name: · revision pack (please keep this pack with you) ... heat using bunsen burner so most but...
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Name: __________________
C2 Revision Pack (Please keep this pack with you) Follow all the steps below...
1) Practice all the maths and ‘working scientifically’ questions – PRACTICE ALL THESE QUESTIONS!
Maths and Science Skills Questions
Foundation Questions - http://NUCOWUB.exampro.net Standard Questions – http://DUAUIEJ.exampro.net Higher Questions - http://AOKIOED.exampro.net
2) Practice Quiz – short answer questions (included in this pack)
3) Practice QWC questions – long answer questions (included in this pack)
4) Practice all the Popplet questions
C2 1 Structure and Bonding
Foundation Questions - http://D416847D.exampro.net Standard Questions - http://1C3278F2.exampro.net Higher Questions – http://CE300923.exampro.net
C2 2 Structure, Properties & Uses of Substances
Foundation Questions - http://A754B9FD.exampro.net Standard Questions - http://EBE97493.exampro.net Higher Questions – http://63679610.exampro.net
C2 3 Quantitative Chemistry & Analysis
Foundation Questions - http://3E919235.exampro.net Standard Questions - http://5664E254.exampro.net Higher Questions – http://AF67F3CF.exampro.net
C2 4 Rates of Reaction
Foundation Questions - http://5E3BB7FD.exampro.net Standard Questions - http://A20362E9.exampro.net Higher Questions – http://2D12B53D.exampro.net
C2 5 Exothermic and Endothermic Reactions
Foundation Questions - http://6B44E863.exampro.net Standard Questions - http://F51B185E.exampro.net Higher Questions – http://22CE4FB4.exampro.net
C2 6 Acids, Bases and Salts
Foundation Questions - http://5770CD46.exampro.net Standard Questions - http://A9A4619E.exampro.net Higher Questions – http://B3C936BF.exampro.net
C2 7 Electrolysis
Foundation Questions - http://2976C355.exampro.net Standard Questions - http://648C3C7E.exampro.net Higher Questions – http://283F8A63.exampro.net
Our Predictions: Experiments! E.g. Rates of reaction experiments, making salts, electrolysis etc. If this comes up as a 6 mark question – DON’T FORGET
TO WRITE A RISK ASSESSMENT. Graphs – Drawing and interpreting - Practice the maths and ‘working scientifically’ questions above!
C2.3 Quantitative Chemistry & Analysis – Revise this whole topic a lot, e.g. empirical formula, mass calculations, Ions, isotopes Making salts Crystalisation Metallic bonding and linking the structure to the properties of metals Electrolysis and half equations Neutralisation, e.g. equation, ions Ionic vs covalent structures, e.g. structure, linking to properties, drawing bonding Diamond vs graphite, e.g. structure, linking to properties Alloys vs pure metals Gas chromatography and mass spectrometry Thermosetting vs thermosoftening polymers Collision theory and rates of reaction
Nanoparticles
PRACTICE QUIZ
1. Which ion makes ammonia solution alkaline? (1 mark)
OH ion/ hydroxide ion
2. Name the type of reaction between aqueous ammonia solution and an acid (1 mark)
Neutralisation/ exothermic
3. Name the acid needed to produce ammonium nitrate (1 mark)
Nitric acid
4. Write the formula of ammonium sulphate (1 mark)
(NH4)2SO4 (Two ammonium ions are needed to neutralise the 2- charge on the sulphate ion.)
