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1
Q

Best way for filtration
James Chadwick proved the existence of the
Mass number of copper

A

Funnel
Neutron
63

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2
Q

In simple distillation, the mixture is heated to make the liquid

A

evaporate

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3
Q

Bromine is in Group?

A

7

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4
Q

What is the structure of hydrogen bromide?

A

small molecule

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5
Q

Explain how the reactivity of the halogens changes going down Group 7.

A

the reactivity decreases (going down Group 7)

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6
Q

The two types of particle in the centre of the atom are the proton and the

A

Neutron

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7
Q

Niels Bohr suggested particles orbit the centre of the atom. This type of particle is the

A

Electron

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8
Q

The two types of particle with the same mass are the neutron and the

A

Proton

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9
Q

What do the dots and crosses represent in the diagram

A

Electrons

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10
Q

formula for the molecule of ammonia

A

NH3

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11
Q

Ammonia manufactured by?

A

Haber process

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12
Q

>

A

reversible (reaction) / reaction can go both ways

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13
Q

Produces ammonium nitrate

A

Ammonia reacts with nitric acid

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14
Q

Nitrate need

A

Nitric acid

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15
Q

why farmers spread ammonium nitrate on their fields.

A

as a fertiliser (1) • contains (a high percentage of) nitrogen (1) • help promote plant growth / increases crop yield (1)

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16
Q

pic pipette

A

apple

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17
Q

pic conical flask

A

flats

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18
Q

Describe how the pipette should be used to measure exactly 25.00 cm3 of sodium hydroxide solution into the conical flask.

A

use a pipette filler (1) • wash pipette with sodium hydroxide solution (1) • draw the liquid up so (the bottom of the meniscus) touches the line (1)

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19
Q

pic burette

A

hairdressers

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20
Q

Titration

A

determine the concentration of an identified analyte

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21
Q

Give a reason why universal indicator is not a suitable indicator to use in an acid-alkali titration.

A

it does not show sharp colour change at end point / not known which colour change gives correct end point

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22
Q

relative mass of a proton?

A

1

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23
Q

Argon group

A

0

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24
Q

Period

A

Row

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25
Q

empirical formula of butene

A

CH2

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26
Q

Test for CO2

A

(bubble gas through) limewater (1)

• (limewater) turns {milky / cloudy / white precipitate} (1)

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27
Q

Fire symbol

A

Flammable

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28
Q

Elements in barium sulfide

A

Barium sulfur

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29
Q

Safety when toxic substance

A

wear gloves (1) • {so does not contact/to protect your} skin (1) OR • wear goggles (1) • {so does not contact/to protect} the eyes (1) OR • use in fume cupboard / mask (1) • so you do not inhale it (1)

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30
Q

condenser is used.

A

to cool (1)

• so (water) {vapour/gas} turns to liquid (1)

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31
Q

pic Bunsen burner.

A

School side

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32
Q

Explain why these changes are called physical changes rather than chemicalchanges.

A

physical changes do not result in formation of a new substance / chemical change results in formation of a new substance (1)

• physical change is easily reversed / chemical change is not easily reversed (1)

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33
Q

Solid to liquid

A

Melting

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34
Q

Liquid gas

A

Evaporation

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35
Q

Explain how alloying changes these pure metals to make the alloys more suitable for the given uses.
(

A

an alloy is a mixture of metals • because larger/different sized atoms introduced in alloying, • stop layers moving easily over one another • therefore individual alloy is stronger/harder • an aluminium alloy is magnalium • pure aluminium is not suitable for making aircraft as it bends too easily / too weak • aluminium alloy stronger • magnesium atoms lighter than aluminium atoms, • therefore alloy still low density / lower density than aluminum alone • an iron alloy is stainless steel • pure iron is not suitable for cutlery as it bends too easily / too weak • iron corrodes, • corrosion would contaminate food • stainless steel does not corrode • gold alloy harder • therefore more hard wearing • gold alloys less likely to change shape when worn • alloying can change the colour of the gold

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36
Q

what is meant by oxidation.

A

gain of oxygen lose electrons

37
Q

Explain why painting iron objects prevents corrosion.

A

the paint {excludes/acts as a barrier/protective layer/shield} (1)

• (excludes) air / oxygen / water (1)

38
Q

Protect iron corrosion

A

Sacrificial protection

39
Q

State two characteristic properties of metals

A

• high melting points (1) • high boiling points (1) • malleable (1) • conduct electricity (1) • conduct heat (1) • high density (1) • shiny (1) • ductile (1) • strong (1) • sonorous (1)

40
Q

acid used to make chlorides.

A

Hydrochloric acid

41
Q

make salts

A

Acids

42
Q

Explain structure changes nickel atom, Ni, changes when it forms a nickel ion, Ni2

A

loss of electron(s) (1)

• two electrons (1)

43
Q

Iron ore contains

A

iron oxide.

44
Q

thermometer measures

A

Temperature

45
Q

polystyrene cup pic

A

Alsatger town

46
Q

exothermic heat

A

release of heat

47
Q

Best way to measure liquid

A

measuring cylinder

48
Q

a yellow flame

A

Sodium

49
Q

the limewater goes milky what gas

A

CO2

50
Q

Inner pack solid with pack of water in it.

