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1
Q

Which element is used to sterilise water? (1)

A

Chlorine (Cl)

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2
Q

Name a metal that can be made by heating its oxide with carbon? (1)

A

Iron (Fe)

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3
Q

Explain why a powdered form is used rather than large pieces to increase rate of reaction. (2)

A

They have a larger Surface Area

Leading to a faster reaction.

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4
Q

When dilute HCl is added to a solid, a gas forms.

Which of these ions is present in the solid? (1)

A

Carbonate (CO3)

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5
Q

In an experiment on the anaerobic respiration of yeast to produce ethanol.

State the purpose of the yeast. (1)

A

The yeast acts like a catalyst. The zymase enzyme acts as the catalyst.

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6
Q

What method is used to obtain water from a mixture containing salt and water? (1)

A

Simple Distillation

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7
Q

State why the solvent level should not be above the base line at the start of the experiment. (1)

A

To prevent the inks mixing in the solvent trough.

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8
Q

(In paper chromatography), State why ink D does not move during the experiment. (1)

A

As the ink is insoluble in the solvent

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9
Q

Water is the name used for H2O(l).

Give the two names used for H2O(g). (2)

A

Steam

Water Vapour

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10
Q

Name the to gases that react to form nitrogen oxides. (1)

A

Nitrogen and Oxygen

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11
Q

State a physical property of Na that shows it is a metal. (1)

A

Good conductor of electricity

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12
Q

State an observation that can be made when adding Potassium (K) to a trough of water. (1)

A

A flame burns (as the hydrogen produced ignites)

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13
Q

Name an element that is a liquid at room temperature. (1)

A

Bromine

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14
Q

What element is used in fire extinguishers? (1)

A

Carbon Dioxide

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15
Q

Name a hydrocarbon compound used as a fuel. (1)

A

Methane

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16
Q

State the name of the mesh heating guard used above Bunsen Burners in heating. (1)

A

Gauze

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17
Q

State the name of the equipment that holds a gauze above a bunsen burner. (1)

A

Tripod

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18
Q

Name two elements in Period 2 that form acidic oxides. (2)

A

Carbon
Nitrogen
Fluorine

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19
Q

What are the elements arranged by in the periodic table?

A

Atomic Number

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20
Q

State what is meant by the term covalent bond? (2)

A

Attracted to the nuclei of both atoms.

Electrostatic attraction of bonding through sharing electrons.

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21
Q

Explain why carbon dioxide has a low boiling point. (2)

A

There are weak intermolecular forces between molecules.

Little thermal energy is required to overcome forces.

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22
Q
              • Blast Furnace - - - - - - -

Give the name of the Iron ore that contains Fe2O3. (1)

A

Haematite

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23
Q

State two condition required fir industry cracking. (2)

A

600 - 700 *C

Alumina or Silica

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24
Q

State the molecular formula of Decane. (1)

A

C10 H22

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25
Q

State the general formula of the homologous series that includes Decane. (1)

A

Cn H2n+2

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26
Q

State the observation made when platinum is added to cold water. (1)

A

No Change - Platinum is not very reactive

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27
Q
              • Haber Process - - - - - - -

Name the type of reaction that occurs between ammonia and sulfuric acid. (1)

A

Nuetralisation

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28
Q

State the formula of Ammonium Sulfate. (1)

A

(NH4)2SO4

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29
Q

Nitric acid and ammonia are used to produce ammonium nitrate.

Explain why ammonium nitrate is used in agriculture.(2)

A

Ammonium nitrate contains nitrogen, which stimulates plant growth and development as a chemical fertiliser.

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30
Q

Give a test to show that the potassium nitrate solution in the test tube contains potassium ions. (2)

A
  • Carry out a flame test.

- Lilac colour given out.

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31
Q

Name the gas which is necessary for rusting to occur. (1)

A

Oxygen

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32
Q

Name the gas which bleaches moist litmus paper. (1)

A

Chlorine

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33
Q

Name the gas which has the highest percentage by volume in the air. (1)

A

Nitrogen

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34
Q

Explain how decreasing the concentration of the hydrochloric acid affects the rate of reaction.

Refer to particle collision theory in your answer. (3)

A
  • As the concentration decreases, there are less particles per unit measure.
  • Meaning there are less particle collisions per unit time.
  • Therefore less successful collision per unit time, reaction rate has decreased.
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35
Q

In a titration, suggest why it is not necessary to dry the flask (after washing it) before repeating the titration. (1)

A

Water does not effect the number of moles.

