Chemistry is all about understanding the building blocks of everything...
Chemistry361 views·Updated 18 Jul 2026·8 pagesGCSE Chemistry Paper 1 Higher Notes
B
B.Y.@erranur_shsqboxebbht
1 / 8
1
of 8
Atoms and Basic Chemistry Concepts
Everything you touch is made of atoms - they're literally the building blocks of the universe. An element contains only one type of atom (like pure oxygen or magnesium), whilst a compound has different atoms chemically bonded together (like water, which is hydrogen and oxygen stuck together).
Mixtures are completely different because the substances aren't chemically bonded - think of air, which is just different gases floating about together. You can separate mixtures using various techniques, but compounds need chemical reactions to break apart.
Matter exists in three main states - solid, liquid, and gas. In solids, particles vibrate in fixed positions like people in assigned cinema seats. Liquids let particles move past each other freely, whilst gases have particles zooming around randomly at high speeds with loads of space between them.
Remember: You need energy (heat) to overcome the forces holding particles together when melting or evaporating substances!
The history of atomic structure is like a detective story. John Dalton started it all, then JJ Thompson proposed the "plum pudding model." Ernest Rutherford discovered the tiny, positively charged nucleus by firing particles at gold foil, and Niels Bohr worked out that electrons exist in energy levels around the nucleus.
2
of 8
Atomic Structure and the Periodic Table
Protons have a +1 charge and mass of 1, neutrons are neutral with mass 1, and electrons have a -1 charge but virtually no mass. Think of the atom like a football stadium - the nucleus is a marble in the centre, and electrons orbit around the outside.
The atomic number tells you how many protons an element has (carbon always has 6). The mass number is protons plus neutrons added together. For an atom to be neutral, it needs equal numbers of protons and electrons - if not, it becomes an ion.
Isotopes are like twins with different weights - same element, but different numbers of neutrons. Some relative atomic masses aren't whole numbers because they're averages of all the isotopes that exist naturally.
Top tip: The periodic table is arranged by atomic number, not mass - Dmitri Mendeleev figured this out!
Metals always donate electrons to get empty outer shells, forming positive ions (like Na+). Non-metals accept electrons to get full outer shells, forming negative ions or sharing electrons instead.
3
of 8
Groups in the Periodic Table and Chemical Bonding
Group 1 metals (alkali metals) get more reactive as you go down because their outer electron is further from the nucleus, making it easier to lose. They all form +1 ions and react vigorously with water.
Group 7 elements (halogens) do the opposite - they get less reactive going down the group but their boiling points increase. They form -1 ions by accepting one electron. Group 0 (noble gases) are practically unreactive because they already have full outer shells.
Metallic bonding creates a lattice of metal ions surrounded by a "sea" of delocalised electrons. Since electrons can move freely, metals conduct electricity and heat brilliantly - that's why your radiators are metal!
Key concept: In ionic bonding, metals donate electrons to non-metals, creating oppositely charged ions that attract each other strongly.
Ionic compounds have high melting points because you need loads of energy to break those strong ionic bonds. The charges in any ionic compound must always add up to zero - it's like balancing a equation!
4
of 8
Covalent Bonding and Giant Structures
Covalent bonding happens when non-metals share electrons to get full outer shells - it's like sharing your lunch so you both get fed! Every covalent bond consists of a pair of shared electrons, and you can show this using dot and cross diagrams.
Simple covalent substances have low boiling points because you only need to break weak forces between molecules, not the actual covalent bonds. Think of it like unsticking Post-it notes rather than tearing them in half.
Giant covalent structures are massive networks of atoms all bonded together - imagine a spider's web that goes on forever! These have very high melting points because you'd have to break actual covalent bonds.
Amazing fact: Diamond is one of the hardest substances known because of its incredibly strong covalent bonds in all directions!
Graphite can conduct electricity because it has delocalised electrons, and its layers can slide past each other (that's why pencils work). Alloys are stronger than pure metals because different-sized atoms disrupt the regular structure, preventing layers from sliding easily.
5
of 8
Chemical Reactions and the Reactivity Series
Displacement reactions happen when a more reactive metal kicks out a less reactive one from a compound - it's like queue-jumping but for atoms! Most metals react with acids to produce a salt and hydrogen gas, whilst metal carbonates give you a salt, carbon dioxide, and water.
The reactivity series is like a league table for metals - the higher up, the more reactive. You can use this to predict which displacement reactions will happen and which won't.
