Chemistry Retrieval Practice QuestionsTopic 0 – Chemistry Fundamentals

Spec Ref No. Question Answer

1Define atom The smallest part of an element that can still be

recognised as that element 2 Define element A substance made of only one type of atom

3Define compound A substance made of two or more different atoms

chemically bonded together

4Define molecule A substance made of more than one atom chemically

bonded together (can be atoms of the same type!)

0.1 5 What is the formula of the hydroxide ion? OH-

0.1 6 What is the formula of the sulphate ion? SO42-

0.1 7 What is the formula of the nitrate ion? NO3-

0.1 8What is the formula of the group 1 metal ions? Li+, Na+, K+

0.1 9What is the formula of the group 2 metal ions? Be2+, Mg2+, Ca2+

0.1 10 What is the formula of the oxide ion? O2-

0.1 11 What is the formula of the ammonium ion? NH4+

0.5 12 What does this hazard symbol mean? Corrosive

0.5 13 What does this hazard symbol mean? Environmental hazard

0.5 14 What does this hazard symbol mean? Toxic

0.5 15 What does this hazard symbol mean? Irritant

0.3 16What does (aq) stand for? Aqueous: when something is dissolved in water. E.g.

NaCl(aq) is salt water

0.3 17What does (s) stand for?

solid

0.3 18What does (l) stand for?

liquid

0.3 19What does (g) stand for?

Gas

20What safety measures should you use if a practical produces a toxic gas? Use a fume cupboard

Topic 1 – Atomic Structure

1.2 21 State the three subatomic particles Protons, neutrons, electrons1.3 22 State the masses of the subatomic particles Protons: 1, neutrons: 1, electrons: 0

1.3 23State the relative charges of the subatomic particles Protons: +1, neutrons: 0, electrons: -1

1.3 24How are the subatomic particles arranged in an atom?

Protons and neutrons in the nucleus, electrons orbiting in shells

1.7 25What is the mass number of an atom? The number of protons + the number of neutrons in

an atom

1.1 26How do you calculate the number of neutrons in an atom? Mass number - atomic number

1.3 27 What is the mass and charge of a neutron? Mass = 1 Charge =0

1.4 28 Why do atoms have no overall charge?Because they have the same number of electrons as protons so the charges cancels each other out.

1.5 29How does the size of the nucleus compare to the size of the atom? Nucleus is very small

1.12 30How can you calculate relative atomic mass given isotopes masses and abundances? (mass 1 x abundance) + (mass2 x abundance) / 100

1.9 31What are isotopes? Atoms of the same element with different mass

numbers

1.9 32What are the similarities and differences between isotopes?

Same number of electrons and protons but a different number of neutrons.

1.10. 33

Sodium has a mass number of 23, and an atomic number of 11. How many electrons, protons and neutrons? 11 protons, 11 electrons, 12 neutrons

1.10. 34

Aluminium has a mass number of 27, and an atomic number of 13. How many electrons, protons and neutrons? 13 protons, 13 electrons, 14 neutrons

35 What makes an atom a particular type of atom?

Each type of atom has a number of protons, a different number of protons would make something a different type of atom.

1.11 36

What are some of the values for relative atomic mass not whole numbers?

They are the average mass of an atom of that isotope, there are several kinds each present in a different amount. So the average is not a whole number.

37How do you work out the mass number of an element? no. protons + no. Neutrons

38What do you do when asked to compare 2 atoms given atomic number and mass number?

State how many electrons, protons and neutrons they both have.

39

Neon has a mass number of 20, and an atomic number of 10. How many electrons, protons and neutrons? 10 protons, 10 electrons, 10 neutrons

40

Nitrogen has a mass number of 14, and an atomic number of 7. How many electrons, protons and neutrons? 7 protons, 7 electrons, 7 neutrons

Topic 1 – Periodic Table

1.16 41 What is the atomic number of an atom? The number of protons in an atom

1.16 42What can the period tell you about the electrons in an atom?

How many shells an atom has. E.g. carbon is in the second period so has two shells

1.13 43Why did Mendeleev put some elements in groups?

Because they had similar chemical properties (e.g. they reacted violently with water)

1.15 44What did Mendeleev put the elements in order of? Increasing atomic mass

1.15 45 How is the modern periodic table organised? In order of increasing atomic number

1.14 46Why did Mendeleev leave gaps in his periodic table? For elements that had not been discovered yet

47 What are groups in the periodic table? The columns, numbered 1, 2, 3, 4, 5, 6, 7, 0

1.16 48

What can the group tell you about the electrons in an atom?

How many electrons in the outer shell. E.g. carbon is in group 4 so has 4 electrons in the outer shell

1.19 49 How are the electrons arranged in atoms? Orbiting the nucleus in shells

1.19 50Where are the metals found on the periodic table? on the left hand side

1.19 51 How many electrons does calcium have? 20 (same as atomic number!)1.19 52 How many electrons does silicon have? 14 (same as atomic number!)1.19 53 How are the electrons in sulphur arranged? 2.8.6 (18 electrons total)

1.19 54How are the electrons in magnesium arranged? 2.8.2 (12 electrons total)

1.19 55How many electrons are in the outer shell of boron? 3 (it is in group 3!)

1.19 56How many electrons are in the outer shell of phosphorous? 5 (it is in group 5!)

1.19 57How many electrons are in the outer shell of sodium? 1 (it is in group 1!)

1.20. 58

An element has three shells and three electrons in the outer shell. What element is it? Aluminium (group 3, period 3

1.19 59How many electrons are in the outer shell of Gallium? 3 (it is in group 3!)

1.19 60How many electrons can go in the first shell? How many in the second shell? 2 = 1st shell, 9 = second shell

Topic 1 – Bonding – Part 1

1.21 61Why do atoms transfer electrons in ionic bonding? So that they can have full outer shells

1.24 62Explain in terms of electrons what occurs when lithium bonds with fluorine One electron transferred from lithium to fluorine

1.24 63Explain in terms of electrons what occurs when magnesium bonds with oxygen

Two electrons transferred from magnesium to oxygen

1.24 64Explain in terms of electrons what occurs when beryllium bonds with oxygen (3 marks) Two electrons transferred from beryllium to oxygen

1.24 65Explain in terms of electrons what occurs when magnesium bonds with chlorine

One electron transferred from magnesium to two different chlorine atoms

1.24 66Explain in terms of electrons what occurs when sodium bonds with oxygen

Two electrons transferred to an oxygen atom from two different sodium atoms

1.24 67Why do sodium ions and chlorine ions form an ionic bond?

There is an electrostatic force of attraction between oppositely charged ions

1.24 68Why don't sulphur ions and oxygen ions form ionic bonds with each other? Both have negative charges so would repel

1.22 69

What is the name for a substance made of billions of oppositely charged ions joined together?

Giant ionic lattice

1.27 70 Define giant ionic lattice A huge 3D network of ions1.33 71 State the melting points of ionic substances High

1.33 72Explain why ionic substances have high melting points.

