The particle model of matterhelps explain how substances behave... Show more
Sign up to see the contentIt's free!
Access to all documents
Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Subjects
Careers
Energy transfers (a2 only)
Infection and response
Homeostasis and response
Responding to change (a2 only)
Cell biology
Organisms respond to changes in their internal and external environments (a-level only)
Biological molecules
Organisation
Substance exchange
The control of gene expression (a2 only)
Bioenergetics
Genetic information & variation
Inheritance, variation and evolution
Ecology
Cells
Show all topics
World war two & the holocaust
2m wars and welfare: britain in transition, 1906-1957
1f industrialisation and the people: britain, c1783-1885
Medieval period: 1066 -1509
1l the quest for political stability: germany, 1871-1991
Britain & the wider world: 1745 -1901
2d religious conflict and the church in england, c1529-c1570
The cold war
1c the tudors: england, 1485-1603
Inter-war germany
2j america: a nation divided, c1845-1877
2n revolution and dictatorship: russia, 1917-1953
2s the making of modern britain, 1951-2007
World war one
Britain: 1509 -1745
Show all topics
86
•
6 May 2023
•
Grace
@grace_tkup
The particle model of matterhelps explain how substances behave... Show more
The particle model of matter provides a fundamental framework for understanding how materials behave in different states. This model is crucial for students studying particle model states of matter Physics and chemistry at various levels.
In solids, particles are arranged in a rigid, organized pattern with strong forces holding them in fixed positions. These particles can only vibrate in place, which explains why solids maintain their shape and volume. This arrangement is why solids cannot be compressed - there's simply no space between particles to squeeze together further.
Liquids demonstrate an intermediate state where particles have enough energy to move past one another while maintaining relatively close proximity. This unique arrangement allows liquids to flow and take the shape of their container while remaining incompressible. The particle model states of matter explanation ks2 helps younger students visualize these concepts through simple diagrams and real-world examples.
Definition: The particle model represents matter as collections of tiny spheres that can be atoms, molecules, or ions, depending on the substance's composition.
Gases exhibit the most energetic state, with particles having sufficient energy to overcome most attractive forces between them. This explains why gases can both flow and be compressed - their particles are spread far apart with significant space between them. Understanding these principles is essential for particle model of matter Grade 8 curriculum standards.
Phase changes occur when energy is added or removed from a substance, affecting particle behavior. During melting, particles gain enough energy to break from their fixed positions in a solid to become a liquid. Conversely, freezing happens when particles lose energy and lock into fixed positions.
The process of evaporation or boiling involves particles gaining enough energy to overcome liquid phase attractions completely, becoming a gas. Condensation occurs when gas particles lose energy and return to the liquid state. These transitions are crucial concepts in the particle model states of matter explanation gcse.
Example: Water demonstrates all three states naturally on Earth: ice , liquid water, and water vapor . The transitions between these states perfectly illustrate the particle model's principles.
Understanding the difference between ionic and covalent bonds examples is crucial for comprehending matter at the molecular level. Ionic bonds form between metals and non-metals through electron transfer, while covalent bonds involve sharing electrons between non-metal atoms.
The difference between ionic and covalent compounds Class 10 becomes apparent in their properties. Ionic compounds typically form crystalline structures, have high melting points, and can conduct electricity when molten or dissolved. Covalent compounds usually exist as molecules with lower melting points and generally don't conduct electricity.
Highlight: Do ionic compounds conduct electricity when molten or dissolved? Yes, because their ions become free to move and carry charge. However, they don't conduct electricity as solids because the ions are fixed in place.
The question "Do ionic compounds conduct electricity when dissolved in water" is fundamental to understanding ionic behavior. When dissolved, ionic compounds separate into their component ions, allowing electrical current to flow. This property is crucial for many biological and industrial processes.
Why do ionic compounds not conduct electricity when solid? In their solid state, ions are locked in a crystal lattice, preventing the movement necessary for electrical conduction. However, when melted or dissolved, these ions become mobile, enabling conductivity. This explains why ionic compounds conduct electricity when molten.
Can covalent compounds conduct electricity? Generally, pure covalent compounds don't conduct electricity because they don't have free electrons or ions to carry charge. However, some exceptions exist, such as graphite, which has delocalized electrons that can carry current.
Vocabulary: Electrical conductivity in compounds depends on the presence of mobile charged particles that can carry current through the material.
