Chemistry starts with understanding the tiny building blocks that make... Show more
Chemistry1,757 views·Updated May 19, 2026·9 pagesAQA Chemistry Paper 1 Study Guide
leema .@leema.x
1 / 9
1
of 9
Atomic Structure Basics
Everything you see, touch, and breathe is made of atoms - the fundamental building blocks of all matter. Think of them as incredibly tiny Lego bricks that combine in different ways to create everything in the universe.
Elements are pure substances made of identical atoms, each with the same number of protons. Iron, oxygen, and carbon are all elements - they can't be broken down into simpler substances. Compounds form when different types of atoms chemically bond together, like iron and oxygen combining to create iron oxide (rust).
Inside every atom, you'll find three types of subatomic particles. Protons carry a positive charge and sit in the nucleus, neutrons have no charge and also live in the nucleus, and electrons are negatively charged particles that whizz around the nucleus in energy levels called shells.
Key Point: The nucleus is incredibly small but contains nearly all the atom's mass - imagine a marble in the centre of a football stadium!
2
of 9
Atomic Numbers and Atomic History
The atomic number tells you how many protons an atom has, whilst the mass number shows the total protons plus neutrons. To find neutrons, simply subtract the atomic number from the mass number - it's that straightforward!
Scientists didn't always understand atoms like we do today. Democritus first suggested matter could be broken into tiny pieces around 450 BC. Much later, J.J. Thomson discovered electrons in 1897 and proposed his "plum pudding" model - imagine electrons like raisins scattered through a positively charged pudding.
Rutherford completely changed our understanding in 1909 by firing particles at gold foil. Most passed straight through, but some bounced back - proving atoms have a tiny, dense nucleus with electrons orbiting around it. Finally, Chadwick discovered neutrons in 1932, completing our picture of atomic structure.
Key Point: Each discovery built on previous work - science is like a giant puzzle where each piece helps reveal the bigger picture!
3
of 9
Mixtures and Separation Techniques
Mixtures are completely different from compounds because the substances aren't chemically bonded together. Think of sand mixed with salt - you can still see both substances, and they keep their individual properties.
The brilliant thing about mixtures is that you can separate them using physical methods. Filtration works perfectly for separating solids from liquids - the liquid passes through filter paper whilst the solid gets trapped. Simple distillation separates a liquid from a solution by heating it until it evaporates, then cooling the vapour back into liquid.
For more complex separations, you've got chromatography to separate different dyes in ink, and fractional distillation to separate mixtures of liquids with different boiling points. Even magnetism works brilliantly - you can pull iron filings away from sulfur using a magnet.
Key Point: Choose your separation method based on the physical properties that differ between your substances!
4
of 9
Pure vs Impure Substances
Pure substances contain only one type of particle and have fixed properties throughout. Water is pure when it's 100% H₂O molecules - it will always melt at exactly 0°C and boil at exactly 100°C under standard conditions.
Impure substances contain different types of particles mixed together, which completely changes their behaviour. Instead of melting at one specific temperature, impure substances melt over a range of temperatures because different components melt at different points.
You can easily test purity by measuring melting points. Pure substances show a sharp melting point on a temperature graph, whilst impure substances show a gradual slope as different components melt at different temperatures.
Key Point: Melting point is like a fingerprint for pure substances - each one has its own unique temperature!
5
of 9
Groups in the Periodic Table
The periodic table organises elements into groups (columns) that share similar properties, making it incredibly useful for predicting how elements will behave.
Group 1 (alkali metals) are incredibly reactive metals that get more dangerous as you go down the group. They all have one electron in their outer shell, making them desperate to lose it and form positive ions. Lithium fizzes gently in water, but potassium explodes violently!
Group 7 (halogens) are reactive non-metals with seven outer electrons, making them keen to gain one more electron. Unlike Group 1, halogens get less reactive as you go down - fluorine is viciously reactive whilst iodine is relatively calm. Group 0 (noble gases) are the lazy ones - they're so stable they rarely react with anything because they already have full outer shells.
Key Point: An element's group number often tells you how many outer electrons it has - this determines most of its chemical behaviour!
6
of 9
Chromatography Practical
Chromatography is your go-to technique for separating different coloured substances, like the various dyes mixed together in black ink. It's surprisingly simple but incredibly effective.
Start by drawing a pencil line near the bottom of filter paper (pencil won't dissolve and mess up your results). Add a small spot of your ink sample to this line, then place the paper in a beaker with a shallow layer of solvent - water or ethanol work well.
The magic happens as the solvent creeps up the paper, carrying different dyes at different speeds. Smaller molecules travel faster, whilst larger ones lag behind. When the solvent reaches the top, you'll see a chromatogram - a pattern showing all the separated dyes.
Key Point: Different dyes travel at different speeds because they have different molecular sizes and attractions to the paper!
7
of 9
Filtration and Crystallisation
Filtration is perfect when you need to separate an insoluble solid from a liquid. Simply pour your mixture through filter paper in a funnel - the liquid passes through whilst the solid stays behind on the paper.
