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Ionic Bonds

Ionic Bonds. Chemistry Mrs. Coyle. Part A:. Ions Lewis Dot Structure Stable Octet (or Duet). The Periodic Table and Atomic Radius. Valence Electrons. Valence electrons are the electrons in the highest occupied energy level of the atom.

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Ionic Bonds

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  1. Ionic Bonds Chemistry Mrs. Coyle

  2. Part A: • Ions • Lewis Dot Structure • Stable Octet (or Duet)

  3. The Periodic Table and Atomic Radius

  4. Valence Electrons • Valence electrons are the electrons in the highest occupied energy level of the atom. • Valence electrons are the only electrons generally involved in bond formation.

  5. Electron Configuration of Sodium • 1s2 2s2 2p6 3s1 • Which is the valence electron for Na? • Answer: 1s2 2s2 2p63s1

  6. Na , 11 e

  7. Na + , 10e

  8. A Positive Ion (Cation): • An atom that has lost one or more electrons. • + charge

  9. Electron Dot Structure or Lewis Dot Diagram A notation showing the valence electrons surrounding the atomic symbol.

  10. Elements within the same group have the same electron-dot structure.

  11. A Negative Ion (Anion) • An atom that has gained one or more electrons. • Negatively (-) charged.

  12. Chlorine Atom  Chlorine Ion

  13. When Na, (Z= 11) loses its valence electron, what element does its configuration look like ? Check your Neighbor • Neon • Potassium • Beryllium • Sodium

  14. When Na, (Z= 11) loses its valence electron, what element does its configuration look like ? Check your Neighbor • Neon • Potassium • Beryllium • Sodium

  15. A Stable Octet When the valence shell is full, the atom is stable, less likely to react. Example: Noble (Inert Gases) Kr

  16. Note • Atoms tend to react in a way that would lead them to have a stable octet.

  17. Part B: • Equations for Formation of Ions and Naming Ions • Ionic Bonds and Ionic Compounds

  18. Equations for the Formation of Cations H. H+ + e- Li. Li+ + e- Mg: Mg2+ + 2e-

  19. Equations for the Formation of Anions . .. : F : + e-:F -: ....

  20. Naming cations (+). • Use the name of the metal. • Example: Na+ • Sodium ion.

  21. Naming Anions(-) • Use the name of the nonmetal with the ending –ide. • Example: F- • Fluoride

  22. Ionic Compounds • Are made up of: • a metal and a nonmetal ion. • polyatomic ions.

  23. Naming Ionic Compounds, a First Look • Example: NaF • Sodium Fluoride

  24. Example: • Which of the following compounds are ionic? • NaCl • CO2 • CO • KF • KNO3

  25. Some Common Ions

  26. Bonding • Elements that do not have a complete octet, tend to react. • When the elements react bonds are formed.

  27. Types of Bonds • Ionic • Metallic • Covalent

  28. Ionic Bonds • Bonds that are formed by transfer of electrons from one element to the other. • Each element (now an ion) will have a complete octet after the transfer of electrons.

  29. The Ionic Bond • The electrical force of attraction between oppositely charged ions. F− Na+

  30. Example: Formation of Lithium Fluoride . .. Li. +: F : Li+:F -: ....

  31. Is an Ionic Compound Electrically Neutral or Charged?

  32. Movie Clip • http://www.youtube.com/watch?v=Kj3o0XvhVqQ&NR=1

  33. Chemical Formula • A representation of the kinds and number of atoms in a substance.

  34. Formula Unit • A chemical formula that shows the lowest whole number ratio of the atoms (ions) in an ionic compound. • Example:KCl, Mg Cl2

  35. The formula unit is used because ionic compounds have a lattice arrangement of ions. Ex: NaCl • Which ball represents the Na?

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