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2012 Chemistry 1 NEAP Exam-2
Physical Science
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Neap Trial Exams are licensed to be photocopied or placed on the school intranet and used only within the confines of the school purchasing them, forthe purpose of examining that school’s students only. They may not be otherwise reproduced or distributed. The copyright of Neap Trial Exams remains with Neap. No Neap Trial Exam or any part thereof is to be issued or passed on by any person to any party inclusive of other schools, non-practisingteachers, coaching colleges, tutors, parents, students, publishing agencies or websites without the express written consent of Neap. Copyright © 2012 Neap ABN 49 910 906 643 96–106 Pelham St Carlton VIC 3053 Tel: (03) 8341 8341 Fax: (03) 8341 8300 TEVCHEMU1_QA_2012
Trial Examination 2012
VCE Chemistry Unit 1
Written Examination
Question and Answer Booklet
Reading time: 15 minutes Writing time: 1 hour 30 minutes Student’s Name: ______________________________ Teacher’s Name: ______________________________ Structure of Booklet Section Number ofquestions questions to beNumber ofanswered Marks Suggested time(minutes) A Multiple-choice 20 20 20 25 B Short-answer 4 4 50 65 Total 70 Total 90 Students are permitted to bring into the examination room: pens, pencils, highlighters, erasers, sharpeners, rulers and one scientific calculator. Students are NOT permitted to bring into the examination room: blank sheets of paper and/or white out liquid/tape. Materials supplied Question and answer booklet of 14 pages with a detachable data sheet in the centrefold. Data booklet of 3 pages. Answer sheet for multiple-choice questions. Instructions Please ensure that you write your name and your teacher’s name in the space provided on this booklet and in the space provided on the answer sheet for multiple-choice questions. All written responses must be in English. At the end of the examination Place the answer sheet for multiple-choice questions inside the front cover of this booklet and hand them in. Students are NOT permitted to bring mobile phones and/or any other unauthorised electronic communication devices into the examination room.
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SECTION A: MULTIPLE-CHOICE QUESTIONS
Question 1 Which of the following compounds have an empirical formula which is the same as the molecular formula? I C 6 H 5 Cl II C 2 H 5 COOH III C 6 H 12 O 6 IV C 10 H 8 A. I and II only B. I, III and IV only C. II, III and IV only D. III and IV only
Question 2 Which of the following contains the smallest number of oxygen atoms? A. 2 × 10 23 molecules of sulfur trioxide gas B. 19 g of ice C. 0 mol of oxygen atoms D. 0 mol of oxygen gas
Question 3 Which one of the following statements about thermosetting plastics is incorrect? A. The number of crosslinks will influence the temperature at which these plastics soften and can be moulded. B. These plastics tend to be rigid, brittle materials which can be used in applications that require the use of moderate heat. C. If a high enough temperature is used, these plastics will char and burn, leaving a black residue which is mostly carbon. D. These plastics are quite difficult to recycle and many are disposed of in landfill waste.
Question 4 Alkanes are compounds composed of carbon and hydrogen. Silicon also forms compounds with hydrogen, known as silanes. How many different molecular structures are expected for the silane compound Si 4 H 10? A. 1 B. 2 C. 3 D. 4
Instructions for Section A Answer all questions in pencil on the answer sheet provided for multiple-choice questions. Choose the response that is correct or that best answers the question. A correct answer scores 1, an incorrect answer scores 0. Marks will not be deducted for incorrect answers. No marks will be given if more than one answer is completed for any question.
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Question 9 The properties of metals can be modified by heat treatment. If a metal is heated to red hot and then cooled slowly in air, which of the following crystal sizes and properties is the heat treated metal likely to have?
Question 10 Element X has the following properties:
- high electronegativity
- small atomic radius
- one of the highest first ionisation energies of any element The location of element X in the Periodic Table is most likely to be in A. Period 2 and Group 17. B. Period 3 and Group 3. C. Period 4 and Group 18. D. Period 5 and Group 16.
Question 11 A substance is insoluble in water, and melts at a high temperature. The substance does not conduct electricity in the solid state, but conducts when molten. The substance is most likely to be A. NaCl. B. Ni. C. CuO. D. S.
