1 / 43

Understanding Ions and Ionic Bonding

Learn about ions, their formation, and ionic bonding. Discover how ions are charged particles and how atoms gain or lose electrons to form ions. Understand the properties of ionic compounds and the forces of attraction between ions in lattice structures.

wbays
Download Presentation

Understanding Ions and Ionic Bonding

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. S2 Science Ions and Ionic Bonding

  2. Learning Outcomes • We are Learning about ionic bonding

  3. Success Criteria • I can describe what an ion is and describe their formation • I can describe an ionic bond and explain that it usually consists of a metal/non-metal combination • I can state that ionic substances form lattice structures • I can state that the forces of attraction between oppositely charged ions in a lattice structure are strong • I can state the properties of ionic compounds

  4. Ions • Ions are charged particles

  5. Ions • Ions are charged particles • The simplest ions are atoms that have lost or gained electrons

  6. Ions • Ions are charged particles • The simplest ions are atoms that have lost or gained electrons • Atoms lose or gain electrons to become like the noble gasses

  7. Why Ions Form • The lithium atom has the electron configuration 2,1 • The target diagram would be - Li 3+ 2,1

  8. Why Ions Form • To achieve the stable electron arrangement of the noble gas the lithium atom would have to lose its outer electron.

  9. Why Ions Form • The lithium ion has the electron configuration of just 2 • The target diagram would be - 3+ 2 Li+

  10. Why Ions Form • The lithium ion now has the same electron configuration as helium and so is very stable.

  11. Why Ions Form • It has 3 protons but only 2 electrons • The extra proton gives it a positive charge.

  12. Why Ions Form • The fluorine atom has 7 electrons in its outer shell • The target diagram would be - 9+ 2,7 F

  13. Why Ions Form • To become like the noble gases it must either lose or gain electrons.

  14. Why Ions Form • To become like the noble gases it must either lose or gain electrons. • It cannot lose 7 electrons so it must gain just 1 to complete the shell

  15. Why Ions Form • The fluoride ion has 8 electrons in its outer shell • The target diagram would be - 9+ 2,8 F-

  16. Why Ions Form • The fluorine ion has 10 electrons and 9 protons.

  17. Why Ions Form • The fluoride ion has 10 electrons and 9 protons. • The extra electron gives it a negative charge.

  18. Ions Summary • Metals lose electrons to form positive ions.

  19. Ions Summary • Metals lose electrons to form positive ions. • Non metals gain electrons to become negative ions.

  20. Ions Summary • Metals lose electrons to form positive ions. • Non metals gain electrons to become negative ions. • Metal and non-metal ions attract each other to form ionic compounds

  21. Ions Summary • Metals lose electrons to form positive ions. • Non metals gain electrons to become negative ions. • Metal and non-metal ions attract each other to form ionic compounds • The attraction between positive and negative ions is called the ionic bond.

  22. Ions Summary

  23. Ions Summary

  24. Ions Summary

  25. The Ionic Bond • Sodium chloride is a typical ionic compound • Sodium forms a positive ion Na+ • Chlorine forms a negative ion Cl- • The negative chloride ion is attracted strongly to the positive sodium ion

  26. Conductivity tests

  27. Conductivity tests

  28. Conductivity tests • Compounds which contain only non metals do not conduct electricity.

  29. Conductivity tests • All metals conduct electricity

  30. Conductivity tests • All metals conduct electricity • Compounds containing metals do not conduct when solid but do conduct when molten or in solution

  31. Conductivity tests • All metals conduct electricity • Compounds containing metals do not conduct when solid but do conduct when molten or in solution • These compounds are called ionic compounds

  32. Compounds • Ionic compounds contain ions

  33. Compounds • Ionic compounds contain ions • Only when the ions can move freely will the compound conduct electricity

  34. Compounds • Ionic compounds contain ions • Only when the ions can move freely will the compound conduct electricity • In a solid the ions cannot move and so cannot conduct electricity

  35. Electrolysis • Electrolysis means the breaking up of a compound by the action of electricity. (‘electro’ = electricity; ‘lysis’ = breaking apart)

  36. Electrolysis DC Carbon electrodes copper chloride

  37. Electrolysis of copper chloride

  38. Electrolysis of copper chloride

  39. Electrolysis of copper chloride • The metal copper was formed at the negative rod • The gas chlorine was formed at the positive rod.

  40. Ions on the move • An electrolyte is a liquid or solution that conducts electricity by ions moving through it. • An electrode is a rod where the electricity enters or leaves the electrolyte.

  41. Ions on the move • The ions always move towards oppositely charged electrodes.

  42. Ions on the move • The ions always move towards oppositely charged electrodes. • Positive metal ions move towards the negative electrode

  43. Ions on the move • The ions always move towards oppositely charged electrodes. • Positive metal ions move towards the negative electrode • Negative non metal ions move towards the positive electrode

More Related