Explain why the pack goes cold. when burst

A

the solid {dissolves/ reacts with the water} (1)

• {takes in /absorbs} heat / is endothermic (1)

51
Q

Why the pack can be used only once.

A

reaction) irreversible

52
Q

Line of best fit

A

Straight line through most

53
Q

Hydrogen peroxide decomposes to form

A

water and oxygen.

54
Q

gas) syringe pic

A

Keats walk

55
Q

atom has a radius of about

A

0.1 nm.

56
Q

A useful property of nanoparticles in sunscreens is that they

A

prevent harmful UV radiation reaching the skin

57
Q

Nanoparticle surface area of 38 400 nm2 and a volume of 51 200 nm3. Calculate the surface area to volume ratio.

A

allow 2 for correct answer with or without working

51200 (1) 38400 1 : 1.33 (1)

58
Q

State why ethane is described as a hydrocarbon.

A

contains carbon and hydrogen (atoms) (1) only (1)

59
Q

Draw a molecule of ethane showing all covalent bonds.

A

CC H’s around

60
Q

crude oil is a

A

finite resource

61
Q

The substances ethane, C2H6, octane, C8H18, and pentadecane, C15H32, are all found in crude oil. These substances

A

are in the same homologous series

62
Q

Crude oil passed of to the column it is

A

Heated

63
Q

transition metal? density

A

High

64
Q

transition metal? catalyst?

A

YES

65
Q

transition metal? colour

A

Coloured

66
Q

Lubricating bike chain prevents corrosion of the steel chain.

A

air/oxygen} excluded / {water/moisture} excluded / oil acts as a barrier (1)

• {air/oxygen} and {water/moisture/damp conditions} both needed (for iron to rust / corrosion) (1)

67
Q

Iron fences can be galvanised by coating them with a layer of zinc. When the layer of zinc is scratched exposing the iron to the weather, the iron does not rust. Explain why the exposed iron does not rust.

A

zinc corrodes {easier than / in preference to / OWTTE} iron / zinc reacts with air and water instead (1)

• zinc is more reactive than iron / zinc is sacrificial / zinc has a higher tendency to form ions (1)

68
Q

Metals have high melting points. Explain, in terms of their structure and bonding, why metals have high melting points.

A

metal ions / cations} surrounded by (delocalised) electrons (1)

  • strong {forces of attraction / bonding} (between (delocalised) electrons and {metal ions / cations}) (1)
  • needs lots of energy to {separate the particles / break bonds / break forces of attraction} (1)
69
Q

Describe the test to show the gas is hydrogen.

A

apply lighted splint (1)

• (squeaky) pop (1)

70
Q

Explain how the structure of a nickel atom, Ni, changes when it forms a nickelion,Ni2+.

A
  • loss of electron(s) (1)

* two electrons (1)

71
Q

Aluminium cannot be extracted by heating its oxide with carbon. Aluminium has to be extracted from its oxide by electrolysis. Explain why.

A

aluminium is high in reactivity / aluminium oxide is (very) stable (1)
• aluminium (oxide) cannot be reduced by carbon (1)

72
Q

Describe how growing plants can result in the phytoextraction of copper

A

plants absorb {copper/metal} (ions) from the {soil/ores} / plants concentrate copper ions (1)

• plants (harvested and) burned (to leave copper/metal compound) (1)

73
Q

Hydrogen burns in

A

air

74
Q

Boiling point of water

A

100d

75
Q

Boiling point of hydrogen

A

-253d

76
Q

Lead can be obtained by heating its oxide with

A

Carbon

77
Q

In most reactions, the percentage yield of any product is less than 100%. Give two reasons why the percentage yield is less than 100%.
(

A

incomplete / reversible reactions

  • competing/unwanted/side reactions
  • practical losses during the experiment / loss on transfer from one piece of equipment to another
78
Q

Molten zinc chloride is an

A

electrolyte.

79
Q

Covalent substances can be

A

simple molecular covalent or giant covalent.

80
Q

Ammonia, NH3, is made by reacting nitrogen with hydrogen. Write the balanced equation for this reaction.

A

N2 + 3H2 → 2NH3 (2)

left hand side formulae (1) balancing of correct formulae (1)

81
Q

Why should the student use a pencil and not a pen to draw the start line? Chromatography

A

Smudge

82
Q

Water level …. the line

A

Below

83
Q

The mixture of compounds in gas chromatography is

A

separated

84
Q

Give one advantage of using instrumental methods of analysis.

A

accurate • sensitive • rapid / fast • small sample

85
Q

Which of these values could be the pH of sulfuric acid?

1, 7, 14, 8

A

1

86
Q

Funnel drawn

A

y

87
Q

What type of bonding holds the atoms together in oxygen?

A

covalent

88
Q

Oxygen boiling point

A

Low

89
Q

Oxygen consists of

A

Small molecules

GCSE papers (10 decks)

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