1. Chemistry Chapter 1 – Atomic structure and the periodic table – atoms, elements, compounds, mixtures, periodic table
Draw and label the structure of the atom.
State the 5 different methods used to separate out mixtures.
Labels the groups, high-light the metals and non-metals, identify the atomic number and relative atomic mass on the below Periodic table.
State the technique used to separate out the below:
Ethanol and water
Salt and water
Sand and ethanol
Crude oil fractions
Inky water
State the relative mass and relative charge of a proton, electron and neutron.
Define the terms:
Element
Compound
Mixture
Atom
Molecule
Balance the below equations:
Mg O2  MgO
Al + O2  Al2O3
HIGHER TIER: Describe why the radius of the atom increases within a group of elements.

2. Chemistry Chapter 1 – Atomic structure and the periodic table – periodic table, metals and non-metals
What does the group number and the period tell you about the element.
Describe the pattern Newlands noticed in 1865 and how he ordered the Periodic table.
State the properties of metals and non-metals.
Describe why Mendeleev’s Periodic table is still used today. Include in your answer what he did differently to the previous scientists before him.
How many electrons are able to go in the 1st, 2nd, 3rd and 4th shell.
Draw an electron shell diagram for sodium.
State the oxide formed from metals
Describe Rutherford’s theory for the atom and describe the experiment that allowed him to come up with this theory.
State the number of electrons, neutron and protons found in Na, F, Cl, Mg and H.
State the oxide formed from non-metals
Describe how you could prove an unknown metal oxide was metal or non-metal.
Describe the pattern Döbereiner noticed in 1829 and the order of his Periodic table.

3. Chemistry Chapter 1 – Atomic structure and the periodic table – Group 1, 7, 0 and maths skills
Name the elements found in Group 1.
Name the elements found in Group 7.
Name the elements found in Group 0.
Complete the word equations for the below reactions:
Sodium + oxygen 
Lithium + water 
Potassium + iodine 
Sodium + chlorine 
Lithium + fluorine 
State the name of Group 1.
State the name of Group 7.
State the name of Group 0.
Describe how the reactivity changes as you go down Group 1.
Describe how the reactivity changes as you go down Group 7.
Explain why Group 0 is relatively unreactive.
Which of the following displacement reactions will happen? (Tick/circle the ones that will).
Fluorine + sodium chloride  chlorine + sodium fluoride
Astatine + potassium bromide  bromine + potassium
astatide
Bromine + potassium iodide  iodine + potassium bromide
Group 1 reacts with water and oxygen to make what?
Group 7 elements react to make what?
State the general trends found in Group 0.
Write these numbers in standard form:
100
100000
1050
0.0004
0.105
Convert these numbers from standard form:
1 x10-2
5.5 x 104
6 x106
9.87 x 10-4
x 103
6.1 x 10-3
9 x 10-6
5.007 x 102
2 x 100
State the colour and state for the below at room temperature.
Fluorine
Chlorine
Bromine
Iodine
Astatine
Explain why Group 1 metals lose an electron.
Describe some uses of Group 0 elements in everyday life.