Trial Examination 2017 VCE Chemistry Unit 1 · 2019. 5. 16. · VCE Chemistry Unit 1 Written Examination Question and Answer Booklet Reading time: 15 minutes Writing time: 1 hour

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Trial Examination 2017

VCE Chemistry Unit 1Written 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 of questions

Number of questions to be

answeredNumber of

marksSuggested time

(minutes)

A 20 20 20 25

B 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 correction fluid/tape.

Materials supplied

Question and answer booklet of 13 pages.

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 bookletand in the space provided on the answer sheet for multiple-choice questions.Unless otherwise indicated, the diagrams in this booklet are not drawn to scale.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 devices into the examination room.

VCE Chemistry Unit 1 Trial Examination Question and Answer Booklet

2 CHEMU1_QA_2017.FM Copyright © 2017 Neap

SECTION A – MULTIPLE-CHOICE QUESTIONS

Question 1

Which one of the following is identical for each of the isotopes 36Ar, 38Ar and 40Ar?A. number of electrons and mass numberB. atomic number and number of neutronsC. number of nuclear particles and number of protonsD. ground state electron configuration and nuclear charge

Use the following information to answer Questions 2 and 3.

The structural formula of a compound of hydrogen, oxygen and carbon is shown below.

Question 2

Some properties of organic compounds include:

I Decolourises red-brown coloured bromine water.

II Reacts with reactive metals.

III Can be used as a monomer in polymerisation reactions.

Which of these properties apply to the compound shown?A. I and II onlyB. II and III onlyC. I, II and IIID. none of I, II and III

Question 3

Which one of the following statements about the compound (M = 72 g mol–1

) is correct?A. The empirical formula is different to the molecular formula.

B. In 3.6 g of the compound, there is 0.45 mole of atoms present.

C. In a sample of the compound, dispersion forces are the only intermolecular bonding.

D. There are 6.02 × 1023

oxygen atoms in 2 mole of the compound.

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.

Unless otherwise indicated, the diagrams in this booklet are not drawn to scale.

HOHC

H

C

H

C

O


Copyright © 2017 Neap CHEMU1_QA_2017.FM 3

Question 4

Which one of the following features applies to transition metals but not to the main group metals?A. Transition metals form compounds which are often coloured.B. Transition metals can be hammered into shapes without fracturing.C. Transition metals conduct electricity in the solid state, but not when molten.D. Transition metals usually have a shiny surface and can be drawn into wires.

Question 5

The scientist Niels Bohr studied the emission spectrum of hydrogen and made deductions aboutA. the types of particles in the nucleus.B. the arrangement of electrons.C. how subshells fill with electrons.D. isotopes and their mass numbers.

Question 6

The formula of a compound is C7H14O2.

Which one of the following could not be the name of the compound?A. ethyl pentanoateB. butyl propanoateC. methyl heptanoateD. heptanoic acid

Question 7

Isomers of a compound haveA. similar chemical properties and the same molecular formula. B. the same molecular formula and structural formula.C. similar physical properties and identical chemical properties.D. the same structural formula and identical physical properties.

Question 8

How many orbitals does the 4p subshell contain?A. 2B. 3C. 6D. 16

Question 9

A compound is composed of carbon, 26.7% oxygen and 13.3% hydrogen.

What conclusion can be made about the molecular formula of the compound?A. The number of hydrogen atoms is eight times the number of oxygen atoms.B. The number of carbon atoms is half the number of hydrogen atoms.C. The total number of carbon atoms and oxygen atoms equals the number of hydrogen atoms.D. From the data given, no valid conclusion can be made about the molecular formula.



Question 10

Information about the two isotopes of element X is shown in the table below.

Which of the following methods should be used to calculate the relative atomic mass of element X?

A.

B. (69 × 0.6011) + (71 × 0.3989)

C.

D. (68.926 × 0.6011) + (70.925 × 0.3989)


Using the equipment shown in the diagram, 7.53 g of an oxide of copper was reacted with ammonia gas until no further reaction occurred and only copper metal remained in the reaction tube. The mass of copper formed was found to be 6.01 g.

Question 11

Based on the results of this experiment, what is the empirical formula of the oxide of copper?A. CuO

B. Cu2O

C. CuO2

D. Cu3O4

Question 12

If insufficient ammonia had been used in the experiment, which one of the following would not be affected?A. the mass of water vapour formed in the reactionB. the amount of oxygen released from the oxide of copperC. the number of copper ions in the reaction tubeD. the calculated empirical formula of the oxide of copper

Question 13

Which group of compounds consists of molecules which all have the same shape?A. NH3; BF3; CH3Cl

B. PF5; SiCl4; C2F4

C. C2H4; CCl4; SF6

D. HCl; CS2; C2H2

Isotope % abundance Relative isotopic mass

69X 60.11 68.926

71X 39.89 70.925

69 71+( )2

-----------------------

68.926 70.925+( )2

--------------------------------------------

oxide of copper

heat

ammonia waste gases

(water vapour andnitrogen gas)



Question 14

Potassium fluoride melts at a slightly lower temperature than lithium fluoride.