Diamond is incredibly hard due to its strong bonds in all directions. Graphite has delocalised electrons forming weak bonds between layers, so it conducts electricity and the layers can slide (making it perfect for pencil lead).
Cool applications: Fullerenes and nanotubes are used in electronics, composites, and medical purposes because of their unique cage-like structures.
Understanding these structures helps explain why different forms of carbon have such different properties despite being made of exactly the same atoms!
6
of 8
Oxidation, Reduction, and Electrolysis
Remember "OILRIG" - Oxidation Is Loss, Reduction Is Gain (of electrons). Even when oxygen isn't involved, we still use these terms for any reaction where electrons are transferred between atoms or ions.
Neutralisation happens when acids (pH < 7) react with alkalis (pH > 7) to produce a salt and water . The pH scale runs from 1-14, and each step represents a 10× change in hydrogen ion concentration - that's a massive difference!
Electrolysis uses electrical current to force chemical reactions by attracting ions to oppositely charged electrodes. The positive anode and negative cathode cause oxidation and reduction respectively.
Important: Electrolysis only works when ions can move freely - so ionic compounds must be molten or dissolved in solution.
For molten compounds, you get the pure elements. With solutions, it's trickier because water interferes - halide ions are always oxidised at the anode, whilst hydrogen ions (being less reactive than most metals) are reduced at the cathode.
7
of 8
Electrolysis of Solutions Continued
When electrolyzing solutions, halide ions (F⁻, Cl⁻, Br⁻) are always oxidised at the anode. If there's no halide present, oxygen gets oxidised instead, producing oxygen gas. Meanwhile, H⁺ ions are usually reduced at the cathode because they're less reactive than most metal ions.
The more reactive metal ions stay dissolved in solution whilst the less reactive ones get reduced. This is why you can extract some metals but not others using electrolysis of solutions.
Exothermic reactions release energy and get hot because there's a net decrease in potential energy, which converts to kinetic energy (heat). Endothermic reactions absorb energy and get cold as kinetic energy converts to potential energy.
Practical tip: You can find the exact neutralisation point by reacting acid with increasing volumes of alkali and measuring maximum temperature - the peak shows perfect neutralisation!
Activation energy is like the initial push needed to get a reaction started - imagine pushing a boulder over a hill before it rolls down the other side.
8
of 8
Energy Changes and Bond Energies
The energy change in a reaction depends on the difference between energy needed to break bonds and energy released when forming new bonds. If more energy is released than used, the reaction is exothermic (gets hot). If more energy is needed than released, it's endothermic (gets cold).
You can calculate energy changes using bond energies - just add up all the energy needed to break reactant bonds, then subtract all the energy released making product bonds. A negative answer means exothermic, positive means endothermic.
Required practical work involves reacting acids with alkalis and measuring temperature changes. Plot a graph of temperature against volume of alkali added - the peak shows you the exact neutralisation point.
Exam tip: Always show your working clearly in bond energy calculations - even if you get the final answer wrong, you can still get marks for the correct method!
Understanding energy changes helps explain why some reactions happen spontaneously whilst others need constant heating. It's all about energy balance and whether the products are more or less stable than the reactants.
We thought you’d never ask...
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.
You can download the app from Google Play Store and Apple App Store.
That's right! Enjoy free access to study content, connect with fellow students, and get instant help – all at your fingertips.
Similar content
Most popular content: Covalent Network Solids
5ChemistryBonding and Structure Overview
Explore the key concepts of chemical bonding, including ionic, covalent, and metallic bonds, as well as the properties of various structures such as giant covalent and molecular compounds. This summary covers essential topics for GCSE Chemistry Unit 2, focusing on the relationships between bonding types and material properties.
1086120
ChemistryUnderstanding Giant Covalent Structures
Explore the properties and characteristics of giant covalent structures, including diamond, graphite, graphene, and fullerenes. This summary covers key concepts such as covalent bonds, carbon allotropes, and their electrical conductivity. Ideal for GCSE Chemistry students seeking to grasp the fundamentals of covalent network solids.
92145
ChemistryChemical Bonding Explained
Explore the fundamentals of chemical bonding, including ionic, covalent, and metallic structures. This summary covers the properties of solids, liquids, and gases, the formation of compounds, and the significance of giant covalent structures and nanoparticles. Ideal for AQA GCSE Chemistry Higher students seeking to understand the intricacies of molecular interactions and material properties.