When substances change state, energy transfer through heating is essential. The particle model of matter explains how particles behave during these transformations. During state changes, particles must gain sufficient energy to overcome the forces holding them together.
During melting, particles acquire energy to break some of their bonds. This allows them to move more freely while maintaining some structure. The particle model states of matter explanation gcse shows that during evaporation or boiling, particles gain even more energy to completely overcome the attractive forces between them, enabling them to escape into the gaseous state.
Definition: State changes occur when particles gain enough energy to overcome intermolecular forces, allowing them to transition between solid, liquid, and gas phases.
Ionic compounds conduct electricity when molten because ions become free to move. These compounds form when metal atoms lose electrons to become positive ions, while non-metal atoms gain electrons to form negative ions. This transfer creates strong ionic bonds between oppositely charged ions.
Do ionic compounds conduct electricity when dissolved in water? Yes, because water molecules separate the ions, allowing them to move freely and carry electrical charge. However, do ionic compounds conduct electricity when solid? No, because the ions are fixed in a crystal structure and cannot move.
Example: Table salt conducts electricity when melted or dissolved in water, but not as a solid crystal.
Covalent bonds form when non-metal atoms share electron pairs to achieve stable outer electron shells. This type of bonding is fundamental to understanding what is a particle model in Chemistry. Unlike ionic compounds, most covalently bonded substances form discrete molecules.
The difference between ionic and covalent bonds examples is clear in their structure and properties. While ionic compounds form crystal lattices, covalent compounds typically exist as individual molecules. This explains why can covalent compounds conduct electricity usually results in "no" - they lack the free charged particles necessary for electrical conduction.
Highlight: Covalent bonds involve electron sharing between non-metals, while ionic bonds involve electron transfer between metals and non-metals.
The 3 differences between ionic and covalent compounds include their bonding mechanism, electrical conductivity, and physical properties. Ionic compounds typically have higher melting points than covalent compounds due to the strong electrostatic forces between ions.
Understanding how ionic compounds conduct electricity class 10 involves recognizing that electrical conductivity requires both charged particles and mobility. This explains why do ionic compounds not conduct electricity when solid - the ions are locked in place. The similarities between ionic and covalent bonds include their goal of achieving stable electron configurations, though they accomplish this through different mechanisms.
Vocabulary: Ionic bonds result from electron transfer between metals and non-metals, while covalent bonds involve electron sharing between non-metals.
The particle model of matter Physics helps us understand how different substances behave at various temperatures and their ability to conduct electricity. When examining substances with simple molecular structures, we observe distinct patterns in their physical properties and behavior.
Simple molecular substances typically exhibit low melting and boiling points due to the weak intermolecular forces between their particles. This characteristic of the particle model states of matter explains why many of these substances exist as liquids or gases at room temperature. For instance, water molecules have relatively weak bonds between them, allowing them to transition between states more easily than substances with stronger intermolecular forces.
Definition: Melting and boiling points are specific temperatures at which substances change their state of matter. These changes require energy transfer to overcome the forces holding particles together.
The ability of substances to conduct electricity depends on specific conditions related to their particle arrangement. Do ionic compounds conduct electricity when molten is a common question, and the answer lies in understanding two crucial factors. First, the substance must contain charged particles . Second, these charged particles must have the freedom to move within the substance. This explains why ionic compounds conduct electricity when dissolved in water but not in their solid state.
Example: Table salt is an excellent illustration of these principles:
Understanding the difference between ionic and covalent bonds examples is crucial for predicting a substance's electrical properties. Ionic compounds form through the transfer of electrons between metals and non-metals, creating oppositely charged ions held together by electrostatic forces. In contrast, covalent compounds share electrons between non-metal atoms.
The 3 differences between ionic and covalent compounds become particularly evident when examining their electrical conductivity. Ionic compounds, when molten or dissolved, can conduct electricity because their charged particles become mobile. However, can covalent compounds conduct electricity is typically answered no, as they generally lack free charged particles. This fundamental difference stems from their bonding structure and particle arrangement.
Highlight: Why do ionic compounds not conduct electricity when solid? In their solid state, ionic compounds have their ions fixed in a rigid crystal lattice, preventing the movement necessary for electrical conduction. However, how ionic compounds conduct electricity gcse studies show that when these compounds melt or dissolve, the ions become free to move, enabling electrical conductivity.
