GCE Chemistry Data Sheet

1338 Pages·2014·19.01 MB·English

GCE Chemistry Data Sheet
W
M
P
/In Table 1 Table 2 Table 3
s
e
rt to Infrared absorption data 1H n.m.r. chemical shift data 13C n.m.r. chemical shift data
A
-lev Bond Wavenumber Type of proton δ/ppm Type of carbon δ/ppm
e
l C /cm–1
he ROH 0.5 – 5.0
mis N H 3300 – 3500 C C 5 – 40
try (amines) RCH3 0.7 – 1.2
RNH 1.0 – 4.5
O H 3230 – 3550 2 R C Cl or Br 10 – 70
(alcohols) R2CH2 1.2 – 1.4
R CH 1.4 – 1.6
C H 2850 – 3300 3
R C C 20 – 50
O H 2500 – 3000
R C C 2.1– 2.6
O
(acids)
O H
C N 2220 – 2260
R C N 25 – 60
C O 1680 – 1750 R O C 3.1 – 3.9
C C 1620 – 1680 H alcohols,
C O 1000 – 1300 RCH2Cl or Br 3.1 – 4.2 C O ethers or 50 – 90
esters
C C 750 – 1100
R C O C 3.7 – 4.1
C C 90 – 150
O H
R H
R C N 110 – 125
C C 4.5 – 6.0
110 – 160
O
R C 9.0 – 10.0 esters or
R C 160 – 185
acids
H
O
O
aldehydes
R C 190 – 220
R C 10.0 – 12.0
or ketones
O H O
The Periodic Table of the Elements
1 2 3 4 5 6 7 0
(18)
1.0 4.0
H He
hydrogen helium
(1) (2) Key (13) (14) (15) (16) (17)
1 2
6.9 9.0 relative atomic mass 10.8 12.0 14.0 16.0 19.0 20.2
Li Be symbol B C N O F Ne
lithium beryllium name boron carbon nitrogen oxygen fluorine neon
3 4 atomic (proton) number 5 6 7 8 9 10
23.0 24.3 27.0 28.1 31.0 32.1 35.5 39.9
Na Mg Al Si P S Cl Ar
sodium magnesium (3) (4) (5) (6) (7) (8) (9) (10) (11) (12) aluminium silicon phosphorus sulfur chlorine argon
11 12 13 14 15 16 17 18
39.1 40.1 45.0 47.9 50.9 52.0 54.9 55.8 58.9 58.7 63.5 65.4 69.7 72.6 74.9 79.0 79.9 83.8
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton
19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36
85.5 87.6 88.9 91.2 92.9 96.0 [98] 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon
37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54
132.9 137.3 138.9 178.5 180.9 183.8 186.2 190.2 192.2 195.1 197.0 200.6 204.4 207.2 209.0 [209] [210] [222]
Cs Ba La * Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
caesium barium lanthanum hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon
55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86
[223] [226] [227] [267] [268] [271] [272] [270] [276] [281] [280]
Fr Ra Ac † Rf Db Sg Bh Hs Mt Ds Rg Elements with atomic numbers 112-116 have been reported but
francium radium actinium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium not fully authenticated
87 88 89 104 105 106 107 108 109 110 111
140.1 140.9 144.2 [145] 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.1 175.0
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
* 58 – 71 Lanthanides
cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium
58 59 60 61 62 63 64 65 66 67 68 69 70 71
232.0 231.0 238.0 [237] [244] [243] [247] [247] [251] [252] [257] [258] [259] [262]
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
† 90 – 103 Actinides
thorium protactinium uranium neptunium plutonium americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium
90 91 92 93 94 95 96 97 98 99 100 101 102 103
For Examiner’s Use
Centre Number Candidate Number
Surname
Other Names
Examiner’s Initials
Candidate Signature
Question Mark
General Certificate of Education
1
Advanced Subsidiary Examination
January 2010 2
3
Chemistry CHEM1
4
5
Unit 1 Foundation Chemistry
6
Thursday 14 January 2010 9.00am to 10.15am
TOTAL
For this paper you must have:
(cid:2) the Periodic Table/Data Sheet,provided as an insert
(enclosed)
(cid:2) a calculator.
