1. Atomic Structure and Periodic Table - Mixtures
Define the following:
Mixture:
Chromatogram:
Solute:
Solvent:
Solution:
Differentiate between the formation of a compound and a mixture: x A B
What are A,B,C and D?
Proton
Neutron
Electron
Atom
Nucleus
Ion x C D .
Label the following models of the atom with a title and annotate the diagrams to describe them
A mixture contains methanol, ethanol and propanol. The boiling points of the components are 65℃, 78℃ and 97℃ respectively. Describe a process that could be used to separate the mixture.

2. Relative electrical charges of subatomic particles and Size and mass of atoms
What is the relative size of the nucleus compared to the atom
Atoms are uncharged particles. Explain why
What are isotopes?
Explain with reference to subatomic particles why Carbon 12 and Carbon 13 are isotopes of each other 2

3. Relative atomic mass Ar
You can use this formula to work out the relative atomic masses of an element:
The relative atomic mass of copper is Explain why this is not a whole number.
92.5% of lithium atoms are Li-7 and the remaining 7.5% are Li-6. Calculate the relative atomic mass of Lithium to one decimal place.
Boron has two stable isotopes – 10B and 11B. 10B has an abundance of 19.9%. Calculate the relative atomic mass of boron to 1 decimal place. 3

4. Development of the periodic table Development of the periodic table
Before Mendeleev’s table, how were the elements arranged in order to classify them?
State one problem with early periodic tables that came before Mendeleev’s table
How did Mendeleev overcome some of the early problems of the periodic table
Give one piece of evidence that strongly suggested Mendeleev’s system of ordering elements was correct
Describe how elements are arranged in the periodic table
What do the following features tell you about the electron configuration of an element
The period number
The group number
Why do elements in the same group of the periodic table have similar chemical properties 4

5. Group 1 What is Group 1 also known as? Appearance of Group 1 elements?
How are they stored?
How are they handled? Why?
How many electrons are on their outer shell? How dense are they?
Why does reactivity increase as you go down the group?
What type of ion do they form, positive or negative? Why?
Complete the reaction word equations
Sodium + water  _______________ + ___________
Write a balanced symbol equation for the reaction above.
Evidence a reaction has taken place:
Gas formed is ___________ which is tested by ___________________
and result in a __________sound. Universal indicator solution test will turn green to
purple as the alkali metal dissolves in the water to give an _________ solution.
_______ Reactive
_______ Melting point
_______ Boiling point
_______ Relative Atomic Mass
_______ Reactive
_______ Melting point
_______ Boiling point
_______ Relative Atomic Mass

6. Group 7 What are they group 7 elements also known as? _______ Reactive
How many electrons do they have in their outer shell?
Why do the Group 7 elements decrease in reactivity as you go down the group? What is the term used to describe this?
Complete these displacement reaction equations and balance them:
Chlorine + potassium bromide  _______ + _________
Cl KBr  _______ + _________
Bromine + lithium iodide  ______ + __________
Br LiI  _________+ ________
Bromine + Sodium chloride  no reaction. Why not?
_______ Reactive
_______ Melting point
_______ Boiling point
_______ Relative Atomic Mass
_______ Reactive
_______ Melting point
_______ Boiling point
_______ Relative Atomic Mass

7. Group 0 What are the group 0 elements commonly known as?
Describe the appearance of the Group 0 elements at room temperature?
Define ‘inert’ gas
Define ‘monatomic’
How many electrons do group 0 have in their outer shell? Any exceptions?
What happens to the boiling point of the group 0 elements as you go down the group? Explain why
Argon is an inert gas.
(a)How many electrons does it have in its outer shell?
(b) Explain how the electron arrangement of argon affects it’s reactivity
The Boiling point of argon is -186℃. Predict whether neon will be a solid, liquid or gas at this temperature
The boiling points of neon, argon and krypton are -246℃, -186℃ and -153℃ respectively. Estimate the boiling point of xenon. 7

8. Your mind map