This GCSE Chemistry cheat sheet covers the essential concepts you'll...
Chemistry4,528 views·Updated 10 Sept 2026·2 pagesAQA GCSE Chemistry: Must-Know Cheat Sheet for Paper 1 Higher
Rebecca Thenderton@rebecca_mvvh
1
of 2
Chemical Changes and Energy
Acids and bases are everywhere in chemistry, and understanding them is crucial for your exams. Acids have a low pH because they produce H⁺ ions, while bases neutralise acids with their OH⁻ ions. The key equation to remember is: acid + base → salt + water.
When it comes to strong vs weak acids, don't confuse strength with concentration. Strong acids like hydrochloric acid (HCl) completely break apart in water, whilst weak acids like ethanoic acid only partially split up. This affects how they react, not how much acid you've got.
Electrolysis might seem tricky, but remember PANIC - Positive Anode Negative Is Cathode. Metals form positive ions and head to the negative cathode, while non-metals form negative ions and go to the positive anode. You'll need this for describing what happens during electrolysis.
Quick Tip: For electrolysis questions, always mention the ion, its charge, electrons gained/lost, and the element formed!
Energy changes split into two camps: exothermic reactions (release energy, temperature goes up) like combustion, and endothermic reactions (absorb energy, temperature drops) like dissolving. Fuel cells are brilliant because they only produce water as waste, though storing hydrogen is still a challenge.
2
of 2
Atomic Structure and Bonding
Your periodic table knowledge starts with knowing that proton number determines the element - this never changes. Isotopes are the same element with different neutrons, which is why relative atomic mass calculations pop up in exams using abundance percentages.
Mendeleev was clever enough to leave gaps in his periodic table and predict missing elements, unlike earlier scientists who just arranged by mass. Today's version uses atomic number, where group number equals outer shell electrons and period equals number of shells.
Chemical bonding comes in three flavours: ionic (metal + non-metal, electrons transferred), covalent (non-metals sharing electrons), and metallic (delocalised electrons). Each creates different properties - giant structures have high melting points, while simple covalent molecules have low melting points.
Memory Aid: Remember "I Have No Clever Or Brainy Friends" for diatomic elements (I₂, H₂, N₂, Cl₂, O₂, Br₂, F₂)!
Quantitative chemistry calculations follow the same pattern: work out Mr, calculate moles of what you know, find the ratio, then calculate what you need. For concentration calculations, remember that 1000 cm³ = 1 dm³, and always show your working - you'll get marks even if the final answer isn't perfect.
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Chemistry4,528 views·Updated 10 Sept 2026·2 pagesAQA GCSE Chemistry: Must-Know Cheat Sheet for Paper 1 Higher
Rebecca Thenderton@rebecca_mvvh
This GCSE Chemistry cheat sheet covers the essential concepts you'll need for Paper 1, focusing on chemical changes, energy reactions, atomic structure, bonding, and quantitative chemistry. These topics form the foundation of chemistry and directly link to exam questions you'll...
1
of 2
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Chemical Changes and Energy
Acids and bases are everywhere in chemistry, and understanding them is crucial for your exams. Acids have a low pH because they produce H⁺ ions, while bases neutralise acids with their OH⁻ ions. The key equation to remember is: acid + base → salt + water.
When it comes to strong vs weak acids, don't confuse strength with concentration. Strong acids like hydrochloric acid (HCl) completely break apart in water, whilst weak acids like ethanoic acid only partially split up. This affects how they react, not how much acid you've got.
Electrolysis might seem tricky, but remember PANIC - Positive Anode Negative Is Cathode. Metals form positive ions and head to the negative cathode, while non-metals form negative ions and go to the positive anode. You'll need this for describing what happens during electrolysis.
Quick Tip: For electrolysis questions, always mention the ion, its charge, electrons gained/lost, and the element formed!
Energy changes split into two camps: exothermic reactions (release energy, temperature goes up) like combustion, and endothermic reactions (absorb energy, temperature drops) like dissolving. Fuel cells are brilliant because they only produce water as waste, though storing hydrogen is still a challenge.
2
of 2Sign up to see the content. It's free!
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By signing up you accept Terms of Service and Privacy Policy
Atomic Structure and Bonding
Your periodic table knowledge starts with knowing that proton number determines the element - this never changes. Isotopes are the same element with different neutrons, which is why relative atomic mass calculations pop up in exams using abundance percentages.
Mendeleev was clever enough to leave gaps in his periodic table and predict missing elements, unlike earlier scientists who just arranged by mass. Today's version uses atomic number, where group number equals outer shell electrons and period equals number of shells.
Chemical bonding comes in three flavours: ionic (metal + non-metal, electrons transferred), covalent (non-metals sharing electrons), and metallic (delocalised electrons). Each creates different properties - giant structures have high melting points, while simple covalent molecules have low melting points.
Memory Aid: Remember "I Have No Clever Or Brainy Friends" for diatomic elements (I₂, H₂, N₂, Cl₂, O₂, Br₂, F₂)!
Quantitative chemistry calculations follow the same pattern: work out Mr, calculate moles of what you know, find the ratio, then calculate what you need. For concentration calculations, remember that 1000 cm³ = 1 dm³, and always show your working - you'll get marks even if the final answer isn't perfect.
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Students love us, and so will you.
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