1. Question and Answer Sheets
Remember, you can also use Seneca to keep revising
You’ll have a weekly quiz on these questions
Use these on Quizlet – Search “King’s Chem Revision”
Make flashcards of the questions and answers
Ask somebody at home to test you
Test yourself regularly
Things to do
Question and Answer Sheets
Paper 1 Revision
Mr King – Chemistry

2. Chemistry Revision Sheets - Topic 1 – The Atom
History of the Atom
400 BC First Idea
Spheres
Early Greece
Questions
Answers
What are the three subatomic particles?
Proton, Neutron, Electron
State the masses of the three subatomic particles
Proton (1), Neutron (1), Electron (0)
State the charges of the three subatomic particles
Proton (+1), Neutron (0), Electron (-1)
What information does the ‘atomic number’ give you?
Number of protons in an atom
What information does the ‘mass number’ give you?
Number of protons and neutrons
How can you calculate the number of neutrons in an atom?
Mass number – atomic number
What is the approximate radius of an atom?
0.1 nm (1 x m)
What is the approximate size of a nucleus?
1/10000th of the atom (or 1 x m)
What is an isotope?
Atom of the same element with the same number of protons but a different number of neutrons
In what order were the subatomic particles discovered?
Electron  Proton  Neutron
Describe the plum pudding model
Ball of positive charge containing negative electrons
What did the alpha particle scattering experiment prove?
Atoms have a dense nucleus with a positive charge
Which scientist adapted the nuclear model of the atom by discovering electrons orbit in shells?
Niels Bohr
Which scientist’s experimental work proved that neutrons exist within the nucleus?
James Chadwick
1897
Plum Pudding
JJ Thompson
Gold foil experiment showed atoms have a dense, positively charged nucleus
1905
Nuclear Model
Ernest Rutherford
1913
Niels Bohr
Electrons in shells
1932
James Chadwick
Neutrons exist
34werfef
Current Atomic Model

3. Chemistry Revision Sheets - Topic 2 – Elements, Compound and Mixtures
Terminology
Compound of Element X and Element Y
Mixture of Element X and Element Y
Element X
Element Y
Questions
Answers
Define the term ‘Atom’
The smallest part of an element that can still be recognised as that element
Define the term ‘Element’
Substance made of one type of atom only
Approximately how many elements are organised into the periodic table?
100
Define the term ‘Compound’
A substance made of two or more
different atoms chemically bonded together
Define the term ‘Mixture’
Two or more
different elements or compounds, not chemically bonded together.
What type of bonding would you find in a molecule?
Simple covalent bonding
How can you separate an insoluble solid and a liquid?
Filtration
How can you separate a soluble solid and a liquid?
Crystallisation
How can you separate the colours in an ink?
Chromatography
How does distillation work?
Evaporation then condensing
Separating Mixtures
Chromatography
Distillation
Separate mixtures of soluble substances (ink, food colourings)
Separate mixtures of two or more substances with different boiling points. The mixture is heated until one substance evaporated and removed, then cooled to condense back to a liquid.
Filtration
Crystallisation
Separates a mixture of a liquid and an insoluble solid
Separating a mixture of a soluble solid and a liquid

4. Chemistry Revision Sheets - Topic 3 – Periodic Table, Groups and Trends
Group 1 – Alkali Metals
One electron in outer shell.
As you go down the group, the reactivity of the elements increases. This is because… more shells = more shielding = easier to lose electrons
Group Group Group
Questions
Answers
What are the columns in the periodic table called?
Groups
What can the group tell you about the electrons in an atom?
Number of electrons in outer shell
What are the rows in the periodic table called?
Periods
What can the period tell you about the electrons in an atom?
How many shells an atom has
How did scientists originally organise the periodic table?
Atomic weight
Why did Mendeleev group some elements together?
Similar chemical properties
Why did Mendeleev leave gaps in his periodic table?
For elements that hadn’t been discovered yet
How was Mendeleev proved correct?
Elements matching his predictions were found.
Which alkali metal (Group 1) is more reactive, sodium or lithium?
Sodium
Which halogen (Group 7) is more reactive, chlorine or bromine?
Chlorine
Why are noble gases (Group 0) unreactive?
Full outer shells so do not need to gain/lose electrons
What is a displacement reaction?
A more reactive element can take the place of a less reactive element in a compound
Group 7 – Halogens
Seven electron in outer shell.
Non-metals.
As you go down the group, the reactivity of the elements decreases. This is because… more shells = more shielding = harder to gain electrons
As you go down the group melting/boiling points increase. At room temp. F/Cl = Gas. Br = Liquid. I = Solid.
Group 0 – Noble Gases
Unreactive. Full outer shells of electrons.
As you go down the group, the boiling points of the noble gases increases.