Evaporation and crystallisation both help you recover dissolved solids from solutions, but crystallisation gives you better results. Heat your solution gently until you see crystals starting to form, then stop heating and let it cool slowly. This produces larger, purer crystals than just evaporating everything to dryness.
You can combine these techniques brilliantly to separate rock salt. First, dissolve the mixture in water so only the salt dissolves. Filter out the sand, then use crystallisation to recover pure salt crystals from the salty water.
Key Point: Crystallisation produces purer products than evaporation because impurities often stay dissolved in the remaining solution!
8
of 9
Development of the Periodic Table
Mendeleev created the first successful periodic table in 1869 by arranging elements in order of atomic mass. Brilliantly, he left gaps for undiscovered elements and even predicted their properties - most of his predictions proved spot-on when these elements were eventually found.
The modern periodic table arranges elements by atomic number instead of mass, which fixes some problems with Mendeleev's version. This arrangement perfectly explains why isotopes (atoms with different numbers of neutrons) don't mess up the pattern.
Metals dominate the left side and bottom of the table - they're typically strong, shiny, and conduct electricity well. Non-metals cluster on the right side and tend to be brittle, dull, and poor conductors. This clear pattern helps you predict an element's properties just from its position.
Key Point: The periodic table is like a giant cheat sheet - an element's position tells you almost everything about how it will behave!
9
of 9
Chemical Bonding
Ions form when atoms gain or lose electrons to achieve a full outer shell - nature's way of making atoms more stable. Metals lose electrons to form positive ions, whilst non-metals gain electrons to form negative ions.
Ionic bonding happens when metals meet non-metals. The metal atom loses electrons whilst the non-metal gains them, creating oppositely charged ions that attract each other strongly through electrostatic forces. This creates incredibly strong bonds that hold ionic compounds together.
Covalent bonding occurs when non-metal atoms share pairs of electrons instead of transferring them completely. Each shared pair creates one covalent bond, and atoms share just enough electrons to fill their outer shells. These shared electrons belong to both atoms simultaneously.
Key Point: Think of ionic bonding as "giving and taking" electrons, whilst covalent bonding is "sharing" electrons between atoms!
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Chemistry1,757 views·Updated May 19, 2026·9 pagesAQA Chemistry Paper 1 Study Guide
leema .@leema.x
Chemistry starts with understanding the tiny building blocks that make up everything around you - from the air you breathe to your mobile phone. This guide covers atomic structure, the periodic table, and how different substances behave and combine together.
1
of 9Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
Atomic Structure Basics
Everything you see, touch, and breathe is made of atoms - the fundamental building blocks of all matter. Think of them as incredibly tiny Lego bricks that combine in different ways to create everything in the universe.
Elements are pure substances made of identical atoms, each with the same number of protons. Iron, oxygen, and carbon are all elements - they can't be broken down into simpler substances. Compounds form when different types of atoms chemically bond together, like iron and oxygen combining to create iron oxide (rust).
Inside every atom, you'll find three types of subatomic particles. Protons carry a positive charge and sit in the nucleus, neutrons have no charge and also live in the nucleus, and electrons are negatively charged particles that whizz around the nucleus in energy levels called shells.
Key Point: The nucleus is incredibly small but contains nearly all the atom's mass - imagine a marble in the centre of a football stadium!
2
of 9Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
Atomic Numbers and Atomic History
The atomic number tells you how many protons an atom has, whilst the mass number shows the total protons plus neutrons. To find neutrons, simply subtract the atomic number from the mass number - it's that straightforward!
Scientists didn't always understand atoms like we do today. Democritus first suggested matter could be broken into tiny pieces around 450 BC. Much later, J.J. Thomson discovered electrons in 1897 and proposed his "plum pudding" model - imagine electrons like raisins scattered through a positively charged pudding.
Rutherford completely changed our understanding in 1909 by firing particles at gold foil. Most passed straight through, but some bounced back - proving atoms have a tiny, dense nucleus with electrons orbiting around it. Finally, Chadwick discovered neutrons in 1932, completing our picture of atomic structure.
Key Point: Each discovery built on previous work - science is like a giant puzzle where each piece helps reveal the bigger picture!
3
of 9Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
Mixtures and Separation Techniques
Mixtures are completely different from compounds because the substances aren't chemically bonded together. Think of sand mixed with salt - you can still see both substances, and they keep their individual properties.
The brilliant thing about mixtures is that you can separate them using physical methods. Filtration works perfectly for separating solids from liquids - the liquid passes through filter paper whilst the solid gets trapped. Simple distillation separates a liquid from a solution by heating it until it evaporates, then cooling the vapour back into liquid.
For more complex separations, you've got chromatography to separate different dyes in ink, and fractional distillation to separate mixtures of liquids with different boiling points. Even magnetism works brilliantly - you can pull iron filings away from sulfur using a magnet.
Key Point: Choose your separation method based on the physical properties that differ between your substances!