Time allowed
(cid:2) 1 hour 15 minutes
Instructions
(cid:2) Use black ink or black ball-point pen.
(cid:2) Fill in the boxes at the top of this page.
(cid:2) Answer all questions.
(cid:2) You must answer the questions in the spaces provided. Answers
written in margins or on blank pages will not be marked.
(cid:2) All working must be shown.
(cid:2) Do all rough work in this book. Cross through any work you do not
want to be marked.
Information
(cid:2) The marks for questions are shown in brackets.
(cid:2) The maximum mark for this paper is 70.
(cid:2) The Periodic Table/Data Sheet is provided as an insert.
(cid:2) Your answers to the questions in Section B should be written in
continuous prose, where appropriate.
(cid:2) You will be marked on your ability to:
– use good English
– organise information clearly
– use accurate scientific terminology.
Advice
(cid:2) You are advised to spend about 50 minutes on Section A and about
25 minutes on Section B.
(JAN10CHEM101) CHEM1
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SECTION A
Answer all questions in the spaces provided.
1 Ionisation energies provide evidence for the arrangement of electrons in atoms.
1 (a) Complete the electron configuration of the Mg+ ion.
1s2 ......................................................................................................................................
(1 mark)
1 (b) (i) State the meaning of the term first ionisation energy.
...................................................................................................................................
...................................................................................................................................
...................................................................................................................................
(2 marks)
1 (b) (ii) Write an equation, including state symbols, to show the reaction that occurs
when the second ionisation energy of magnesium is measured.
...................................................................................................................................
(1 mark)
1 (b) (iii) Explain why the second ionisation energy of magnesium is greater than the first
ionisation energy of magnesium.
...................................................................................................................................
...................................................................................................................................
...................................................................................................................................
(1 mark)
1 (b) (iv) Use your understanding of electron arrangement to complete the table by
suggesting a value for the third ionisation energy of magnesium.
First Second Third Fourth Fifth
Ionisation energies of
736 1450 10500 13629
magnesium/kJmol–1
(1 mark)
(02)
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1 (c) State and explain the general trend in the first ionisation energies of the Period 3
elements sodium to chlorine.
Trend ..................................................................................................................................
Explanation ........................................................................................................................
.............................................................................................................................................
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(3 marks)
(Extra space) ......................................................................................................................
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1 (d) State how the element sulfur deviates from the general trend in first ionisation energies
across Period 3. Explain your answer.
How sulfur deviates from the trend ...................................................................................
.............................................................................................................................................
Explanation ........................................................................................................................
.............................................................................................................................................
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(3 marks)
(Extra space) ......................................................................................................................
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1 (e) A general trend exists in the first ionisation energies of the Period 2 elements lithium
to fluorine. Identify one element which deviates from this general trend.
.............................................................................................................................................
(1 mark)
13
Turn over (cid:2)
(03)
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2 Ammonium sulfate reacts with sodium hydroxide to form ammonia, sodium sulfate and
water as shown in the equation below.
→
(NH ) SO (s) + 2NaOH(aq) 2NH (g) + Na SO (aq) + 2H O(l)
4 2 4 3 2 4 2
2 (a) A 3.14g sample of ammonium sulfate reacted completely with 39.30cm3 of a sodium
hydroxide solution.
2 (a) (i) Calculate the amount, in moles, of (NH ) SO in 3.14g of ammonium sulfate.
4 2 4
...................................................................................................................................
...................................................................................................................................
...................................................................................................................................
(2 marks)
2 (a) (ii) Hence calculate the amount, in moles, of sodium hydroxide which reacted.
...................................................................................................................................
(1 mark)
2 (a) (iii) Calculate the concentration, in moldm–3, of the sodium hydroxide solution used.
...................................................................................................................................
...................................................................................................................................
