Sixth Form Entrance 2017 CHEMISTRY

- 1 -

Sixth Form Entrance 2017

CHEMISTRY

1 hour

Name (Capital Letters): ......................................................................

Present School: ……………………………………………………….

Answer ALL the questions

TOTAL MARK = 60

Answers to Section A should be answered on the question paper.

Answers to Section B should be written on the blank pages at the end of the question paper.

A copy of the Periodic Table is included with the question paper (back page).

If you know the name of the examination board and the title of the chemistry course you are

currently studying e.g. AQA Chemistry, Edexcel, OCR Gateway or 21st Century Science,

IGCSE write it below. Indicate if you are doing Triple Science (i.e. you will get separate

grades in Biology, Chemistry and Physics) or Double Science.

Board_________________ Course________________________ Triple/Double __________

- 2 -

SECTION A

Q1 Use the Periodic Table to help you with this question.

Complete the table below by putting in the missing symbols or numbers.

Symbol Number of

protons

Number of

neutrons

Mass

number

Electron

arrangement

P 15 16

11 23 2.8.1

Ca2+ 20

[TOTAL = 7]

Q2 (a) You are given the formulae of the following ions. Write the chemical formula of

the following substances. The first one is shown as an example.

Ion Formula Ion Formula

Ammonium NH4+ Iodide I−

Magnesium Mg2+ Nitride N3−

Lithium Li+ Hydroxide OH−

Potassium K+ Hydrogencarbonate HCO3−

Lead(II) Pb2+ Carbonate CO32−

Iron(III) Fe3+ Sulfate SO42−

Barium Ba2+ Nitrate NO3−

Example: barium hydroxide Ba(OH)2

(i) Ammonium iodide..........................................................................

(ii) Magnesium hydroxide....................................................................

(iii) Iron (III) nitrate.............................................................................

(iv) Lithium sulfate..............................................................................

(v) Barium nitride................................................................................

[5]

- 3 -

(b) Put numbers in front of the formulae as necessary to balance the equations

below:

(i) ........K + .........H2O .........KOH + .........H2

(ii) ........Fe2O3 + ........CO ........Fe + ..........CO2

(iii) ........C10H22 + ........O2 ........CO2 + ........H2O

[3]

[TOTAL = 8]

Q3 The following table gives some information about several substances.

Substance Melting

point /

°C

Boiling

point /

°C

Electrical

conductivity

when solid

Electrical

conductivity

when molten

Solubility in

water

A 1410 2355 poor poor insoluble

B -25 144 poor poor insoluble

C 712 1418 poor good soluble

D -101 -35 poor poor soluble

E 1660 3287 good good insoluble

For each of the substances, A to E, decided the type of bonding and structure present. Circle

the correct answers below.

(a) A: Bonding – Covalent / Ionic / Metallic

Structure – Giant / Simple Molecular

(b) B: Bonding – Covalent / Ionic / Metallic


(c) C: Bonding – Covalent / Ionic / Metallic


(d) D: Bonding – Covalent / Ionic / Metallic


(e) E: Bonding – Covalent / Ionic / Metallic


[TOTAL = 5]

- 4 -

Q4 The table shows the names of some common pieces of laboratory apparatus used to

make measurements.

(a) Complete the table to show the name of the quantity that can be measured by each piece

of apparatus, and a common unit used for that quantity. One example of each has been done

for you.

[6]

(b) Which piece of apparatus is needed to make measurements in a paper chromatography

experiment?

[1]

A balance

B gas syringe

C ruler

D stop clock

[TOTAL = 7]

- 5 -

Q5 The table shows the displayed formulae of six organic compounds, P, Q, R, S, T and U.

(a) (i) What is the molecular formula of compound S?

[1]

......................................................................................................................................................

(ii) What is the empirical formula of compound T?

[1]

......................................................................................................................................................

(b) (i) Give the letters of two compounds that belong to the homologous series of alkenes.

[1]

....................................................................... and .......................................................................

(ii) The general formula of this homologous series is

[1]

A CnH2n–2

B CnH2n+2

C Cn + H2n

D CnH2n

- 6 -

(c) Which of these conversions is an example of an addition reaction?

