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 133-137

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

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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

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

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

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

Ionization energy image 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

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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

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

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

Electron Affinity image 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

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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

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

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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

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

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

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

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

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 150-164 Chapter 5 Section 1 History of the Periodic Table pages 133-137

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

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