Strong bonds between oppositely charged ions are hard to break

1.33 73 Will NaCl(s) conduct electricity? No

1.33 74Will NaCl (aq) conduct electricity? Yes (aq stands for aqueous which means it is

dissolved in water)1.33 75 Will NaCl (l) conduct electricity? Yes1.33 76 What does molten mean? Melted

1.33 77Explain why ionic compounds do not conduct electricity when solid Because the ions are not free to move

1.33 78Explain why ionic compounds conduct electricity in solution Because the ions are free to move

1.33 79Explain why ionic compounds conduct electricity when molten Because the ions are free to move

1.29 80Explain why chlorine and fluorine form covalent bonds They are both non-metals

Topic 1 – Bonding – Part 2

1.28 81Complete the sentence: In covalent bonds, electrons are _______________________ Shared

1.34 82In ionic bonds, electrons are ___________________ Transferred

1.35 83What is the name given to the structure of diamond, graphite and silicon dioxide? Giant covalent

1.36 84How many bonds does each carbon have in diamond? 4

1.37 85Explain why diamond has a high melting point Giant structure, Strong covalent bonds between the

atoms, requires a lot of energy to break

1.37 86Explain why most giant covalent substances do not conduct electricity (3 marks)

There are no electrons/ions/charged particles that are free to move

1.37 87Explain why graphite conducts electricity Has delocalised electrons between the layers that

can move through the graphite

1.37 88Explain why graphite can act as a lubricant Weak forces between layers which are free to slide

over each other1.38 89 What is graphene? One layer of graphite

1.38 90What is a fullerene? Substance made of carbon atoms arranged in a cage

1.32 91What type of substance are methane and water? Simple molecular (or simple molecules)

1.29 92 What is a molecule? A group of atoms chemically bonded together

1.31 93Describe the structure of simple covalent molecules

Strong covalent bonds between atoms, weak forces holding the molecules together

1.34 94What are intermolecular forces? Weak forces between molecules which hold them

together

1.34 95Explain why methane has a low melting point It is a simple molecular substance with weak forces

between the molecules (which are easy to break)

1.39 96What is a polymer? Millions of small molecules joined together in a chain

to form a large molecule

1.40. 97Describe the main features of metals in terms of their structure

Positive metal ions arranged in layers with delocalised electrons

1.42 98 Explain why metals can conduct electricity Delocalised electrons are free to carry charge

1.42 99Explain why pure metals are soft Layers of metal ions are free to slide over each other

1.21 100Explain in terms of electrons what occurs when lithium bonds with chlorine One electron transferred from lithium to chlorine

Topic 1 – Bonding – Part 3

1.21 101What charge will an ion of lithium take? 1+ (one electron in the outer shell, needs to lose it)

1.21 102What charge will an ion of beryllium take? 2+ (two electrons in the outer shell, needs to lose

them both)

1.21 103What charge will an ion of barium take? 2+ (group 2 so two electrons in the outer shell,

needs to lose them both)

1.21 104What charge will an ion of fluorine take? 1- (7 electrons in the outer shell, needs to gain one)

1.21 105If something has gained electrons, what charge will it have? Negative

1.21 106If something has lost electrons, what charge will it have? Positive (because they have lost a negative!)

1.21 107What charge will an ion of oxygen take? 2- (6 electrons in outer shell so needs to gain two)

1.24 108 What is an ion? an atom which has lost or gained an electron

1.23 109How many electrons, protons and neutrons in a sodium ion Na+ ? 11 protons, 12 neutrons, 10 electrons

1.41 110What are the limitations of dot and cross diagrams.

It does not show the shape of the molecule or the size of the atoms.

1.25 111If a compound name ends in -ate what does this show?

It is a molecule made of the other elements in the name and oxygen.

1.41 112What are the limitations of a ball and stick model

It does not show the electrons involved in the bonds. It does not show the 3d shape

1.25 113 What elements are in sodium sulfate? Sodium, sulfur and oxygen

1.25 114If a compound name ends in -ide what does this show? It is a molecule made of 2 elements only.

1.23 115How many electrons, protons and neutrons in an oxygen ion O2- ? 8 protons, 8 neutrons, 10 electrons

1.23 116How many electrons, protons and neutrons in a chloride ion Cl- ? 17 protons, 18 neutrons, 18 electrons

1.23 117How many electrons, protons and neutrons in a magnesium ion Mg2+ ? 12 protons, 12 neutrons, 10 electrons

1.25 118What elements are in potassium hydroxide? potassium, oxygen and hydrogen

1.25 119What elements are in sulfuric acid? hydrogen, sulfur and oxygen

1.25 120What elements are in iron carbonate iron, carbon and oxygen

Topic 2 – States of Matter

2.2 121Define mixture A substance made of more than one thing not

chemically bonded together 122 What are the 3 states of matter? Solid, liquid and gas

2.2 123What is the change from a solid to a liquid called? Solid liquid – melting

2.4 124

If the temperature is above the melting point of a substance but below the boiling point of a substance what state will it be in?

Liquid

2.4 125

If the temperature is below the melting point of a substance and below the boiling point of a substance what state will it be in?

Solid

2.4 126

If the temperature is above the melting point of a substance and above the boiling point of a substance what state will it be in?

Gas

2.2 127What is the change from a liquid to a gas called? Liquid gas – evaporation

2.2 128What is the change from a gas to a liquid called? gas liquid – condensation

2.2 129What is the change from a liquid to a solid called? liquid solid – freezing

2.1 130Describe the arrangement of the particles in a solid particles closely packed, in a regular arrangement

2.1 131Describe the arrangement of the particles in a liquid

particles closely packed, but in a random arrangement

2.1 132Describe the arrangement of the particles in a gas particles spaced far apart in a random arrangement

2.4 133A substance has a melting point of 25 oC and a boiling point of 235 oC. What state is it at 5oC? Solid

2.4 134

A substance has a melting point of -125 oC and a boiling point of -35 oC. What state is it at 15oC? Gas

2.4 135A substance has a melting point of -25 oC and a boiling point of 35 oC. What state is it at 25oC? liquid

2.32 136Describe how the particles change in arrangement when a solid turns into a liquid

Forces between particles weaken and they move more freely. The particles are not arranged in order

2.32 137Describe how the particles change in arrangement when a liquid turns into a solid

Forces between particles weaken and they move freely. They are spaced far apart

2.32 138Describe how the particles change in arrangement when a gas turns into a liquid Forces strengthen, particles move closer together

2.32 139Describe how the particles change in arrangement when a liquid turns into a gas

Forces strengthen, particles move close together in ordered rows

2 140

Describe the melting and boiling points of pure substances

One very specific temperature

Topic 2 – Separating Techniques

2.7c 141What is chromatography? A process to separate the constituents of a mixture

2.9 142

In paper chromatography, what is the stationary phase and what is the mobile phase

Paper is stationary, solvent (usually water or ethanol) is mobile

2.1 143How can chromatography show the difference between pure and impure substances? Pure ones will not separate into a number of spots

2.10. 144How is the Rf value calculated? distance moved by spot/distance moved by solvent

2.10. 145 What does a substance's Rf value depend on? How soluble it is in the solvent

2.9 146In chromatography, why must the substances be placed on a pencil line? Pencil will not dissolve in the solvent

2.9 147In chromatography why must the solvent height be lower than the pencil line?

