GCSE Chemistry - What is an Ionic Compound? Ionic Compounds Explained #15

[@Cognitoedu]

If you’d like to practise the material covered in this video, check out our platform at www.cognitoedu.org - it's totally free, and has been built to make learning and revision as easy as possible. The main features are: - Lessons organised by topic, only the lessons relevant to your specific exam board and tier are shown. - Automatic progress tracking. Progress bars tell you what you’re doing well at, and what you need to spend some time on. - Practise quizzes so you can test your knowledge. You can quiz yourself on any combination of topics you like. - A huge number of fully-hinted questions that take you step-by-step through some of the trickiest calculations & concepts. - A comprehensive bank of past exam papers, organised both by year, and also by topic. Amadeus & Tom

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Getting ahead of the game a bit Alpha! Good luck with all your work - and great to hear they’re helping :))

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Thanks aBurntNugget, glad you're enjoying them!

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[@imperialrover]

1:10 I still don't get it. If each Na+ donates one e- to each Cl-, how can one Na+ being surrounded by 6 Cl-? I mean they should be in 1:1 ratio, right?

[@Dariakll]

Hello. Thank you for the video it was very useful and easy to follow. But I have a question I couldn't find an answer to: So, if the charge of a Catbon atom is 4+ and the charge of an Oxygen atom is 2-, in order for them to be stable, one Carbon atom would need to form an ionic compound with 2 oxygen atoms. But why is the formula for a Carbonate C03? I understand it's because it has 3 oxygen atoms and 1 carbon atom but if all a carbon needs to be stable is 2 Oxygens, why is the 3rd one there? Sorry for grammar English isn't my first language 😅

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Well we really appreciate you taking the time to comment, thanks Malak 😊

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Thank you very much very useful. I was wondering how in depth these chemistry videos are. Are they more to recap key ideas? or are they in depth enough to be everything a student would need to know for the exams?

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Thanks Alex! They're made to include everything you need to know for the exams - that said, it is worth doing further reading for deeper understanding, and practising lots of questions :)

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Haha thanks Clara! To be fair comments really help bump them up the algorithm so thanks so much for leaving one!

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Learnt more from Cognito than I ever did from my actual chemistry teachers over the course of ~4 years.

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Aw thanks jelly comments like this really do help, we appreciate it a lot 🤩

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Great to hear Abdul, good luck! 🤞

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Glad you think so! 👍

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Glad you think so, thanks for taking the time to let us know!

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Cheers, well i'm from the midlands, but lived in Australia for a few years

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Great video! i have a question: Chlorine reacts with aqueous FeCl2 to form a FeCl3 solution. Write a balanced ionic equation to show this reaction. (3 marks) could you please explain how you would get to the answer? Thank you.

[@pushparadhakrishnan7343]

Bit late but for anyone interested: Cl2 +FeCl2 -> FeCl3 Now to balance it: Cl2 + 2FeCl2 -> 2FeCl3 And with state symbols for higher tier: Cl2 (g) + 2FeCl2(aq) -> 2FeCl3 (aq)

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Thanks Timber! We're glad its making a little more sense now 😁

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Would the formula for cation and anion of an compund be the same? If not then how would we take that out?

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1:13 Amadeus is obsessed with NaCl he uses it in every example ever lol

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Hey Cognito, wouldn't it be easier to use "Criss-cross" method to show ionic compound's formula rather than using "LCM" method? I personally feel that the Criss-Cross method is easier to use... Like if you agree...

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He's showing it the long route purely for understanding purposes, otherwise criss cross method only takes a few seconds. He's going the long mile so that students understand WHY the criss cross method works.

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are these only in triple and not combined?

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Hi but how does the ionic compound structure differ from another ionic bond which is not a compond

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