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Complete GCSE Chemistry Study Guide
Matilda Gant
@atildaant_rvlgyqbimq
1 / 10
The Atom and Elements
Ever wondered what makes up absolutely everything around you? Atoms are incredibly tiny - about 1×10⁻¹⁰ metres in radius - yet they're the building blocks of our entire universe.
Scientists have spent centuries figuring out what atoms actually look like. Dalton thought they were solid spheres, Thomson proposed the "plum pudding" model with electrons stuck in positive charge, but Rutherford's alpha scattering experiment changed everything. He fired particles at gold foil and was shocked when some bounced straight back - proving atoms have a dense, positive nucleus at their centre.
Elements contain only one type of atom, whilst compounds have different atoms chemically bonded together. Mixtures are just different substances mixed up without chemical bonds - you can separate them using physical methods like filtration for solids and liquids, or distillation for different liquids.
Key insight: Isotopes are atoms of the same element with different numbers of neutrons - they're like identical twins with different weights!
Covalent Bonding
When non-metals get together, they share electrons through covalent bonding - it's like atomic teamwork to get full outer shells. Picture two hydrogen atoms overlapping their electron shells to form H₂, sharing a pair of electrons between them.
Most covalent substances form simple molecules like water (H₂O) or methane (CH₄). These have surprisingly low melting points because whilst the covalent bonds within molecules are incredibly strong, the forces between different molecules are really weak.
However, some non-metals form giant covalent structures instead. These are completely different beasts - they have high melting points and usually don't conduct electricity because all the electrons are locked into strong covalent bonds.
Remember: Strong bonds within molecules, weak forces between molecules - that's why water boils at just 100°C!
Carbon Allotropes
Carbon is the ultimate shape-shifter - the same element can form completely different structures called allotropes, each with unique properties that'll blow your mind.
Diamond has each carbon bonded to four others in a super-strong tetrahedral network. This makes it incredibly hard with a massive melting point, but it can't conduct electricity because all electrons are tied up in bonds. Graphite takes a different approach - carbon atoms form layers of hexagons with only three bonds each, leaving delocalised electrons free to move between layers.
This gives graphite some weird properties: it's soft (layers slide over each other), conducts electricity (those free electrons!), and works great as pencil "lead". Graphene is just a single layer of graphite - incredibly strong and an excellent conductor.
Cool fact: Fullerenes like buckyballs can carry drugs safely through your body, then break apart to release them exactly where needed!
Ionic Bonding
When metals meet non-metals, electrons don't get shared - they get completely transferred in ionic bonding. The metal loses electrons to become a positive ion, whilst the non-metal gains them to become negative.
Take lithium fluoride: lithium gives up one electron (becoming Li⁺) and fluorine grabs it (becoming F⁻). These oppositely charged ions are pulled together by electrostatic attraction - imagine tiny magnets that can't let go of each other.
Ionic compounds form giant lattices with high melting points because breaking all those electrostatic attractions needs loads of energy. They only conduct electricity when molten or dissolved because the ions need to be free to move around.
Watch out: Ionic compounds are brittle - tap them wrong and the structure shifts, putting like charges next to each other, causing the whole thing to shatter!
Metallic Bonding
Pure metals have their own special bonding system that explains why they're so useful. Metal atoms lose their outer electrons, creating positive ions surrounded by a "sea" of delocalised electrons that can move freely.
The electrostatic attraction between positive metal ions and the negative electron sea creates strong bonds, giving metals high melting points. Those mobile electrons are why metals conduct electricity so well - it's like having a highway for electric current.
Group 3 metals have the highest melting points because each atom contributes three electrons to the sea, creating much stronger attractions than Group 1 or 2 metals. The mobile electrons also explain why metals are malleable - the atoms can slide past each other without breaking bonds.
Think of it: Metallic bonding is like positive ions floating in an electron soup - the ions can move positions but stay glued together by the soup!
The Periodic Table
Mendeleev was brilliant but had problems - his periodic table had gaps and some elements seemed in wrong places when arranged by atomic mass. The modern table fixes this by using atomic number instead, creating perfect patterns.
Group 1 (alkali metals) have one outer electron, making them incredibly reactive - and reactivity increases down the group. They react violently with water, producing hydrogen gas and metal hydroxides. Group 7 (halogens) need one electron to complete their shells, but reactivity decreases down the group as atoms get larger.
