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Grace Chemistry IGCSE > Exam Notes > Flashcards

Exam Notes Flashcards

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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
Q

How to heat flammable liquids

A

In a water bath

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26
Q

Chromatography original dot

A

Doesn’t appear in after diagram

Also label spots

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27
Q

Temperature in rates

A

More successful collisions per unit time!!

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28
Q

SA rates

A

Temperature increases because more energy transferred to mixture

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29
Q

Volume affect on temperature change

A

Increase in volume decreases temperature change because there is more to heat up

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30
Q

Why use distillation

A

Smaller / bigger BPs

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31
Q

Equilibrium

A

Concentration of reactants and products remain constant

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32
Q

Endothermic reactions

A

Release thermal energy

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33
Q

Ionic substances and melting points

A

Define ionic

Mention oppositely charged ions

34
Q

Substance responsible for bubbles

A

Not ion

Substance

35
Q

Calculating empirical formula

A

Percentage / RFM

36
Q

No temperature decrease in neutralisation at higher volumes

A

Volume of acid larger

37
Q

Condensation polymerisation

A

Involves loss of water molecules

38
Q

Biodegradable

A

Can be broken down by bacteria

39
Q

Method of separation for separating copper(II) sulphate from a mixture with water

A

Crystallisation

40
Q

Leave chromatogram until

A

Solvent front reaches top of paper

41
Q

AgCl

A

Prevents false positives by preventing other precipitates from forming

42
Q

Why do you relight flame in reduction of metal oxides

A

Hydrogen poses risk of explosion

43
Q

What steps are taken to confirm an accurate value for the mass of a metal

A

Heat solid again, reweigh to check constant mass

44
Q

Rock salt equipment

A

Evaporating basin

45
Q

Why is the mixture of rock salt and water warmed and stirred

A

Sodium chloride dissolves more quickly

46
Q

Colour of halogens afterwards

A

Always colour of element

47
Q

Crystallisation method

A

1) heat until crystals form
2) cool
3) filter of crystals
4) dry crystals using filter paper

48
Q

Obtaining pure, dry water from sea water

A

Simple distillation

49
Q

Properties of carbon

A

High melting point

Giant structure

50
Q

Using a Burette

A

Acid must be added before

Better resolution

51
Q

Why is there no reaction between a metal and acid

A

Think about reactivity

52
Q

Repeats

A

Increase validity

53
Q

Dynamic equilibrium

A

Rates of forwards and backwards reactions are equal

54
Q

Order of reactivity in halogen reactions

A

Have they been vaporised?

55
Q

Magnesium ribbon

A

Silver solid strip

56
Q

Lithium removed from oil, dried and cut

The exposed surface….

A

Changes from shiny to dull

57
Q

Metal + water

A

Metal hydroxide + hydrogen

58
Q

Exothermic reactions

A

Reactant temperature increases

59
Q

Universal indicators in weak acids

A

Orange-yellow

60
Q

Carbonic acid

A

H2CO3

61
Q

How to figure out which of two solutions has a greater concentration when given volume and equation

A

Compare molar ratio with volumes

62
Q

Galvanising

A

Zinc

63
Q

Simple distillation equipment

A

Flask

64
Q

Why is iron powder mixture with water when creating oxygen

A

Too slow without water

65
Q

How to calculate percentage of oxygen in air

A

Volume of oxygen reacting x 100

Divided by total volume of air in conical flask, glass tube and syringe reading at start

66
Q

Bromine + sodium iodide

A

Displacement -> solution becomes darker

67
Q

Why is a glass rod used in heated solutions

A

To see if crystals form, indicates crystallisation point

68
Q

Why is solution heated

A

To evaporate water (to reach crystallisation point)

69
Q

Label above tripod in distillation

A

Gauze

70
Q

Group

A

Column - same number of outer-shall electors

71
Q

CO2 production

A

Stops because insoluble CaSO4 coats the marble chips

72
Q

Condensation

A

Discuss cooling

73
Q

Zinc solutions

A

Colourless

74
Q

Copper colour

A

Brown

75
Q

Reasons for anomalous results in precipitation

A
  • start mass to small
  • to little reactant
  • precipitate not left to settle for long enough
76
Q

ANHYDROUS copper(II) sulphate

A

Nice

77
Q

Preparation of water

A

Collect using gas syringe

78
Q

Is a solution more acidic or more alkali?

A

Is one solid?

79
Q

Nitric acid

A

Removes carbonate and sulfite ions

80
Q

Crude oil separating in a

A

Fractionating column

81
Q

Cotton wool

A

Stops liquid escaping, let gas escape

82
Q

Control variables for CaCO3 + HCl

A

Mass

Surface area

Grace Chemistry IGCSE (21 decks)

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