Syllabus: Periodic Table, (Inorganic Chemistry): Chemistry 2261, 1261 Spring 2015

Keith H. Pannell, PS 309, 747-5796; [email protected] (Cell phone 539-3730)

Room PS 403: Tuesday/Thursday; 10.30 – 11.50; Monday 4.00 – 700 PM.

Office Hours: Tu, Tr. 9.30 – 10.15 AM; Fri. 3.00 – 4.00 PM or by appointment

Book: The Periodic Table, Pannell and Haiduc, available from the Library Copy Center.

There will be a final comprehensive examination which includes an interactive oral portion involving, inter alia, a Periodic Table “Darts” segment. Homework may be given as may be student presentations, and quizzes. Remember the drop date is APRIL 6th. The topics outlined below in blue are a small extension from your coverage in the Introductory Freshman Chemistry courses. I anticipate you will need to refresh your memory prior to the Periodic Table class next week. Please do so since I will not extend much coverage to these previously covered aspects.

ATOMIC PROPERTIES The electronic structure of atoms: The Periodic Table Periodic relationships of the properties of the atomic elements. Shielding and Effective Nuclear Charge. Electron movement: ionization energies, electron affinity, electronegativity.

ATOMIC BONDING Simple molecular orbital theory of bonding The valence bond approach Hypervalency or valence shell expansion Other forms of bonding interactions Dipole-dipole interactions Hydrogen bonding London dispersion forces (Van der Waals interactions) Bond energies

THE SIZES OF ATOMS AND MOLECULES Bond lengths Atomic sizes

THE SHAPES OF MOLECULES Structures of predominantly covalent molecules The valence shell electron pair repulsion theory (VSEPR) Structures of predominantly ionic molecules The radius ratio rule Covalency of ionic compounds

REPRESENTATIVE CHEMISTRY OF THE GROUPS 1 – 18.

Group 1: Enthalpy of hydration; electrostatic potentials; solution “size” versus solid state size; ionophore selectivity.

Group 2: Enthalpy of hydration continued; bridging Cl in BeCl2; BeMe2 (polymeric organometallic compound with 3 center 2 electron bonds).

Group 13: 3 center 2 electron bonds for boranes; AlCl3 dimer structure with bridging Cl atoms; 2 exchange of Cl and F in BF3 / BCl3 mixtures; “inert” 6s pair for Tl (also for Pb and Bi in groups 14 and 15).

Group 14: Singlet and triplet ER2; thermodynamic stability of, but kinetic lability of, Si-Cl cf C- Cl bonds; reaction mechanisms; increased coordination numbers by acid-base interactions. The nature of a “double bond”

Group 15: Hypervalency ( e.g. PF3, PF5); Berry pseudo rotation via square pyramid transition states; the nature of “structure” as a function of T; fluxional molecules.

Group 16: Your call.

Group 17: Hypervalency, polyhalides (cations and anions); mono-, tri-, penta- and hepta-valency

Group 18: Not so inert!; I and Xe very similar behaviour; the rôle of π- bonding in O compounds. charged compounds.

Transition metals: Crystal Field approach; breaking of d-orbital degeneracy (non-equivalence of d-electrons (shielding or deshielding wrt to size?); hydration energy variations as a function of d-orbital electron count. Always remember that your communication skills must be on a par with your knowledge, otherwise your knowledge can remain a secret!