Group 0 (noble gases) have full outer shells, making them almost completely unreactive - they exist as single atoms. Displacement reactions happen when a more reactive halogen kicks out a less reactive one from compounds.
Pattern spotting: Down Group 1, melting points decrease but reactivity increases. Down Group 7, it's the opposite - melting points increase but reactivity decreases!
Quantitative Chemistry
Conservation of mass means atoms can't be created or destroyed in reactions - if your equation doesn't balance, you've probably got a gas escaping or being used up that you've forgotten about.
One mole contains 6.02×10²³ particles (that's Avogadro's constant) - it's chemistry's way of counting enormous numbers of atoms. Molar calculations follow a simple pattern: write the balanced equation, work out the molar ratios, calculate what you know, then use ratios to find what you need.
Concentration measures how much solute you've dissolved in a given volume of solvent. High concentration means lots of solute in little solvent - like really strong squash. Calculate it using: concentration = mass ÷ volume.
Top tip: Always convert cm³ to dm³ by dividing by 1000 - it's the most common mistake in concentration calculations!
Metal Reactions and Extraction
The reactivity series ranks metals from most reactive (potassium) to least reactive (gold). The most reactive metals explode with water, whilst unreactive ones like gold don't even react with acids.
Metal extraction depends on reactivity. Unreactive metals like gold exist naturally and can just be mined. Metals less reactive than carbon can be extracted by reduction with carbon - carbon steals oxygen from metal oxides, leaving pure metal behind.
Really reactive metals need electrolysis because carbon isn't strong enough to reduce them. In these reactions, oxidation means gaining oxygen (or losing electrons), whilst reduction means losing oxygen (or gaining electrons).
Memory trick: "OILRIG" - Oxidation Is Loss (of electrons), Reduction Is Gain (of electrons)!
Displacement Reactions
In displacement reactions, more reactive elements bully less reactive ones out of compounds - it's all about which element forms ions more easily. A reactive metal will kick out a less reactive one because it's more desperate to lose electrons.
Ionic equations show what's really happening by writing dissolved compounds as separate ions. Spectator ions don't change during the reaction, so you can remove them to see the actual chemistry happening.
Half equations show each part of the electron transfer separately. In copper sulfate + iron, the iron loses electrons (oxidation): Fe → Fe²⁺ + 2e⁻, whilst copper ions gain electrons (reduction): Cu²⁺ + 2e⁻ → Cu.
Real-world example: Iron nails go rusty in copper sulfate solution and get coated with copper metal - you can literally see the displacement happening!
Electrolysis
Electrolysis uses electricity to split up ionic compounds - it's like using electric power to force chemical reactions backwards. You need the compound molten or dissolved so ions can move freely to the electrodes.
At the cathode (negative electrode), positive metal ions gain electrons and become pure metals - this is reduction. At the anode (positive electrode), negative ions lose electrons to form pure non-metals - this is oxidation.
Aluminium extraction uses electrolysis because aluminium is too reactive for carbon reduction. The aluminium oxide gets mixed with cryolite to lower the melting point from 2000°C to 960°C, saving loads of energy.
Industrial reality: The graphite anodes slowly get eaten away because carbon reacts with oxygen to form CO₂ - they need regular replacement!
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This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.
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Anna
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Thomas R
iOS user
Just amazing. Let's me revise 10x better, this app is a quick 10/10. I highly recommend it to anyone. I can watch and search for notes. I can save them in the subject folder. I can revise it any time when I come back. If you haven't tried this app, you're really missing out.
Basil
Android user
This app has made me feel so much more confident in my exam prep, not only through boosting my own self confidence through the features that allow you to connect with others and feel less alone, but also through the way the app itself is centred around making you feel better. It is easy to navigate, fun to use, and helpful to anyone struggling in absolutely any way.
David K
iOS user
The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!
Sudenaz Ocak
Android user
In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.
Greenlight Bonnie
Android user
very reliable app to help and grow your ideas of Maths, English and other related topics in your works. please use this app if your struggling in areas, this app is key for that. wish I'd of done a review before. and it's also free so don't worry about that.