5. Chemistry Revision Sheets - Topic 4a – Ionic Bonding
Questions
Answers
What form of bonding is between a metal and non-metal?
Ionic
In ionic bonding, are electrons transferred or shared?
Transferred
What is an ion?
Atom which has lost/gained electron(s)
Do metals form positive or negative ions?
Positive
Do non-metals form positive or negative ions?
Negative
If an atom gains electrons, what will the charge on the ion be?
If an atom loses electrons, what will the charge on the ion be?
What term describes the attraction between oppositely charged ions?
Electrostatic Attraction
What term describes a large structure of charged ions joined together?
Giant Ionic Lattice
What is the melting point of ionic substances? High/Low?
High
Why do ionic substances have high melting points?
Strong bonds between oppositely charged ions are in a giant lattice structure. This requires a lot of energy to break.
Can ionic substances conduct electricity as a solid? Why/why not?
No, ions are not free to move.
Can ionic substances conduct electricity as a liquid? Why/why not?
Yes, ions are free to move and carry charge through the whole structure
Which two forms can an ionic substance be in to conduct electricity?
Molten and dissolved in water (aqueous)
Ionic Bonding – Dot Cross Diagram Example
Oxygen will gain two electrons from calcium atom to become a negative oxide ion (O2-).
Oxygen has been reduced.
Calcium will transfer two electrons to an oxygen atom to become a positive calcium ion (Ca2+). Calcium has been oxidised.
Giant Ionic Lattice

6. Chemistry Revision Sheets - Topic 4b – Covalent Bonding
Questions
Answers
What form of bonding is between non-metals only?
Covalent
In covalent bonding, are electrons transferred or shared?
Shared
What is a molecule?
A small group of atoms, covalently bonded together
What are intermolecular forces?
Weak forces between covalent molecules
Why do simple covalent molecules have low boiling points?
They have weak forces between molecules which take little energy to overcome.
Why can’t simple covalent molecules conduct electricity?
No charged particles (ions/delocalised electrons)
How would you describe the bonding in diamond, graphite and silicon dioxide?
Giant Covalent
How many bonds can each carbon atom form? 4
Why can graphite conduct electricity?
Each carbon only forms 3 covalent bonds. One electron from each carbon atom is delocalised and can carry charge through the whole structure
Why is graphite soft?
Weak forces between layers. Layers can slide
What is graphene?
One layer of graphite
Give a use of fullerenes/nanotubes?
Drug delivery. Conductors. Catalysts. Lubricants.
Why is diamond hard/why does it have a high melting point?
Each carbon forms 4 covalent bonds. It has a giant structure and these bonds require a lot of energy to break.
Simple Covalent Bonding – Dot Cross Diagram Examples
Shared pair of electrons, single bond
Two shared pairs of electrons, double bond
Giant Covalent Structures
Diamond Graphite

7. Chemistry Revision Sheets - Topic 5 – Metallic Bonding, Alloys and Polymers
Questions
Answers
Describe the structure/bonding of a metal.
It has positive metal ions, arranged in layers, with delocalised electrons.
Why do metals have high melting points?
Strong electrostatic attraction between negative delocalised electrons and positive metal ions.
Why can metals conduct electricity?
Delocalised electrons carry charge through the whole structure.
Why are metals soft?
Metal ions are in layers which can slide.
What is an alloy?
A mixture of two or more elements ((at least one must be a metal).
Why are alloys harder than metals?
Different sizer atoms disrupt the layers. This stops sliding.
Why would you use an alloy instead of a metal?
Alloys are harder, look better and are less reactive.
What is each unit of a polymer called?
Monomer
What type of bonding is between the atoms in one polymer molecule?
Covalent
What type of bonding is between polymer molecules?
Intermolecular forces
Why do polymers have high melting points?
Although intermolecular forces are weak, because polymers are long, they have a lot of these forces to break.
Negative delocalised electrons
Positive metal ions
Alloy
Different sized atoms.
No layers.
No Sliding.
Harder.
Monomer Polymer

