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Understanding Ionic Bonds and Ion Formation in Chemistry

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francis-conley
35 diapositives · 519 Views · Nov 07, 2014

This guide covers essential concepts in chemistry, focusing on ionic bonds, the formation of cations and anions, and the significance of stable electron configurations. Learn about valence electrons, electron dot structures, and how elements interact to achieve stable octets. The guide explains the naming conventions for ions, examines ionic compounds, and how they differ from covalent bonds. Through examples such as sodium and chlorine ions, you will grasp the intricacies of ionic relationships within the periodic table.

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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?