[1]

A compound P → compound Q

B compound Q → compound T

C compound R → compound Q

D compound R → compound U

(d)

Complete the table to show the displayed formula and name of the isomer of compound T.

[2]

(e) The equation represents a reaction between compound P and bromine.

(i) Complete the equation to show the displayed formula of the organic product.

[1]

(ii) State the name of this organic product.

[1]

......................................................................................................................................................

(iii) State the condition used in this reaction.

[1]

......................................................................................................................................................

- 7 -

(iv) What term is used for this type of reaction?

[1]

A addition

B hydration

C neutralisation

D substitution

[TOTAL = 11]

Q7. Some students investigated the rate of reaction between sodium thiosulfate solution

and hydrochloric acid. The equation for the reaction is

Na2S2O3(aq) + 2HCl(aq) → 2NaCl(aq) + H2O(l) + S(s) + SO2(g)

The precipitate of sulfur makes the reaction mixture go cloudy.

The students used this method.

Place a mixture of sodium thiosulfate solution and water in a conical flask

Add some dilute hydrochloric acid, swirl the mixture and start a timer

Place the flask over a black cross marked on a piece of paper

Record the time taken for the cross to disappear when viewed from above. The

students used 10 cm3 of dilute hydrochloric acid in each experiment.

They carried out all the experiments at the same temperature.

They used different volumes of sodium thiosulfate solution and water in each experiment.

They were told to keep the total volume of sodium thiosulfate solution and water constant.

The table shows their results.

- 8 -

(a) Explain why the results of student 7 should not be used.

[1]

..............................................................................................................................................

(b) Plot the results of the six other students on the grid below. Draw a curve of best fit

through the points.

[4]

- 9 -

(c) The students used this equation to calculate the rate of each reaction in their investigation.

Calculate the rate of reaction for student 1's experiment.

Give your answer to one decimal place.

[2]

Rate = ...............................................

(d) Another group of students used the same method but with different solutions of sodium

thiosulfate and hydrochloric acid. They calculated the rate of reaction for each experiment

they did. Their results are shown on the following graph.

- 10 -

(i) Describe the relationship between rate and concentration as shown by the graph.

[2]

......................................................................................................................................................

......................................................................................................................................................

......................................................................................................................................................

......................................................................................................................................................

(ii) Explain why increasing the concentration has this effect on the rate.

[3]

......................................................................................................................................................

......................................................................................................................................................

......................................................................................................................................................

......................................................................................................................................................

......................................................................................................................................................

......................................................................................................................................................

......................................................................................................................................................

[TOTAL = 12]

- 11 -

SECTION B

Write your answers to this section on the blank pages which follow.

Write notes on TWO of the following [5 marks each]. Use diagrams and chemical equations

where relevant.

(a) Cracking

(b) The structures, properties and uses of TWO polymers

(c) Catalysts

(d) The bonding and structure of graphite and diamond

(e) The manufacture of aluminium from its ore

(f) The industrial manufacture of ammonia

SECTION B ANSWER

- 12 -

SECTION B ANSWER (continued)

- 13 -

3 11

19

37

55

87

4 12

20

38

56

88

21

39

57

89

22

40

72

104

23

41

73

105

24

42

74

106

25

43

75

58

90

59

91

60

92

61

93

62

94

63

95

64

96

65

97

66

98

67

99

68

100

69

101

70

102

71

103

26

44

76

27

45

77

28

46

78

29

47

79

30

48

80

5 13

31

49

81

6 14

32

50

82

7 15

33

51

83

8 16

34

52

84

9 17

35

53

85

10

18

36

54

86

Li

Na K Rb

Cs

Fr7 23

39

85

133

(223

)

9 24

40

88

137

(226

)

45

89

139

(227

)

48

91

178

(261

)

51

93

18

1

(26

2)

52

96

184

(263

)

55

(99

)

18

6

140

232

141

(231)

14

4

23

8

(14

7)

(23

7)

15

0

(24

2)

15

2

(24

3)

15

7

(24

7)

159

(245

)

163

(251

)

165

(254

)

167

(253

)

169

(256

)

173

(254)

17

5

(25

7)