So that the substances do not dissolve into the solvent off the paper

2.6 148How is the melting point of a pure substance different from that of an impure substance?

Pure substance has one specific melting point. Impure substance has a melting range.

2.7a 149 What is simple distillation used to separate? A liquid from a solid

2.7b 150What is fractional distillation used to separate? Two liquids with different boiling points.

2.7c 151 What is filtration used to separate? An insoluble solid from a liquid

2.7d 152What is crystallisation? Forming crystals of a soluble solid from a solution.

2.12 153 What is potable water? Drinking water2.12 154 How can sea water be made potable? By distillation

2.12 155What are the stages used to make water potable. Sedimentation, filtration and chlorination

2.5 156 What is a pure substance?A substance made of one type of atom or molecule only.

2.8 157How would you separate water from salt water? Simple distillation

2.8 158 How would you separate salt from salt water? Crystallisation

2.12 159 Why must analysis be done with pure water?Because dissolved salts in non pure water would give false positive results.

2.5 160How is the melting point of a mixture different from a pure substance?

A pure substance has a single melting temperature, a mixture has a range of melting points.

Topic 3 – Acids – Part 1

3.19 161What does soluble mean? What does insoluble mean? Dissolves in water. Does not dissolve in water

3.1 162 Define acid in terms of pH A substance with a pH of less than 73.1 163 Define acids in terms of ions A substance which releases H⁺ ions in solution

164State the three common acids and give their formulae

Hydrochloric acid, HCl(aq), Sulphuric acid, H₂SO₄(aq), Nitric acid, HNO₃

165Which ions do the common acids form in solution?

HCl forms H⁺ and Cl⁻, H₂SO₄ forms 2H⁺ and SO₄²⁻, HNO₃ forms H⁺ and NO₃⁻

3.2 166 What is a neutral solution? A solution with a pH of 7. Water is an example.3.3 167 How do you measure pH? With an indicator or pH probe.

3.10. 168What is a base? A metal oxide, hydroxide or carbonate that will react

with an acid. E.g. copper oxide3.10. 169 What is an alkali? A soluble base. E.g. sodium hydroxide

3.1 170Which ions are always present in a solution of an alkali? OH⁻

3.9 171

What is a salt?

A compound formed when some or all of the hydrogen from an acid is replaced by a metal. E.g. CuSO₄, copper sulphate, where copper has replaced H from H₂SO₄

172What type of salts are formed by the three main acids?

Hydrochloric acid produces chlorides, sulphuric acid = sulphates, nitric acid = nitrates

3.14 173What is a neutralisation reaction? Write an ionic equation for neutralisation.

A reaction involving an acid that results in a neutral solution. H⁺ + OH⁻ → H₂O

3.14 174

Which ions always react together in a neutralization reactions between acids and alkalis?

H⁺ and OH⁻

3.11a 175 metal + acid → → salt + hydrogen gas3.11c 176 metal hydroxide + acid → → salt + water3.11b 177 metal oxide + acid → → salt + water3.11d 178 metal carbonate + acid → → salt + water + carbon dioxide

3.15 179How do you make a soluble salt from an acid? React the acid with a base. E.g. to make copper

sulphate react copper oxide with sulphuric acid

3.21 180If a salt is in solution, how do you extract it as a solid?

Allow the water to evaporate off and it will leave the salt behind as a solid.

Topic 3 – Acids – Part 2

3.8 181What is a strong acid?

An acid which completely splits up into its ions in water. E.g. when HCl is in water all the HCl molecules split up into H⁺ and Cl⁻.

3.8 182

What is a weak acid?

An acid which will have some molecules which do not split up into their ions. E.g. in ethanoic acid only some of the molecules will have split up into the ethanoate ion and H⁺ ions.

3.4 183What is the relationship between an acid of pH2 and an acid of pH 3? pH 2 is 10 times more hydrogen ions than pH 3

3.7 184What is a concentrated acid? An acid where there are lots of acid particles in the

water.

3.7 185What is a dilute acid? An acid where there are fewer acid particles in the

water.

3 186How is pH measured? pH is related to the concentration of H⁺ in a solution.

3.12 187How can hydrogen be tested for? Makes a squeaky pop when a splint is placed in it

3.12 188How can carbon dioxide be tested for? Bubble through limewater, turns it milky (cloudy)

3.3 189 What colour is litmus in acid and alkali? Acid – red, alkali – blue

3.3 190What colour is methyl orange in acid and alkali? Acid – red, alkali – yellow

3.3 191What colour is phenol phthalein in acid and alkali? Acid – colourless, alkali – pink

3.17 192How do you prepare a sample of a soluble salt from a base and an acid? Neutralisation, filtration, crystallisation

3.16 193How do you prepare a sample of a soluble salt from an acid and an alkali?

Titration, repeat titration without indicator, crystallisation

3.21 194How do you prepare a sample of an insoluble salt from two solutions Combine, filtration.

3.19 195 Soluble or insoluble? nitrates Soluble3.19 196 Soluble or insoluble? Sodium salts Soluble3.19 197 Soluble or insoluble? Chloride salts Soluble, except silver and lead compounds

3.19 198Soluble or insoluble? sulphates Soluble, except lead, barium and calcium compounds

3.19 199Soluble or insoluble? carbonates Insoluble, except sodium, potassium and ammonium

3.19 200Soluble or insoluble? hydroxides Insoluble, except sodium, potassium and ammonium

3.22 201

Magnesium carbonate is insoluble. What do you need to do before it will conduct electricity?

Melt it

Topic 3 – Electrolysis – Part 1

3.22 202Sodium fluoride is soluble. Explain what the easiest way for it to conduct electricity is

Dissolve it in water because this does not require high temperatures

203 Which ions are in NaCl Na⁺ and Cl⁻ 204 Which ions are in CuCl₂ Cu²⁺ and two Cl⁻ 205 Which ions are in Na₂SO₄ 2 ions of Na⁺ and one SO₄²⁻

3.29 206Is this process oxidation or reduction? Al → Al³⁺ + 3e⁻ Oxidation

3.29 207Is this process oxidation or reduction? Na⁺ + e⁻ → Na Reduction

3.29 208Is this process oxidation or reduction? F₂ + 2e⁻ → 2F⁻ Reduction

3.29 209Is this process oxidation or reduction? Fe²⁺ → Fe³⁺ + e⁻ Oxidation

3.29 210

In this reaction, what has been oxidised and what has been reduced? Mg²⁺ + 2Na → 2Na⁺ + Mg

Na has been oxidised, Mg²⁺ has been reduced

3.29 211

In this reaction, what has been oxidised and what has been reduced? 2Al + 3Ca²⁺ → 2Al³⁺ + 3Ca

Al has been oxidised, Ca²⁺ has been reduced

3.29 212In this reaction, what has been oxidised and what has been reduced? K + Na⁺ → K⁺ + Na K has been oxidized, Na⁺ has been reduced