Question 12 Which of the following shows the correct molecular polarity and molecular shape of the listed molecules?
Size of metal crystals Properties of the treated metal A. tiny hard and brittle B. tiny soft and malleable C. large hard and flexible D. large soft and ductile
Molecule Molecular polarity Molecular shape A. CO 2 polar V-shaped B. NH 3 polar tetrahedral C. CCl 4 non-polar trigonal pyramidal D. SF 6 non-polar octahedral
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Question 13 An experiment was conducted to determine the percentage by mass of the elements in a compound consisting of tin and oxygen. The mass of oxygen reacting with a sample of tin can be determined by heating the metal in a crucible until no further reaction occurs. Some steps in the experiment are shown below in the incorrect order.
- Weigh the metal and record its mass.
- Ignite the burner and heat the metal.
- Allow the crucible to cool and then weigh it.
- Remove any oxide layer on the metal by scrubbing.
- Continue heating the crucible until any reaction is complete.
- Put metal into crucible of known mass and cover with lid. What order of steps should be used to conduct an accurate experiment? A. 1, 4, 6, 2, 3, 5 B. 6, 2, 5, 3, 4, 1 C. 4, 1, 6, 2, 5, 3 D. 2, 5, 3, 4, 1, 6
Question 14 The total number of atoms in 90 g of (NH 4 ) 3 PO 4 is A. 3 × 10 23. B. 1 × 10 24. C. 6 × 10 24. D. 7 × 10 24.
Question 15 Which of the following shows the correct order of discovery of the listed items, beginning with the earliest discovered? A. proton, neutron, nucleus, electron, isotopes B. electron, proton, nucleus, isotopes, neutron C. electron, neutron, proton, isotopes, nucleus D. nucleus, proton, neutron, isotopes, electron
Question 16 Which of the following substances could not be used to form an addition polymer? A. ClCH 2 CHCl 2 B. CH 3 CHCCl 2 C. CH 3 CH 2 C(OH)CH 2 D. C 2 H 2 Br 2
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SECTION B: SHORT-ANSWER QUESTIONS
Question 1 Analysis of a mixture of equimolar quantities of argon and potassium produced the data shown in the table and the spectrum displayed below.
a. Using the notation , give the symbol for the chemical species that produced the result in the spectrum marked Q. _________________________________________________________________________________ 2 marks
Instructions for Section B Answer all questions in the spaces provided. To obtain full marks for your responses you should
- give simplified answers with an appropriate number of significant figures to all numerical questions; unsimplified answers will not be given full marks.
- show all working in your answers to numerical questions. No credit will be given for an incorrect answer unless it is accompanied by details of the working.
- make sure chemical equations are balanced and that the formulas for individual substances include an indication of state; for example H 2 (g); NaCl(s).
Element Atomic number Relative isotopicmass abundance (%)Relative
Argon 18 35.97837.97439 99.6330.
Potassium 19 38.97539.97640 0.01193.
relative isotopic mass
relative abundance (%)
0 34 35 36 37 38 39 40 41
20
40
60
80
100
Q
A Z X x
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b. Relative isotopic mass has no units. Explain why. ________________________________________________________________________________ ________________________________________________________________________________ ________________________________________________________________________________ 1 mark c. When asked to calculate the relative atomic mass of argon, a student used the method:
The accepted value for the relative atomic mass of argon is 39. i. Identify the error in the student’s method. ___________________________________________________________________________ ___________________________________________________________________________ ii. Show how the relative atomic mass of argon should be calculated using the data provided. ___________________________________________________________________________ ___________________________________________________________________________ 1 + 1 = 2 marks d. Potassium has a higher atomic number than argon, but a smaller relative atomic mass. Explain how this situation occurs.
2 marks e. A similar situation occurs with the elements tellurium and iodine, with the higher atomic number iodine having a smaller mass than tellurium. In the Periodic Table produced by Mendeleev in 1869, elements were ordered horizontally by increasing atomic mass. However, in Mendeleev’s table, the element tellurium was placed before iodine (just as it is in the modern table). On what basis did Mendeleev place tellurium before iodine?
1 mark Total 8 marks
( 35 + 37 +39)
------------------------------------------------------------------ 3 - =37.