Rohan U
Android user
I know a lot of apps use fake accounts to boost their reviews but this app deserves it all. Originally I was getting 4 in my English exams and this time I got a grade 7. I didn’t even know about this app three days until the exam and it has helped A LOT. Please actually trust me and use it as I’m sure you too will see developments.
Xander S
iOS user
THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮
Elisha
iOS user
This apps acc the goat. I find revision so boring but this app makes it so easy to organize it all and then you can ask the freeeee ai to test yourself so good and you can easily upload your own stuff. highly recommend as someone taking mocks now
Paul T
iOS user
The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.
Stefan S
iOS user
This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.
Samantha Klich
Android user
Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.
Anna
iOS user
Best app on earth! no words because it’s too good
Thomas R
iOS user
Just amazing. Let's me revise 10x better, this app is a quick 10/10. I highly recommend it to anyone. I can watch and search for notes. I can save them in the subject folder. I can revise it any time when I come back. If you haven't tried this app, you're really missing out.
Basil
Android user
This app has made me feel so much more confident in my exam prep, not only through boosting my own self confidence through the features that allow you to connect with others and feel less alone, but also through the way the app itself is centred around making you feel better. It is easy to navigate, fun to use, and helpful to anyone struggling in absolutely any way.
David K
iOS user
The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!
Sudenaz Ocak
Android user
In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.
Greenlight Bonnie
Android user
very reliable app to help and grow your ideas of Maths, English and other related topics in your works. please use this app if your struggling in areas, this app is key for that. wish I'd of done a review before. and it's also free so don't worry about that.
Rohan U
Android user
I know a lot of apps use fake accounts to boost their reviews but this app deserves it all. Originally I was getting 4 in my English exams and this time I got a grade 7. I didn’t even know about this app three days until the exam and it has helped A LOT. Please actually trust me and use it as I’m sure you too will see developments.
Xander S
iOS user
THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮
Elisha
iOS user
This apps acc the goat. I find revision so boring but this app makes it so easy to organize it all and then you can ask the freeeee ai to test yourself so good and you can easily upload your own stuff. highly recommend as someone taking mocks now
Paul T
iOS user
Complete GCSE Chemistry Study Guide
Matilda Gant
@atildaant_rvlgyqbimq
Chemistry at GCSE level covers the fundamental building blocks of matter and how they interact. You'll explore everything from the tiny structure of atoms to large-scale chemical reactions that power our world.
The Atom and Elements
Ever wondered what makes up absolutely everything around you? Atoms are incredibly tiny - about 1×10⁻¹⁰ metres in radius - yet they're the building blocks of our entire universe.
Scientists have spent centuries figuring out what atoms actually look like. Dalton thought they were solid spheres, Thomson proposed the "plum pudding" model with electrons stuck in positive charge, but Rutherford's alpha scattering experiment changed everything. He fired particles at gold foil and was shocked when some bounced straight back - proving atoms have a dense, positive nucleus at their centre.
Elements contain only one type of atom, whilst compounds have different atoms chemically bonded together. Mixtures are just different substances mixed up without chemical bonds - you can separate them using physical methods like filtration for solids and liquids, or distillation for different liquids.
Key insight: Isotopes are atoms of the same element with different numbers of neutrons - they're like identical twins with different weights!
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Covalent Bonding
When non-metals get together, they share electrons through covalent bonding - it's like atomic teamwork to get full outer shells. Picture two hydrogen atoms overlapping their electron shells to form H₂, sharing a pair of electrons between them.
Most covalent substances form simple molecules like water (H₂O) or methane (CH₄). These have surprisingly low melting points because whilst the covalent bonds within molecules are incredibly strong, the forces between different molecules are really weak.
However, some non-metals form giant covalent structures instead. These are completely different beasts - they have high melting points and usually don't conduct electricity because all the electrons are locked into strong covalent bonds.
Remember: Strong bonds within molecules, weak forces between molecules - that's why water boils at just 100°C!
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Carbon Allotropes
Carbon is the ultimate shape-shifter - the same element can form completely different structures called allotropes, each with unique properties that'll blow your mind.
Diamond has each carbon bonded to four others in a super-strong tetrahedral network. This makes it incredibly hard with a massive melting point, but it can't conduct electricity because all electrons are tied up in bonds. Graphite takes a different approach - carbon atoms form layers of hexagons with only three bonds each, leaving delocalised electrons free to move between layers.