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36
Q

What are concordant results? (1)

A

Those results within 0.20 cm^3 of each other.

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37
Q

What type of polymers are poly(ethene) and poly(chloroethene)

A

Addition Polymers

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38
Q

Name the polymerisation process used to form Nylon. (1)

A

Condensation

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39
Q

In titrations, state why zinc should not be used for the electrodes. (1)

A

Zinc is not an inert element and may react.

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40
Q

Name a process that takes place in a Hofmann voltameter. (1)

A

Electrolysis

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41
Q

Which particles is furthest from the centre of each atom. (1)

A

An electron

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42
Q

What makes two atoms neutral? (1)

A

Electrons and Protons

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43
Q

What method of separation is used to separate red ink from a mixture of coloured inks? (1)

A

Chromatography

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44
Q

What method of separation is used to separate ethanol from a mixture of ethanol and water? (1)

A

Fractional Distillation

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45
Q

What method of separation is used to separate a mixture of sand and water? (1)

A

Filtration

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46
Q

What method of separation is used to separate water from a copper (II) Sulfate solution? (1)

A

Simple Distillation

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47
Q

Describe a Chemical test to show that the colourless liquid contains water. (2)

A

Test … Anhydrous Copper (II) Sulfate

Result … Changes to a blue colour (from white)

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48
Q

Describe a Physical test to show that the colourless liquid is pure water. (2)

A

Test … Boiling point and Freeing point

Result … B.P = 100 *C, F.P = 0 *C

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49
Q
              • Not on New Spec - - - - - - -

Explain why Carbon Dioxide is sometimes used in fire extinguishers. (2)

A

The CO2 blankets the fire

Stopping oxygen getting to the fire and developing it

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50
Q

Incomplete combustion of propane leads to the formation of a poisonous gas.

Identify this gas. (1)

A

Carbon Monoxide (CO)

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51
Q

During the combustion of propane at high temperatures, gases represented by the formula NOx can form.

Which two elements combine to form these gases? (1)

A

Nitrogen (N) and Oxygen (O)

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52
Q

The disposal of most addition polymers is a problem because they do not biodegrade.

What is meant by the term biodegrade? (2)

A

breaks down / decomposes / decays

by bacteria / microbes / microorganisms

53
Q

Complete the sentence. (1)

Lithium reacts with water to form an ……….

A

Alkali

54
Q

Which group contains the noble gases? (1)

A

0

55
Q

Identify the group whose atoms form ions with a charge of +1. (1)

A

1

56
Q

Identify the group whose atoms form ions with a charge of -1. (1)

A

7

57
Q

State the process that occurs as ethene changes t poly(ethene). (1)

A

Deposition - Gas -> Solid

58
Q

Describe what is done to the crude oil before it enters the fractionating column. (2)

A

Heated

Until Vaporised

59
Q

When potassium is heated in gas X, potassium chloride solid is formed. State Gas X. (1)

A

Chlorine

60
Q

When water is added to Potassium, colourless solution Y forms. State Y. (1)

A

Potassium Hydroxide

61
Q

When Potassium Hydroxide has acid Z added to it, potassium chloride solution forms. State acid Z. (1)

A

Hydrochloric Acid

62
Q

Give a test to show that an aqueous solution of sodium iodide contains iodide ions. (3)

A
  • Add dilute nitric acid.
  • Add (aqueous) silver nitrate.
  • Yellow precipitate formed.
63
Q

Sulfur Dioxide dissolves in water to form an acidic solution.
Identify the ion that causes this solution to be acidic. (1)

A

H+

64
Q

State how litmus paper can be used to tell your solution is acidic. (1)

A

Blue litmus paper will turn red in acid.

65
Q

Give two observations that are made when a piece of magnesium ribbon is added to the acidic solution. (2)

A

Effervescence.
Dissolves into acid.
ACCEPT gas produced and named (H2).

66
Q

State why metals such as titanium are good electricity conductors. (1)

A

Their delocalised electrons can flow.