This observation is best explained by considering theA. difference in electronegativity of the elements.B. type of bonding holding each lattice together.C. differences in charges on the ions present.D. comparative sizes of the ions involved.

Question 15

Pieces of three different metals were placed in test tubes containing hydrochloric acid. The observations made are summarised in the table below.

Based on these observations, the likely identity of metals X, Y and Z respectively isA. magnesium, gold, iron.B. copper, silver, lead.C. iron, gold, sodium.D. lead, copper, magnesium.

Question 16

A red blood cell has a diameter of 7 micrometers (7 μ m). A hydrogen molecule has a length of approximately 0.15 nanometers (0.15 nm).

Approximately how many times larger is the red blood cell than the hydrogen molecule?A. 500

B. 5000

C. 50 000

D. 500 000

Question 17

When the particle size of a substance is reduced to the nanoscale, properties of the nanomaterial may be different to those of the corresponding bulk material.

Which of the following changes in properties is least likely to occur when particle size is reduced to the nanoscale?A. altering the visible properties, such as colourB. increasing catalytic propertiesC. changing an opaque material to a transparent materialD. increasing the melting temperature of the substance

Metal Observations

X Bubbles of gas are rapidly produced. The metal disappears.

Y No signs of any chemical reaction occurs.

Z Bubbles of gas are slowly produced. The metal slowly disappears.




The first ionisation energies of seven consecutive elements in the periodic table are shown in the graph below. The elements are identified by letters that are not the correct elemental symbols.

Question 18

Which element is likely to be located in group 18?A. QB. SC. TD. W

Question 19

The first ionisation of element U is greater than that of element T becauseA. an atom of U contains more neutrons than an atom of T.B. the core charge of U is greater than the core charge of T.C. the outermost electron of U is further from the nucleus than the outermost electron in T.D. U is a transition metal, while T is a main group metal.

Question 20

Which electron configuration does not correctly match the corresponding description of the chemical entity?

END OF SECTION A

Electron configuration of the chemical entity

Description of the chemical entity

A. 1s22s

22p

63s

23p

4an uncharged atom with 16 protons in the nucleus

B. 1s22s

22p

43s

2an atom with excited electrons ready to emit energy

C. 1s22s

22p

63s

23p

2a negatively charged ion with atomic number of 15

D. 1s22s

22p

63s

23p

63d

54s

1an atom of chromium in the ground state

ionisation energy

(kJ mol–1

)

atomic number

2000

1600

1200

800

400

0

Q

R

S

T

U

V

W



SECTION B – SHORT-ANSWER QUESTIONS

Question 1 (14 marks)

A range of processes are used to extract various metals from their ores.

a. Electricity is used to melt and electrolyse magnesium chloride ore to allow magnesium metal to be formed.

i. Describe the structure and bonding in magnesium chloride. 3 marks

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ii. What happens to the magnesium particles in molten magnesium chloride in order to produce magnesium metal? 1 mark

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iii. Solid calcium chloride is usually mixed with magnesium chloride to lower its melting temperature.

Why is this an advantage in the industrial production of magnesium metal? 1 mark

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b. Copper is produced by roasting its ore in air to produce the overall chemical reaction shown below.

Cu2S(l) + O2(g) → 2Cu(l) + SO2(g)

Calculate the mass of copper (in g) present in 1.00 tonne of Cu2S. (1 tonne = 106 g) 2 marks

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Instructions for Section B

Answer all questions in the spaces provided. Write using blue or black pen.

Give simplified answers to all numerical questions, with an appropriate number of significant figures; unsimplified answers will not be given full marks.

Show all working in your answers to numerical questions; no marks will be given for an incorrect answer unless it is accompanied by details of the working.

Ensure chemical equations are balanced and that the formulas for individual substances include an indication of state; for example, H2(g), NaCl(s).

Unless otherwise indicated, the diagram in this booklet are not drawn to scale.



c. Iron is produced by heating iron oxide and carbon monoxide at very high temperatures to produce a chemical reaction shown by the following equation.

Fe2O3(s) + 3CO(g) → 2Fe(l) + 3CO2(g)

i. Three of the four chemical substances in this reaction will not conduct electricity.

Select one of these three substances and explain why it is a non-conductor of electricity. (Indicate the chosen substance by circling its formula in the equation above and providing your explanation in the space below.) 2 marks

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ii. Draw the structural formula of a carbon dioxide molecule, showing all bonding and non-bonding pairs. 1 mark

iii. Is the carbon dioxide molecule polar or non-polar? Explain your choice. 2 marks

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d. Mining for metal ores can cause land degradation.