957512
ChemistryBonding Structures & Properties
Explore the intricacies of bonding structures and their properties in matter. This summary covers giant covalent structures, ionic bonds, metallic bonds, and the unique characteristics of materials like graphite, diamond, and polymers. Understand how these structures influence conductivity, melting points, and physical states. Ideal for AQA Combined Science students preparing for exams.
111065
ChemistryGraphite Properties Overview
Explore the unique properties of graphite, a carbon allotrope known for its high melting and boiling points, softness, and excellent conductivity. This summary covers the structure of graphite, including covalent bonding and the role of delocalised electrons in its electrical and thermal conductivity. Ideal for students studying carbon allotropes and covalent network solids.
9521
Most popular content in Chemistry
9G
ChemistryGCSE AQA Chemistry Topic 1- The Atom
The Atom
101,2910
Chemistrychem paper 1
higher
112,10444
ChemistryA-level OCR A Chemistry summary sheets
Everything from snaprevise for OCR chemistry a-level
122,32379
C
Chemistrychem paper 1
Unlock the secrets of chemical reactions with this comprehensive flashcard set designed to help you conquer complex concepts and ace your Chemistry exams.
117261
ChemistryChemistry paper 2
Chem paper 2 notes
1172714
A
ChemistryAQA GCSE Chemistry 4.4 Chemical changes
4.4 Reactions of acids with bases or carbonates
97621
ChemistryEssential Chemistry Practicals
Explore key AQA GCSE Chemistry practicals, including flame tests, titration, and gas identification. This resource covers essential techniques for analyzing ions, making salts, and understanding reaction kinetics. Perfect for students preparing for exams and practical assessments.
1011,973902
A
ChemistryAtomic Mass and Atomic Number Calculations
Calculate the number of protons, neutrons, and electrons for different elements and isotopes.
S34950
F
ChemistryFundamentals of Atomic Structure
Practice identifying subatomic particles, calculating neutrons, and defining isotopes and atomic/mass numbers.
123460
Most popular content
9
SociologySociology of Education Overview
Explore comprehensive A-Level Sociology notes on the education system, covering key theories, policies, and sociological perspectives. This resource includes insights on marketisation, gender roles, cultural deprivation, and educational inequalities, providing a thorough understanding of how education shapes social stratification and individual achievement. Ideal for exam preparation and in-depth study.
12102,9583,041
SociologySociology of Families: Comprehensive Revision
Dive into an extensive overview of family dynamics, perspectives, and patterns in sociology. This resource covers key concepts such as family diversity, gender roles, marriage, and the impact of social policies on family structures. Perfect for A-Level Sociology students preparing for Paper 2.
1273,7532,307
CriminologyCriminology: Crime & Punishment Overview
Comprehensive mindmaps covering key concepts in the Crime and Punishment topic for WJEC Criminology Unit 4. This resource includes detailed insights into the Criminal Justice System, crime prevention strategies, sentencing models, and the roles of various agencies. Ideal for A-Level revision, ensuring you grasp essential theories and legislative processes to excel in your exams.
1254,8941,060
SociologyComprehensive Crime & Deviance Overview
Explore an extensive revision of crime and deviance topics, including theories, types of crime, and the impact of media. This resource covers key concepts such as Marxism, functionalism, gender and crime, and the influence of globalization on criminal behavior. Ideal for students seeking a thorough understanding of criminology and its various theories. Type: Full Topic Revision.
1251,6691,400
C
BiologyCell Biology and Cell structure
cell structures
93,2810
CriminologyWJEC Unit 4 Criminology
Criminology unit 4 detailed revision note
127,176125
SociologySociological Theories Overview
Comprehensive revision of key sociological theories including Functionalism, Marxism, Feminism, and Interpretivism. Explore concepts like value freedom, identity formation, and the critique of social control. Ideal for AQA A-Level Sociology students preparing for exams. This summary covers essential theories and their implications in sociology, providing a clear understanding of each perspective.
1231,480846
T
BiologyThe functions of subcellular structures - B1 Biology
Flashcards on the different functions of subcellular structures: cell membrane, nucleus, mitochondria, ribosomes, cytoplasm, permant vacuole, chloroplasts and cell wall.
102,8215
1
Biology1.cells Gcse biology question cards
combined science higher biology
92,3644
Students love us — and so will you.
4.6/5App Store
4.7/5Google Play
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 SiOS 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 KlichAndroid 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.
