year 11-12 transition task - chemistry · web viewthe chemist did the experiment but only made...

Eggbuckland Community College

Year 11 – 12 Chemistry Transition Questions

Q1.This question is about atoms and isotopes.

(a) Atoms contain protons, neutrons and electrons.

A lithium atom has the symbol

Explain, in terms of sub-atomic particles, why the mass number of this lithium atom is 7. (3)

(b) Amounts of substances can be described in different ways.

Complete the sentences.

One mole of a substance is the relative formula mass in

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

The relative atomic mass of an element compares the mass of an atom of an element with the mass of an atom of

........................................................................................................................(2)

(c) Two isotopes of oxygen are and

Describe the similarities and differences between the isotopes and

You should refer to the numbers of sub-atomic particles in each isotope. (3)

(Total 8 marks)

Q2. Graphite and diamond are different forms of the element carbon.Graphite and diamond have different properties.

The structures of graphite and diamond are shown below.

Graphite Diamond

(a) Graphite is softer than diamond.

Explain why. (4)

(b) Graphite conducts electricity, but diamond does not.


Explain why. (3)

(Total 7 marks)

Q3. This question is about calcium hydroxide.

Ancient artworks and monuments can be protected from acid rain if the surface is sprayed with calcium hydroxide nanoparticles.

By Svilen Enev (Own work) [GFDL or CC-BY-SA-3.0], via Wikimedia Commons

(a) Calcium hydroxide has the formula Ca(OH)2

Why are there two hydroxide ions for each calcium ion in the formula? (1)

(b) The calcium hydroxide is used in the form of nanoparticles.

What are nanoparticles? (1)

(c) A student added water to calcium oxide to make calcium hydroxide.

The equation for the reaction is shown below.

CaO + H2O → Ca(OH)2

Calculate the maximum mass of calcium hydroxide which could be made from 2.00 g of calcium oxide.

Relative atomic masses (Ar): H = 1; O = 16; Ca = 40.

Maximum mass of calcium hydroxide = ............................... g(3)

(Total 5 marks)

Q4. Aspirin tablets have important medical uses.


(a) Aspirin is made when salicylic acid reacts with ethanoic anhydride.

The equation for this reaction is:

C7H6O3 + C4H6O3 → C9H8O4 + CH3COOH salicylic acid aspirin

Calculate the maximum mass of aspirin that could be made from 100 g of salicylic acid.

Show clearly how you work out your answer.

The relative formula mass (Mr) of salicylic acid (C7H6O3) is 138.The relative formula mass (Mr) of aspirin (C9H8O4) is 180.

Maximum mass of aspirin = .................................... g(2)

(b) (i)In an experiment a chemist calculated that the maximum yield of aspirin is 400 g.

The chemist did the experiment but only made 250 g of aspirin.

Calculate the percentage yield of aspirin for this experiment.

Show clearly how you work out your answer.

Percentage yield of aspirin = ........................... %(2)

(ii) Suggest one possible reason why the chemist did not have a percentage yield of 100%.

(1)

(c) The use of a catalyst might reduce costs in the industrial production of aspirin.

Suggest how. (1)

(Total 6 marks)

Q5. The picture shows a painting which was painted in a cave in France about 17 000 years ago.


By Carla Hufstedler [CC-BY-SA-2.0], via Wikimedia Commons

One of the pigments in this painting contains:

70 % of iron (Fe) and 30 % of oxygen (O)

Calculate the simplest (empirical) formula of this substance.

Relative atomic masses: O = 16; Fe = 56. (4)

(Total 4 marks)

Q6.Glass is made from silicon dioxide.

© Velirina/iStock/Thinkstock

(a) Silicon dioxide has a very high melting point.

Other substances are added to silicon dioxide to make glass. Glass melts at a lower temperature than silicon dioxide.

Suggest why. (1)

(b) Sodium oxide is one of the substances added to silicon dioxide to make glass.


(i) Sodium oxide contains Na+ ions and O2– ions.

Give the formula of sodium oxide. (1)

(ii) Sodium oxide is made by heating sodium metal in oxygen gas.

Complete the diagram to show the outer electrons in an oxygen molecule (O2).

(2)

(c) Glass can be coloured using tiny particles of gold. Gold is a metal.