Identify one environmental issue (other than land degradation) associated with the production of one of the metals listed below from its ores and explain how the environment is affected by this issue. Circle the metal you have chosen. 2 marks

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magnesium copper iron




Recently, element 117 was officially named tennessine and given the symbol Ts. The isotopic symbol of the

standard used for determination of the relative atomic masses of the elements is

a. i. Give the isotopic symbol for an atom of tennessine containing 180 neutrons. 1 mark

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ii. Give one reason why carbon-12 was selected as the standard used for determination of the relative atomic masses. 1 mark

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b. Using the atomic number of tennessine, the element can be placed in the periodic table.

i. By considering its position in the periodic table, write the outer shell subshell configuration of an atom of tennessine. 1 mark

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ii. Would you expect the electronegativity of tennessine to be greater than or less than other elements in the same group in the periodic table? 1 mark

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iii. Explain why the atomic radius of an atom of tennessine would be expected to be less than that of an atom of element number 116. 2 marks

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c. Tennessine is a man-made element which was produced by firing high-energy 48

Ca

nuclei at atoms of 249Bk. The new element was formed when a 48Ca nucleus joined

with the 249Bk nucleus.

i. Suggest a reason why it was necessary to use high-energy nuclei. 2 marks

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C.12

6



ii. 48Ca is one of six naturally occurring isotopes of calcium. The other isotopes of calcium have the following mass numbers: 40, 42, 43, 44 and 46.

By referring to the relative atomic mass of calcium, identify which isotope is most abundant. Explain your choice. 2 marks

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The main steps in the production of some polymer products are shown in the flow chart below.

a. The starting material is a complex mixture of hydrocarbons found deep below ground level.

Give the common name of this complex mixture. 1 mark

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b. Give the formula of a compound from the same homologous series as butane which contains seven carbon atoms per molecule. 1 mark

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c. Polypropene is a linear polymer. The structure of one of its forms (type 1) is shown below.

i. Describe the intermolecular and intramolecular bonding in a sample of solid polypropene. 2 marks

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complex mixture

recycle

step 1butane propene polypropene consumer products

step 2 step 3 step 4

C

H

CH3

C C C C C C C C C C C

CH3

CH3

CH3

CH3

CH3H H H H H H H

H H HH H H H H H

H



ii. Another form of polypropene (type 2) has all of the methyl groups (–CH3) on one side of the polymer chain, as shown below.

Which form of polypropene, type 1 or type 2, is likely to melt at the higher temperature? Explain your choice. 2 marks

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iii. Describe a simple laboratory experiment to show that polypropene is thermoplastic.Include the expected results of the experiment. 2 marks

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d. i. One of the advantages of polypropene is that it is easily recycled.

Give one reason why this recycling is beneficial. 1 mark

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ii. Give one disadvantage of using a polymer material such as polypropene. 1 mark

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e. Propene can be used to generate the compounds propanol and propanoic acid.

i. Write the semi-structural formulas of both isomers of propanol. 2 marks

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ii. Draw the structural formula of propanoic acid and show all bonds. 1 mark

C

H

CH3

C C C C C C C C C C C

CH3 CH3 CH3 CH3 CH3

H H H H H H H

H HH H H H

HH HH




The building industry uses the properties of a range of materials in a diverse selection of applications.

a. Silicon carbide (SiC) has a similar structure to that of diamond.

i. Draw a small section of the solid to show the structure of silicon carbide. 2 marks

ii. Grains of silicon carbide are glued onto reinforced paper backing to produce a type of sandpaper which is used to remove rust from metal. Alternatively, the grains are compressed with a bonding agent into a grinding wheel to grind stone or metal.

Explain how the structure and bonding in silicon carbide makes it suitable for these purposes. 2 marks

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b. Lubricants are used to allow one surface to slide over another surface with minimal friction.

i. A particular oil has the formula C20H42.

Using structure and bonding, explain why this compound is suitable as a lubricant. 2 marks

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ii. This oil is not used in locks as dirt and dust stick to it and clog up the lock. Instead, the dry lubricant graphite is used.

Using structure and bonding, explain why graphite is suitable as a lubricant. 2 marks

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iii. For high-temperature applications, suggest a reason why hydrocarbons are not used as lubricants. 1 mark

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c. Metals are often modified before use in the building industry. A range of these modifications are shown in the table below.

Select and circle one number (1–6) in the table above. For your selected modification, identify the property of the modified metal which was achieved by the modification, and explain, in terms of structure and bonding, how the modification resulted in this property of the metal. 2 marks

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d. Pipes carrying water in very cold weather conditions must be heavily insulated to prevent the water from freezing and causing the pipes to burst.

Explain what happens to water molecules during the freezing process that may cause the pipes to burst. 2 marks

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END OF QUESTION AND ANSWER BOOKLET

1. Taps are made of brass – an alloy of copper and zinc.

2. The cutting edge of a chisel is specially heat treated.

3. Iron roofing sheets are coated with zinc.

4. Steel support beams are made from iron with some carbon.

5. A layer of cadmium is plated onto steel screws.

6. Copper piping is heat treated before its use in plumbing.

Documents

Trial Examination 2017 VCE Chemistry Unit 1 · 2019. 5. 16. · VCE Chemistry Unit 1 Written Examination Question and Answer Booklet Reading time: 15 minutes Writing time: 1 hour