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1543202
GCSE AQA Chemistry Atomic Structure and Bonding
Description
A mixture of Unit 1 and Unit 2 AQA Chemistry for GCSE level
No tags specified
gcse
aqa
chemistry
ion
molecule
bonding
atomic
a-level
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Joseph Tedds
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Joseph Tedds
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Resource summary
GCSE AQA Chemistry Atomic Structure and Bonding
Atoms
Atoms consist of a nucleus orbited by electrons
Protons, neutrons and electrons are sub-atomic particles
Protons
The number of protons determines the element
If an element has only 1 proton it is hydrogen
If an element has 2 protons it is helium etc....
Protons have a relative charge of +
Protons have a relative atomic mass of 1
Neutrons
Neutrons have a relative charge of 0
Neutrons have a relative atomic mass of 1
Electrons
Electrons have a relative charge of -
Electrons have a relative atomic mass of 0
The nucleus is made up of protons and neutrons
An atom contains the same number of protons as electrons
The relative atomic mass is determined by the number of protons added to the number of neutrons
The Periodic Table
The periodic table is an information source that displays various properties of different elements and groups them accordingly
Elements are listed with symbols that represent them and are used in all formulas
Hydrogen's symbol is H
These can be one or two letters, the first always capitalised
Helium's symbol is He
These symbols are usually either taken directly from the name or from the same name in a different language
Gold is Au taken from its Latin name aurum
Hydrogen is H taken from he start of the word
Groups
Groups on the periodic table are columns
Groups of elements have similar properties because they have the same number of outer shell electrons
Group 8/0 the Noble Gases
Helium
Argon
Krypton
Radon
Xenon
Neon
These are unreactive because they have a full outer shell of electrons
Group 1 the Alkali Metals
Potassium
Francium
Caesium
Hydrogen (technically)
Rubidium
Lithium
Sodium
These are very reactive as they only have one electron in their outer shell
The group number is the number of electrons in the outer shell
Periods
Periods are rows on the periodic table
The period is the number of energy shells or layers an atom has
Electron shells
Electrons orbit the nucleus in energy layers or shells
The shells can only contain a certain amount of electrons
The first shell can contain 2 electrons
The second shell can only contain 8 electrons
The third shell can hold more than 8 electrons but at GCSE level you only need to know it can hold 8
Energy shells are filled from the lowest level upwards
Atoms want to gain a full outer shell of electrons and so this is why they react
Electronic Structure
Electronic structures are diagrams of the energy shells of an atom
The diagram is then described by a series of numbers that show the electron is each shell
Carbon is 2.4
Method 1
Draw a nucleus, no detail is necessary
To calculate the electronic structure find the number of protons as this is equal to the number of electrons
Look at the number of electrons each shell can hold and calculate how many shells you need
Look at the number of electrons each shell can hold and place accordingly filling from the lowest shell
Method 2
Draw the nucleus, no detail is necessary
Look at the period of the atom and draw that many of energy shells
Look at the group number and fill all the other energy shells up to the outer shell which you put the group number of electrons in
Ionic Bonding
Ions give or take electrons
This is held together by electromagnetic forces
This is between metals and non-metals
Giant Ionic Lattices
An ion is a charged particle
High melting point
High Boiling Point
Will carry a current in solution and melted
Covalent Bonding
This is between non-metals
Atoms share electrons
Molecules
Giant Structure
High Melting Point
High Boiling Point
No conduction of electricity (except graphite)
Strong covalent bonds
Simple Structure
Low Melting Points
Low Boiling Points
No conduction of electricity
Weak intermolecular bonds
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