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Modern Chemistry Chapter 5 The Periodic Law

Modern Chemistry Chapter 5 The Periodic Law. Sections 1-3 History of the Periodic Table Electron Configurations and the Periodic Table Electron Configurations and Periodic Properties. Section 3. Electron Configurations and periodic properties.

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Modern Chemistry Chapter 5 The Periodic Law

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  1. Modern ChemistryChapter 5The Periodic Law Sections 1-3 History of the Periodic Table Electron Configurations and the Periodic Table Electron Configurations and Periodic Properties Chapter 5 Section 1 History of the Periodic Table pages 133-137

  2. Section 3 Electron Configurations and periodic properties Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  3. Section 3 Vocabulary Atomic radius Ion Ionization Ionization Energy Electron affinity Cation Anion Valence electrons Electronegativity Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  4. Atomic Radii • One half the distance between the nuclei of identical atoms bonded together p. 150 Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  5. Atomic Radii • Period Trend  • Atomic radii decreases across a period • Electrons are added to the s and p in the same energy level • Protons are added to the nucleus • The nucleus is stronger and pulls in the electrons making the atom smaller Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  6. Atomic Radii • Group Trend  • Atomic radii increases down a group • Exeption Al to Ga in group 13 • Electrons exist in higher energy levels further from the nucleus Practice on page 152 Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  7. Atomic radius image p. 151* Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  8. Ionization Energy • Ion: an atom or group of bonded atoms that has a positive or negative charge • Ionization: any process that results in the formation of an ion • Ionization energy: The energy required to remove one electron from a neutral atom. Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  9. ion animation Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  10. Ionization Energy • First ionization energy = IE1 (energy to remove one electron) • Diagram on Page 153 and 154 • A + energy  A+ + e- Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  11. Ionizaiton Energy Comic p. ## Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  12. Ionization energy animation Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  13. Ionization energy vs. atomic number graph p. 154 Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  14. Ionization Energy • Period Trend  • IE increases across a period • Increased nuclear charge holds e- thighter • Elements with low IE lose e- easily • Elements with high IE do not lose e- • Generally nonmetals have higher IE than metals Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  15. Ionization Energy • Group Trend  • IE decreases down a group • An electron is removed from higher energy levels further from the nucleus • In elements with many electron, the inner electrons in lower energy levels shield the outer electrons in the higher energy levels from the attraction of the nucleus Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  16. Ionization energy image Ionization Energy p. 153* Decrease Increase Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  17. Ionization Energy • Removing electrons from positive ions • More than one electron can be removed from an atom • Second ionization energy = IE2 • IE2 is higher than IE1 • Because few electrons remain to shield the outer electrons from the nucleus • Table on page 155 Practice page 156 Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  18. 1st- 5th Ionization energy chart p. 55 Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  19. Electron Affinity • The energy change that occurs when an electron is acquired by a neutral atom A + e-  A- + energy or A + e- + energy  A- • Positive or less negative EA won’t likely gain electrons • More negative EA will gain electrons easily Energy is released negative number Energy is absorbed positive number Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  20. Electron Affinity animation Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  21. Electron affinity • Period Trend  • EA increases across the period (more neg.) • Exception between group 14 and 16 Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  22. Electron affinity • Group Trend  • EA decreases down a group (less neg.) • An increase in protons increases EA but an increase in radius decreases EA Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  23. Electron Affinity image Electron Affinity p. 157* Decrease Increase Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  24. Electron affinity • Adding electrons to negative ions • More difficult to add a second eletron • All second EA are positive Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  25. Ionic Radii • Positive Ions • Cation • Loss of electron • Smaller electron cloud; loss of highest energy level • Electrons are drawn closer to the nucleus Na Na+ Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  26. Ionic Radii • Negative ion • Anions • Gaining of electrons • The electron cloud spreads out because of the repeling of electrons Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  27. ions Cation - positive Anion - negative Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  28. Ionic Radii • Period Trend  • Ionic radii decreases across a period • As protons increase the electrons are pulled in Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  29. Ionic Radii • Group Trend  • Ionic Radii increases down a group • More electrons in higher energy levels Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  30. Ionic RADIUS Image p. 159* Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  31. Valence electrons • Electrons available to be lost, gained or shared in the formation of compounds. • Located in the incompletely filled main energy level • For main group elements – outer s & p sublevels Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  32. Valence electrons animation p. ## Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  33. electronegativity • A measure of an atom in a compound to attract electrons from another atom in the compound • Linus Pauling devised a scale from 0-4. • Fluorine is the most electronegative EN = 4.0 Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  34. Electronegativities p.161 Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  35. electronegativity animation Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  36. electronegativity • Period Trend  • EN increases across a period • There are exceptions. Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  37. electronegativity • Group Trend  • EN decreases down a group Practice Page 162 Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  38. Electronegativity Electronegativity p. 160* Decrease Increase Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  39. Periodic Properties of the d and F block elements • Many exceptions in atomic radii, IE, and EN • Most d block elements from 2+ ions • Group 3 from 3+ ions • Copper forms 1+ and 2+ ions • Iron forms 2+ and 3+ ions Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

  40. Summary of trends Image Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 1 History of the Periodic Table pages 133-137

  41. Section 3 Homework Chapter 5 Section 1 History of the Periodic Table pages 133-137 Chapter 5 Section 3 Periodic Properties pages 150-164

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