AnnaiOS user
Chemistry361 views·Updated 18 Jul 2026·8 pagesGCSE Chemistry Paper 1 Higher Notes
B
B.Y.@erranur_shsqboxebbht
Chemistry is all about understanding the building blocks of everything around you - from the air you breathe to your mobile phone! This unit covers the fundamental concepts that explain how atoms combine to form compounds, how energy changes in...
1
of 8
Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Atoms and Basic Chemistry Concepts
Everything you touch is made of atoms - they're literally the building blocks of the universe. An element contains only one type of atom (like pure oxygen or magnesium), whilst a compound has different atoms chemically bonded together (like water, which is hydrogen and oxygen stuck together).
Mixtures are completely different because the substances aren't chemically bonded - think of air, which is just different gases floating about together. You can separate mixtures using various techniques, but compounds need chemical reactions to break apart.
Matter exists in three main states - solid, liquid, and gas. In solids, particles vibrate in fixed positions like people in assigned cinema seats. Liquids let particles move past each other freely, whilst gases have particles zooming around randomly at high speeds with loads of space between them.
Remember: You need energy (heat) to overcome the forces holding particles together when melting or evaporating substances!
The history of atomic structure is like a detective story. John Dalton started it all, then JJ Thompson proposed the "plum pudding model." Ernest Rutherford discovered the tiny, positively charged nucleus by firing particles at gold foil, and Niels Bohr worked out that electrons exist in energy levels around the nucleus.
2
of 8Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Atomic Structure and the Periodic Table
Protons have a +1 charge and mass of 1, neutrons are neutral with mass 1, and electrons have a -1 charge but virtually no mass. Think of the atom like a football stadium - the nucleus is a marble in the centre, and electrons orbit around the outside.
The atomic number tells you how many protons an element has (carbon always has 6). The mass number is protons plus neutrons added together. For an atom to be neutral, it needs equal numbers of protons and electrons - if not, it becomes an ion.
Isotopes are like twins with different weights - same element, but different numbers of neutrons. Some relative atomic masses aren't whole numbers because they're averages of all the isotopes that exist naturally.
Top tip: The periodic table is arranged by atomic number, not mass - Dmitri Mendeleev figured this out!
Metals always donate electrons to get empty outer shells, forming positive ions (like Na+). Non-metals accept electrons to get full outer shells, forming negative ions or sharing electrons instead.
3
of 8Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Groups in the Periodic Table and Chemical Bonding
Group 1 metals (alkali metals) get more reactive as you go down because their outer electron is further from the nucleus, making it easier to lose. They all form +1 ions and react vigorously with water.
Group 7 elements (halogens) do the opposite - they get less reactive going down the group but their boiling points increase. They form -1 ions by accepting one electron. Group 0 (noble gases) are practically unreactive because they already have full outer shells.
Metallic bonding creates a lattice of metal ions surrounded by a "sea" of delocalised electrons. Since electrons can move freely, metals conduct electricity and heat brilliantly - that's why your radiators are metal!
Key concept: In ionic bonding, metals donate electrons to non-metals, creating oppositely charged ions that attract each other strongly.
Ionic compounds have high melting points because you need loads of energy to break those strong ionic bonds. The charges in any ionic compound must always add up to zero - it's like balancing a equation!
4
of 8Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Covalent Bonding and Giant Structures
Covalent bonding happens when non-metals share electrons to get full outer shells - it's like sharing your lunch so you both get fed! Every covalent bond consists of a pair of shared electrons, and you can show this using dot and cross diagrams.
Simple covalent substances have low boiling points because you only need to break weak forces between molecules, not the actual covalent bonds. Think of it like unsticking Post-it notes rather than tearing them in half.
Giant covalent structures are massive networks of atoms all bonded together - imagine a spider's web that goes on forever! These have very high melting points because you'd have to break actual covalent bonds.
Amazing fact: Diamond is one of the hardest substances known because of its incredibly strong covalent bonds in all directions!
Graphite can conduct electricity because it has delocalised electrons, and its layers can slide past each other (that's why pencils work). Alloys are stronger than pure metals because different-sized atoms disrupt the regular structure, preventing layers from sliding easily.
5
of 8Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Chemical Reactions and the Reactivity Series
Displacement reactions happen when a more reactive metal kicks out a less reactive one from a compound - it's like queue-jumping but for atoms! Most metals react with acids to produce a salt and hydrogen gas, whilst metal carbonates give you a salt, carbon dioxide, and water.
The reactivity series is like a league table for metals - the higher up, the more reactive. You can use this to predict which displacement reactions will happen and which won't.