3.23 213What is electrolysis? Using a dc electric current to decompose (break

down) a substance

3.23 214What is an electrolyte? An ionic compound in the molten state or dissolved

in water

3.22 215What happens to an ionic substance when it is melted or dissolved in water? The ions become free to move around

3.24 216 What is the name for the positive electrode? The anode3.24 217 What is the name for the negative electrode? The cathode

3.24 218Do positive ions move to the anode or the cathode? Cathode

3.24 219Do negative ions move to the anode or the cathode? Anode

3.24 220 Where does reduction occur? Cathode

Topic 3 – Electrolysis Part 2

3.24 221 Where does oxidation occur? Anode

3.24 222At which electrode would Zn²+(aq) turn into Zn(s)? Cathode (needs to gain electrons)

3.24 223At which electrode would Cl⁻(aq) turn into Cl₂(g)? Anode (needs to lose electrons)

3.27 224 Balance the equation: Al³⁺ + e⁻ → Al Al³⁺ + 3e⁻ → Al3.27 225 Balance the equation: Cl⁻ → Cl₂ + e⁻ 2Cl⁻ → Cl₂ + 2e⁻3.27 226 Balance the equation: O²⁻ → O₂ + e⁻ 2O²⁻ → O₂ + 4e⁻

3.26 227What will be the products for the electrolysis of molten iron bromide? Iron and bromine

3.26 228What will be the products for the electrolysis of molten zinc oxide? Zinc and oxygen

3.28 229 Define oxidation in terms of electrons Oxidation is the loss of electrons4 230 Define reduction in terms of electrons Reduction is the gain of electrons

3.25 231What will be the products for the electrolysis of sodium sulfate solution? Hydrogen gas and Oxygen gas

3.25 232What will be the products for the electrolysis of acidified water? Hydrogen gas and Oxygen gas

3.31 233What happens to the change in mass of the electrodes if you increase the current? As current increases so does the change in mass.

3.31 234

When copper sulphate solution is electrolysed using copper electrodes. What happens to the mass of the electrodes?

The cathode mass increases. The anode mass decreases.

3.31 235Why use propanone to dry the electrodes when reweighing them after the electrolysis.

It evaporates drying the electrodes, no need to physically dry them.

3.25 236What will be the products for the electrolysis of copper chloride solution? Copper and chlorine

3.25 237What will be the products for the electrolysis of molten lead bromide? lead and bromine

3.25 238In the electrolysis of sodium chloride solution, what are the products? Chlorine gas and hydrogen gas

3.25 239Why is sodium not produced in the electrolysis of sodium chloride solution?

It is more reactive than hydrogen so hydrogen is produced instead.

3.25 240What is produced at the anode in electrolysis of solutions?

Either a halogen or oxygen (when there is no halogen present)

Topic 4 – Metals

4.2 241For the extraction of which metals is electrolysis needed? Ones more reactive than carbon, e.g. aluminium

4.7b 242

What are the two main disadvantages of using electrolysis to extract metals?

Requires a large amount of energy to melt the compounds and to produce the necessary electricity

4.7b 243Why is aluminium oxide mixed with cryolite when extracting aluminium? To lower the melting point

4.7b 244What is produced at the anode and cathode in the electrolysis of aluminium oxide? Aluminium at the cathode and oxygen at the anode

4.7b 245Why does the anode need to be replaced in the electrolysis of aluminium oxide?

The oxygen reacts with the carbon electrode to produce carbon dioxide.

4.3 246What is the reactivity series? A list of elements ordered by their reactivity. (K, Na,

Ca, Mg, Al, (C), Zn, Fe, (H), Cu, Ag, Au)

4.1 247How can metals be placed in order of their reactivity?

Add the metals to water or acid and see which ones react the most (by how much fizzing there is)

4.5 248What is the name for a reaction where oxygen is removed from a compound? Reduction

4.7a 249

Explain why zinc can be extracted from zinc oxide with carbon but magnesium cannot be extracted from magnesium oxide with carbon

Magnesium is more reactive than carbon (1), Zinc is less reactive than carbon (1), Carbon can therefore remove oxygen from zinc oxide but not magnesium oxide (1)

4.4a 250Explain why gold and silver can be found naturally in the Earth's crust It is very unreactive

4.7b 251What process is used to extract metals more reactive than carbon? Why? Electrolysis. It is a stronger form of reduction.

4.4a 252Define an ore A material containing enough metal in it for it to be

economically worthwhile to extract the metal.

4.2 253Define a displacement reaction

A reaction in which a more reactive element takes the place of a less reactive element in one of its compounds or in solution

4.2 254

Which of the substances below has been oxidized and which has been reduced? Al³⁺ + Fe → Fe³⁺ + Al

Aluminium has been reduced and iron has been oxidised

4.2 255Show two half equations for the reaction below: Al³⁺ + Fe → Fe³⁺ + Al Al³⁺ + 3e⁻ → Al, Fe → Fe³⁺ + 3e-

4.8 256What is phytoextraction

Growing plants on areas of low grade ore, to concentrate the metal in the plant then extracting the metal from the plant.

4.8 257Why use phytoextraction Allows us to extract ores from sites where it would

not otherwise be cost effective.

4.11 258What are the stages of a life cycle assessment?

Effect on the environment of; obtaining raw materials, manufacturing the product, using the product and disposing of the product.

4.2 259 How is copper extracted from its ore? Heating with carbon.

4.6 260

In this displacement reaction. What is oxidised and what is reduced? CuSO4 + Mg → MgSO4 + Cu

Copper gains electrons and is reduced. Magnesium loses electrons and is oxidised.

Topic 4 – Equilibrium

4.13 261What is a reversible reaction? A reaction which can go from reactants to products but

also from products to reactants

4.13 262What chemical symbol represents a reversible reaction? ⇌

263

If a reaction is exothermic in the forward direction what will it be in the reverse direction?

Endothermic

264

Two reactants require 30kJ to turn into products. What energy transfer is involved when the products turn into reactants?

30kJ is released

4.14 265What is equilibrium? The point in a reversible reaction when the forward and

reverse reactions are occurring at the same rate

4.14 266How is the amount of reactant changing at equilibrium? It is not changing

4.14 267How is the amount of product changing at equilibrium? It is not changing

4.17a 268

A reaction is exothermic in the forward direction. What will occur if the temperature is increased?

The backward reaction will increase as it is endothermic and will reduce the temperature

4.17a 269

A reaction is endothermic in the forward direction. What will occur if the temperature is increased?

The forward reaction will increase as it is endothermic and will reduce the temperature

4.17c 270A reaction is at equilibrium when some product is removed. What will occur?

The forward reaction will increase as that will increase the amount of product

4.17c 271

A reaction is at equilibrium when the concentration of a reactant is increased. What will occur?

It will move in the forward reaction to reduce the amount of the reactant.

4.17b 272

The reaction below is at equilibrium. What will occur when the pressure is increased?2H₂(g) + O₂(g) ⇌ 2H₂O(g)

The forward reaction will increase as there are fewer molecules on the right. This will reduce the total number of molecules and therefore the pressure.