5. Suggest a PH value for sulphuric acid solution (1 mark)
0-6.9 (7 is neutral, 8-14 is alkali)
6. Name the ion which makes sulphuric acid solution acidic (1 mark)
H+ ion / hydrogen ion
7. Why do some farmers put ammonium nitrate on their farmland? (1 mark)
To fertilise the soil and to help plants grow
8. Why should the start line on chromatography paper be drawn in pencil not ink? (1 mark)
ink dissolves in the solvent, graphite does not
9. Give 2 advantages of gas chromatography compared with paper chromatography. (2 marks)
rapid / quick
accurate
sensitive / detects very small quantities
10. What does gas chromatography do to the mixture of solvents? (1 mark)
separates
11. What information does mass spectrometry give? (1 mark)
identifies solvents / compounds / substances
12. What is an exothermic reaction? (1 mark)
gives out energy / heat
13. Why does a solution of sodium thiosulfate and dilute HCL go cloudy? ( 2Mrks)
Because sulphur forms (1) which is insoluble (1)
14. Increase in temp of hydrogen peroxide increases the rate of the reaction, why? (3 marks)
The particles have more energy so move faster (1) so particles collide more often (1) and more of
collisions are successful (1)
15. How does a gold atom (Au) become a gold ion (Au3+)? (2 marks)
It loses / transfers (1) 3 electrons (1)
16. Why is the positive electrode in the cell used up during electrolysis? (2 marks)
because the electrode reacts with oxygen (1) to form carbon dioxide (1)
17. Why do hydrogen ions move to the negative electrode? (1 mark)
because they are positively charged
18. How does a hydrogen ion change into a hydrogen atom?
gains one electron
19. How do you remove unreacted copper oxide in the preparation of copper sulphate crystals?
Filtration
20. Why does the catalyst work for a long time before it needs replacing?
It is not used up
21. Why wouldn’t thermosoftening polymers be suitable for packaging very hot food? (2 marks)
They would melt / have a low melting point (1)
There are weak intermolecular forcer / no cross links (1)
22. How can gas chromatography separate substances in a mixture of compounds? (3 marks)
Substances carried by gas (1)
Through column packed with solids (1)
At different speeds (1)
23. What information does the molecular ion peak give about the molecule? (1 mark)
(relative) molecular mass/ Mr
24. What happens when sodium atoms react iodine atoms to produce sodium iodide? (3 marks)
sodium atom loses electron and iodine atom gains (1) one electron (1) electrostatic attraction (1)
25. Why does sodium iodide solution conduct electricity? (1 mark)
Ions can move in the solution
26. What formed at negative electrode when sodium iodide solution is electrolysed? (2 marks)
Hydrogen is formed (1) because sodium is more reactive (1)
27. Explain why silicon dioxide is a suitable material for lining furnaces. (4 marks)
high melting point (1)
because a lot of energy needed to break bonds (1)
because it is covalent or has strong bonds (1)
and because it is a giant structure or a macromolecule or a lattice (1)
28. Explain why copper is a good conductor of electricity. (2 marks)
copper has delocalized electrons (1) which can move through the metal / structure (1)
29. why doesn’t electrolysis of solid potassium salts to produce potassium work? (2 marks)
Current couldn’t flow (1) because the ions couldn’t move (1)
30. Describe how potassium atoms are formed from potassium ions. (2 marks)
Gain (1) 1 electron (1)
31. Carbon dioxide has a very low boiling point, explain why (3 marks)
Carbon dioxide is simple molecular (1)
There are intermolecular forces between the molecules (1)
Small amount of energy is needed to separate molecules / intermolecular forces are weak (1)
32. Suggest three reasons why gold is still used in industrial processes. (3 marks)
Gold is the only catalyst for some reactions.