(1 mark)
2 (b) Calculate the percentage atom economy for the production of ammonia in the reaction
between ammonium sulfate and sodium hydroxide.
.............................................................................................................................................
.............................................................................................................................................
.............................................................................................................................................
(2 marks)
(04)
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2 (c) Ammonia is manufactured by the Haber Process.
N + 3H 2NH
2 2 3
Calculate the percentage atom economy for the production of ammonia in this process.
.............................................................................................................................................
.............................................................................................................................................
(1 mark)
2 (d) A sample of ammonia gas occupied a volume of 1.53 × 10–2 m3 at 37°C and a
pressure of 100 kPa.
(The gas constant R = 8.31JK–1 mol–1)
Calculate the amount, in moles, of ammonia in this sample.
.............................................................................................................................................
.............................................................................................................................................
.............................................................................................................................................
(3 marks)
(Extra space) ......................................................................................................................
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2 (e) Glauber’s salt is a form of hydrated sodium sulfate that contains 44.1% by mass of
sodium sulfate. Hydrated sodium sulfate can be represented by the formula
Na SO .xH O where x is an integer. Calculate the value of x.
2 4 2
.............................................................................................................................................
.............................................................................................................................................
.............................................................................................................................................
.............................................................................................................................................
(3 marks)
(Extra space) ......................................................................................................................
.............................................................................................................................................
13
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Turn over (cid:2)
(05)
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3 The table below shows the boiling points of some hydrogen compounds formed by Group 6
elements.
H O H S H Se H Te
2 2 2 2
Boiling point/K 373 212 232 271
3 (a) State the strongest type of intermolecular force in water and in hydrogen sulfide (H S).
2
Water ..................................................................................................................................
Hydrogen sulfide ................................................................................................................
(2 marks)
3 (b) Draw a diagram to show how two molecules of water are attracted to each other by the
type of intermolecular force you stated in part (a). Include partial charges and all lone
pairs of electrons in your diagram.
(3 marks)
3 (c) Explain why the boiling point of water is much higher than the boiling point of
hydrogen sulfide.
.............................................................................................................................................
.............................................................................................................................................
(1 mark)
3 (d) Explain why the boiling points increase from H S to H Te
2 2
.............................................................................................................................................
.............................................................................................................................................
(2 marks)
(06)
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3 (e) When H+ ions react with H O molecules, H O+ ions are formed.
2 3
Name the type of bond formed when H+ ions react with H O molecules.
2
Explain how this type of bond is formed in the H O+ ion.
3
Type of bond ......................................................................................................................
Explanation ........................................................................................................................
.............................................................................................................................................
(2 marks)
3 (f) Sodium sulfide (Na S) has a melting point of 1223K.
2
Predict the type of bonding in sodium sulfide and explain why its melting point is
high.
Type of bonding .................................................................................................................
Explanation ........................................................................................................................
.............................................................................................................................................
.............................................................................................................................................
(3 marks)
(Extra space) ......................................................................................................................
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13
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Turn over for the next question
Turn over (cid:2)
(07)
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4 Alkanes are saturated hydrocarbons which can be obtained from crude oil.
Pentane is an example of an alkane. A molecule of pentane contains five carbon atoms.
4 (a) (i) State the meaning of the term saturated and of the term hydrocarbon as applied
to alkanes.
Saturated ...................................................................................................................
...................................................................................................................................
Hydrocarbon .............................................................................................................
...................................................................................................................................
(2 marks)
4 (a) (ii) Give the general formula for the alkanes.
...................................................................................................................................
(1 mark)
4 (b) Pentane burns completely in oxygen.
4 (b) (i) Write an equation for this reaction.
...................................................................................................................................
(1 mark)
4 (b) (ii) State how the products of this reaction may affect the environment.
...................................................................................................................................
...................................................................................................................................
(1 mark)
4 (c) Give the name of a solid pollutant which may form when pentane burns incompletely
in air.
.............................................................................................................................................
(1 mark)
(08)
WMP/Jan10/CHEM1