4.15 273 What is the Haber process reaction 3H2(g) + N2 (g) ⇌ 2NH3(g)

4.16 274What temperature is used for the Haber process? 450 oC

4.15 275Where does the nitrogen for the Haber Process come from? Nitrogen from the atmosphere

4.15 276Where does the hydrogen for the Haber Process come from? Hydrogen from natural gas

277Why are the products of the reaction cooled?

To turn the ammonia into a liquid and remove it, so driving the equilibrium in the forward reaction some more.

4.14 278 What is a dynamic equilibrium?A reversible reaction where the forward reaction and the backward reaction happen at the same rate

4.16 279 What catalyst is used for the Haber process? Iron catalyst4.16 280 What pressure is used for the Haber process? 200 atmospheres

Topic 6 – Periodic Table

6.1 281In terms of electrons, what do group 1 elements have in common? 1 electron in the outer shell

6.1 282In terms of electrons, what do group 7 elements have in common? 7 electrons in the outer shell

6.1 283In terms of electrons, what do group 0 elements have in common? Full outer shell

6.4 284 What is more reactive, lithium or sodium? Sodium6.11 285 What is more reactive, chlorine or bromine? Chlorine

286 Define inert Un-reactive

6.14 287Explain why the noble gases are inert They have full outer shells, so do not need to gain or

lose electrons

6.2 288State the trend in the melting points of the alkali metals Gets lower down the group

6.6 289What state are fluorine, chlorine, bromine and iodine at room temperature? Gas, gas, liquid, solid

6.3 290 Balance the equation: Li + H₂O → LiOH + H₂ 2Li + 2H₂ → 2LiOH + H₂

6.7 291

State the trend in melting and boiling points for the halogens as you go down the group. Predict what state astatine will be.

As you go down the group melting point increases. F2

and Cl2 are gases, Br2 is a liquid, I2 is a solid. At2 will be a solid

6.8 292 How can chlorine be tested for? Bleaches damp litmus paper white

6.3 293Explain why the group 1 elements are called alkali metals

They are metals that form alkalis when they react with water

6.11 294What is a displacement reaction? A reaction in which a more reactive element takes

the place of a less reactive element in a compound

6.11 295Explain why the following reaction does not proceed: KBr + I₂

Iodine is less reactive than bromine so cannot displace it

6.11 296

Balance the below equation and explain why it is a displacement reaction: KBr + Cl₂ → KCl + Br₂

2KBr + Cl₂ → 2KCl + Br₂ , chlorine has displaced bromine as it is more reactive

6.13 297

Explain why fluorine is more reactive than chlorine

Fewer shells/electrons, less shielding (or stronger attraction from nucleus), easier to gain electrons

6.5 298

Explain why potassium is more reactive than lithium (3 marks)

More shells/electrons, less shielding (or weaker attraction from nucleus), easier to lose electrons

6.9 299 How do halogens react with magnesium? Mg (s) + Cl2 → MgCl2 (s)

6.1 300

What happens with halogens react with hydrogen? What is the pH when the product dissolves in water?

H2 (g) + Cl2 (g) → 2HCl (g) - pH will be low as forms an acid

Topic 7 – Rates of Reaction

7.2 301What is the rate of a chemical reaction in terms of reactants? How quickly the reactants in a reaction are used up

7.2 302What is the rate of a chemical reaction in terms of products? How quickly the products in a reaction are formed

7.2 303What is the formula for a mean rate of reaction in terms of reactants? quantity of reactant used/time taken

7.2 304What is the formula for a mean rate of reaction in terms of products? quantity of reactant product formed/time taken

7.2 305How can you measure the quantity of a reactant or product? In grams or in cm³

7.2 306What are the two possible units for rate of reaction? g/s or cm³/s (where s is seconds)

7.5 307How could you measure the rate of a reaction from a graph?

Draw a tangent to the curve and calculate the gradient.

7.3 308What is "collision theory"? The theory that chemical reactions only occur when

particles collide with sufficient energy

7.4 309What factors can affect the rate of a reaction? Temperature, surface area of a solid, concentration

or reactants in solution, pressure of gases

7.4 310State the effect of increasing the surface area on the rate of a reaction Increases the rate

7.4 311

Explain why increasing the surface area increases the rate of a reaction

More particles are available to collide, there are therefore more frequent collisions between reactants.

7.4 312State the effect of increasing the concentration on the rate of reaction Increases

7.4 313

Explain why increasing the concentration increases the rate of reaction

More concentrated means more particles in solution, therefore more frequent collisions between reactants.

7.4 314State the effect on increasing the pressure of a gas on the rate of reaction Increases

7.4 315Explain why increasing the pressure of a gas increases the rate of a reaction

Less space for the particles to move around in, therefore more frequent collisions

7.4 316State the effect of increasing the temperature on the rate of reaction Increases

7.4 317What is the activation energy?

The amount of energy a particle needs before it will be able to react when it collides with another particle

7.4 318

Explain why increasing the temperature increases the rate of reaction

Increases the speed at which particles move therefore more frequent collisions. Increases the number of particles which have the activation energy therefore more collisions result in a reaction.

7.6 319What is a catalyst? Something which changes the rate of a reaction but

is not used up in that reaction

7.6 320How do catalysts speed up reactions? They provide another route for the reaction to take

place which has a lower activation energy.

Topic 7 – Energy in Reactions

7.8 321What supplies the enzyme for producing alcoholic drinks Yeast

322

How does the law of conservation of energy apply to chemistry?

In all chemical reactions, energy is either transferred to the surroundings or from the surroundings.

7.10. 323What is an exothermic reaction? A reaction where energy is transferred to the

surroundings.7.9 324 Give two examples of exothermic reactions. Combustion, respiration

7.10. 325

What happens to the temperature of the surroundings during an exothermic reaction?

They increase. The thermometer is included in "the surroundings" so shows the temperature increasing.

7.11 326What is an endothermic reaction? A reaction where energy is transferred from the

surroundings.

7.9 327Give two examples of endothermic reactions. Thermal decomposition reactions, citric acid and

sodium hydrogencarbonate.

7.11 328

What happens to the temperature of the surroundings during an endothermic reaction?

They decrease. The thermometer is included in "the surroundings" so shows the temperature decreasing.

329 State two uses of exothermic reactions Self-heating cans, hand warmers 330 State two uses of endothermic reactions Some cooling sports injury packs 331 What are reactants? The substances involved in a chemical reaction

332What are products? The substances formed when reactants have a

chemical reaction

7.16 333What is a reaction profile? A diagram which shows whether the reactants have

more or less energy than the products.

7.10. 334

If the reactants have more energy than the products, what kind of a reaction must have taken place?

An exothermic one. The missing energy has been transferred to the surroundings.

7.11 335

If the reactants have less energy than the products, what kind of a reaction must have taken place?

An endothermic one. The extra energy has been taken in by the surroundings.

7.12 336

Is breaking bonds endothermic or exothermic?Endothermic. Chemical bonds are strong so require energy to break (like when you have to put energy in to separate magnets from each other)

7.12 337Is making bonds endothermic or exothermic?