The practical applications of these properties are extensive in both industry and everyday life. For example, understanding ionic vs covalent metal or non-metal interactions helps in designing better batteries, developing more efficient electrical systems, and creating new materials with specific conductivity properties. This knowledge forms the foundation for many modern technological advances in electronics and materials science.
App Store
Google 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 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
Grace
@grace_tkup
The particle model of matter helps explain how substances behave in different states and how chemical bonds form between atoms. This fundamental concept is crucial for understanding both basic and advanced chemistry concepts.
In the particle model of matter,... Show more
Access to all documents
Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
The particle model of matter provides a fundamental framework for understanding how materials behave in different states. This model is crucial for students studying particle model states of matter Physics and chemistry at various levels.
In solids, particles are arranged in a rigid, organized pattern with strong forces holding them in fixed positions. These particles can only vibrate in place, which explains why solids maintain their shape and volume. This arrangement is why solids cannot be compressed - there's simply no space between particles to squeeze together further.
Liquids demonstrate an intermediate state where particles have enough energy to move past one another while maintaining relatively close proximity. This unique arrangement allows liquids to flow and take the shape of their container while remaining incompressible. The particle model states of matter explanation ks2 helps younger students visualize these concepts through simple diagrams and real-world examples.
Definition: The particle model represents matter as collections of tiny spheres that can be atoms, molecules, or ions, depending on the substance's composition.
Access to all documents
Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Gases exhibit the most energetic state, with particles having sufficient energy to overcome most attractive forces between them. This explains why gases can both flow and be compressed - their particles are spread far apart with significant space between them. Understanding these principles is essential for particle model of matter Grade 8 curriculum standards.
Phase changes occur when energy is added or removed from a substance, affecting particle behavior. During melting, particles gain enough energy to break from their fixed positions in a solid to become a liquid. Conversely, freezing happens when particles lose energy and lock into fixed positions.
The process of evaporation or boiling involves particles gaining enough energy to overcome liquid phase attractions completely, becoming a gas. Condensation occurs when gas particles lose energy and return to the liquid state. These transitions are crucial concepts in the particle model states of matter explanation gcse.
Example: Water demonstrates all three states naturally on Earth: ice , liquid water, and water vapor . The transitions between these states perfectly illustrate the particle model's principles.
Access to all documents
Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Understanding the difference between ionic and covalent bonds examples is crucial for comprehending matter at the molecular level. Ionic bonds form between metals and non-metals through electron transfer, while covalent bonds involve sharing electrons between non-metal atoms.
The difference between ionic and covalent compounds Class 10 becomes apparent in their properties. Ionic compounds typically form crystalline structures, have high melting points, and can conduct electricity when molten or dissolved. Covalent compounds usually exist as molecules with lower melting points and generally don't conduct electricity.
Highlight: Do ionic compounds conduct electricity when molten or dissolved? Yes, because their ions become free to move and carry charge. However, they don't conduct electricity as solids because the ions are fixed in place.
Access to all documents
Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
The question "Do ionic compounds conduct electricity when dissolved in water" is fundamental to understanding ionic behavior. When dissolved, ionic compounds separate into their component ions, allowing electrical current to flow. This property is crucial for many biological and industrial processes.
Why do ionic compounds not conduct electricity when solid? In their solid state, ions are locked in a crystal lattice, preventing the movement necessary for electrical conduction. However, when melted or dissolved, these ions become mobile, enabling conductivity. This explains why ionic compounds conduct electricity when molten.
Can covalent compounds conduct electricity? Generally, pure covalent compounds don't conduct electricity because they don't have free electrons or ions to carry charge. However, some exceptions exist, such as graphite, which has delocalized electrons that can carry current.
Vocabulary: Electrical conductivity in compounds depends on the presence of mobile charged particles that can carry current through the material.
Access to all documents
Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
When substances change state, energy transfer through heating is essential. The particle model of matter explains how particles behave during these transformations. During state changes, particles must gain sufficient energy to overcome the forces holding them together.
During melting, particles acquire energy to break some of their bonds. This allows them to move more freely while maintaining some structure. The particle model states of matter explanation gcse shows that during evaporation or boiling, particles gain even more energy to completely overcome the attractive forces between them, enabling them to escape into the gaseous state.
