1. 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
Chapter 5 Section 1 History of the Periodic Table pages

2. Electron Configurations and periodic properties
Section 3
Electron Configurations and periodic properties
Chapter 5 Section 3 Periodic Properties pages
Chapter 5 Section 1 History of the Periodic Table pages

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

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

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 3 Periodic Properties pages
Chapter 5 Section 1 History of the Periodic Table pages

6. Atomic Radii Group Trend  Practice on page 152
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 3 Periodic Properties pages
Chapter 5 Section 1 History of the Periodic Table pages

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

8. Ionization: any process that results in the formation of an ion
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 3 Periodic Properties pages
Chapter 5 Section 1 History of the Periodic Table pages

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

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

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

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

13. Ionization energy vs. atomic number graph
Chapter 5 Section 1 History of the Periodic Table pages
Chapter 5 Section 1 History of the Periodic Table pages

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 3 Periodic Properties pages
Chapter 5 Section 1 History of the Periodic Table pages

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 3 Periodic Properties pages
Chapter 5 Section 1 History of the Periodic Table pages

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

17. Removing electrons from positive ions
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 3 Periodic Properties pages
Chapter 5 Section 1 History of the Periodic Table pages

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

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 3 Periodic Properties pages
Chapter 5 Section 1 History of the Periodic Table pages

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

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

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 3 Periodic Properties pages
Chapter 5 Section 1 History of the Periodic Table pages

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

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

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 3 Periodic Properties pages
Chapter 5 Section 1 History of the Periodic Table pages

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

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

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

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

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

31. Located in the incompletely filled main energy level
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 3 Periodic Properties pages
Chapter 5 Section 1 History of the Periodic Table pages

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

33. Linus Pauling devised a scale from 0-4.
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 3 Periodic Properties pages
Chapter 5 Section 1 History of the Periodic Table pages

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

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

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

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

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

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 3 Periodic Properties pages
Chapter 5 Section 1 History of the Periodic Table pages

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

41. Section 3 Homework
Chapter 5 Section 3 Periodic Properties pages
Chapter 5 Section 1 History of the Periodic Table pages