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23 Dec 2025
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Understanding Relative Atomic Mass
Safir Yafi Chowdury
@safirchowdury_positiveskills
1 / 10
Understanding Isotopes and Atomic Structure
You'll often see elements like chlorine, copper, and bromine written with different numbers after their names - this isn't random! Isotopes are atoms of the same element that have identical numbers of protons and electrons but different numbers of neutrons.
Take chlorine as an example: Chlorine-35 has 17 protons, 17 electrons, and 18 neutrons, whilst Chlorine-37 has the same protons and electrons but 20 neutrons instead. Both are still chlorine because they have 17 protons, but their different neutron counts give them different mass numbers.
This concept is crucial for understanding why atomic masses aren't always whole numbers on your periodic table.
Quick Check: Remember that the number of protons determines what element you're dealing with - change that number and you get a completely different element!
What Makes Isotopes Special
Isotopes are simply different versions of the same element - think of them as siblings in the same family. They share the same number of protons and electrons (which gives them their chemical properties), but they've got different numbers of neutrons tucked away in their nucleus.
This difference in neutron count means isotopes have different mass numbers. The mass number is just the total count of protons plus neutrons in an atom's nucleus.
Here's the brilliant bit: because isotopes of the same element behave almost identically in chemical reactions, they occur together naturally in the environment. You can't separate them easily, so when you find an element in nature, you're actually getting a mixture of its isotopes.
Real World Connection: This is why a sample of chlorine from your school lab contains both Chlorine-35 and Chlorine-37 atoms mixed together!
Why Atomic Masses Aren't Whole Numbers
Here's where things get interesting - if you look at chlorine on the periodic table, its atomic mass is 35.453, not 35 or 37. You might think "hang on, you can't have half a neutron!" and you'd be absolutely right.
The answer lies in the fact that chlorine exists naturally as a mixture of isotopes. About 75% of chlorine atoms are Chlorine-35, whilst 25% are Chlorine-37.
Since we can't separate these isotopes in everyday chemistry, scientists need to use an average that reflects this natural mixture. That's why the relative atomic mass is a decimal - it's the weighted average of all the isotopes found in nature.
Key Point: The decimal atomic mass on your periodic table represents the average mass you'd actually encounter when working with that element in real life!
Understanding Relative Atomic Mass
Relative atomic mass is chemistry's way of dealing with isotope mixtures scientifically. It's defined as the average mass of an element's atoms compared to 1/12th the mass of a carbon-12 atom (which scientists use as their standard reference point).
This measurement takes into account two crucial factors: the mass numbers of all the isotopes and how abundant each isotope is in nature. It's not just a simple average - it's a weighted average that reflects real-world proportions.
Think of it like calculating your overall grade when different assignments are worth different percentages. The more common an isotope is in nature, the more it influences the final relative atomic mass value.
Study Tip: Don't confuse relative atomic mass (the average) with mass number (the mass of a single isotope) - they're related but definitely not the same thing!
Relative Atomic Mass vs Mass Number
Understanding the difference between relative atomic mass and mass number is essential for exam success. Mass number is straightforward - it's just the total protons and neutrons in one specific atom or isotope.
Relative atomic mass, however, is much more sophisticated. It's the weighted average mass of all an element's naturally occurring isotopes, compared against the carbon-12 standard.
Mass number depends only on counting particles in a single atom's nucleus. Relative atomic mass depends on the masses of different isotopes and how commonly each one appears in nature. This is why relative atomic mass values are rarely whole numbers.
Exam Alert: Questions often test whether you understand this distinction, so make sure you can explain both concepts clearly!
Real Examples: Hydrogen and Bromine
Let's look at some concrete examples that show how isotope abundance affects relative atomic mass. Hydrogen has a relative atomic mass of essentially 1 because 99% of hydrogen atoms in nature are Hydrogen-1 (just one proton, no neutrons).
Bromine tells a different story entirely. It has a relative atomic mass of about 80 because nature gives us roughly 50% Bromine-79 and 50% Bromine-81. When isotopes are present in similar amounts, the relative atomic mass sits roughly halfway between their mass numbers.
These examples show how the abundance of isotopes in nature directly determines what you see on the periodic table.
Memory Hook: If one isotope dominates (like hydrogen), the relative atomic mass stays close to that isotope's mass number. If isotopes are evenly split (like bromine), you get a value roughly in the middle!