Definition: State changes occur when particles gain enough energy to overcome intermolecular forces, allowing them to transition between solid, liquid, and gas phases.
Access to all documents
Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Ionic compounds conduct electricity when molten because ions become free to move. These compounds form when metal atoms lose electrons to become positive ions, while non-metal atoms gain electrons to form negative ions. This transfer creates strong ionic bonds between oppositely charged ions.
Do ionic compounds conduct electricity when dissolved in water? Yes, because water molecules separate the ions, allowing them to move freely and carry electrical charge. However, do ionic compounds conduct electricity when solid? No, because the ions are fixed in a crystal structure and cannot move.
Example: Table salt conducts electricity when melted or dissolved in water, but not as a solid crystal.
Access to all documents
Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Covalent bonds form when non-metal atoms share electron pairs to achieve stable outer electron shells. This type of bonding is fundamental to understanding what is a particle model in Chemistry. Unlike ionic compounds, most covalently bonded substances form discrete molecules.
The difference between ionic and covalent bonds examples is clear in their structure and properties. While ionic compounds form crystal lattices, covalent compounds typically exist as individual molecules. This explains why can covalent compounds conduct electricity usually results in "no" - they lack the free charged particles necessary for electrical conduction.
Highlight: Covalent bonds involve electron sharing between non-metals, while ionic bonds involve electron transfer between metals and non-metals.
Access to all documents
Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
The 3 differences between ionic and covalent compounds include their bonding mechanism, electrical conductivity, and physical properties. Ionic compounds typically have higher melting points than covalent compounds due to the strong electrostatic forces between ions.
Understanding how ionic compounds conduct electricity class 10 involves recognizing that electrical conductivity requires both charged particles and mobility. This explains why do ionic compounds not conduct electricity when solid - the ions are locked in place. The similarities between ionic and covalent bonds include their goal of achieving stable electron configurations, though they accomplish this through different mechanisms.
Vocabulary: Ionic bonds result from electron transfer between metals and non-metals, while covalent bonds involve electron sharing between non-metals.
Access to all documents
Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
The particle model of matter Physics helps us understand how different substances behave at various temperatures and their ability to conduct electricity. When examining substances with simple molecular structures, we observe distinct patterns in their physical properties and behavior.
Simple molecular substances typically exhibit low melting and boiling points due to the weak intermolecular forces between their particles. This characteristic of the particle model states of matter explains why many of these substances exist as liquids or gases at room temperature. For instance, water molecules have relatively weak bonds between them, allowing them to transition between states more easily than substances with stronger intermolecular forces.
Definition: Melting and boiling points are specific temperatures at which substances change their state of matter. These changes require energy transfer to overcome the forces holding particles together.
The ability of substances to conduct electricity depends on specific conditions related to their particle arrangement. Do ionic compounds conduct electricity when molten is a common question, and the answer lies in understanding two crucial factors. First, the substance must contain charged particles . Second, these charged particles must have the freedom to move within the substance. This explains why ionic compounds conduct electricity when dissolved in water but not in their solid state.
Example: Table salt is an excellent illustration of these principles:
Access to all documents
Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Understanding the difference between ionic and covalent bonds examples is crucial for predicting a substance's electrical properties. Ionic compounds form through the transfer of electrons between metals and non-metals, creating oppositely charged ions held together by electrostatic forces. In contrast, covalent compounds share electrons between non-metal atoms.
The 3 differences between ionic and covalent compounds become particularly evident when examining their electrical conductivity. Ionic compounds, when molten or dissolved, can conduct electricity because their charged particles become mobile. However, can covalent compounds conduct electricity is typically answered no, as they generally lack free charged particles. This fundamental difference stems from their bonding structure and particle arrangement.
Highlight: Why do ionic compounds not conduct electricity when solid? In their solid state, ionic compounds have their ions fixed in a rigid crystal lattice, preventing the movement necessary for electrical conduction. However, how ionic compounds conduct electricity gcse studies show that when these compounds melt or dissolve, the ions become free to move, enabling electrical conductivity.
The practical applications of these properties are extensive in both industry and everyday life. For example, understanding ionic vs covalent metal or non-metal interactions helps in designing better batteries, developing more efficient electrical systems, and creating new materials with specific conductivity properties. This knowledge forms the foundation for many modern technological advances in electronics and materials science.
App Store
Google 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 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