8. Chemistry Revision Sheets – Topic 6 – Quantitative Chemistry
Relative Formula Mass (Mr)
Questions
Answers
What is the law of conservation of mass?
No atoms are lost or made in a chemical reaction
In a reaction, the mass of reactants is less than / equal to / more than / the mass of the products.
Equal to
Why might a reaction appear to have a decrease in mass?
One product is a gas which escapes
How do you calculate relative formula mass (Mr)?
Add up all mass numbers of each atom in the formula
What unit is used to measure the amount of substance?
Moles
How many particles are in one mole of a substance?
6.02 x 1023
6.02 x 1023, the number of particles in one mole, is known as…
Avogadro's Constant
What is the formula that links mass, moles and relative formula mass (Mr)?
Moles = Mass / Mr
What is the formula that links concentration, mass and volume?
Concentration = Mass / Volume
What unit is used for volume in calculations involving solutions?
Decimetre cubed (dm3 )
How do you convert from cm3 to dm3?
Divide by 1000
What is the unit for concentration?
g/dm3
What is a limiting reactant?
The reactant that is used up first in a reaction.
Mr of CaCO3?
(16x3) = 100
Moles
If you have 20g of CaCO3, how many moles is this?
Moles = Mass / Mr  20 / 100 = 0.2 moles
Reacting Masses
0.5g of lithium reacts with oxygen. How much lithium oxide is made?
2Li + O2  Li2O
Step 1) moles of lithium = mass / Mr
= 0.5 / 7 = moles
Step 2) mole ratio Li : Li2O
2 : 1
0.071 : moles of lithium oxide
Step 3) mass of lithium oxide = moles X Mr
= x (7+7+16)
= 1.065g Li2O
From equation
Concentration
What is the concentration if 1.5g of potassium iodide dissolves in 150cm3 of solution?
Step 1) Convert units. 150cm3 = 0.150dm3
Step 2) Concentration = Mass / Volume
= 1.5 / = 10g/dm3

9. Chemistry Revision Sheets - Topic 7 – Reactivity Series and Metal Extraction
Questions
Answers
What experiment can you do to order metals by reactivity?
Add metals to water/acid to see which reacts the most (amount of fizzing)
Which type of reaction is oxygen removed?
Reduction
Define oxidation in terms of electrons
Loss of electrons
Define reduction in terms of electrons
Gain of electrons
What is a displacement reaction?
A more reactive element takes the place of a less reactive element in a compound
Why can carbon displace zinc from zinc oxide?
Carbon is more reactive than zinc
Why can’t carbon displace magnesium from magnesium oxide?
Magnesium is more reactive than carbon
What is an ore?
Material containing enough metal for it to be economically worth extracting
Why is gold found naturally in the Earth’s crust, and not need extracting?
It is unreactive
How do you extract metals which are less reactive than carbon?
Reduction with carbon
How do you extract metals which are more reactive than carbon?
Electrolysis
Describe bioleaching
Bacteria can break down low-grade copper ores to produce an acidic solution containing copper ions (a leachate).
Describe phytomining
Plants are grown in soil that contains low grade copper ore. Plants absorb metal ions, they’re burnt and ash contains metal compounds.
Reaction with cold water
Reaction with acid
How to extract
Electrolysis
Reduction with carbon
Unreactive
Reduction with Carbon
Copper oxide + carbon → copper + carbon dioxide
2CuO(s) + C(s) → 2Cu(l) + CO2(g)
This is displacement; the carbon has displaced the copper.
This is a redox reaction; the carbon has been oxidised and the copper has been reduced.