Describe the structure of a metal. (3)

(Total 7 marks)

Q7.Spacecraft have been to the planets Venus and Mars. The spacecraft have sent back information about the atmosphere of each planet.

© Tristan3D/Shutterstock

(a) The main gas in the atmosphere of Mars is carbon dioxide.

Explain why, in terms of structure, carbon dioxide is a gas, even at low temperatures.

(3)

(b) Gas chromatography linked to a mass spectrometer (GC-MS) is used to identify substances found on Mars.

(i) What is the purpose of gas chromatography? (1)


(ii) What information do the molecular ion peaks from the mass spectrometer give about the substances?

(1)

(c) The atmosphere on Venus contains droplets of sulfuric acid solution.

(i) Suggest a pH value for sulfuric acid solution.

pH = ...........................(1)

(ii) Name the ion which makes sulfuric acid solution acidic. (1)

(d) The atmosphere of Venus contains the isotopes and

Describe the similarities and the differences in the isotopes and

You should refer to the sub-atomic particles in each isotope. (3)

(Total 10 marks)

Q8.This question is about sodium chloride and iodine.

(a) Describe the structure and bonding in sodium chloride.(4)

(d) The bonding in iodine is similar to the bonding in chlorine.

(i) Complete the diagram below to show the bonding in iodine.

Show the outer electrons only.

(2)

(ii) Explain why iodine has a low melting point. (3)

(iii) Explain, in terms of particles, why liquid iodine does not conduct electricity. (2)

(Total 11 marks)

Q9.Aluminium has many uses.

(a) An aluminium atom has 13 electrons.

(i) Draw the electronic structure of an aluminium atom.


(1)

(ii) Name the two sub-atomic particles in the nucleus of an aluminium atom.

................................................... and ................................................... (1)

(iii) Why is there no overall electrical charge on an aluminium atom? (1)

(b) Rail tracks are made from steel. Molten iron is used to weld rail tracks.

The reaction of aluminium with iron oxide is used to produce molten iron.

(i) Balance the chemical equation for the reaction.

(1)

(ii) Why does aluminium react with iron oxide? (1)

(Total 5 marks)

Q10. Crude oil is a mixture of hydrocarbons. Most of these hydrocarbons are alkanes.

(a) The general formula of an alkane is CnH2n+2

Complete the structural formula for the alkane that has six carbon atoms in its molecules.

(1)

(b) The boiling points of alkanes are linked to the number of carbon atoms in their molecules.


(i) Describe the link between the number of carbon atoms in an alkane molecule and its boiling point. (1)

(ii) Suggest two reasons why all of the alkanes in the bar chart are better fuels than the alkane with the formula C30H62

(2)

(c) During the last 200 million years the carbon cycle has maintained the percentage of carbon dioxide in the atmosphere at about 0.03 %.Over the last 100 years the percentage of carbon dioxide in the atmosphere has increased to about 0.04 %.Most of this increase is caused by burning fossil fuels to heat buildings, to generate electricity and to power our transport.Fossil fuels contain carbon that has been locked up for millions of years.

(i) Burning fossil fuels, such as petrol, releases this locked up carbon. Balance the chemical equation for the combustion of one of the alkanes in petrol.

2 C8H18 + 25 O2 ........ CO2 + ........ H2O

(1)


(ii) Where did the carbon that is locked up in fossil fuels come from? (1)

(iii) The burning of fossil fuels has caused the percentage of carbon dioxide in the atmosphere to increase to above 0.03 %.Explain why.

(2)(Total 8 marks)

Q11. (a) Balance these chemical equations.

(i) H2 + O2 → H2O(1)

(ii) Al + O2 → Al2O3

(1)

(b) Briefly explain why an unbalanced chemical equation cannot fully describe a reaction. (2)

(Total 4 marks)

Q12. This information was taken from a label on a packet of crisps.

Main ingredients:

Potatoes, vegetable oil, Worcester sauce flavour,

colourings, flavourings, salt.

Nutritional information (per 100 g):

Energy 2040 kJ

Protein 6.5 g

Carbohydrate 55 g

of which sugars 3 g

Fat 27 g

of which saturates 9 g

unsaturates 18 g

Fibre 4.5 g

Sodium 1.2 g

Saturated fats are linked to heart problems. In order to claim that their crisps are healthy, the manufacturer keeps the proportion of saturated fats low.