67
Q

Explain why metals such as titanium are malleable. (1)

A

(Cat)ion layers

Can slide / slip over one another

68
Q

Slaked Lime, Ca(OH)2, forms when water is added to calcium oxide.
Give the chemical name of Slaked Lime. (1)

A

Calcium Hydroxide

69
Q 
Which of these is the formula for a molecule of an element? (1)
H
H2
H2O
H2O2
A

H2

70
Q

What method of separation is used to separate dyes from a food colouring? (1)

A

Chromatography

71
Q

Describe how to carry out a test to show that an (aqueous) sample contains chloride ions. (3)

A
  • add (dilute) nitric acid
  • add silver nitrate (solution)
  • white precipitate forms
72
Q

A brown solid contains hydrated iron(III) oxide.

What is the common name for this brown solid? (1)

A

Rust

73
Q

Identify two substances that react with Iron to form rust. (2)

A

Water

Oxygen

74
Q

What process involves coating iron with zinc? (1)

A

Galvanisation

75
Q

What is the correct name for the compound with formula CuSO4? (1)

A

Copper(II) Sulfate

76
Q

What colour is NH4Cl(s)? (1)

A

White

77
Q

What colour is NH4Cl(aq)? (1)

A

Colourless

78
Q

What is formed when sodium hydroxide solution is added to a sample of iron(III) sulfate solution? (1)

A

Brown Precipitate forms - [Iron(III)]

79
Q

What is the general formula of an Alkene? (1)

A

Cn H2n

80
Q

T/F: (1)

Halogens an be obtained by electrolysing molten metal halides.

A

True - Electrolysis

81
Q

T/F: (1)

The first Halogens are diatomic.

A

True

82
Q

T/F: (1)

The halogens form covalent bonds with other non-metals.

A

True

83
Q

T/F: (1)

All halogens are liquid at room temperature

A

False - based on boiling points

84
Q

T/F: (1)

The boiling points of group 7 elements decrease as the group develops.

A

False - B.P increases down the group

85
Q

T/F: (1)

Cracking is used because of different demands for each hydrocarbon.

A

True - Petrol is high demand

86
Q

T/F: (1)

Molecules used in cracking are all hydrocarbons.

A

True

87
Q

T/F: (1)

Catalytic cracking uses iron as a catalyst.

A

False

88
Q

T/F: (1)

Cracking reactions are addition reactions.

A

False

89
Q

T/F: (1)

Cracking produces molecules with shorter chains.

A

True

90
Q

Explain why magnesium metal is malleable. (2)

A

(magnesium) ions in layers / rows

that can slip / slide (over each other).

91
Q

Explain why magnesium metal is a good electricity conductor. (2)

A

(sea of) delocalised electrons

that can flow / move through metal.

92
Q

In a reaction, Magnesium is ignited and placed in a jar of oxygen gas.
State two observations that would be made. (2)

A

Bright / white flame produced.

White solid collects at base

93
Q

Name the state change from; (1)

Solid to Liquid

A

melting

94
Q

Name the state change from; (1)

Liquid to Gas

A

evaporation

95
Q

Name the state change from; (1)

Solid to Gas

A

sublimation

96
Q

What is the name of the equipment piece that that the filter paper fits in? (1)

A

Filter Funnel

97
Q

Name the industrial process used to separate crude oil. (1)

A

Fractional Distillation

98
Q

State a use for Kerosene and Bitumen. (2)

A

Kerosene - Aircraft fuel

Bitumen - Road surfacing

99
Q

State a catalyst used in the industrial cracking of eicosane. (1)

A

Silica (Silicon Dioxide);
or
Alumina (Aluminium Oxide).

100
Q

A molecule of the hydrocarbon eicosane has the formula C20 H42.
Explain which homologous series eicosane belongs to. (2)

A

Alkanes;

General formula Cn H2n+2.

101
Q

The hydrocarbon eicosane has 20 Carbons, how many Hydrogens does it have? (2)

A

42;

Cn H2n+2 -> H (2 x 20) + 2 = 42

102
Q

Suggest what it means if a hydrocarbon is saturated. (1)

A

The hydrocarbon has no carbon-carbon double bonds.

103
Q

Describe a chemical test used to distinguish between unsaturated and saturated hydrocarbons. (3)

A

test: Adding bromine water.
result: Decolourisation = alkene (unsaturated);
Stays orange = alkane (saturated).

104
Q

Does the isomer;

But-3-ene exist?

A

No: only But-1-ene, and But-2-ene.

105
Q

Substance A and B are both covalently bonded, simple molecular structures. A has a much higher boiling point than B, suggest why. (1)

A

The molecular mass is greater.