56

10

1

19

0

59

10

3

19

2

59

10

6

19

5

63

.5

10

8

19

7

65

.4

112

201

11

27

70

11

5

204

12

28

73

11

9

207

14

31

75

122

209

16

32

79

12

8

(21

0)

19

35.5

80

12

7

(21

0)

20

40

84

13

1

(22

2)

Lith

ium

So

diu

m

Po

tassiu

m

Ru

bid

ium

Ca

esiu

m

Fra

nciu

m

Bery

lium

Mag

ne

siu

m

Ca

lciu

m

Str

on

tium

Ba

riu

m

Ra

diu

m

Sca

ndiu

m

Ytt

riu

m

Lanth

an

um

Actiniu

m

Titaniu

m

Zircon

ium

Hafn

ium

Un

nilq

ua

diu

m

Va

na

diu

m

Nio

biu

m

Tan

talu

m

Un

nilp

entium

Ch

rom

ium

Mo

lybd

en

um

Tun

gste

n

Un

nilh

exiu

m

Mang

an

ese

Te

chn

etiu

m

Rh

en

ium

Ceriu

m

Tho

riu

m

Pra

seo

dym

ium

Pro

tactiniu

m

Neo

dim

ium

Ura

niu

m

Pro

me

thiu

m

Ne

ptu

niu

m

Sa

mari

um

Plu

toniu

m

Euro

piu

m

Am

eri

ciu

m

Gad

olin

ium

Curi

um

Terb

ium

Be

rke

lium

Dyspro

siu

m

Ca

lifo

rniu

m

Ho

lmiu

m

Ein

ste

iniu

m

Erb

ium

Fe

rmiu

m

Thu

lium

Men

dele

viu

m

Ytte

rbiu

m

Nob

eliu

m

Lute

tiu

m

Law

renciu

m

Iron

Ru

the

niu

m

Osm

ium

Co

ba

lt

Rho

diu

m

Irid

ium

Nic

kel

Pa

llad

ium

Pla

tin

um

Co

pp

er

Silv

er

Go

ld

Zin

c

Cad

miu

m

Me

rcury

Boro

n

Alu

min

ium

Ga

llium

Indiu

m

Tha

lliu

m

Carb

on

Sili

con

Germ

aniu

m

Tin

Lea

d

Nitro

gen

Ph

osp

ho

rus

Ars

en

ic

An

tim

on

y

Bis

mu

th

Oxyg

en

Su

lph

ur

Sele

niu

m

Tellu

riu

m

Polo

niu

m

Flu

ori

ne

Chlo

rin

e

Bro

min

e

Iodin

e

Asta

tine

Ne

on

Arg

on

Kry

pto

n

Xen

on

Rad

on

Heliu

mH

ydro

gen

12

14

H

Be

Mg

Ca

Sr

Ba

Ra

Sc Y La

Ac

Ti

Zr

Hf

Un

q

V Nb

Ta

Un

p

Cr

Mo

W

Un

h

Mn

Tc

Re

Ce

Th

Pr

Pa

Nd U

Pm

Np

Sm

Pu

Eu

Am

Gd

Cm

Tb

Bk

Dy

Cf

Ho

Es

Er

Fm

Tm

Md

Yb

No

Lu

Lr

Fe

Ru

Os

Co

Rh Ir

Ni

Pd

Pt

Cu

Ag

Au

Zn

Cd

Hg

B Al

Ga

In Ti

C Si

Ge

Sn

Pb

N P As

Sb

Bi

O S Se

Te

Po

F Cl

Br I At

Ne

Ar

Kr

Xe

Rn

He

Ato

mic

Num

ber

Sym

bo

l

Nam

e

Mola

r m

ass in

g m

ol–

1

Peri

od

Ke

y

Gro

up

TH

E P

ER

IOD

IC T

AB

LE

12

34

56

70

1 2 3 4 5 6 7

La

nth

an

ide

ele

me

nts

Ac

tin

ide

ele

me

nts

- 1 -

Sixth Form Entrance 2015

CHEMISTRY

1 hour


Present School: ……………………………………………………….


TOTAL MARK = 70









- 2 -

SECTION A



Symbol Number of

protons

Number of

neutrons

Mass

number

Electron

arrangement

O 8 8

17 37 2.8.7

S2- 32

[TOTAL = 7]












(i) ammonium nitrate............................................................................

