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Chemical Properties: Diamond 💎 GCSE Chemistry Learning & Revision

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Manage episode 474863442 series 3139602
Content provided by Seneca Learning. All podcast content including episodes, graphics, and podcast descriptions are uploaded and provided directly by Seneca Learning or their podcast platform partner. If you believe someone is using your copyrighted work without your permission, you can follow the process outlined here https://ppacc.player.fm/legal.

In this episode, we will discuss diamonds.

Diamond, a form of carbon, is characterised by its unique structure and resulting properties.

Each carbon atom within a diamond forms strong covalent bonds with four neighbouring carbon atoms, establishing an extensive network.

This robust bonding arrangement is the underlying reason for a diamond's exceptional hardness, making it suitable for cutting applications.

Furthermore, the absence of mobile electrons within this structure means that a diamond does not conduct electricity.

Finally, due to the sheer strength and quantity of its covalent bonds, diamond exhibits a very high melting point, requiring substantial energy to break down its lattice.

Don't miss out on subscribing for more educational content tailored to help you succeed in your exams. Perfect for AQA, OCR, Edexcel, CIE and WJEC exam boards.

⁠Click here to see all of our GCSE Chemistry content!

  continue reading

196 episodes

Artwork
iconShare
 
Manage episode 474863442 series 3139602
Content provided by Seneca Learning. All podcast content including episodes, graphics, and podcast descriptions are uploaded and provided directly by Seneca Learning or their podcast platform partner. If you believe someone is using your copyrighted work without your permission, you can follow the process outlined here https://ppacc.player.fm/legal.

In this episode, we will discuss diamonds.

Diamond, a form of carbon, is characterised by its unique structure and resulting properties.

Each carbon atom within a diamond forms strong covalent bonds with four neighbouring carbon atoms, establishing an extensive network.

This robust bonding arrangement is the underlying reason for a diamond's exceptional hardness, making it suitable for cutting applications.

Furthermore, the absence of mobile electrons within this structure means that a diamond does not conduct electricity.

Finally, due to the sheer strength and quantity of its covalent bonds, diamond exhibits a very high melting point, requiring substantial energy to break down its lattice.

Don't miss out on subscribing for more educational content tailored to help you succeed in your exams. Perfect for AQA, OCR, Edexcel, CIE and WJEC exam boards.

⁠Click here to see all of our GCSE Chemistry content!

  continue reading

196 episodes

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