10. Chemistry Revision Sheets - Topic 8 – Electrolysis
Aqueous – Cathode Rule
Aqueous – Anode Rule
Questions
Answers
What is electrolysis?
Using electricity to break down a substance
What happens to an ionic substance when it is melted or dissolved in water?
The ions become free to move around
What is the name for the positive electrode?
The anode
What is the name for the negative anode?
The cathode
Do positive ions move to the anode or the cathode?
Cathode
Do negative ions move to the anode or the cathode?
Anode
Metals that are ____ reactive than carbon need to be extracted using electrolysis
More
What is the main disadvantage of using electrolysis to extract metals?
Requires a large amount of energy to melt the compounds.
Why is aluminium oxide mixed with cryolite when extracting aluminium?
To lower the melting point
What is produced at the anode and cathode in the electrolysis of aluminium oxide?
Aluminium at the cathode and oxygen at the anode
Why does the anode need to be replaced in the electrolysis of aluminium oxide?
The oxygen reacts with the carbon electrode to produce carbon dioxide.
In electrolysis of an aqueous substance, what is the rule for what is formed at the positive anode?
Oxygen is formed, unless a halogen is present.
In electrolysis of an aqueous subtance, what is the rule for what is formed at the negative cathode?
It the metal is more reactive than hydrogen, hydrogen is produced instead.
At negative cathode, hydrogen is made, unless the metal present is less reactive than hydrogen.
At positive anode, oxygen is made, unless there is a halogen present (Cl-, Br- or I-)
Electrolyte must be molten or dissolved in water (aqueous) so that ions are free to move.
In aqueous substances, hydrogen and hydroxide ions are formed by some water molecules breaking down. H2O  OH- + H+
As a solid (giant ionic lattice) ions are not free to move so this substance cannot conduct electricity.
Half Equations
Reduction at anode. e.g.) Cu2+ + 2e-  Cu
Copper ions have gained electrons to become copper element.
Oxidation at cathode. e.g.) 2Cl-  Cl2 + 2e-
Chloride ions have lost electrons to become chlorine element.
Oxygen production at cathode: Oxygen is produced in electrolysis of aqueous substances which don’t contain a halide ion:
4OH-  O2 + 2H2O + 4e-

11. Chemistry Revision Sheets - Topic 9 – Acids, Salts and Neutralisation
Strong Acids
Questions
Answers
Define acid in terms of pH
A substance with a pH of less than 7
Define acids in terms of ions
A substance which releases H⁺ ions in solution
State the three common acids and give their formulae
Hydrochloric acid, HCl(aq), Sulphuric acid, H₂SO₄(aq), Nitric acid, HNO₃
What is a neutral solution?
A solution with a pH of 7. Water is an example.
How do you measure pH?
With an indicator or pH probe.
What is a base?
A metal oxide, hydroxide or carbonate that will react with an acid. E.g. copper oxide
What is an alkali?
A soluble base. E.g. sodium hydroxide
Which ions are always present in a solution of an alkali?
OH⁻
What type of salts are formed by the three main acids?
Hydrochloric acid produces chlorides, sulphuric acid = sulphates, nitric acid = nitrates
What is a neutralisation reaction?
A reaction involving an acid that results in a neutral solution
Which ions always react together in a neutralization reactions between acids and alkalis?
H⁺ and OH⁻
Write the equation showing the reaction between H⁺ and OH⁻ ions
H⁺ + OH⁻ → H₂O
metal + acid →
→ salt + hydrogen gas
metal hydroxide + acid →
→ salt + water
metal oxide + acid →
metal carbonate + acid →
→ salt + water + carbon dioxide
What is a strong acid?
An acid which completely ionises in water.
What is a weak acid?
An acid which partially ionises in water.
What is a concentrated acid?
An acid where there are lots of acid particles in the water.
What is a dilute acid?
An acid where there are fewer acid particles in the water.
Fully dissociate in solution:
Weak Acids
Partially dissociate in water:

12. Chemistry Revision Sheets - Topic 10 – Endothermic and Exothermic
Reaction Profiles
Questions
Answers
State the law of conservation of energy.
Energy cannot be created or destroyed, it can only transferred from one place to another.
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.
What is an exothermic reaction?
A reaction where energy is transferred to the surroundings.
Give two examples of exothermic reactions.
Combustion, respiration
What happens to the temperature of the surroundings during an exothermic reaction?
It increases.
What is an endothermic reaction?
A reaction where energy is transferred from the surroundings.
Give two examples of endothermic reactions.
Thermal decomposition reactions, citric acid and sodium hydrogencarbonate.
What happens to the temperature of the surroundings during an endothermic reaction?
It decreases.
State two uses of exothermic reactions
Self-heating cans, hand warmers
State two uses of endothermic reactions
Some cooling sports injury packs
What are reactants?
The substances involved in a chemical reaction
What are products?
The substances formed when reactants have a chemical reaction
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 as heat.
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.
Is breaking bonds endothermic or exothermic?
Endothermic. (Chemical bonds are strong so require energy to break).
Is making bonds endothermic or exothermic?
Exothermic. (Energy is released when chemical bonds are formed)
Endothermic
Exothermic
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.