(ii) Magnesium nitride..........................................................................

(iii) Barium hydrogencarbonate............................................................

(iv) Iron(III) hydroxide.........................................................................

(v) Lead nitride.....................................................................................

[5]

- 3 -


below:

(i) ........Cs + .........H2O .........CsOH + .........H2

(ii) ........Fe2O3 + ........C ........Fe + ..........CO

(iii) ........C9H20 + ........O2 ........CO2 + ........H2O

(iv) ........ Al2(SO4)3 + ........Mg(OH)2 ........Al(OH)3 + .........MgSO4

[4]

[TOTAL = 9]

Q3 Atoms are made of electrons, neutrons and protons.

(a) Complete the table to show the relative mass and charge of an electron,

neutron and proton.

particle relative mass relative charge

electron -1

neutron 1

proton

[4]

(b) The diagram shows the electronic structure of an atom of an element.

(i) Name the element of which this is an atom.

Explain your answer.

..........................................................................................................................

..........................................................................................................................

[2]

×

×

××

× ×

×

×

×

×

×

××

×

×

×

×

- 4 -

(ii) What is the atomic number of this element?

..........................................................................................................................

[1]

(c) The table below shows some information about the isotopes of neon.

Isotope Mass

Number

Abundance

Lead - 207 207 90.1%

Lead - 208 208 3.4%

Lead - 210 210 6.5%

(i) What is the definition of an isotope?

…………………………………………………………………………..........

…………………………………………………………………………..........

…………………………………………………………………………..........

…………………………………………………………………………..........

[2]

(ii) Calculate the relative atomic mass of lead.

…………………………………………………………………………..........

…………………………………………………………………………..........

……………...…………………………………………………………...........

…………………………………………………………………………..........

[2]

[TOTAL = 11]

- 5 -


Substance Melting

point /

°C

Boiling

point /

°C

Electrical

conductivity

when solid

Electrical

conductivity

when molten

Solubility in

water

A 705 1445 poor good soluble

B 1635 3350 good good insoluble

C -111 -45 poor poor soluble

D -25 154 poor poor insoluble

E 1435 2295 poor poor insoluble













[TOTAL = 5]

Q5 (a) Draw a dot-cross diagram to show the bonding in an methane molecule. Show the

outer shell electrons only. Name the type of bonding.

[3]

- 6 -

(b) Draw one molecule of butane and one molecule of butene, showing all the

bonds.

butane butene

[4]

(c) Define the term isomerism

………………………………………………………………………………

………………………………………………………………………………

[2]

[TOTAL = 9]

Q6 Sodium nitrate decomposes on strong heating as shown:

2KNO3(s) 2KNO2(s) + O2(g)

If 51.0 g of potassium nitrate was completely decomposed by heating, what mass

of solid would remain? Show full working including relevant equations used with

appropriate units for each calculation.

[TOTAL = 6]

- 7 -

Q8 Hydrogen peroxide (H2O2) decomposes slowly at room temperature to form oxygen

and water.

(a) Write a balanced equation for this reaction including the relevant state

symbols.

..........................................................................................................................

[3]

(b) Iron (III) oxide acts as a catalyst for this reaction.

Andy added 1.0 g of Iron (III) oxide to 35 cm3 of hydrogen peroxide

solution at room temperature.

He measured the total volume of oxygen given off at one minute intervals.

His results are shown in the table.

Time (minutes) 0 1 2 3 4 5

Total volume of oxygen

(cm3)

0 62 80 94 96 96

Draw a graph of total volume of oxygen produced against time.

3

Totalvolumeof oxygenin cm

Time in minutes

- 8 -

[3]

(c) At the end of the experiment Andy filtered off the oxide.

What mass of oxide would you expect to be left?

..........................................................................................................................

[1]

(d) Define catalyst

..........................................................................................................................

..........................................................................................................................

[1]

(e) Andy then added 1.0 g of a different oxide to a fresh 20 cm3 sample of

hydrogen peroxide solution at the same temperature.

Again he measured the volume of oxygen produced at one minute intervals.

