I.         Periodic Properties of the Elements

II.        Periodic Properties

            A.        Related to repeating e^- configuration

            B.        Increase in valence e^-

            C.        Shielding

            D.        Properties repeat

III.       Examples

            A.        Density

            B.        Atomic Radius

            C.        Boiling Point

            D.        Melting Point

IV.      Reaction Tendencies

            A.        Ionization Energy

            B.        Electron Affinity

V.        Patterns in Size: Atomic Radius

            A.        Distance from nucleus to outer level

VI.      Atomic Radius: Down column

            A.        Increases

            B.        Distance inverse to force

            C.        Full levels shield e^- from nucleus

VII.     Atomic Radius: Across row

            A.        Decreases

            B.        Both p⁺ and e^- increase

            C.        Increase q direct to force

VIII.    Transition Metals

            A.        Filling d sublevel increases shielding

            B.        Atomic radius increases

IX.      Noble Gas Exception

            A.        Outer e^- on adjacent atoms interact

            B.        Atom compressed

            C.        Noble gas outer level full

            D.        No interaction, no compression

X.        Ionic Radius

            A.        Mimic noble gas configuration

            B.        Lose e^-, greater attraction

            C.        Gain e^-, lower attraction

            D.        Increase down column

            E.        Decrease across row

XI.      Oxidation Numbers

            A.        Gain or lose e^- to produce noble gas configuration

XII.     Groups 1,2,13

            A.        Matches number of e^- in outer level

            B.        Outer level only s and p

XIII.    Groups 3-12

            A.        Lose outer level e^- first

            B.        d1 to d5: lose e^- until d empty

            C.        d6 to d9: lose e^- until d half full

XIV.   Group 14

            A.        Have 4 e^-

            B.        Share e^-

XV.     Groups 15 to 17

            A.        Gain e^- to fill outer level

            B.        Oxidation number in number needed to fill level

XVI.   Chemical Reactivity

            A.        Related to gain or loss of electrons

            B.        Metals: Ionization Energy

            C.        Non-Metals: Electron Affinity

XVII.  Ionization Energy

            A.        Energy required to remove an electron

XVIII. Factors Affecting Ionization Energy

            A.        Nuclear charge

            B.        Radius

            C.        Shielding effect

            D.        Sublevel

XIX.   First Ionization Energy

            A.        Increases across row

                        1.         Nuclear charge increases

                        2.         Field Strength increases

            B.        Decreases down row

                        1.         Radius increases

                        2.         Shielding increases

            C.        Low for metals, high reactivity

XX.     Other Ionization Energies

            A.        Fewer e^-, stronger nuclear pull

            B.        Atom more stable, need more energy

XXI.   An Example: Al

            A.        1s²2s²2p⁶3s²3p¹

            B.        3p¹ electron easily removed

            C.        3s subshell is full and stable

            D.        More energy required to remove

XXII.  Metals

            A.        Lose electrons

            B.        Good conductors

            C.        Form ionic bonds

XXIII. Alkali Metals

            A.        Soft, silver/white, good conductors

            B.        Lose s¹ electron

            C.        Reactivity increases down column

            D.        React readily with O

            E.        React violently with H₂O

XXIV. Alkaline Earth Metals

            A.        Too reactive to occur in nature

            B.        Must lose 2 s electrons, more energy needed

            C.        More stable than Alkali

            D.        Denser, harder, higher BP and MP

XXV.  Electron Affinity

            A.        Attraction of an atom for more e^-

            B.        Affected by same factors as Ionization Energy

            C.        Decreases as e^- are gained

XXVI. Electron Affinity: Columns

            A.        r increases

            B.        Field strength drops

            C.        Electron affinity drops

XXVII.           Electron Affinity: Rows

            A.        Charge increases

            B.        Field strength increases

            C.        Electron affinity increases

XXVIII.          Exceptions to Trend

            A.        Be: Full 2s sublevel

            B.        N: ½ full 2p sublevel

            C.        Ne: full outer level

XXIX. Non-Metals

            A.        Gain electrons

            B.        Poor conductors

            C.        Form covalent bonds

            D.        Group 14 shares or gains

XXX.  Most Reactive

            A.        Halogens: gain 1

            B.        Oxygen: gain 2