This gives graphite some weird properties: it's soft (layers slide over each other), conducts electricity (those free electrons!), and works great as pencil "lead". Graphene is just a single layer of graphite - incredibly strong and an excellent conductor.
Cool fact: Fullerenes like buckyballs can carry drugs safely through your body, then break apart to release them exactly where needed!
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Ionic Bonding
When metals meet non-metals, electrons don't get shared - they get completely transferred in ionic bonding. The metal loses electrons to become a positive ion, whilst the non-metal gains them to become negative.
Take lithium fluoride: lithium gives up one electron (becoming Li⁺) and fluorine grabs it (becoming F⁻). These oppositely charged ions are pulled together by electrostatic attraction - imagine tiny magnets that can't let go of each other.
Ionic compounds form giant lattices with high melting points because breaking all those electrostatic attractions needs loads of energy. They only conduct electricity when molten or dissolved because the ions need to be free to move around.
Watch out: Ionic compounds are brittle - tap them wrong and the structure shifts, putting like charges next to each other, causing the whole thing to shatter!
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Metallic Bonding
Pure metals have their own special bonding system that explains why they're so useful. Metal atoms lose their outer electrons, creating positive ions surrounded by a "sea" of delocalised electrons that can move freely.
The electrostatic attraction between positive metal ions and the negative electron sea creates strong bonds, giving metals high melting points. Those mobile electrons are why metals conduct electricity so well - it's like having a highway for electric current.
Group 3 metals have the highest melting points because each atom contributes three electrons to the sea, creating much stronger attractions than Group 1 or 2 metals. The mobile electrons also explain why metals are malleable - the atoms can slide past each other without breaking bonds.
Think of it: Metallic bonding is like positive ions floating in an electron soup - the ions can move positions but stay glued together by the soup!
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The Periodic Table
Mendeleev was brilliant but had problems - his periodic table had gaps and some elements seemed in wrong places when arranged by atomic mass. The modern table fixes this by using atomic number instead, creating perfect patterns.
Group 1 (alkali metals) have one outer electron, making them incredibly reactive - and reactivity increases down the group. They react violently with water, producing hydrogen gas and metal hydroxides. Group 7 (halogens) need one electron to complete their shells, but reactivity decreases down the group as atoms get larger.
Group 0 (noble gases) have full outer shells, making them almost completely unreactive - they exist as single atoms. Displacement reactions happen when a more reactive halogen kicks out a less reactive one from compounds.
Pattern spotting: Down Group 1, melting points decrease but reactivity increases. Down Group 7, it's the opposite - melting points increase but reactivity decreases!
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Quantitative Chemistry
Conservation of mass means atoms can't be created or destroyed in reactions - if your equation doesn't balance, you've probably got a gas escaping or being used up that you've forgotten about.
One mole contains 6.02×10²³ particles (that's Avogadro's constant) - it's chemistry's way of counting enormous numbers of atoms. Molar calculations follow a simple pattern: write the balanced equation, work out the molar ratios, calculate what you know, then use ratios to find what you need.
Concentration measures how much solute you've dissolved in a given volume of solvent. High concentration means lots of solute in little solvent - like really strong squash. Calculate it using: concentration = mass ÷ volume.
Top tip: Always convert cm³ to dm³ by dividing by 1000 - it's the most common mistake in concentration calculations!
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Metal Reactions and Extraction
The reactivity series ranks metals from most reactive (potassium) to least reactive (gold). The most reactive metals explode with water, whilst unreactive ones like gold don't even react with acids.
Metal extraction depends on reactivity. Unreactive metals like gold exist naturally and can just be mined. Metals less reactive than carbon can be extracted by reduction with carbon - carbon steals oxygen from metal oxides, leaving pure metal behind.
Really reactive metals need electrolysis because carbon isn't strong enough to reduce them. In these reactions, oxidation means gaining oxygen (or losing electrons), whilst reduction means losing oxygen (or gaining electrons).
Memory trick: "OILRIG" - Oxidation Is Loss (of electrons), Reduction Is Gain (of electrons)!
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Displacement Reactions
In displacement reactions, more reactive elements bully less reactive ones out of compounds - it's all about which element forms ions more easily. A reactive metal will kick out a less reactive one because it's more desperate to lose electrons.