Catalysts are not used up
Improve speed of reaction
Only small quantities of catalyst needed
33. Why does an electrolyte contain cryolite? (2 marks)
Because it lowers the melting point of the aluminium oxide (1)
So less energy is needed to melt is (1)
34. Why is the positive electrode in the cell used up during electrolysis? (2 marks)
because the electrode reacts with oxygen (1) to form carbon dioxide (1)
35. Why are there two hydroxide ions for each calcium ion in the formula Ca(OH)2? (1 mark)
Because calcium is +2 and hydroxide is -1 / to make the compound neutral charge
36. What are nanoparticles? (1 marks)
particles of size 1-100 nm
37. Why is graphite softer than diamond? (4 marks)
Because the layers (of carbon atoms) in graphite can move / slide (1) this is because there are only weak
intermolecular forces or weak forces between layers (1) however, in diamond, each carbon atom is
(strongly / covalently) bonded to 4 others (1) so no carbon atoms able to move (1)
38. Explain why graphite conducts electricity but diamond does not (3 marks)
because graphite has delocalized, sea of electrons (1) which can carry charge / current (1) however,
diamond has no delocalised electrons (1)
39. Explain why alloys are harder than pure metals. (3 marks)
because atoms in alloy are different sizes
so layers distorted
and layers don’t slide or slide less easily
40. Describe the structure and bonding in diamond. (4 marks)
giant structure / lattice / macromolecule (1)
strong bonds between carbon atoms (1)
covalent bonds (1)
each carbon / atom forms 4 bonds (1)
QWC 6 MARK QUESTIONS
KEY POINTS TO INCLUDE IN YOUR ANSWER:
Aluminium oxide is melted / made liquid
Aluminium ions are attracted to the negative electrode
At the negative electrode aluminium is formed
At the negative electrode aluminium ions gain electrons
Oxide ions are attracted to the positive electrode
Oxygen is formed at the positive electrode or oxide
Oxide ions lose electrons
The oxygen reacts with carbon to make carbon dioxide at positive electrode
KEY POINTS TO INCLUDE IN YOUR ANSWER:
Each carbon is covalently bonded to three other carbon atoms
There are only weak forces of attraction between layers
Layers can slide over each other
One electron on each carbon is not used for bonding
There are free electrons / delocalised electrons that carry the electric charge
KEY POINTS TO INCLUDE IN YOUR ANSWER:
Chemistry points made in the response:
Sulfuric acid is heated in a beaker and copper oxide is added whilst stirring
Keep on adding the copper oxide until the copper oxide is in excess
Filter the mixture / Pour the mixture through a funnel and filter paper
Filtering will remove the excess copper oxide
Some of the solution is then evaporated / heated in an evaporating basin
The solution is allowed to crystallise / cool down
Risk assessment points made in the response:
Wear safety goggles – to protect eyes because sulfuric acid is corrosive / an irritant
Take care when heating – to protect against burns
Wash hands after the preparation – copper sulfate is harmful
Take care when handling glass apparatus – to protect against cuts
KEY POINTS TO INCLUDE IN YOUR ANSWER:
Carbon dioxide is a simple covalent molecule
The intermolecular forces between carbon dioxide molecules are weak
Only a small amount of energy is needed to overcome the weak intermolecular forces
REMEMBER IT IS NOT THE COVALENT BONDS THAT ARE WEAK!
KEY POINTS TO INCLUDE IN YOUR ANSWER:
One reagent in beaker (or similar)
Add (any named) indicator, e.g. universal indicator
Add other reagent
Swirl or mix
Add dropwise near end point
Stop addition at change of indicator colour, e.g. when universal indicator turns green = neutral
Note volume of reagent added
Repeat without indicator, adding same volume of reagent
Pour solution into basin / dish
Heat using Bunsen burner so most but not all of the water evaporates
Leave remaining solution to crystallise
KEY POINTS TO INCLUDE IN YOUR ANSWER:
Thermosoftening polymers are made up of long chains
They have no cross links
They have weak intermolecular forces between the chains
Only a small amount of heat energy is needed to break these weak intermolecular forces
KEY POINTS TO INCLUDE IN YOUR ANSWER:
In alloys...
Atoms are different sizes
This distorts the layers
Layers cannot slide over each other
This makes them hard
In pure metals...
Atoms are all the same size
This means they form neat layers
Layers can easily slide over each other
This makes them soft
KEY POINTS TO INCLUDE IN YOUR ANSWER:
Diamond has a giant structure / lattice structure / is a macromolecule
Diamond has strong covalent bonds between atoms
Each carbon atom in diamond forms 4 covalent bonds
KEY POINTS TO INCLUDE IN YOUR ANSWER:
Add magnesium to acid
Dependant variable (measure) could be: (PICK ONLY ONE)
o Time for reaction
o Counting bubbles released
o Measuring the volume of gas released
Independent variable (change) could be: (PICK ONLY ONE)
o Concentration of acid
o Volume of acid
Control variables (keep the same) make it a fair test. They could be:
o Amount / mass / length / size of the magnesium
o Concentration / Volume of acid
o Try to think of at least three – make sure they are not your dependent/independent variable!