More Examples: Chlorine and Copper
Chlorine provides a classic example of weighted averages in action. With 75% Chlorine-35 and 25% Chlorine-37, the relative atomic mass works out to 35.5 - closer to 35 because that isotope is more abundant.
Copper shows a similar pattern with 69% Copper-63 and 31% Copper-65. The relative atomic mass reflects this uneven split, sitting closer to 63 than to 65.
These percentages aren't random - they reflect billions of years of natural processes that have determined how much of each isotope exists on Earth.
Pattern Spot: Notice how the relative atomic mass always leans towards the more abundant isotope - this makes intuitive sense when you think about averages!
Understanding Chlorine's Decimal Mass
The mystery of chlorine's 35.5 relative atomic mass becomes crystal clear when you understand isotope mixing. Most chlorine atoms (about 75%) are Chlorine-35, but a significant minority (25%) are Chlorine-37.
Because a quarter of all chlorine atoms are the heavier isotope, this pulls the average mass up from 35 towards 37. The result is 35.5 - not a whole number, but a realistic reflection of what you'd actually find in a sample of chlorine.
This decimal value appears on your periodic table because it represents the mass you'd measure if you could weigh a large sample of chlorine atoms. You're not weighing individual atoms - you're weighing the mixture that exists in nature.
Real World: Every time you encounter chlorine - in swimming pools, table salt, or lab experiments - you're dealing with this 75:25 mixture of isotopes!
Calculating Relative Atomic Mass
Now for the maths bit - calculating relative atomic mass from isotope data is actually quite straightforward once you get the hang of it. For chlorine, you take 75% of 35 plus 25% of 37, then divide by 100.
The calculation looks like this: (75 × 35) + (25 × 37) ÷ 100 = 35.5. Each isotope contributes to the final answer based on how common it is in nature.
This weighted average approach means more abundant isotopes have a bigger influence on the final relative atomic mass value. It's not just adding and dividing by 2 - the percentages matter enormously.
Calculation Tip: Always multiply each mass number by its percentage abundance first, add these products together, then divide by 100 for your final answer!
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David K
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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!
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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
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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
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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
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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
Understanding Relative Atomic Mass
Safir Yafi Chowdury
@safirchowdury_positiveskills
Ever wondered why some elements on the periodic table have decimal atomic masses instead of nice whole numbers? It's all down to isotopes - atoms of the same element that have different numbers of neutrons, creating a natural mix that... Show more
Understanding Isotopes and Atomic Structure
You'll often see elements like chlorine, copper, and bromine written with different numbers after their names - this isn't random! Isotopes are atoms of the same element that have identical numbers of protons and electrons but different numbers of neutrons.
Take chlorine as an example: Chlorine-35 has 17 protons, 17 electrons, and 18 neutrons, whilst Chlorine-37 has the same protons and electrons but 20 neutrons instead. Both are still chlorine because they have 17 protons, but their different neutron counts give them different mass numbers.
This concept is crucial for understanding why atomic masses aren't always whole numbers on your periodic table.
Quick Check: Remember that the number of protons determines what element you're dealing with - change that number and you get a completely different element!
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What Makes Isotopes Special
Isotopes are simply different versions of the same element - think of them as siblings in the same family. They share the same number of protons and electrons (which gives them their chemical properties), but they've got different numbers of neutrons tucked away in their nucleus.
This difference in neutron count means isotopes have different mass numbers. The mass number is just the total count of protons plus neutrons in an atom's nucleus.
Here's the brilliant bit: because isotopes of the same element behave almost identically in chemical reactions, they occur together naturally in the environment. You can't separate them easily, so when you find an element in nature, you're actually getting a mixture of its isotopes.
Real World Connection: This is why a sample of chlorine from your school lab contains both Chlorine-35 and Chlorine-37 atoms mixed together!
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Why Atomic Masses Aren't Whole Numbers
Here's where things get interesting - if you look at chlorine on the periodic table, its atomic mass is 35.453, not 35 or 37. You might think "hang on, you can't have half a neutron!" and you'd be absolutely right.
The answer lies in the fact that chlorine exists naturally as a mixture of isotopes. About 75% of chlorine atoms are Chlorine-35, whilst 25% are Chlorine-37.
Since we can't separate these isotopes in everyday chemistry, scientists need to use an average that reflects this natural mixture. That's why the relative atomic mass is a decimal - it's the weighted average of all the isotopes found in nature.