From his results he concluded that this different oxide was a better catalyst

than manganese(IV) oxide.

Add a line to your graph to show results which would support this

conclusion. Label this new line “Oxide”.

[2]

(f) Draw a labelled diagram to illustrate the apparatus you would use to investigate

this reaction and collect and measure the volume of gas produced.

[3]

[TOTAL = 13]

- 9 -

SECTION B



where relevant.

(a) Fractional distillation

(b) The industrial manufacture of sulphuric acid

(c) The mole concept

(d) The bonding and structure of sodium and water

(e) The formation of soluble salts

(f) The manufacture of iron from its ore (include all relevant equations)

(g) The structures, properties and uses of TWO polymers

SECTION B ANSWER

- 10 -


- 11 -


- 12 -

3 11

19

37

55

87

4 12

20

38

56

88

21

39

57

89

22

40

72

104

23

41

73

105

24

42

74

106

25

43

75

58

90

59

91

60

92

61

93

62

94

63

95

64

96

65

97

66

98

67

99

68

100

69

101

70

102

71

103

26

44

76

27

45

77

28

46

78

29

47

79

30

48

80

5 13

31

49

81

6 14

32

50

82

7 15

33

51

83

8 16

34

52

84

9 17

35

53

85

10

18

36

54

86

Li

Na K Rb

Cs

Fr7 23

39

85

133

(223

)

9 24

40

88

137

(226

)

45

89

139

(227

)

48

91

178

(261

)

51

93

18

1

(26

2)

52

96

184

(263

)

55

(99

)

18

6

140

232

141

(231)

14

4

23

8

(14

7)

(23

7)

15

0

(24

2)

15

2

(24

3)

15

7

(24

7)

159

(245

)

163

(251

)

165

(254

)

167

(253

)

169

(256

)

173

(254)

17

5

(25

7)

56

10

1

19

0

59

10

3

19

2

59

10

6

19

5

63

.5

10

8

19

7

65

.4

112

201

11

27

70

11

5

204

12

28

73

11

9

207

14

31

75

122

209

16

32

79

12

8

(21

0)

19

35.5

80

12

7

(21

0)

20

40

84

13

1

(22

2)

