1
Q
Test for metal cations
A
Flame test
2
Q
Test for lithium
A
Flame test - crimson red
3
Q
Test for potassium
A
Flame test - lilac
4
Q
Test for sodium
A
Flame test - yellow/orange
5
Q
Test for calcium
A
Flame test - red/orange
6
Q
Test for copper
A
Flame test - green
7
Q
Test for water
A
Using anhydrous copper(II) sulfate
Positive - clear to blue colour change
8
Q
Composition of dry air
A
Nitrogen 78%
Oxygen 21%
Argon 1%
Other gases 0.04%
9
Q
Formula for enthalpy change
A
Q = mc ΔT
10
Q
Test for carbon dioxide
A
Bubble through limewater, limewater turns milky when shaken with the gas
11
Q
Group 1 metals (down the group)
A
Li, Na, K
12
Q
Group 2 (down the group)
A
Be, Mg, Ca
13
Q
Group 13 (down the group)
A
B, Al, (Ga)
14
Q
Group 14 (down the group)
A
C, Si
15
Q
Group 15 (down the group)
A
N, P
16
Q
Group 16 (down the group)
A
O, S
17
Q
Group 17 (down the group)
A
F, Cl, Br, I
18
Q
Group 18 (down the group)
A
Ne, Ar
19
Q
Which one is exothermique and which one is endothermic: bond breaking and bond making?
A
Bond breaking = endothermic
Bond making = exothermic
20
Q
Pale yellow gas - which halogen?
A
Fluorine
21
Q
Green gas - which halogen?
A
Chlorine
22
Q
Red-brown liquid - which halogen?
A
Bromine
23
Q
Grey solid - which halogen?
A
Iodine
24
Q
Disproportionation reaction
A
Redox reaction where a single species is reduced and oxidided simultaneously
25
Convert 1mm to micrometers
1000 micrometers
26
Mass number
protons + neutrons
26
Atomic number
proton number
27
how are elements arranged
In order of increasing atomic number
28
Avogadro's constant (number of particles in one mole)
6.022 x 10^23
29
convert tonnes to kilograms
1 tonne = 1000 kilograms
29
convert kg to g
1kg = 1000 g
30
percentage yield
(actual yield/predicted yield) x 100
31
oxidation state of metal(II)
+2
32
ammonium ion with charge
NH4+
33
hydroxide ion with charge
OH-
34
hydrogen ion with charge
H+
35
nitrate ion with charge
NO3-
36
sulfate ion with charge
SO4 2-
37
phosphate ion with charge
PO4 3-
38
carbonate ion with charge
CO3 2-
39
physical properties of ionic compounds
generally solid at room temperature
high melting points and boiling points (due to strong electrostatic attraction)
conducts electricity when molten or dissolved in aqueous solutions
40
physical properties of small covalently bonded molecules
41
structure of ionic compounds
giant lattice structure of positive and negative ions, that are continuous and regular
42
physical properties of giant covalent structures
43
physical properties of metals
43
which metal is liquid at rtp
mercury
44
which forces must be overcome in melting and boiling
intermolecular forces
45
order ionic, covalent (not giant), and metallic structures in increasing order of mp
covalent, metallic, ionic
46
diamond structure
46
graphite structure
47
order ionic, covalent (except graphite), and metallic structures in increasing order of conductivity
covalent (no conductivity), ionic, metallic
47
silicon dioxide structure
48
when should you use fractional distillation over simple distillation
When the boiling points of miscible liquids differ by less than 25 degrees Celcius
49
When should centrifugation be used in the separation of mixtures
If the mixtures contain components of different densities or sizes that would not easily settle on their own (especially for solid-liquid mixtures, emulsions and suspensions hat are difficult to filter)
50
ways to establish impure substances
chromatography (but may be just one spot by coincidencce)
range of bp or mp (pure substances should have a sharp bp or mp) (higher bp or lower fp)
evaporation for dissolved impurities
51
oxygen gas test
glowing splint relights
52
hydrogen gas test
burning splint held at the open end of a test tube, explodes with a 'squeaky pop'
53
chlorine gas test
damp blue litmus paper. turns red and then is bleached
53
test for Al3+
react with aqueous sodium hydroxide, forms a white precipitate
54
test for metal cations (Al3+, Ca2+, Mg2+, Cu2+, Fe2+, Fe3+)
test usiing aqueous sodium hydroxide (NaOH)
55
test for Ca2+
react with aqueous sodium hydroxide, forms a white precipitate
flame test - red-orange flame
56
test for Mg2+
react with aqueous sodium hydroxide, forms a white precipitate
57
test for Cu2+
react with aqueous sodium hydroxide, forms a blue precipitate
58
test for Fe2+
react with aqueous sodium hydroxide, forms a green precipitate
59
test for Fe3+
react with aqueous sodium hydroxide, forms a brown precipitate
60
test for carbonates
