1. Using the Quantum Model

2. Periodic Table

3. Periodic Trends Atomic Radius: Increases down a group and decreases across a period Ionization Energy (energy required to remove an electron from the atom): Decreases down a group and increases across a period

4. Ions Cations: lose electrons, electron configuration of the cation is the noble gas core General group 1: [NG]ns 1  [NG] + +1e - Anions: gain electrons, electron configuration of anion is the following noble gas on the periodic table General group 17: [NG] ns 2 np 5 +1e -  [NG] ns 2 np 6 Become isoelectric to the noble gas (same number of electrons)

5. Magnetism: classified by strongest magnetic property Diamagnetic: weak interaction with a magnetic field, material is slightly repelled by magnetic field – All material has diamagnetic properties Paramagnetic: material is attracted into the magnetic field, single electron in an orbital (unpaired electron) Ferromagnetic: material is attracted to a magnet or form magnetic material. Higher number of unpaired electrons.

6. Anomelies Pairing raises the energy slightly, a half filled subshell and a full filled subshell lower the energy (gaining some stability) Possibilities: Will half fill both s and d orbitals (Cr, Mo, W) Will half fill s orbital and fill d orbital (Cu, Ag, Au) Will fill d orbital and have empty s orbital (Pd)

7. Applications of Quantum Mechanics

8. Lasers Uses Planks theory: excite electrons and when they relax back to ground state the photon released produces light

9. MRI’s Magnetic resonance imaging: uses nuclear magnetic resonance principles Aligns the spins to one direction in the body using a large magnet, followed by a pulse to alter the alignment Nuclei produce a magnetic field which is detected to create an image when they relax