Lith

ium

So

diu

m

Po

tassiu

m

Ru

bid

ium

Ca

esiu

m

Fra

nciu

m

Bery

lium

Mag

ne

siu

m

Ca

lciu

m

Str

on

tium

Ba

riu

m

Ra

diu

m

Sca

ndiu

m

Ytt

riu

m

Lanth

an

um

Actiniu

m

Titaniu

m

Zircon

ium

Hafn

ium

Un

nilq

ua

diu

m

Va

na

diu

m

Nio

biu

m

Tan

talu

m

Un

nilp

entium

Ch

rom

ium

Mo

lybd

en

um

Tun

gste

n

Un

nilh

exiu

m

Mang

an

ese

Te

chn

etiu

m

Rh

en

ium

Ceriu

m

Tho

riu

m

Pra

seo

dym

ium

Pro

tactiniu

m

Neo

dim

ium

Ura

niu

m

Pro

me

thiu

m

Ne

ptu

niu

m

Sa

mari

um

Plu

toniu

m

Euro

piu

m

Am

eri

ciu

m

Gad

olin

ium

Curi

um

Terb

ium

Be

rke

lium

Dyspro

siu

m

Ca

lifo

rniu

m

Ho

lmiu

m

Ein

ste

iniu

m

Erb

ium

Fe

rmiu

m

Thu

lium

Men

dele

viu

m

Ytte

rbiu

m

Nob

eliu

m

Lute

tiu

m

Law

renciu

m

Iron

Ru

the

niu

m

Osm

ium

Co

ba

lt

Rho

diu

m

Irid

ium

Nic

kel

Pa

llad

ium

Pla

tin

um

Co

pp

er

Silv

er

Go

ld

Zin

c

Cad

miu

m

Me

rcury

Boro

n

Alu

min

ium

Ga

llium

Indiu

m

Tha

lliu

m

Carb

on

Sili

con

Germ

aniu

m

Tin

Lea

d

Nitro

gen

Ph

osp

ho

rus

Ars

en

ic

An

tim

on

y

Bis

mu

th

Oxyg

en

Su

lph

ur

Sele

niu

m

Tellu

riu

m

Polo

niu

m

Flu

ori

ne

Chlo

rin

e

Bro

min

e

Iodin

e

Asta

tine

Ne

on

Arg

on

Kry

pto

n

Xen

on

Rad

on

Heliu

mH

ydro

gen

12

14

H

Be

Mg

Ca

Sr

Ba

Ra

Sc Y La

Ac

Ti

Zr

Hf

Un

q

V Nb

Ta

Un

p

Cr

Mo

W

Un

h

Mn

Tc

Re

Ce

Th

Pr

Pa

Nd U

Pm

Np

Sm

Pu

Eu

Am

Gd

Cm

Tb

Bk

Dy

Cf

Ho

Es

Er

Fm

Tm

Md

Yb

No

Lu

Lr

Fe

Ru

Os

Co

Rh Ir

Ni

Pd

Pt

Cu

Ag

Au

Zn

Cd

Hg

B Al

Ga

In Ti

C Si

Ge

Sn

Pb

N P As

Sb

Bi

O S Se

Te

Po

F Cl

Br I At

Ne

Ar

Kr

Xe

Rn

He

Ato

mic

Num

ber

Sym

bo

l

Nam

e

Mola

r m

ass in

g m

ol–

1

Peri

od

Ke

y

Gro

up

TH

E P

ER

IOD

IC T

AB

LE

12

34

56

70

1 2 3 4 5 6 7

La

nth

an

ide

ele

me

nts

Ac

tin

ide

ele

me

nts

- 1 -

THE KING’S SCHOOL, CANTERBURY

SIXTH FORM ENTRANCE EXAMINATION

2014-2015

CHEMISTRY

1 Hour


Present School: ……………………………………………………….


TOTAL MARK = 70









- 2 -

SECTION A



Symbol Number of

protons

Number of

neutrons

Mass

number

Electron

arrangement

Si 14 14

13 27 2.8.2

O2- 16

[TOTAL = 7]












(i) lead(II) carbonate....................................................................

(ii) Potassium nitride....................................................................

(iii) ammonium hydroxide............................................................

(iv) ammonium sulfate..................................................................

(v) iron(III) hydrogencarbonate....................................................

[5]

- 3 -


below:

(i) ........Na + .........H2O .........NaOH + .........H2

(ii) ........Fe2O3 + ........CO ........Fe + ..........CO2

(iii) ........C7H16 + ........O2 ........CO2 + ........H2O

(iv) ........ Al2(SO4)3 + ........NaOH ........Al(OH)3 + .........Na2SO4

[4]

[TOTAL = 9]

Q3 Atoms are made of electrons, neutrons and protons.

(a) Complete the table to show the relative mass and charge of an electron,

neutron and proton.

particle relative mass relative charge

electron 1/1840

neutron 0

proton

[4]

(b) The diagram shows the electronic structure of an atom of an element.

(i) Name the element of which this is an atom.

Explain your answer.

..........................................................................................................................

..........................................................................................................................

[2]

×

×

××

× ×

×

×

×

×

×

××

×

×

×

×

- 4 -

(ii) What is the atomic number of this element?

..........................................................................................................................

[1]

(c) The table below shows some information about the isotopes of neon.

Isotope Mass

Number

Abundance

arsenic-74 74 9%

arsenic-75 75 91%

(i) What is the definition of an isotope?

…………………………………………………………………………..........

…………………………………………………………………………..........

…………………………………………………………………………..........

…………………………………………………………………………..........

[2]

(ii) Calculate the relative atomic mass of arsenic.

…………………………………………………………………………..........

…………………………………………………………………………..........

……………...…………………………………………………………...........

…………………………………………………………………………..........

[2]

[TOTAL = 11]

- 5 -


Substance Melting

point /

°C

Boiling

point /

°C

Electrical

conductivity

when solid

Electrical

conductivity

when molten

Solubility in

water

A 1410 2355 poor poor insoluble

B -25 144 poor poor insoluble

C 712 1418 poor good soluble

D -101 -35 poor poor soluble

E 1660 3287 good good insoluble













[TOTAL = 5]

Q5 (a) Draw a dot-cross diagram to show the bonding in an ammonia molecule. Show the

outer shell electrons only. Name the type of bonding.