Exothermic. Energy is released when chemical bonds are formed (like how two magnets move together when close and generate kinetic energy)

7.14 338

How do we work out the overall energy change of a reaction?

Work out the difference between the energy needed to break all the bonds in the reactants and the energy released to form all the bonds in the products.

7.13a 339

If more heat energy is released forming bonds than is required for breaking bonds in a reaction what kind of reaction is it? exothermic

7.13b 340

If less heat energy is released forming bonds than is required for breaking bonds in a reaction what kind of reaction is it? endothermic

Topic 8 – Fuels – Part 1

8.2a 341 What is crude oil? A mixture of hydrocarbons

342What is crude oil formed from? The remains of ancient biomass (mostly plankton)

that was buried in mud

8.2d 343What is a finite resource? Why is crude oil a finite resource?

One that will run out. Because it takes longer to form than the rate at which we are using it up

8.1 344What is a hydrocarbon? A compound made of atoms of carbon and hydrogen

only8.6 345 What is an alkane? A hydrocarbon with only single bonds8.6 346 Name the first four alkanes Methane, ethane, propane, butane

8.6 347 What is the general formula for alkanes? CnH2n+2 (the n and 2n are small)

8.6 348How does boiling point change with the length of an alkane? The longer the alkane, the higher its boiling point

8.5 349How does viscosity change with the length of an alkane?

The longer the alkane, the more viscous (the thicker) it is

8.5 350How does flammability change with the length of an alkane? The longer the alkane, the less flammable it is

8.3 351What is fractional distillation? A process used to separate mixtures of substances

with different boiling points

8.3 352

What are the steps involved in fractional distillation?

Crude oil is vaporised, different molecules rise up the fractionating column and cool down. Condense at different points on the column.

8.3 353Why is fractional distillation important? Because the different fractions have different uses

8.4 354What is a fuel? A substance which when reacted with oxygen releases

energy

8.4 355Name five fuels we obtain from crude oil Petrol, diesel oil, kerosene, fuel oil and liquefied

petroleum gases

8.4 356What other uses are there for products of fractional distillation? Solvents, lubricants, polymers and detergents

8.7 357 What is combustion? The reaction of a fuel with oxygen

8.7 358What are the products of complete combustion? Carbon dioxide and water

8.8 359 When does incomplete combustion occur? When there is not enough oxygen present8.8 360 What is formed in incomplete combustion Carbon monoxide

Topic 8 – Fuels – Part 2

8.9 361Why is carbon monoxide dangerous It is toxic, taken up by red blood cells in preference to

oxygen.

8.16 362What is cracking? The process of breaking down a long hydrocarbon into

smaller hydrocarbons8.16 363 What are the products of cracking? Short alkanes and alkenes

8.17 364Why is cracking important? Because smaller hydrocarbons are more useful than

longer ones8.6 365 What are alkenes A hydrocarbon with a double bond

8.6 366What are alkenes used for? As a starting material to make more useful chemicals

8.6a 367 What is the general formula for alkenes? CnH2n

9.12 368 What are the first four alkenes? Ethene, propene, butene, pentene

8.6 369

What do members of a homologous series have in common?

Same general formula, differ by CH2 for neighbouring compounds in the series, boiling points increase with chain length, have similar chemical properties and reactions.

8.11 370How is sulphur dioxide produced? Sulphur impurities in fuels form it when the fuel is

burnt

8.12 371What happens when the sulphur dioxide dissolves in rain water? Acid rain is formed

8.13 372How are oxides of nitrogen formed?

When the nitrogen and oxygen in the air react together at the high temperatures created in combustion engines

8.14 373

State three advantages of hydrogen fuel cells over petrol

Do not need to be recharged, no pollutants are produced only H2O, water is a renewable resource

8.14 374

State three disadvantages of hydrogen fuel cells over petrol

Hydrogen is highly flammable, hydrogen is sometimes produced through non-renewable means, hydrogen is difficult to store and transport

8.2d 375 What does finite mean? It wil run out.

8.5c 376How does ease of ignition change with the length of an alkane? The longer the alkane, the harder it is to ignite.

8.5b 377How are members of a homologous series different from each other? Their chain length differs by a number of CH2

8.15 378Where do petrol, kerosene and diesel oil come from? They are obtained by fractional distillation of crude oil

8.15 379 Where does methane come from? It is found in natural gas?

8.15 380Are petrol, kerosene, diesel and methane renewable or non renewable? non-renewable

Topic 8 – Atmosphere

8.23 381 How can oxygen be tested for? Relights a glowing splint

8.19 382What gases made up the Earths initial atmosphere

Large amount of carbon dioxide, water vapour, small amounts of other gases

8.20. 383What happened to the water vapour as the earth cooled? Water vapour condensed forming oceans

8.21 384

What affect did the formation of the oceans have on the amount of carbon dioxide in the atmosphere?

Carbon dioxide dissolves in water so some dissolved and the amount in the atmosphere decreased

8.22 385How did the growth of primitive plant affect the atmosphere?

They used carbon dioxide and released oxygen in photosynthesis

8.26 386What is the composition of our atmosphere today? Nitrogen about 78%, Oxygen 21%, 1% other gases

8.24 387 Name 3 greenhouse gases Carbon dioxide, methane and water vapour

8.24 388What is the greenhouse effect Greenhouse gases absorb heat radiated from the

earth and release it keeping the earth warm8.26b 389 Name 2 effects of global warming Polar ice caps melting, sea levels rising

8.18 390Where did the gases that formed our early atmosphere come from? They were produced by volcanic activity.

8.19 391What gas, in today's atmosphere was missing from our early atmosphere? oxygen

8.25 392 What does correlation mean?There is a link between them. (eg. As one increases so does the other)

8.22 393When did oxygen begin to be formed in our atmosphere? When the first plants began photosynthesising

8.24 394 What do greenhouse gases do? Trap heat in our atmosphere

8.26 395Name one man made cause of the greenhouse effect Deforestation

8.25 396

What has happened to the amount of carbon dioxide in our atmosphere in the last 200 years? It has increased

8.25 397What human activity might have increased the amount of carbon dioxide in our atmosphere? Burning fossil fuels

8.25 398

What human activity, other than burning fossil fuels, might have increased the amount of carbon dioxide in our atmosphere? Respiration (as population increases so does this)

399If a sample of the atmosphere is reacted with copper, what gas will react? Oxygen

400If all the oxygen is removed from a sample of the atmosphere how much is removed? 21%

Topic 5 – Transition Metals

5.6 401What is an alloy? A mixture of two or more elements, at least one of

which is a metal5.5 402 Give a reason for alloying a metal To make it harder, to make it less reactive

5.5 403Explain why alloys can be harder than pure metals

Different size of atoms disturb the layers to stop them sliding over each other

5.1 404

What are the typical properties of transition metals?

High melting point, high density, form coloured compounds, act as catalysts for particular reactions.

5.3 405 How can rusting of iron be prevented? By excluding water and oxygen

5.3 406What can you exclude to reduce rusting of iron. water and oxygen

5.3 407 How else can rusting of iron be prevented? By sacrificial protection

5.3c 408What is sacrificial protection? Coating the metal in a more reactive metal that will

react in preference to the one you are trying to protect

5.4 409What is electroplating? Using electrolysis to coat the metal to be protected in a

thin layer of another metal

5.4 410Why is electroplating used? It improves appearance and increases resistance to

corrosion.