(i) What type of fat contains double carbon carbon bonds? (1)


(ii) The colour of bromine water is orange.

What is seen when bromine water is shaken with:

an unsaturated fat .......................................................................................................

a saturated fat? ..........................................................................................................(2)

(iii) Unsaturated vegetable oils can be hardened to make them useful as spreads. Describe how unsaturated vegetable oils are hardened.

(2)(Total 5 marks)

Q13. Crude oil is a complex mixture of hydrocarbons, mainly alkanes. The number of carbon atoms in the molecules ranges from 1 to over 100.

(a) How does the boiling point change as the number of carbon atoms in the molecules increases?

(1)

(b) Name the method used to separate petroleum into fractions.(1)

(c) The simplest hydrocarbon is methane, CH4. Its structure can be represented:

Draw the structure of ethane, C2H6.(1)

(Total 3 marks)

Q14. The molecular formulae of two hydrocarbons M and N are given.

M = C4H10

N = C4H8

(a) M reacts with chlorine to form C4H9Cl.

(i) Write a balanced chemical equation for the reaction of chlorine with M. (2)

(ii) Name this type of reaction.(1)

(b) A displayed structural formula for N is:


Draw a displayed structural formula of a compound which is an isomer of N.

(1)

(c) Complete the boxes to show the displayed structural formula for each of the products formed.

(2)(Total 6 marks)

Q15. Propane and ethene are both important hydrocarbons.

(a) Complete the table by adding the formula of the ethene molecule and the structure of the propane molecule.

(2)

(c) Ethene can be changed into a plastic. The equation shown below represents the reaction in which ethene is polymerised.


(i) What is the name of the plastic formed in this reaction? (1)

(ii) What type of polymerisation reaction is shown in the equation? (1)

(Total 4 marks)

Modem window frames are often made from uPVC which contains the plastic poly(chloroethene).

Replace your old wooden windowswith our super high quality uPVC

windows!

(a) State why plastic window frames need no painting or maintenance. (1)

(b) Poly(chloroethene) is a polymer formed by the addition polymerisation of chloroethene.

(i) Chloroethene is an unsaturated molecule. Why is this molecule said to be unsaturated? (1)

(ii) Complete the diagram to represent how poly(chloroethene) is formed from chloroethene.

(3)

(iii) Explain what is meant by the term polymerisation. (2)

(Total 7 marks)


M1.(a) because this lithium atom has

3 protons1

and 4 neutrons1

mass number is total of neutrons and protonsaccept protons and neutrons have a mass of 1accept number of neutrons = 7 - 3(protons)ignore mass of electron is negligible

1

(b) gramsaccept g

1

12Callow carbon-12 or C-12ignore hydrogen or H

1

(c) any three from:max 2 if no numbers givennumbers if given must be correct

• both have 8 protonsaccept same number of protons

• 18O has 10 neutrons• 16O has 8 neutrons

accept different number of neutrons or 18O has two more neutrons for 1 mark

• both have 8 electrons.accept same number of electrons

3[8]

M2. (a) Graphite:

because the layers (of carbon atoms) in graphite can move / slideit = graphite

Eggbuckland Community College1

this is because there are only weak intermolecular forces or weak forces between layers

accept Van der Waals’ forces allow no covalent bonds between layers

1

Diamond:

however, in diamond, each carbon atom is (strongly / covalently) bonded to 4 othersallow diamond has three dimensional / tetrahedral structure

1

so no carbon / atoms able to move / slideallow so no layers to slide or so diamond is rigid

1

(b) because graphite has delocalised electrons / sea of electronsallow free / mobile / roaming electrons

1

which can carry charge / current or move through the structure1

however, diamond has no delocalised electronsaccept however, diamond has all (outer) electrons used in bonding

1

[7]

M3. (a) because calcium is +2 and hydroxide is –1


accept to balance the charges

orto make the compound neutral (in terms of charges)

allow calcium needs to lose 2 electrons and hydroxide needs to gain one electron

1

(b) particles of size 1-100 nm allow clear comparison to ‘normal’ size particles

or particles with a few hundred atoms / ions

or particles with a high surface area (to volume ratio)

or as different properties to ‘normal’ size particles of the same substance1

(c) Mr CaO = 56and

Mr Ca(OH)2= 741

2/56 (x74) or 0.036 (x74)or

allow ecf from step 1

74/56 (x2) or 1.3(214…) (x2)1

2.6(428…) in range 2.6 to 2.96correct answer with or without working gains 3 marksallow ecf carried through from step 1ignore final rounding to 3