[3]

- 6 -

(b) Draw one molecule of ethane and one molecule of ethene, showing all the

bonds.

ethane ethene

[4]

[TOTAL = 7]

Q6 Molten, impure iron is made from iron ore in the blast furnace.

(a) In the blast furnace, reducing agents change iron ore into iron.

Give the name of ONE substance which can act as a reducing agent in the

blast furnace.

………………………………………………………………………………

[1]

(b) The main impurity in iron ore is silicon dioxide (SiO2).

Describe how this is removed.

Give the name of the raw material which must be present to remove this

impurity and describe the reactions involved, naming the waste product

formed.

You should include equations for the chemical reactions taking place.

………………………………………………………………………………

………………………………………………………………………………

………………………………………………………………………………

………………………………………………………………………………

………………………………………………………………………………

………………………………………………………………………………

………………………………………………………………………………

………………………………………………………………………………

………………………………………………………………………………

[5] [TOTAL = 6]

- 7 -

Q7 Sodium nitrate decomposes on strong heating as shown:

2KNO3(s) 2KNO2(s) + O2(g)

If 51.0 g of potassium nitrate was completely decomposed by heating, what mass

of solid would remain? Show full working.

[TOTAL = 4]

Q8 Hydrogen peroxide (H2O2) decomposes slowly at room temperature to form oxygen

and water.

(a) Write a balanced equation for this reaction.

..........................................................................................................................

[2]

(b) Manganese(IV) oxide acts as a catalyst for this reaction.

Andy added 1.0 g of manganese(IV) oxide to 20 cm3 of hydrogen peroxide

solution at room temperature.

He measured the total volume of oxygen given off at one minute intervals.

His results are shown in the table.

Time (minutes) 0 1 2 3 4 5

Total volume of oxygen

(cm3)

0 31 41 46 48 48

Draw a graph of total volume of oxygen produced against time.

- 8 -

[3]

(c) At the end of the experiment Andy filtered off the oxide.

What mass of oxide would you expect to be left?

..........................................................................................................................

[1]

(d) Andy then added 1.0 g of a different oxide to a fresh 20 cm3 sample of

hydrogen peroxide solution at the same temperature.

Again he measured the volume of oxygen produced at one minute intervals.

From his results he concluded that this different oxide was a better catalyst

than manganese(IV) oxide.

Add a line to your graph to show results which would support this

conclusion. Label this new line “Oxide”.

[2]

(e) Draw a labelled diagram to illustrate the apparatus you would use to investigate

this reaction and collect and measure the volume of gas produced.

[3]

[TOTAL = 11]

3

Totalvolumeof oxygenin cm

Time in minutes

- 9 -

SECTION B



where relevant.

(a) Cracking

(b) The structures, properties and uses of TWO polymers

(c) The mole concept

(d) Catalysts

(e) The bonding and structure of graphite and diamond

(f) The formation of insoluble salts

(g) The manufacture of aluminium from its ore

(h) The industrial manufacture of ammonia

SECTION B ANSWER

- 10 -


- 11 -

3 11

19

37

55

87

4 12

20

38

56

88

21

39

57

89

22

40

72

104

23

41

73

105

24

42

74

106

25

43

75

58

90

59

91

60

92

61

93

62

94

63

95

64

96

65

97

66

98

67

99

68

100

69

101

70

102

71

103

26

44

76

27

45

77

28

46

78

29

47

79

30

48

80

5 13

31

49

81

6 14

32

50

82

7 15

33

51

83

8 16

34

52

84

9 17

35

53

85

10

18

36

54

86

Li

Na K Rb

Cs

Fr7 23

39

85

133

(223

)

9 24

40

88

137

(226

)

45

89

139

(227

)

48

91

178

(261

)

51

93

18

1

(26

2)

52

96

184

(263

)

55

(99

)

18

6

140

232

141

(231)

14

4

23

8

(14

7)

(23

7)

15

0

(24

2)

15

2

(24

3)

15

7

(24

7)

159

(245

)

163

(251

)

165

(254

)