5.6 411Why is iron alloyed to make steel to improve resistance to corrosion and increase

strength.

5.7 412How does alloying gold increase its strength

The different sized atoms mixed with the gold atoms disrupt the layers of identical gold atoms and stop them rolling over one another.

5.7 413What properties of gold make it suitable for its uses unreactive - jewellery lasts well

5.7 414What is copper used for? wires - because it is a good conductor, water pipes -

because it is unreactive5.2 415 What causes corrosion of metals? oxidation5.7 416 What is aluminium used for? Drinks cans - lightweight, ladders - low density5.7 417 What is brass used for? Door fittings - unreactive, attractive

5.7 418What is magnalium used for? Scientific instruments - increased malleable, lower

density than aluminium

5.2 419What is another name for oxidation of metals? corrosion

5.1 420What are irons properties? High melting point, high density, form coloured

compounds, act as catalysts for particular reactions.

Topic 5 – Equilibrium

5.19 421What is the Haber process? A reversible reaction between nitrogen and hydrogen

forming ammonia

5.21 422

In an industrial reaction why would you carry it out at a high temperature even if this would shift the equilibrium to the left hand side and reduce percentage yield?

To increase the rate of the reaction, saving time

5.22 423 What elements do fertilisers contain? Nitrogen, phosphorus and potassium (NPK)5.22 424 What are fertilisers used for? To promote plant growth

5.23 425What is formed when ammonia reacts with nitric acid? Ammonium nitrate

5.23 426Why is ammonium nitrate a good fertiliser? NH4NO3, contains 2 nitrogen atoms per molecule

5.24 427 How would you make ammonium sulphate? From ammonia and sulfuric acid

5.20a 428How will an increase in temperature affect the rate of attainment of equilibrium? Equilibrium will be reached quicker.

5.20a 429How will an decrease in temperature affect the rate of attainment of equilibrium? Equilibrium will be reached slower.

5.20b 430How will an increase in pressure affect the rate of attainment of equilibrium? Equilibrium will be reached quicker.

5.20b 431How will an decrease in pressure affect the rate of attainment of equilibrium? Equilibrium will be reached slower.

5.20c 432How will an increase in concentration affect the rate of attainment of equilibrium? Equilibrium will be reached quicker.

5.20c 433How will an decrease in concentration affect the rate of attainment of equilibrium? Equilibrium will be reached slower.

5.20d 434How will adding a catalyst affect the rate of attainment of equilibrium? Equilibrium will be reached quicker.

5.21b 435

Why would you choose a lower/medium pressure when a high pressure would give a better yield?

To reduce costs and risk.

5.21b 436

Why would you choose a high temperature when a low temperature would give a better yield?

To increase rate of reaction

5.21b 437Why would you use a catalyst in an industrial reaction? To increase rate of reaction and reduce costs.

5.23 438Write a word equation for the reaction of ammonia and nitric acid. ammonia + nitric acid --> ammonium nitrate

439Why does increasing temperature increase rate at which equilibrium is reached?

There are more frequent collisions between particles so the rate of reaction increases.

440Why does increasing pressure increase rate at which equilibrium is reached?

There are more frequent collisions between particles so the rate of reaction increases.

Topic 5 – Fuel Cells

441What is a chemical cell? A unit which contains chemicals which produce

electricity through a reaction

5.25 442What are the main components of a chemical cell? An anode, a cathode and an electrolyte

443What is an electrolyte? A solution containing ions which allows current to flow.

5.25 444What does the potential difference of a cell depend on? The type of electrode and the electrolyte.

5.25 445 What is a battery? Two or more cells connected in series

5.25 446What happens to the electrodes in a chemical cell?

The more reactive metal depletes and the less reactive one increases in size.

5.25 447In non-rechargeable cells, why do the chemical reactions stop over time? One of the reactants becomes used up.

5.25 448 How can certain cells be recharged? Applying an external electric current

5.25 449

How does the reactivity of the metal electrodes affect the size of the potential difference?

The greater the difference in reactivity, the greater the potential difference.

5.26 450What is a fuel cell? A cell which uses a fuel and oxygen (or air) to generate

electricity.5.26 451 What are the products in a hydrogen fuel cell? Water

5.26 452State three advantages of hydrogen fuel cells Do not need to be recharged, no pollutants are

produced, can be different sizes for different uses

5.26 453

State three disadvantages of hydrogen fuel cells

Hydrogen is highly flammable, hydrogen is sometimes produced through non-renewable means, hydrogen is difficult to store

5.26 454

Complete the equation which occurs at the negative electrode of a hydrogen fuel cell 2H₂ + 4OH⁻ →

4H₂O + 4e⁻

5.26 455

Complete the equation which occurs at the positive electrode of a hydrogen fuel cell O₂ + 2H₂O →

4OH⁻

5.26 456What is the overall reaction occurring in a hydrogen fuel cell? O₂ + 2H₂ → 2H₂O

5.27 457Does a hydrogen fuel cell produce greenhouse gases? yes water is a greenhouse gas

5.27 458Does a hydrogen fuel cell produce any carbon emissions?

no, only product Is water, but sometimes CO2 is produced making the hydrogen fuel.

5.27 459Why is hydrogen difficult to store? It is a highly flammable gas so needs pressurised tanks

460 What other fuels can fuel cells run on? methanol

Topic 9 Qualitative Analysis

9.2 461 What is a flame test? A test to identify metal ions (cations)

9.2 462What is the colour of the flame produced from a lithium containing compound? Crimson

9.2 463What is the colour of the flame produced from a copper containing compound? Green

9.2 464What is the colour of the flame produced from a sodium containing compound? Yellow

9.2 465What is the colour of the flame produced from a potassium containing compound? lilac

9.2 466What is the colour of the flame produced from a calcium containing compound? Orange-red

9.3 467Other than flame tests, how can metal ions be identified? Use of sodium hydroxide

9.3 468Which solutions produce white precipitates on addition of sodium hydroxide? Solutions containing aluminium, calcium ions

9.3 469How can a solution of aluminium ions be distinguished from calcium ones? Its precipitate will dissolve in excess sodium hydroxide

9.3 470

What is the colour of the precipitate formed from the addition of sodium hydroxide to a solution containing copper (II) ions?

Blue

9.3 471

What is the colour of the precipitate formed from the addition of sodium hydroxide to a solution containing iron(II) ions?

Green

9.3 472

What is the colour of the precipitate formed from the addition of sodium hydroxide to a solution containing iron(III) ions?

Brown

9.5a 473 What is the test for carbonates? Add an acid to generate carbon dioxide gas

9.5c 474What is the test for halides? Add silver nitrate and nitric acid to generate a solid

silver halide precipitate

9.5c 475What are the colours of the silver halides? Silver chloride white, silver bromide cream, silver iodide

yellow

9.5b 476What is the test for sulphate ions? Add barium chloride and hydrochloric acid, forms white

precipitate9.8 477 How do we test for ammonia gas? Add damp red litmus paper it will turn blue.