add a dilute acid
causes fizzing (effervescence) due to the release of CO2
the gas produced should turn limewater milky/cloudy (CaCO3 formed) (CO2 test)
61
test for halides
acidify the sample with dilute nitric acid (HNO3) to remove interfering ions
add silver nitrate solution (AgNO3 (aq))
white precipitate = chloride ions (AgCl)
cream precipitate - bromide ions (AgBr)
yellow precipitate = iodide ions (AgI)
62
test for sulfates
acidify the sample with dilute acid (HCl) to remove interfering carbonates
add a few drops of barium chloride (BaCl2) solution or barium nitrate solution (Ba(NO3)2)
white precipitate (BaSO4) = sulfate present
63
sublimation
solid to gas
64
disposition
gas to solid
65
What separation technique is used to separate the components of air
fractional distillation
66
3 common properties of transition metals
they are able to form stable ions in different oxidation states
they often form coloured compounds
they are often used as catalyssts (as ions or atoms)
67
reaction of an acid with a base (type of reaction, exothermic or endothermic?)
neutralisation reaction
often exothermic
68
What does an increase or decrease in temperature do to the equilibrium of a reversible reaction
Increase in temperature will favour the endothermic reaction (more of the reaction that is endothermic will take place) and equilibrium will shift to the position of the endothermic reaction
A decrease in temperature will favour the exothermic reaction, shifting the equilibrium to the direction of the exothermic reaction
69
What does a change in pressure do to the equilibrium of a reversible reaction
A change in pressure can only affect the position of the equilibrium when the reaction involves chemicals in the gaseous state.
Pressure can only affect the position of equilibrium if there is a change in the total gas volume.
An increase in pressure favours the side with the lower gas volume.
A decrease in pressure favours the side with the higher gas volume.
e.g. if the RHS produces 2 moles for every 3 moles of reactants on the LHS, an increase in pressure would move the equilibrium to the right and result in more of the lower mass products being formed.
70
What does a change in concentration do to the equilibrium of a reversible reaction
Adding a chemical that is present on either side of the equation will cause a shift in the position of the equilibrium to counteract the change.
e.g. if more of the LHS reactants were added, the equilibrium will shift to the RHS to compensate.
a decrease in concentration on one side will result in a shift to that side of the equilibrium to replace the products that were removed.
71
71
What is the effect on adding a catalyst to a reaction at equilibrium
Adding. a catalyst has no effect on the position of the equilibrium, however, it alloows the equilibrium to be reached more quickly, or established at a lower temperature, making reactions more profitable.
72
convert dm to m
1 dm = 0.1m
73
energy (Joules) formula
Force (N) x Distance (m)
74
Define saturated solution
A solution in which no more solute will dissolve at a given temperature
75
Unit for solubility
g of solute per 100g of solvent
76
describe the change in solubility of gases as temperature increases
solubility decreases
77
describe the change in solubility of salts as temperature increases
solubility increases
78
what polymerisation are polyalkenes formed from
addition polymerisation
79
what polymerisation are polyesters formed from
condensation polymerisation
80
what polymerisation are polyamides formed from
condensation polymerisation
81
products of complete combustion
carbon dioxide and water (+ heat)
82
products of incomplete combustion
carbon monoxide, soot, water, (+ unburnt hydrocarbons)
83
How do greenhouse gases contribute to warming of temperature
It absorbs infrared radiation emitted from Earth, trapping it in the atmosphere
84
carbon monoxide properties and effects
colourless, odourless, poisonous gas
binds to haemoglobin, reducing the amount of oxygen blood can carry. CO exposure can lead to death
85
pH value of solution with 0.1 mol dm-3 H+ concentration
1.0
86
concentration of H+ ions of a solution with pH 2.0
0.01 mol dm-3
87
1 meter in nanometers
10^9 nm
88
___ is added to ____. What do you ask first
Does a reaction occur? If so, balance the equation
89
electrolysis question. Ask if the product is...
diatomic
90
91
91
92
1g in mg
1000mg
92
92
Chemistry
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