1

[5]


M4. (a) 130.4accept 130 to 130.43478………correct answer gains two marks with or without workingan answer of 131 would gain one mark.if answer is not correct then:moles of salicylic acid = 0.7 .......... (1 mark)ormass of aspirin = moles of salicylic acid x 180 (1 mark)or100 x (180/138) (1 mark)

2

(b) (i) 62.5%accept 63%correct answer gains two marks with or without workingif answer is not correct then:250/400 x 100 (1 mark)

2

(ii) any one from:

• reversible reactionaccept not all of the reactant converted to product

• some of product lost1

(c) use lower temperaturesorless energy needed

allow product made faster or more product made in a given time

1[6]

M5. 70/56 30/16division by atomic mass

1


= 1.25 = 1.875proportion

1

2 3ratio (accept 1:1.5 / 4:6 / etc)allow e.c.f from proportion if sensible attempt at step 1

1

Fe2O3

formula allow e.c.f from ratio if sensible attempt at step 1allow correct formula with no working = 1 mark

1[4]

M6.(a) weaker bondsallow (other substances) react with the silicon dioxide

or

fewer bondsignore weaker / fewer forces

or

disruption to latticedo not accept reference to intermolecular forces / bonds

1

(b) (i) Na2Odo not accept brackets or charges in the formula

1

(ii)

electrons can be shown as dots, crosses, e or any combination

2 bonding pairs


accept 4 electrons within the overlap1

2 lone pairs on each oxygenaccept 4 non-bonding electrons on each oxygen

1

(c) lattice / regular pattern / layers / giant structure / close-packed arrangement1

(of) positive ions or (of) atoms1

(with) delocalised / free electronsreference to incorrect particles or incorrect bonding or incorrect structure = max 2

1[7]

M7.(a) has simple / small moleculesaccept molecular covalent

1

the intermolecular forces / intermolecular bonds (are weak)do not accept weak covalent bonds or reference to incorrect bonding

1

only need a small amount of energy to be overcomeaccept only need a small amount of energy to separate the molecules if no other mark awarded, allow it has a low boiling point for 1 mark

1

(b) (i) to separate1

(ii) (relative) molecular massallow Mr / (R)MM / relative mass / mass of molecule / (R)FM

1


(c) (i) any pH value from 0 to 6.91

(ii) hydrogenallow H+

ignore H / H2 / H–

1

(d) any three from:

• same number of protonsaccept same atomic numbernumbers if given must be correct

• 2H has one neutron

• 1H has no neutronsaccept different mass number or different number of neutrons for 1 markignore relative atomic mass

• same number of electronsnumbers if given must be correct

3[10]

M8.(a) lattice / giant structuremax 3 if incorrect structure or bonding or particles

1

ionic or (contains) ions1

Na+ and Cl-

accept in words or dot and cross diagram: must include type and magnitude of charge for each ion

1

electrostatic attractionallow attraction between opposite charges

1


(b) hydrogenallow H2

1

sodium hydroxideallow NaOH

1

(c) any one from, eg:• people should have the right to choose• insufficient evidence of effect on individuals• individuals may need different amounts.

allow too much could be harmfulignore religious reasonsignore costignore reference to allergies

1

(d) (i) one bonding pair of electronsaccept dot, cross or e or − or any combination, eg

1

6 unbonded electrons on each atom1

(ii) simple moleculesmax 2 if incorrect structure or bonding or particlesaccept small moleculesaccept simple / small molecular structure

1

with intermolecular forcesaccept forces between moleculesmust be no contradictory particles

1

which are weak or which require little energy to overcome − must be linked to second marking pointreference to weak covalent bonds negates second and third marking points

1

(iii) iodine has no delocalised / free / mobile electrons or ions1

so cannot carry chargeif no mark awarded iodine molecules have no charge gains 1


mark1

[14]

M9.(a) (i) 2.8.3any sensible symbol can be used to represent an electron

1

(ii) proton(s) and neutron(s)both needed for the mark

1

(iii) number of protons is equal to number of electronsallow positive and negative charges cancel out allow same amount of protons and electrons