9.8 478

What are the three advantages of instrumental methods?

They are accurate (gives correct results), sensitive (only needs a small sample to work), rapid (a lot faster than other tests)

9.9 479What is flame emission spectroscopy? An instrumental analysis tool for identifying metal ions

9.9 480

How is flame emissions spectroscopy carried out?

Sample placed in a flame, light emitted is passed through a spectroscope to give a spectrum which can be compared to a reference

Topic 9 Hydrocarbons

9.15 481 How do you test for an alkene? React it with bromine water.

9.13 482 What is the general formula for alkenes? CnH2n

9.11 483What does unsaturated means? Contains double bonds (which could become C-H

bonds)9.12 484 What are the first four alkenes? Ethene, propene, butene, pentene

9.16 485How is the combustion of alkenes different to combustion of alkanes?

Alkenes usually react by incomplete combustion so burn with smoky flames

9.11 486 What type of hydrocarbon are alkanes? saturated

9.11 487 What is a hydrocarbon? a molecule made of hydrogen and carbon atoms only.9.10. 488 What are the first four alkanes? Methane, Ethane, propane, and butane9.12 489 What functional group do all alkenes contain? C=C

9.10. 490 What is the general formula for alkanes? CnH2n+2

9.15 491What is the colour change when an alkene reacts with bromine water? The bromine water turns from orange to colourless

9.15 492What is the colour change when an alkane is added to bromine water? There is no colour change it remains orange.

9.15 493Which substance will decolourise bromine water, propane or propene? Propene

9.16 494What is produced when an alkane is combusted? carbon dioxide and water

9.16 495Write a balanced equation for the combustion of methane, CH4. CH4 + 2O2 --> CO2 + 2H2O

9.16 496What is happening to the hydrocarbon when it is being combusted? It is being oxidised

9.13 497 Why are alkenes unsaturated compounds? They contain a C=C double bond

9.11 498 Why are alkanes saturated compounds?They contain no C-C double bond. They have only single bonds

9.12 499 How are but-1-ene and but-2-ene different?The position of the double bond. In but-1-ene between C's 1 & 2. In but-2-ene between carbons 2 & 3

9.11 500 Is di-chloroethane a hydrocarbon?No it does not contain just carbon and hydrogen atoms. It also contains chlorine atoms.

Topic 9 Alcohols and Carboxylic acids

9.24 501 What functional group do all alcohols have? OH

9.26 502Name and draw the first four alcohols Methanol, ethanol, propanol, butanol (ethanol

pictured)

503What happens when an alcohol reacts with sodium?

It forms a sodium salt (e.g. sodium ethoxide from ethanol) and releases hydrogen gas.

504What are the products of a combustion reaction involving an alcohol and oxygen? Carbon dioxide and water

505

Write a symbol equation for the reaction of methanol/ethanol/propanol/butanol with oxygen

E.g. CH₃CH₂OH + 5O₂ → 2CO₂ + 3H₂O

506 Do alcohols dissolve in water? Yes, they form neutral solutions9.31 507 How do alcohols react with oxidizing agents? They turn into carboxylic acids

508What are the main uses of alcohols? Solvents, ethanol used as drinking alcohol and a biofuel

9.33 509What is fermentation? The process of turning glucose (a natural sugar) into

ethanol9.33 510 What is required for natural fermentation? Yeast

9.3 511What functional groups do all carboxylic acids have? COOH

9.29 512Name and draw the first four carboxylic acids Methanoic acid, ethanoic acid, propanoic acid, butanoic

acid (image is ethanoic acid)513 Why are carboxylic acids weak acids? Not all their molecules ionise when in water

9.31 514 What is made when ethanol is oxidised? Ethanoic acid

9.28 515

How do you compare the energy released by alcohols when they are combusted.

Burn the alcohol, use the energy to heat water. Measure the temperature change of the water. Calculate the temperature change caused per gram of alcohol burnt.

9.27 516 What is made when ethanol is dehydrated? An alkene9.34 517 How can ethanol be concentrated? Distillation

9.32 518Why do alcohols have the same type of reactions? They are part of the same homologous.

9.27 519What group do molecules with an -OH belong to? alcohols

9.27 520What group do molecules with an -COOH belong to? carboxylic acid

Topic 9 Polymers

9.19 521 What is the monomer in poly(ethene)? ethene

9.18 522What is polymerisation? The process of using small molecules (monomers) to

make long chain molecules (polymers)

9.18 & 9.22 523 What are the two types of polymerisation? Addition and condensation

9.18 524What monomers are involved in addition polymerisation? Alkenes

9.2 525How do we draw polymers? In round brackets with an n [poly(ethene) is shown]

9.22 526What type of monomers are involved in condensation polymerisation? Ones with two functional groups (like a diol)

9.22 527What are the products of condensation polymerization? A polymer and a small molecule (usually water)

9.19 528What is the polymer made from chloroethene monomer? poly(chloroethene)

9.19 529What is the monomer in poly(tetrafluoroethene) (PTFE)? tetrafluoroethene

9.21 530 What is a use of poly(ethene)? carrier bags9.21 531 What is a use of poly(propene)? drain pipes9.21 532 What is a use of poly(chloroethene)? clothing9.21 533 What is a use of PTFE? Non stick coatings on pans

9.20. 534What does the repeating unit for the polymer made of propene look like? (CH3CH-CH)-

9.25c 535What is formed from different amino acids combined in one chain? Proteins

9.25a 536 What does DNA stand for? Deoxyribonucleic acid9.25a 537 What is DNA? A large molecule containing genetic information

9.25a 538What is the structure of DNA? Two polymer chains made from nucleotides in the form

of a double helix9.25 539 Name four naturally occurring polymers DNA, proteins, starch, cellulose

9.25b 540What monomers are starch and cellulose made of? Glucose

Topics 1 Calculations with Mass and Topic 5 Calculations

Ar = Sum of (atomic mass x percentage abundance) / 100

Ar - relative atomic massNo units

Mr = Sum of (Ar atoms x number of atoms of each element)

Mr – relative molecular/formula massNo units

m = n x Mrm – mass (g)n – amount of substance (mol)M – molar mass (g mol-1)

n = V / Vm

n – amount of gas (mol) at RTP (room temperature and pressure)V – volume of gas (dm3)Vm – molar volume of gas (24.0 dm3)

c = n / V c – concentration (mol dm-3)n – amount of substance (mol)V – volume of solution (dm3)

c = m / V c – concentration (g dm-3)m – mass (g)V – volume of solution (dm3)

c(mass) = c(mol) x Mc(mass) – concentration (g dm-3)c(mol) – concentration (mol dm-3)M – molar mass (g / mol)

pV = nRTp – pressure (Pa)V – volume (m3)n – amount of substance (mol)R – molar gas constant (8.314 JK-1mol-1)T – temperature (K)

percentage yield = ( actual yield / theoretical yield ) x 100%

Atom economy = [ (mass of desired products in balanced equation) / (total mass of products in balanced equation) ] x 100