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Ionic BONDING

Discover the unique properties of metals, metalloids, and non-metals in ionic bonding, including noble gases, cations, anions, and the formation of ionic bonds. Learn about the characteristics and interactions of different elements.

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Ionic BONDING

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  1. Ionic • BONDING

  2. MetalsMetalloidsNon-metals

  3. Noble Gases

  4. Noble Gases • Have complete outer shells that cannot accept anymore electrons • Unreactive • Will not combine (form bonds) with any other element 2 2,8 2,8, 8 2,8, 8, 18

  5. Metal atoms • Metal atoms have incomplete outer shells • Have 1, 2 or 3 electrons on their outer shell • Metal atoms want to LOSE these extra electrons in order to have a full outer shell (like the noble gases)

  6. Metal atoms • Metal atoms lose electrons to form a CATION • CATION: when a neutral metal atom loses one or more electrons to form a positively charged ion 2,8,1  2,8

  7. Metal Cations • Possible Metal Cations: Lose 1 electron = +1 eg. K+ Lose 2 electrons = +2 eg. Ca2+ Lose 3 electrons = +3 eg. Al3+ Aluminum metal lost 3 electrons to become stable

  8. Non-metal Atoms • Non-metals have incomplete outer shells • Have 5, 6, or 7 electrons on their outer shell • Non-Metal atoms want to GAIN additional electrons in order to have a full outer shell (like the noble gases) 2, 8, 7 2, 6

  9. Non-Metal atoms • Non-Metal atoms gain electrons to form an ANION • ANION: when a neutral non-metal atom gains one or more electrons to form a negatively charged ion 2,8,7  2,8,8

  10. Non-Metal Anions • Possible Non-Metal Anions: Gain 1 electron = -1 eg. F- Gain 2 electrons = -2 eg. O2- Gain 3 electrons = -3 eg. S3- Sulfur non-metal atom gains 3 electrons to become stable

  11. Ionic Bonds • - results from the TRANSFER of electrons from a metal to a non-metal • Lithium atom needs to lose 1e- where Fluorine atom needs to gain 1e- • What a perfect match! • They will form an ionic bond! • Cations Anions

  12. Opposites Attract!!

  13. Ions are held strongly by opposite charges in a 3D lattice

  14. Properties • Highmelting points because of strong attractions between cations and anions • Soluble in water

  15. Conducts electricity because of the charged ions freely moving in water (but not in solid state)

  16. 4. Brittle – similar ions can repel if they come into contact

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