Ionic equations show what's really happening by writing dissolved compounds as separate ions. Spectator ions don't change during the reaction, so you can remove them to see the actual chemistry happening.
Half equations show each part of the electron transfer separately. In copper sulfate + iron, the iron loses electrons (oxidation): Fe → Fe²⁺ + 2e⁻, whilst copper ions gain electrons (reduction): Cu²⁺ + 2e⁻ → Cu.
Real-world example: Iron nails go rusty in copper sulfate solution and get coated with copper metal - you can literally see the displacement happening!
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Electrolysis
Electrolysis uses electricity to split up ionic compounds - it's like using electric power to force chemical reactions backwards. You need the compound molten or dissolved so ions can move freely to the electrodes.
At the cathode (negative electrode), positive metal ions gain electrons and become pure metals - this is reduction. At the anode (positive electrode), negative ions lose electrons to form pure non-metals - this is oxidation.
Aluminium extraction uses electrolysis because aluminium is too reactive for carbon reduction. The aluminium oxide gets mixed with cryolite to lower the melting point from 2000°C to 960°C, saving loads of energy.
Industrial reality: The graphite anodes slowly get eaten away because carbon reacts with oxygen to form CO₂ - they need regular replacement!
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.
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The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.
Stefan S
iOS user
This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.
Samantha Klich
Android user
Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.
Anna
iOS user
Best app on earth! no words because it’s too good
Thomas R
iOS user
Just amazing. Let's me revise 10x better, this app is a quick 10/10. I highly recommend it to anyone. I can watch and search for notes. I can save them in the subject folder. I can revise it any time when I come back. If you haven't tried this app, you're really missing out.
Basil
Android user
This app has made me feel so much more confident in my exam prep, not only through boosting my own self confidence through the features that allow you to connect with others and feel less alone, but also through the way the app itself is centred around making you feel better. It is easy to navigate, fun to use, and helpful to anyone struggling in absolutely any way.
David K
iOS user
The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!
Sudenaz Ocak
Android user
In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.
Greenlight Bonnie
Android user
very reliable app to help and grow your ideas of Maths, English and other related topics in your works. please use this app if your struggling in areas, this app is key for that. wish I'd of done a review before. and it's also free so don't worry about that.
Rohan U
Android user
I know a lot of apps use fake accounts to boost their reviews but this app deserves it all. Originally I was getting 4 in my English exams and this time I got a grade 7. I didn’t even know about this app three days until the exam and it has helped A LOT. Please actually trust me and use it as I’m sure you too will see developments.
Xander S
iOS user
THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮
Elisha
iOS user
This apps acc the goat. I find revision so boring but this app makes it so easy to organize it all and then you can ask the freeeee ai to test yourself so good and you can easily upload your own stuff. highly recommend as someone taking mocks now
Paul T
iOS user
The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.
Stefan S
iOS user
This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.
Samantha Klich
Android user
Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.
Anna
iOS user
Best app on earth! no words because it’s too good
Thomas R
iOS user
Just amazing. Let's me revise 10x better, this app is a quick 10/10. I highly recommend it to anyone. I can watch and search for notes. I can save them in the subject folder. I can revise it any time when I come back. If you haven't tried this app, you're really missing out.
Basil
Android user
This app has made me feel so much more confident in my exam prep, not only through boosting my own self confidence through the features that allow you to connect with others and feel less alone, but also through the way the app itself is centred around making you feel better. It is easy to navigate, fun to use, and helpful to anyone struggling in absolutely any way.
David K
iOS user
The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!
Sudenaz Ocak
Android user
In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.
Greenlight Bonnie
Android user
very reliable app to help and grow your ideas of Maths, English and other related topics in your works. please use this app if your struggling in areas, this app is key for that. wish I'd of done a review before. and it's also free so don't worry about that.
Rohan U
Android user
I know a lot of apps use fake accounts to boost their reviews but this app deserves it all. Originally I was getting 4 in my English exams and this time I got a grade 7. I didn’t even know about this app three days until the exam and it has helped A LOT. Please actually trust me and use it as I’m sure you too will see developments.
Xander S
iOS user
THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮
Elisha
iOS user
This apps acc the goat. I find revision so boring but this app makes it so easy to organize it all and then you can ask the freeeee ai to test yourself so good and you can easily upload your own stuff. highly recommend as someone taking mocks now
Paul T
iOS user