Diamond is incredibly hard due to its strong bonds in all directions. Graphite has delocalised electrons forming weak bonds between layers, so it conducts electricity and the layers can slide (making it perfect for pencil lead).
Cool applications: Fullerenes and nanotubes are used in electronics, composites, and medical purposes because of their unique cage-like structures.
Understanding these structures helps explain why different forms of carbon have such different properties despite being made of exactly the same atoms!
6
of 8Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Oxidation, Reduction, and Electrolysis
Remember "OILRIG" - Oxidation Is Loss, Reduction Is Gain (of electrons). Even when oxygen isn't involved, we still use these terms for any reaction where electrons are transferred between atoms or ions.
Neutralisation happens when acids (pH < 7) react with alkalis (pH > 7) to produce a salt and water . The pH scale runs from 1-14, and each step represents a 10× change in hydrogen ion concentration - that's a massive difference!
Electrolysis uses electrical current to force chemical reactions by attracting ions to oppositely charged electrodes. The positive anode and negative cathode cause oxidation and reduction respectively.
Important: Electrolysis only works when ions can move freely - so ionic compounds must be molten or dissolved in solution.
For molten compounds, you get the pure elements. With solutions, it's trickier because water interferes - halide ions are always oxidised at the anode, whilst hydrogen ions (being less reactive than most metals) are reduced at the cathode.
7
of 8Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Electrolysis of Solutions Continued
When electrolyzing solutions, halide ions (F⁻, Cl⁻, Br⁻) are always oxidised at the anode. If there's no halide present, oxygen gets oxidised instead, producing oxygen gas. Meanwhile, H⁺ ions are usually reduced at the cathode because they're less reactive than most metal ions.
The more reactive metal ions stay dissolved in solution whilst the less reactive ones get reduced. This is why you can extract some metals but not others using electrolysis of solutions.
Exothermic reactions release energy and get hot because there's a net decrease in potential energy, which converts to kinetic energy (heat). Endothermic reactions absorb energy and get cold as kinetic energy converts to potential energy.
Practical tip: You can find the exact neutralisation point by reacting acid with increasing volumes of alkali and measuring maximum temperature - the peak shows perfect neutralisation!
Activation energy is like the initial push needed to get a reaction started - imagine pushing a boulder over a hill before it rolls down the other side.
8
of 8Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Energy Changes and Bond Energies
The energy change in a reaction depends on the difference between energy needed to break bonds and energy released when forming new bonds. If more energy is released than used, the reaction is exothermic (gets hot). If more energy is needed than released, it's endothermic (gets cold).
You can calculate energy changes using bond energies - just add up all the energy needed to break reactant bonds, then subtract all the energy released making product bonds. A negative answer means exothermic, positive means endothermic.
Required practical work involves reacting acids with alkalis and measuring temperature changes. Plot a graph of temperature against volume of alkali added - the peak shows you the exact neutralisation point.
Exam tip: Always show your working clearly in bond energy calculations - even if you get the final answer wrong, you can still get marks for the correct method!
Understanding energy changes helps explain why some reactions happen spontaneously whilst others need constant heating. It's all about energy balance and whether the products are more or less stable than the reactants.
We thought you’d never ask...
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.
You can download the app from Google Play Store and Apple App Store.
That's right! Enjoy free access to study content, connect with fellow students, and get instant help – all at your fingertips.
Similar content
Most popular content: Covalent Network Solids
5ChemistryBonding and Structure Overview
Explore the key concepts of chemical bonding, including ionic, covalent, and metallic bonds, as well as the properties of various structures such as giant covalent and molecular compounds. This summary covers essential topics for GCSE Chemistry Unit 2, focusing on the relationships between bonding types and material properties.
1086120
ChemistryUnderstanding Giant Covalent Structures
Explore the properties and characteristics of giant covalent structures, including diamond, graphite, graphene, and fullerenes. This summary covers key concepts such as covalent bonds, carbon allotropes, and their electrical conductivity. Ideal for GCSE Chemistry students seeking to grasp the fundamentals of covalent network solids.
92145
ChemistryChemical Bonding Explained
Explore the fundamentals of chemical bonding, including ionic, covalent, and metallic structures. This summary covers the properties of solids, liquids, and gases, the formation of compounds, and the significance of giant covalent structures and nanoparticles. Ideal for AQA GCSE Chemistry Higher students seeking to understand the intricacies of molecular interactions and material properties.