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c. Aluminium oxide is a compound of oxygen and a Period 3 element. Several other oxides of Period 3 elements, together with their melting points, are shown in the table below.
i. SO 3 forms a trigonal planar molecule. Name the bond types present in a sample of liquid SO 3. ___________________________________________________________________________ ___________________________________________________________________________ ii. Explain why the melting point of MgO is much higher than that of Na 2 O. ___________________________________________________________________________ ___________________________________________________________________________ ___________________________________________________________________________ ___________________________________________________________________________ 2 + 2 = 4 marks d. Cryolite is a compound composed of fluorine (54%), aluminium (12%) and sodium. Determine the empirical formula of cryolite.
2 marks e. Aluminium is often combined with other metals to produce alloys. An alloy of aluminium and the element scandium is used in spacecraft manufacture. Scientists have designed this alloy to form nanoparticles, which produces an extremely strong material. i. In terms of structure and bonding, explain why alloying metals often produces a stronger metal.
ii. Explain why the alloy composed of nanoparticles produces a much stronger material.
2 + 2 = 4 marks Total 14 marks
Formula of oxide Na 2 O MgO SiO 2 P 2 O 5 SO 3 Melting point (°C) 920 2800 1700 250 62
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Question 3 a. The element seaborgium (Z = 106) was named in honour of the scientist Glenn Seaborg who was involved in the discovery of elements 94 to 102. Most of these elements were produced by firing a neutron at the nucleus of an atom of another element. If the neutron is captured by the nucleus, the neutron disintegrates to produce a proton and a beta particle which is ejected. i. How are scientists able to claim that a new element has been produced by this neutron capture process? ____________________________________________________________________________ ____________________________________________________________________________ ____________________________________________________________________________ ____________________________________________________________________________ ii. Some of these new elements are produced in minute quantities and exist for as briefly as 10 –14 seconds. Suggest how chemists could predict the properties of these elements. ____________________________________________________________________________ ____________________________________________________________________________ ____________________________________________________________________________ iii. Seaborg also identified the actinides as a separate grouping in the modern Periodic Table. Which type of subshell is being progressively filled in the elements of the actinide series? ____________________________________________________________________________ 2 + 1 + 1 = 4 marks b. An atom of seaborgium can be made by initially forcing a zinc (Z = 30) nucleus to combine with a lead (Z = 82) nucleus. This produces an unstable nucleus which emits an alpha particle to form the nucleus of an atom of a different element. Alpha particles continue to be emitted until a stable nucleus is formed. An alpha particle consists of two protons and two neutrons. i. An alpha particle is simply the nucleus of a particular element. Name this element. ____________________________________________________________________________ ii. In total, how many alpha particles are emitted after the zinc and lead nuclei combine before a seaborgium nucleus is produced? ____________________________________________________________________________ 1 + 1 = 2 marks
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Question 4 The structural formulas of some carbon-based compounds are shown below.
Use the letters A to H to identify compounds when answering the following questions. (Letters may be used more than once.)
a. i. Identify two compounds which have the same molecular formula. ____________________________________________________________________________ ii. Identify one unsaturated hydrocarbon compound.
iii. Identify one compound which would undergo a substitution reaction.
1 + 1 + 1 = 3 marks b. Which of the compounds C, D or F would have the higher boiling point? Explain your choice. _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ 3 marks
A B C D
E F G H
C C C C C
H
H H
H H H H H
H H H
H HC H H H
H C C H
H H
H H
H C C H
H H HO
H
H C C H
H C H C C
H H
H H C O C H
H H H
H H C C
H H OCOCH 3
CH 3
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c. i. Write a balanced chemical equation for the reaction by which compound C is produced from compound F. Include any necessary reaction conditions. ___________________________________________________________________________ ___________________________________________________________________________ ii. Write a balanced chemical equation for the complete combustion of a gaseous sample of compound E.
2 + 2 = 4 marks d. Give the structural formula and systematic name of another isomer of compound A.
2 marks e. Draw a section of the product formed when compound H undergoes addition polymerisation.
2 marks f. Calculate the mass, in grams, of one molecule of compound H.
2 marks Total 16 marks
END OF QUESTION AND ANSWER BOOKLET
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2012 Chemistry 1 NEAP Exam-2
Subject: Physical Science
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