167

(253

)

169

(256

)

173

(254)

17

5

(25

7)

56

10

1

19

0

59

10

3

19

2

59

10

6

19

5

63

.5

10

8

19

7

65

.4

112

201

11

27

70

11

5

204

12

28

73

11

9

207

14

31

75

122

209

16

32

79

12

8

(21

0)

19

35.5

80

12

7

(21

0)

20

40

84

13

1

(22

2)

Lith

ium

So

diu

m

Po

tassiu

m

Ru

bid

ium

Ca

esiu

m

Fra

nciu

m

Bery

lium

Mag

ne

siu

m

Ca

lciu

m

Str

on

tium

Ba

riu

m

Ra

diu

m

Sca

ndiu

m

Ytt

riu

m

Lanth

an

um

Actiniu

m

Titaniu

m

Zircon

ium

Hafn

ium

Un

nilq

ua

diu

m

Va

na

diu

m

Nio

biu

m

Tan

talu

m

Un

nilp

entium

Ch

rom

ium

Mo

lybd

en

um

Tun

gste

n

Un

nilh

exiu

m

Mang

an

ese

Te

chn

etiu

m

Rh

en

ium

Ceriu

m

Tho

riu

m

Pra

seo

dym

ium

Pro

tactiniu

m

Neo

dim

ium

Ura

niu

m

Pro

me

thiu

m

Ne

ptu

niu

m

Sa

mari

um

Plu

toniu

m

Euro

piu

m

Am

eri

ciu

m

Gad

olin

ium

Curi

um

Terb

ium

Be

rke

lium

Dyspro

siu

m

Ca

lifo

rniu

m

Ho

lmiu

m

Ein

ste

iniu

m

Erb

ium

Fe

rmiu

m

Thu

lium

Men

dele

viu

m

Ytte

rbiu

m

Nob

eliu

m

Lute

tiu

m

Law

renciu

m

Iron

Ru

the

niu

m

Osm

ium

Co

ba

lt

Rho

diu

m

Irid

ium

Nic

kel

Pa

llad

ium

Pla

tin

um

Co

pp

er

Silv

er

Go

ld

Zin

c

Cad

miu

m

Me

rcury

Boro

n

Alu

min

ium

Ga

llium

Indiu

m

Tha

lliu

m

Carb

on

Sili

con

Germ

aniu

m

Tin

Lea

d

Nitro

gen

Ph

osp

ho

rus

Ars

en

ic

An

tim

on

y

Bis

mu

th

Oxyg

en

Su

lph

ur

Sele

niu

m

Tellu

riu

m

Polo

niu

m

Flu

ori

ne

Chlo

rin

e

Bro

min

e

Iodin

e

Asta

tine

Ne

on

Arg

on

Kry

pto

n

Xen

on

Rad

on

Heliu

mH

ydro

gen

12

14

H

Be

Mg

Ca

Sr

Ba

Ra

Sc Y La

Ac

Ti

Zr

Hf

Un

q

V Nb

Ta

Un

p

Cr

Mo

W

Un

h

Mn

Tc

Re

Ce

Th

Pr

Pa

Nd U

Pm

Np

Sm

Pu

Eu

Am

Gd

Cm

Tb

Bk

Dy

Cf

Ho

Es

Er

Fm

Tm

Md

Yb

No

Lu

Lr

Fe

Ru

Os

Co

Rh Ir

Ni

Pd

Pt

Cu

Ag

Au

Zn

Cd

Hg

B Al

Ga

In Ti

C Si

Ge

Sn

Pb

N P As

Sb

Bi

O S Se

Te

Po

F Cl

Br I At

Ne

Ar

Kr

Xe

Rn

He

Ato

mic

Num

ber

Sym

bo

l

Nam

e

Mola

r m

ass in

g m

ol–

1

Peri

od

Ke

y

Gro

up

TH

E P

ER

IOD

IC T

AB

LE

12

34

56

70

1 2 3 4 5 6 7

La

nth

an

ide

ele

me

nts

Ac

tin

ide

ele

me

nts

Sixth Form Entrance 2017 CHEMISTRY

Documents

Transcript of Sixth Form Entrance 2017 CHEMISTRY