L)
25
Base vs alkali
Base are oxides or hydroxides of metals
Alkali are soluble bases
26
List the reactivity series
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
27
Group 1 reactions with cold water
More fire and explosives as you go down the group
28
reaction of magnesium with steam
Magnesium burns in steam to produce white magnesium oxide and hydrogen gas
28
Neutralisation equation
acid + alkali = salt + water
29
define ionise
When ions in an ionic solid separate during dissolving
30
When an alkali like sodium hydroxide dissolves give ionic equation
NaOH -> Na+ + OH-
31
The strength of an acid is also a measure of...
How much the acid compound ionises
32
Strong acid will... [2]
Fully ionise
Completely disasscoiate in water
33
Weak acid will... [2]
Partially ionise
partially dissociate in water
34
Ethanoic acid (Vinegar) & Citric acid weak or strong
Weak acid
35
Good method writing [5]
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
36
Calculate mass of water from using crystallisation
Mass of hydrated salt - mass of anhydrous salt
37
Define Precipitation
2 soluble ionic salts are combined, they can form an insoluble salt, a precipitate
38
How is Calcium oxide manufactured from limestone
By thermal decomposition of calcium carbonate
39
Slag
the substance that is formed when impurities in the ore react with calcium hydroxide (Limewater)
40
What gas do K, Li, and Na release when reacting with water
Hydrogen
41
Non-metal oxides are acidic or alkaline
Acidic
42
Ammonium chloride + Base =
Ammonia
43
Name of aluminium ore
Bauxite
44
What is another name for iron ore
Hematite
45
Limestone largely contains...
Calcium carbonate
46
Two functions of the coke used in the blast furnace are
1) To provide heat
2) To produce carbon dioxide
47
Limewater is another name for..
aqueous solution of calcium hydroxide
48
Making salt practical using sulfuric acid and copper oxide [7]
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
Make salt from sulfuric acid and Copper oxide word equation
Sulfuric acid + copper oxide -> copper sulfat + water
50
How to know if gas is sulfur dioxide?
1) Add permenganate paper
2) Turn purple to colourless
51
How to know if gas is ammonia?
1) Add damp red litmus paper
2) Turns blue (Ammonia is an alkali/base)
52
Sulfite vs sulfate
sulfite ion is SO32- and a sulfate ion is SO42-
53
How to know if gas is carbon dioxide?
1) Bubble gas through limewater
2) White precipitate of calcium carbonate forms and turns lime water cloudy white
54
How to know if gas is chlorine?
1) Add damp blue litmus paper
2) Turns bleach
55
How to know if gas is oxygen?
1) Add a glowing splint
2) Relights
56
Flame test barium
Light green
57
Flame test calcium
Orange-red
58
Flame test copper(II)
Blue - green
58
Flame test sodium
yellow
59
Flame test potassium
lilac
59
Flame test lithium
Red
60
How to test for metal ions? [2]
1) Add sodium hydroxide solution
2) Add ammonium NH3
61
How to test for negative ion (Anion) [4]
1) Carbonates test
2) Halides test
3) Sulphate test
4) Nitrate test
62
Describe carbonates test
1) Add dilute acid to a carbonate
2) It should fizz and produce carbon dioxde
63
Describe halides (Group 7) test
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
Describe sulphate test
1) Add dilute hydrochloric acid then barium chloride solution
2) White precipitate to show sulphate ions presence
65
Describe nitrates test
1) Aluminium foil + Sodium hydroxide
2) Ammonia gas
66
Define displacement
When a more reactive element swaps places with a less reactive element in a compound
67
What is released when acid dissoaciates in water?
protons are released when an acid dissociates in water
68
All sodium, potassium and ammonium salts are soluble or insoluble
soluble
69
All nitrates are soluble or insoluble
soluble
70
Most chlorides, bromides, and iodies (Halides) are soluble or insoluble
Soluble
71
Most sulphates, except lead, barium, and calcium are soluble or insoluble
soluble
72
Sodium, potassium, and ammonium carbonates are soluble or insoluble
soluble
73
Sodium, potassium, ammonium, and calcium hydroxide are soluble or insoluble
soluble
74
Silver and lead halides are soluble or insoluble
insoluble
75
lead, barium, and calcium sulphate are soluble or insoluble
insoluble
76
Most carbonates, except sodium, potassium, and ammonium are soluble or insoluble
insoluble
77
Most hydroxides, except sodium, potassium, and ammonium are soluble or insoluble
insoluble
78
Gas test hydrogen
ignites easily and will burn with a 'squeaky pop'
79
Iron(II) and Iron(III) colours and acid used
Iron(II) forms green precipitate
Iron(III) forms brown precipitate
uses sodium hydroxide
80
How many different salts could be made from a supply of dilute sulfuric acid, dilute hydrochloric
acid, copper, magnesium oxide and zinc carbonate?
4 because copper doesnt really react with dilute acids
81
A pungent smelling gas is produced when ammonium carbonate is added. base or acid
Base
82
Reaction of metal oxide with carbon makes a metal more or less reactive
Less reactive because its being replaced in displacement reaction
83
How is carbon dioxide converted into carbon monoxide in the blast furnace?
Carbon dioxide reacts with coke
84
Write the chemical equation of calcium oxide with silicon(IV) oxide and state the type of reaction
CaO + SiO2 -> CaSiO3
Acid-base reaction
85
Why must the high levels of carbon be lowered before the iron becomes a useful material?
Iron becomes too brittle
86
How is carbon removed from the iron?
By oxygen blowing in
87
Equvilance point definition
include graph
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
Ore definition
Rock containing enough metal to make it worthwhile extracting
89
Word equation of the extraction of iron from iron oxide include which gets oxidised and reduced
Iron oxide + carbon -> Iron + carbon dioxide
Carbon gains oxygen oxidation
Iron loses oxygen reduction
90
Define thermal decomposition
Chemical decompisiton by heat
91
Tin nitrate thermal decompose to? Sn(NO3)4
SnO2 + NO2
92
Name an acidic and alkaline oxide
`1) CO2 is acidic
2) NaO alkaline
93
Are non metal oxides acidic or basic
Usually acidic
94
Copper (II) colour
Lilac
95
How are metals above carbon in reactivity series extracted
Electrolysis
96
How are metals below carbon in reactivity series extracted
Displacement
97
1 use of slaked lime
cement
98
How to get hydrogen gas from metals in the reactivity series and hydrochloric acid?
All metals more reactive than hydrogen will release hydrogen when reacting with hydrochloric acid
99
How to test anhydrous copper (II) sulphate with water
White (dry) to blue (water)
