Chemical changes are everywhere around you - from the rust... Show more
Chemistry118 views·Updated Jun 8, 2026·3 pagesGCSE Chemistry: Guide to Unit 4 - Chemical Changes
Erin@erin_agwa
1 / 3
1
of 3
Reactions of Metals
Metal reactivity determines how vigorously metals react with oxygen, water, and acids. When metals react with oxygen, they form metal oxides - think about how iron rusts when exposed to air and moisture.
The most reactive metals like potassium and sodium react explosively with water, producing metal hydroxides (which are alkaline) and hydrogen gas. You can test for hydrogen because it burns with a distinctive "pop" sound when lit.
Acids react with metals to produce salts and hydrogen gas. The type of salt depends on the acid used: hydrochloric acid makes chlorides, sulfuric acid makes sulfates, and nitric acid makes nitrates. For example, zinc + hydrochloric acid → zinc chloride + hydrogen.
Remember: The reactivity series goes potassium, sodium, lithium, calcium, magnesium, zinc, iron, copper (most to least reactive). Carbon and hydrogen fit between zinc and iron.
Metal compounds also react with acids. Metal oxides and carbonates both react with acids, but carbonates also produce carbon dioxide gas, which turns limewater cloudy - a useful test you'll need to remember.
2
of 3
Metal Extraction and Key Reactions
Unreactive metals like gold are found naturally as pure elements in the Earth. More reactive metals need to be extracted from their compounds using reduction with carbon, which displaces oxygen from metal oxides.
OILRIG is your key memory tool: Oxidation Is Loss, Reduction Is Gain (of electrons). When carbon removes oxygen from a metal oxide, the metal is reduced whilst carbon is oxidised.
Neutralisation happens when acids and alkalis react together, moving the pH closer to 7. Strong acids like HCl completely ionise in water, whilst weak acids like citric acid only partially ionise. The key reaction is: H⁺ + OH⁻ → H₂O.
Essential equation: At the heart of neutralisation is hydrogen ions from acids combining with hydroxide ions from alkalis to make water.
Electrolysis uses electricity to split ionic compounds. The compound (called the electrolyte) must be molten or dissolved so ions can move. Positive ions (cations) go to the negative electrode (cathode), whilst negative ions (anions) go to the positive electrode (anode).
3
of 3
Aluminium Extraction and Energy Changes
Aluminium extraction is a perfect example of electrolysis in action. Aluminium oxide is mixed with cryolite to help disrupt the lattice structure, making the process more efficient.
This process is incredibly expensive because it requires massive amounts of energy to melt the aluminium oxide and run the electrical current. The carbon electrodes also wear away and need replacing regularly.
Energy transfers happen in every chemical reaction, and energy is always conserved. Exothermic reactions release energy to the surroundings (heating them up) - think combustion, oxidation, and neutralisation reactions. These are used in self-heating cans and hand warmers.
Energy tip: If a reaction makes things warmer, it's exothermic. If it makes things cooler, it's endothermic.
Endothermic reactions absorb energy from the surroundings, cooling them down. Examples include thermal decomposition (like heating copper carbonate), mixing citric acid with sodium hydrogencarbonate, and photosynthesis in plants.
We thought you’d never ask...
What is the Knowunity AI companion?
Our AI Companion is a student-focused AI tool that offers more than just answers. Built on millions of Knowunity resources, it provides relevant information, personalised study plans, quizzes, and content directly in the chat, adapting to your individual learning journey.
Where can I download the Knowunity app?
You can download the app from Google Play Store and Apple App Store.
Is Knowunity really free of charge?
That's right! Enjoy free access to study content, connect with fellow students, and get instant help – all at your fingertips.
Most popular content: Electrolysis
9Most popular content in Chemistry
9Most popular content
9Can't find what you're looking for? Explore other subjects.
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
Chemistry118 views·Updated Jun 8, 2026·3 pagesGCSE Chemistry: Guide to Unit 4 - Chemical Changes
Erin@erin_agwa
Chemical changes are everywhere around you - from the rust forming on bikes to the energy released when you burn fuel. Understanding how metals react, how we extract them, and how energy moves during reactions will help you make sense... Show more
1
of 3Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
Reactions of Metals
Metal reactivity determines how vigorously metals react with oxygen, water, and acids. When metals react with oxygen, they form metal oxides - think about how iron rusts when exposed to air and moisture.
The most reactive metals like potassium and sodium react explosively with water, producing metal hydroxides (which are alkaline) and hydrogen gas. You can test for hydrogen because it burns with a distinctive "pop" sound when lit.
Acids react with metals to produce salts and hydrogen gas. The type of salt depends on the acid used: hydrochloric acid makes chlorides, sulfuric acid makes sulfates, and nitric acid makes nitrates. For example, zinc + hydrochloric acid → zinc chloride + hydrogen.
Remember: The reactivity series goes potassium, sodium, lithium, calcium, magnesium, zinc, iron, copper (most to least reactive). Carbon and hydrogen fit between zinc and iron.
Metal compounds also react with acids. Metal oxides and carbonates both react with acids, but carbonates also produce carbon dioxide gas, which turns limewater cloudy - a useful test you'll need to remember.
2
of 3Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
Metal Extraction and Key Reactions
Unreactive metals like gold are found naturally as pure elements in the Earth. More reactive metals need to be extracted from their compounds using reduction with carbon, which displaces oxygen from metal oxides.
OILRIG is your key memory tool: Oxidation Is Loss, Reduction Is Gain (of electrons). When carbon removes oxygen from a metal oxide, the metal is reduced whilst carbon is oxidised.
Neutralisation happens when acids and alkalis react together, moving the pH closer to 7. Strong acids like HCl completely ionise in water, whilst weak acids like citric acid only partially ionise. The key reaction is: H⁺ + OH⁻ → H₂O.
Essential equation: At the heart of neutralisation is hydrogen ions from acids combining with hydroxide ions from alkalis to make water.
Electrolysis uses electricity to split ionic compounds. The compound (called the electrolyte) must be molten or dissolved so ions can move. Positive ions (cations) go to the negative electrode (cathode), whilst negative ions (anions) go to the positive electrode (anode).
3
of 3Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
Aluminium Extraction and Energy Changes
Aluminium extraction is a perfect example of electrolysis in action. Aluminium oxide is mixed with cryolite to help disrupt the lattice structure, making the process more efficient.
This process is incredibly expensive because it requires massive amounts of energy to melt the aluminium oxide and run the electrical current. The carbon electrodes also wear away and need replacing regularly.
Energy transfers happen in every chemical reaction, and energy is always conserved. Exothermic reactions release energy to the surroundings (heating them up) - think combustion, oxidation, and neutralisation reactions. These are used in self-heating cans and hand warmers.
Energy tip: If a reaction makes things warmer, it's exothermic. If it makes things cooler, it's endothermic.
Endothermic reactions absorb energy from the surroundings, cooling them down. Examples include thermal decomposition (like heating copper carbonate), mixing citric acid with sodium hydrogencarbonate, and photosynthesis in plants.
We thought you’d never ask...
What is the Knowunity AI companion?
Our AI Companion is a student-focused AI tool that offers more than just answers. Built on millions of Knowunity resources, it provides relevant information, personalised study plans, quizzes, and content directly in the chat, adapting to your individual learning journey.
Where can I download the Knowunity app?
You can download the app from Google Play Store and Apple App Store.
Is Knowunity really free of charge?
That's right! Enjoy free access to study content, connect with fellow students, and get instant help – all at your fingertips.
Most popular content: Electrolysis
9Most popular content in Chemistry
9Most popular content
9Can't find what you're looking for? Explore other subjects.
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