1

(b) (i) 2 Al + Fe2 O3 → 2 Fe + Al2 O3

equation must be balanced1

(ii) aluminium is more reactive (than iron)it = aluminiumaccept converseaccept aluminium displaces ironaccept aluminium is higher in the reactivity series (than iron)

1[5]

M10. (a) complete diagram with 2 carbon atoms and 5 hydrogen atoms each C–Cand each C–H linked by a single line (bond)

1

(b) (i) the greater the number of (carbon) atoms (in an alkane molecule) the


greater its boiling point or vice versaallow as the (carbon) chain gets longer the boiling point increasesignore melting pointsdo not accept reference to greater number of molecules

1

(ii) they = hydrocarbons from the graphit = C30H62

any two from:

• low boiling point / volatileaccept they are gases or liquids

• low viscosity

• high flammabilityaccept easier to burn / ignite

• small molecules accept short chainsignore number of carbon atoms

• burn completelyignore speed of burning

2

(c) (i) 16 (CO2) + 18 (H2O)1

(ii) (carbon dioxide in the Earth’s early) atmosphere accept from volcanoes (millions of years ago)or from dead plants / animalsallow dead sea creatures ignore shells

1

(iii) increase in burning / use of fossil fuels1

locked up carbon (carbon dioxide) is released


allow carbon / carbon dioxide from millions of years ago is releasedaccept extra carbon dioxide is not ‘absorbed’ (by the carbon cycle)

1[8]

M11. (a) (i) H 2 + O2 → H 2O *both circled correctfor 1 mark

1

(ii) A1 + O 2 → A1 2O3 all circled correctfor 1 mark

1

(b) idea that: must end up with the same number of atoms as at the start

any 2 each

otherwise matter is shown to be lost/gainedfor 1 mark

won’t show correct amount of each element/compound2

[4]

M12. (i) (poly)unsaturatedaccept monounsaturated

1

(ii) (turns) colourless or colour disappears / decolourisesdo not accept clear

1

stays the same colour / orange / no changeallow yellow-orange / orange-brown / red-orange

1

(iii) (react) with hydrogen / H2 / hydrogenation1


any one from:

• heated / 60 °C

• catalyst / nickel1

[5]

M13. (a) the more C atoms the higher the b.pt./temperatureAllow just higher. Not answer based on melting point

for 1 mark1

(b) (fractional) distillation/fractionationfor 1 mark

1

(c)

must include H atoms and lines not CH3 – CH3

for 1 mark1

[3]

M14. (a) (i) C4H10 + Cl2 → C4H9Cl + HClreactants

1

productsignore incorrect balancing


no state symbols required1

(ii) substitution / chlorination1

(b)

H atoms not necessary1

(c)

2

[6]

M15. (a) C2H4

1

H H HH C C C H H H H

Accept even if in wrong columns1

(c) (i) polythene or poly(ethene)1


(ii) addition1

[4]

M16. (a) not broken down by microorganisms or not bio-degradableaccept alternative answers such as:do not rot / corrode / fade / react with atmosphere etcany answers which imply the inertness or non-biodegradability of this plasticaccept they don’t react, they are ‘inert’ignore rustingdo not accept weathering

1

(b) (i) (have a) double bond or do not have maximum number of(hydrogen) atoms attached

accept can add / react with hydrogenaccept can take part addition reactionsdo not accept it is a double bonddo not accept additional reactionsdo not accept has ‘spare’ / ‘free’ bonddo not accept alkene alone

1

(ii) single bond between carbon atoms1

all atoms correct + 2 ‘linking’ bonds(linking bonds need not go through bracket)

1

n moved to bottom right of bracket i.e. is below way on the rightfirst 2 marks are possible for chain structuresaccept [– CHCl–CH2–] n

1


(iii) many molecules or many monomers1

joined / bonded / linked or form longchain molecules / large molecules or toform a long chain polymer

accept many alkenes or many (ethene) moleculesdo not accept many ethene alone etc.to form a long polymer is not enough for 2nd mark

1

(iv) no other substances formed(A + B → C)

allow because double bond breaks so other atoms can addallow one product onlydo not accept saturation occurs

1[8]

year 11-12 transition task - chemistry · web viewthe chemist did the experiment but only made...

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