Key Point: The decimal atomic mass on your periodic table represents the average mass you'd actually encounter when working with that element in real life!
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Understanding Relative Atomic Mass
Relative atomic mass is chemistry's way of dealing with isotope mixtures scientifically. It's defined as the average mass of an element's atoms compared to 1/12th the mass of a carbon-12 atom (which scientists use as their standard reference point).
This measurement takes into account two crucial factors: the mass numbers of all the isotopes and how abundant each isotope is in nature. It's not just a simple average - it's a weighted average that reflects real-world proportions.
Think of it like calculating your overall grade when different assignments are worth different percentages. The more common an isotope is in nature, the more it influences the final relative atomic mass value.
Study Tip: Don't confuse relative atomic mass (the average) with mass number (the mass of a single isotope) - they're related but definitely not the same thing!
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Relative Atomic Mass vs Mass Number
Understanding the difference between relative atomic mass and mass number is essential for exam success. Mass number is straightforward - it's just the total protons and neutrons in one specific atom or isotope.
Relative atomic mass, however, is much more sophisticated. It's the weighted average mass of all an element's naturally occurring isotopes, compared against the carbon-12 standard.
Mass number depends only on counting particles in a single atom's nucleus. Relative atomic mass depends on the masses of different isotopes and how commonly each one appears in nature. This is why relative atomic mass values are rarely whole numbers.
Exam Alert: Questions often test whether you understand this distinction, so make sure you can explain both concepts clearly!
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Real Examples: Hydrogen and Bromine
Let's look at some concrete examples that show how isotope abundance affects relative atomic mass. Hydrogen has a relative atomic mass of essentially 1 because 99% of hydrogen atoms in nature are Hydrogen-1 (just one proton, no neutrons).
Bromine tells a different story entirely. It has a relative atomic mass of about 80 because nature gives us roughly 50% Bromine-79 and 50% Bromine-81. When isotopes are present in similar amounts, the relative atomic mass sits roughly halfway between their mass numbers.
These examples show how the abundance of isotopes in nature directly determines what you see on the periodic table.
Memory Hook: If one isotope dominates (like hydrogen), the relative atomic mass stays close to that isotope's mass number. If isotopes are evenly split (like bromine), you get a value roughly in the middle!
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More Examples: Chlorine and Copper
Chlorine provides a classic example of weighted averages in action. With 75% Chlorine-35 and 25% Chlorine-37, the relative atomic mass works out to 35.5 - closer to 35 because that isotope is more abundant.
Copper shows a similar pattern with 69% Copper-63 and 31% Copper-65. The relative atomic mass reflects this uneven split, sitting closer to 63 than to 65.
These percentages aren't random - they reflect billions of years of natural processes that have determined how much of each isotope exists on Earth.
Pattern Spot: Notice how the relative atomic mass always leans towards the more abundant isotope - this makes intuitive sense when you think about averages!
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Understanding Chlorine's Decimal Mass
The mystery of chlorine's 35.5 relative atomic mass becomes crystal clear when you understand isotope mixing. Most chlorine atoms (about 75%) are Chlorine-35, but a significant minority (25%) are Chlorine-37.
Because a quarter of all chlorine atoms are the heavier isotope, this pulls the average mass up from 35 towards 37. The result is 35.5 - not a whole number, but a realistic reflection of what you'd actually find in a sample of chlorine.
This decimal value appears on your periodic table because it represents the mass you'd measure if you could weigh a large sample of chlorine atoms. You're not weighing individual atoms - you're weighing the mixture that exists in nature.
Real World: Every time you encounter chlorine - in swimming pools, table salt, or lab experiments - you're dealing with this 75:25 mixture of isotopes!
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Calculating Relative Atomic Mass
Now for the maths bit - calculating relative atomic mass from isotope data is actually quite straightforward once you get the hang of it. For chlorine, you take 75% of 35 plus 25% of 37, then divide by 100.
The calculation looks like this: (75 × 35) + (25 × 37) ÷ 100 = 35.5. Each isotope contributes to the final answer based on how common it is in nature.
This weighted average approach means more abundant isotopes have a bigger influence on the final relative atomic mass value. It's not just adding and dividing by 2 - the percentages matter enormously.
Calculation Tip: Always multiply each mass number by its percentage abundance first, add these products together, then divide by 100 for your final answer!
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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