4
of 9Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
Pure vs Impure Substances
Pure substances contain only one type of particle and have fixed properties throughout. Water is pure when it's 100% H₂O molecules - it will always melt at exactly 0°C and boil at exactly 100°C under standard conditions.
Impure substances contain different types of particles mixed together, which completely changes their behaviour. Instead of melting at one specific temperature, impure substances melt over a range of temperatures because different components melt at different points.
You can easily test purity by measuring melting points. Pure substances show a sharp melting point on a temperature graph, whilst impure substances show a gradual slope as different components melt at different temperatures.
Key Point: Melting point is like a fingerprint for pure substances - each one has its own unique temperature!
5
of 9Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
Groups in the Periodic Table
The periodic table organises elements into groups (columns) that share similar properties, making it incredibly useful for predicting how elements will behave.
Group 1 (alkali metals) are incredibly reactive metals that get more dangerous as you go down the group. They all have one electron in their outer shell, making them desperate to lose it and form positive ions. Lithium fizzes gently in water, but potassium explodes violently!
Group 7 (halogens) are reactive non-metals with seven outer electrons, making them keen to gain one more electron. Unlike Group 1, halogens get less reactive as you go down - fluorine is viciously reactive whilst iodine is relatively calm. Group 0 (noble gases) are the lazy ones - they're so stable they rarely react with anything because they already have full outer shells.
Key Point: An element's group number often tells you how many outer electrons it has - this determines most of its chemical behaviour!
6
of 9Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
Chromatography Practical
Chromatography is your go-to technique for separating different coloured substances, like the various dyes mixed together in black ink. It's surprisingly simple but incredibly effective.
Start by drawing a pencil line near the bottom of filter paper (pencil won't dissolve and mess up your results). Add a small spot of your ink sample to this line, then place the paper in a beaker with a shallow layer of solvent - water or ethanol work well.
The magic happens as the solvent creeps up the paper, carrying different dyes at different speeds. Smaller molecules travel faster, whilst larger ones lag behind. When the solvent reaches the top, you'll see a chromatogram - a pattern showing all the separated dyes.
Key Point: Different dyes travel at different speeds because they have different molecular sizes and attractions to the paper!
7
of 9Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
Filtration and Crystallisation
Filtration is perfect when you need to separate an insoluble solid from a liquid. Simply pour your mixture through filter paper in a funnel - the liquid passes through whilst the solid stays behind on the paper.
Evaporation and crystallisation both help you recover dissolved solids from solutions, but crystallisation gives you better results. Heat your solution gently until you see crystals starting to form, then stop heating and let it cool slowly. This produces larger, purer crystals than just evaporating everything to dryness.
You can combine these techniques brilliantly to separate rock salt. First, dissolve the mixture in water so only the salt dissolves. Filter out the sand, then use crystallisation to recover pure salt crystals from the salty water.
Key Point: Crystallisation produces purer products than evaporation because impurities often stay dissolved in the remaining solution!
8
of 9Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
Development of the Periodic Table
Mendeleev created the first successful periodic table in 1869 by arranging elements in order of atomic mass. Brilliantly, he left gaps for undiscovered elements and even predicted their properties - most of his predictions proved spot-on when these elements were eventually found.
The modern periodic table arranges elements by atomic number instead of mass, which fixes some problems with Mendeleev's version. This arrangement perfectly explains why isotopes (atoms with different numbers of neutrons) don't mess up the pattern.
Metals dominate the left side and bottom of the table - they're typically strong, shiny, and conduct electricity well. Non-metals cluster on the right side and tend to be brittle, dull, and poor conductors. This clear pattern helps you predict an element's properties just from its position.
Key Point: The periodic table is like a giant cheat sheet - an element's position tells you almost everything about how it will behave!
9
of 9Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
Chemical Bonding
Ions form when atoms gain or lose electrons to achieve a full outer shell - nature's way of making atoms more stable. Metals lose electrons to form positive ions, whilst non-metals gain electrons to form negative ions.
Ionic bonding happens when metals meet non-metals. The metal atom loses electrons whilst the non-metal gains them, creating oppositely charged ions that attract each other strongly through electrostatic forces. This creates incredibly strong bonds that hold ionic compounds together.
Covalent bonding occurs when non-metal atoms share pairs of electrons instead of transferring them completely. Each shared pair creates one covalent bond, and atoms share just enough electrons to fill their outer shells. These shared electrons belong to both atoms simultaneously.
Key Point: Think of ionic bonding as "giving and taking" electrons, whilst covalent bonding is "sharing" electrons between atoms!
We thought you’d never ask...
What is the Knowunity AI companion?
Our AI Companion is a student-focused AI tool that offers more than just answers. Built on millions of Knowunity resources, it provides relevant information, personalised study plans, quizzes, and content directly in the chat, adapting to your individual learning journey.
Where can I download the Knowunity app?
You can download the app from Google Play Store and Apple App Store.
Is Knowunity really free of charge?
That's right! Enjoy free access to study content, connect with fellow students, and get instant help – all at your fingertips.
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