957512
ChemistryBonding Structures & Properties
Explore the intricacies of bonding structures and their properties in matter. This summary covers giant covalent structures, ionic bonds, metallic bonds, and the unique characteristics of materials like graphite, diamond, and polymers. Understand how these structures influence conductivity, melting points, and physical states. Ideal for AQA Combined Science students preparing for exams.
111065
ChemistryGraphite Properties Overview
Explore the unique properties of graphite, a carbon allotrope known for its high melting and boiling points, softness, and excellent conductivity. This summary covers the structure of graphite, including covalent bonding and the role of delocalised electrons in its electrical and thermal conductivity. Ideal for students studying carbon allotropes and covalent network solids.
9521
Most popular content in Chemistry
9G
ChemistryGCSE AQA Chemistry Topic 1- The Atom
The Atom
101,2910
Chemistrychem paper 1
higher
112,10444
ChemistryA-level OCR A Chemistry summary sheets
Everything from snaprevise for OCR chemistry a-level
122,32379
C
Chemistrychem paper 1
Unlock the secrets of chemical reactions with this comprehensive flashcard set designed to help you conquer complex concepts and ace your Chemistry exams.
117261
ChemistryChemistry paper 2
Chem paper 2 notes
1172714
A
ChemistryAQA GCSE Chemistry 4.4 Chemical changes
4.4 Reactions of acids with bases or carbonates
97621
ChemistryEssential Chemistry Practicals
Explore key AQA GCSE Chemistry practicals, including flame tests, titration, and gas identification. This resource covers essential techniques for analyzing ions, making salts, and understanding reaction kinetics. Perfect for students preparing for exams and practical assessments.
1011,973902
A
ChemistryAtomic Mass and Atomic Number Calculations
Calculate the number of protons, neutrons, and electrons for different elements and isotopes.
S34950
F
ChemistryFundamentals of Atomic Structure
Practice identifying subatomic particles, calculating neutrons, and defining isotopes and atomic/mass numbers.
123460
Most popular content
9SociologySociology of Education Overview
Explore comprehensive A-Level Sociology notes on the education system, covering key theories, policies, and sociological perspectives. This resource includes insights on marketisation, gender roles, cultural deprivation, and educational inequalities, providing a thorough understanding of how education shapes social stratification and individual achievement. Ideal for exam preparation and in-depth study.
12102,9583,041
SociologySociology of Families: Comprehensive Revision
Dive into an extensive overview of family dynamics, perspectives, and patterns in sociology. This resource covers key concepts such as family diversity, gender roles, marriage, and the impact of social policies on family structures. Perfect for A-Level Sociology students preparing for Paper 2.
1273,7532,307
CriminologyCriminology: Crime & Punishment Overview
Comprehensive mindmaps covering key concepts in the Crime and Punishment topic for WJEC Criminology Unit 4. This resource includes detailed insights into the Criminal Justice System, crime prevention strategies, sentencing models, and the roles of various agencies. Ideal for A-Level revision, ensuring you grasp essential theories and legislative processes to excel in your exams.
1254,8941,060
SociologyComprehensive Crime & Deviance Overview
Explore an extensive revision of crime and deviance topics, including theories, types of crime, and the impact of media. This resource covers key concepts such as Marxism, functionalism, gender and crime, and the influence of globalization on criminal behavior. Ideal for students seeking a thorough understanding of criminology and its various theories. Type: Full Topic Revision.
1251,6691,400
C
BiologyCell Biology and Cell structure
cell structures
93,2810
CriminologyWJEC Unit 4 Criminology
Criminology unit 4 detailed revision note
127,176125
SociologySociological Theories Overview
Comprehensive revision of key sociological theories including Functionalism, Marxism, Feminism, and Interpretivism. Explore concepts like value freedom, identity formation, and the critique of social control. Ideal for AQA A-Level Sociology students preparing for exams. This summary covers essential theories and their implications in sociology, providing a clear understanding of each perspective.
1231,480846
T
BiologyThe functions of subcellular structures - B1 Biology
Flashcards on the different functions of subcellular structures: cell membrane, nucleus, mitochondria, ribosomes, cytoplasm, permant vacuole, chloroplasts and cell wall.
102,8215
1
Biology1.cells Gcse biology question cards
combined science higher biology
92,3644
Students love us — and so will you.
4.6/5App Store
4.7/5Google Play
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 SiOS 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 KlichAndroid 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.
AnnaiOS user