KEY POINTS TO INCLUDE IN YOUR ANSWER:
One magnesium atom reacts with two iodine atoms
Magnesium loses 2 electrons ...it then becomes a magnesium ion
Each iodine atom gains 1 electron ...it then becomes an iodide ion
Magnesium forms a positive ion
Iodine forms a negative ion
Oppositely charged ions attract
This forms a giant structure / lattice
KEY POINTS TO INCLUDE IN YOUR ANSWER:
Chlorine (In the exam it could be any other simple molecule but the mark scheme is always the
same - water, hydrogen, ammonia, methane, carbon dioxide, oxygen etc.):
Covalent bonds between atoms
Forms a simple molecule
Weak intermolecular forces between molecules (NOT WEAK COVALENT BONDS)
Only a small amount of energy needed to overcome weak intermolecular forces
This means it has a low boiling point and is a gas at room temperature
Sodium Chloride (In the exam it could be any other ionic substance but the mark scheme is
always the same – any group 1/2 metal bonded to a group 7/8 non-metal):
Ionic bonds between atoms
Strong electrostatic forces in all directions between oppositely charged ions
Forms a giant lattice
Large amount of energy needed to break these ionic bonds
This means it has a high boiling point and is a solid at room temperature
KEY POINTS TO INCLUDE IN YOUR ANSWER:
Advantages of using hydrogen:
There are renewable ways of producing hydrogen, e.g. electrolysis of water.
Combustion of hydrogen only produces water
Combustion of hydrogen does not produce carbon dioxide / not contribute to climate change
Combustion of hydrogen does not produce any particulates
Combustion of hydrogen does not contribute to global dimming
Petrol requires much more oxygen to burn so incomplete combustion is possible
Incomplete combustion of petrol produces carbon monoxide
Petrol comes from a non-renewable source
Disadvantages of using hydrogen:
Hydrogen has to be stored at high pressure and there is a risk of explosion
Hydrogen is a gas and this makes it difficult to store
Hydrogen produces much less energy and this means you need to refuel more often
Most methods of producing hydrogen need fossil fuels
KEY POINTS TO INCLUDE IN YOUR ANSWER:
Level 3 (5−6 marks) = There are statements about the results with at least one link and an attempt
at an explanation.
Statements
Concentration of copper sulfate increases
Temperature change increases
There is an anomalous result
The temperature change levels off
Reaction is exothermic
Linked Statements
Temperature change increases as concentration of copper sulfate increases
The temperature change increases, and then remains constant
After experiment 7 the temperature change remains constant
Statements including data
The trend changes at experiment 7
Experiment 3 is anomalous
Attempted Explanation
Temperature change increases because rate increases
Temperature change levels off because the reaction is complete
Explanation
As more copper sulfate reacts, more heat energy is given off
Once copper sulfate is in excess, no further heat energy produced
KEY POINTS TO INCLUDE IN YOUR ANSWER:
Level 3 (5−6 marks) = Correct statements about the effect of at least one condition on rate and yield and
at least one correct statement about compromise conditions.
Temperature
a higher temperature gives a lower yield
a higher temperature gives a faster rate
Pressure
a higher pressure gives a higher yield
increase in yield gets less as pressure increases
a higher pressure gives a faster rate
increase in rate increases as pressure increases
Catalyst
using a catalyst speeds up reaction
catalysts allow a lower temperature to be used and so save energy / reduce energy costs
Compromise
a higher pressure gives a greater yield but increases costs / (safety) risks
a high pressure gives a faster rate but increases costs / risks
a high temperature makes reaction faster but reduces yield
a catalyst makes reaction faster so a lower temperature can be used which will increase the yield
KEY POINTS TO INCLUDE IN YOUR ANSWER:
Level 3 (5−6 marks) = There is a well organised description of a laboratory procedure for obtaining
magnesium chloride that can be followed by another person. The answer must include a way of ensuring
the hydrochloric acid is fully reacted and a method of obtaining magnesium chloride crystals.
Put hydrochloric acid in beaker (or similar)
Add small pieces of magnesium ribbon until magnesium is in excess
Filter the excess magnesium using filter paper and funnel
Pour the solution into evaporating dish
Heat using Bunsen burner to evaporate sum but not all the water
Leave to crystallise while the rest of the water evaporates
Pat the crystals dry using filter paper