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Grace Chemistry IGCSE > Exam Notes > Flashcards

Exam Notes Flashcards

1
Q

Explaining diffusion

A

Don’t confuse with rates technique

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2
Q

Separating a mixture containing salt and water

A

Simple distillation

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3
Q

Preparation of CO2

A

Tap funnel

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4
Q

Colour change when CuCO3 thermally decomposed

A

Green > black

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5
Q

Rust reactions

A

Take a week

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6
Q

Nitric acid

A

HNO3

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7
Q

Water of crystallisation

A

Heat to constant mass to ensure all of the water has been removed from the crystals

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8
Q

Iconic substances don’t conduct when solid

A

Particles only vibrate

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9
Q

Electrolysis

A

Refer to ions

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10
Q

Gold

A

NOT too unreactive, just does not react

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11
Q

Use excess

A

Because…. JEM HELP!!

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12
Q

Ion which caused solutions to be acidic

A

H+

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13
Q

Flame test

A

Dip platinum/nichrome wire in HCl

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14
Q

When naming substance responsible for observations

A

Name compound (not ion!)

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15
Q

Energy level diagrams

A

ΔH is the vertical line

Ea is the bump (draw straight line next to it as label)

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16
Q

Q

A

Remember to add volumes of acid and alkali

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17
Q

Calorimetry variables

A

Distance, insulation

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18
Q

Why is percentage yield small in reversible reactions?

A

Dynamic equilibrium was not reached

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19
Q

Crude oil enters the column,

A

heated, until it is vaporised

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20
Q

Fraction with the largest molecules

A

Bitumen

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21
Q

When drawing ester functional group

A

Include other bonds

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22
Q

Control variables

A

If in doubt, use MOLES not mass

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23
Q

Why repeat?

A

To take a mean average, help identify anomalous results and obtain reliable results

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24
Q

Ethanol used instead of water in solutions because

A

it’s a better solvent

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25
How to heat flammable liquids
In a water bath
26
Chromatography original dot
Doesn’t appear in after diagram | Also label spots
27
Temperature in rates
More successful collisions *per unit time*!!
28
SA rates
Temperature increases because more energy transferred to mixture
29
Volume affect on temperature change
Increase in volume decreases temperature change because there is more to heat up
30
Why use distillation
Smaller / bigger BPs
31
Equilibrium
*Concentration* of reactants and products remain constant
32
Endothermic reactions
Release thermal energy
33
Ionic substances and melting points
Define ionic | Mention oppositely charged ions
34
Substance responsible for bubbles
Not ion | Substance
35
Calculating empirical formula
Percentage / RFM
36
No temperature decrease in neutralisation at higher volumes
Volume of acid larger
37
Condensation polymerisation
Involves loss of water molecules
38
Biodegradable
Can be broken down by bacteria
39
Method of separation for separating copper(II) sulphate from a mixture with water
Crystallisation
40
Leave chromatogram until
Solvent front reaches top of paper
41
AgCl
Prevents false positives by preventing other precipitates from forming
42
Why do you relight flame in reduction of metal oxides
Hydrogen poses risk of explosion
43
What steps are taken to confirm an accurate value for the mass of a metal
Heat solid again, reweigh to check constant mass
44
Rock salt equipment
Evaporating basin
45
Why is the mixture of rock salt and water warmed and stirred
Sodium chloride dissolves more quickly
46
Colour of halogens afterwards
Always colour of element
47
Crystallisation method
1) heat until crystals form 2) cool 3) filter of crystals 4) dry crystals using filter paper
48
Obtaining pure, dry water from sea water
Simple distillation
49
Properties of carbon
High melting point | Giant structure
50
Using a Burette
Acid must be added before | Better resolution
51
Why is there no reaction between a metal and acid
Think about reactivity
52
Repeats
Increase validity
53
Dynamic equilibrium
Rates of forwards and backwards reactions are equal
54
Order of reactivity in halogen reactions
Have they been vaporised?
55
Magnesium ribbon
Silver solid strip
56
Lithium removed from oil, dried and cut | The exposed surface....
Changes from shiny to dull
57
Metal + water
Metal hydroxide + hydrogen
58
Exothermic reactions
Reactant temperature increases
59
Universal indicators in weak acids
Orange-yellow
60
Carbonic acid
H2CO3
61
How to figure out which of two solutions has a greater concentration when given volume and equation
Compare molar ratio with volumes
62
Galvanising
Zinc
63
Simple distillation equipment
Flask
64
Why is iron powder mixture with water when creating oxygen
Too slow without water
65
How to calculate percentage of oxygen in air
Volume of oxygen reacting x 100 Divided by total volume of air in conical flask, glass tube and syringe reading at start
66
Bromine + sodium iodide
Displacement -> solution becomes darker
67
Why is a glass rod used in heated solutions
To see if crystals form, indicates crystallisation point
68
Why is solution heated
To evaporate water (to reach crystallisation point)
69
Label above tripod in distillation
Gauze
70
Group
Column - same number of outer-shall electors
71
CO2 production
Stops because insoluble CaSO4 coats the marble chips
72
Condensation
Discuss cooling
73
Zinc solutions
Colourless
74
Copper colour
Brown
75
Reasons for anomalous results in precipitation
* start mass to small * to little reactant * precipitate not left to settle for long enough
76
ANHYDROUS copper(II) sulphate
Nice
77
Preparation of water
Collect using gas syringe
78
Is a solution more acidic or more alkali?
Is one solid?
79
Nitric acid
Removes carbonate and sulfite ions
80
Crude oil separating in a
Fractionating column
81
Cotton wool
Stops liquid escaping, let gas escape
82
Control variables for CaCO3 + HCl
Mass | Surface area

Grace Chemistry IGCSE (21 decks)

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