106
Q

Hot, molten sulfur reacts with oxygen to form sulfur dioxide gas.
Describe what is seen when a sample of hot, molten sulfur is lowered into a glass jar containing oxygen. (1)

A

(bright), blue flame is produced

107
Q

State a use of silica gel. (1)

A

They are used to dry substances.

108
Q

A sample of sulfur dioxide reacts with water to form an acidic solution.
Identify the acid formation. (1)

A

Sulfuric Acid

109
Q

Describe how a scientist could make sure all the water has been lost. (2)

A

Heat the sample until the mass of the sample does not change.

110
Q

Describe how the scientist could use a solution of the salt to find out if the negative ions are chloride ions. (3)

A
  • Nitric acid
  • Silver nitrate
  • White precipitate
111
Q

Describe how you could use a method of crystallisation to obtain a pure, dry sample of ammonium sulfate from a dilute solution of ammonium sulfate. (4)

A
  • Boil until crystals begin to form;
  • Leave to cool;
  • Filter;
  • Suitable drying method; eg window.
112
Q

Deduce the formula of the compound that is formed when Magnesium (group 2), reacts with Fluorine (halogen). (1)

A

MgF2

113
Q

SiF4 and SiCl4 have simple molecular structures.
SiO2 has a giant covalent structure.

Explain why the boiling point of SiCl4 is greater than the boiling point of SiF4. (2)

A

M1) intermolecular forces (of attraction) / forces (of attraction) between molecules;

M2) stronger in SiCl4 /weaker in SiF4.

114
Q

SiF4 and SiCl4 have simple molecular structures.
SiO2 has a giant covalent structure.

Explain why the boiling point of SiO2 is very much greater than the boiling point of SiCl4. (2)

A

M1 SiO2 has strong covalent bonds (that must be broken);

M2 (whereas) SiCl4 has weak intermolecular forces (of attraction must be overcome).

115
Q

Name the particles that move through the connecting wires to form an electric current. (1)

A

Electrons

116
Q

The electrodes are made of Platinum, which is an inert metal.
State what is meant by inert. (1)

A

not (chemically) reactive / does not react (with the electrolytes/with the products of electrolysis)

117
Q

Explain how you know structure B is being presented as a displayed formula. (1)

A

(because) it shows all the bonds (in the molecule)

118
Q

Explain the meaning of Isomers; (in terms of structure not atomic number).

A
  • (compounds/molecules that have the) same molecular formula;
  • (but have) different structural formula (allow displayed).
119
Q

State the full name of the polymer, PVC. (1)

A

poly(chloroethene) or Polyvinyl Chloride

120
Q

A beaker contains dilute hydrochloric acid.
Litmus indicator is added to the acid.
What is the final colour of the litmus? (1)

A

Red - Litmus is red in acidic solution.

121
Q

A conical flask contains potassium hydroxide solution.
Litmus indicator is added to this alkaline solution.
What is the final colour of the litmus? (1)

A

Blue - Litmus is blue in alkaline solution.

122
Q

Name the two particles found in the nucleus. (2)

A

Proton

Nuetron

123
Q

State the name given to atoms with the same atomic number but different mass numbers. (1)

A

Isotopes

124
Q

In a titration between dilute sulfuric acid and sodium hydroxide, what type of reaction occurs? (1)

A

Neutralisation

125
Q

Ethanol and compound X are members of the homologous series of alcohols.
One property of members of a homologous series is that they have similar chemical reactions.
Give one other property of members of a homologous series. (1)

A 
Any one from:
 have a general formula
 successive members differ by CH2
 trends in physical properties
 same functional group
126
Q

Most chromium is extracted from the ore, chromite, FeCr2O4.

State the names of all the present elements in chromite. (1)

A 
Fe = Iron
Cr = Chromium
O = Oxygen
127
Q

Give the formulae of the two ions in LiF. (1)

A

Li+ and F-

128
Q

Calculate the relative formula mass (Mr) of MgO. (1)

A

2 x 16 = 32

129
Q

Chlorine is used in the manufacture of the addition polymer poly(chloroethene).

Explain how an addition polymer is formed from its monomers. (2)

A

M1 monomers join together/ double bonds
broken (in monomers).

M2 to form a long chain (molecule)/large
molecule.

GCSE Chem (19 decks)

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