1. Period (rows) Group or Family (columns)

2. The discovery of the STM's ability to image variations in the density distribution of surface state electrons created in the artists a compulsion to have complete control of not only the atomic landscape, but the electronic landscape also. Here they have positioned 48 iron atoms into a circular ring in order to "corral" some surface state electrons and force them into "quantum" states of the circular structure. The ripples in the ring of atoms are the density distribution of a particular set of quantum states of the corral. The artists were delighted to discover that they could predict what goes on in the corral by solving the classic eigenvalue problem in quantum mechanics -- a particle in a hard-wall box.

4. Principal Energy Level Generally symbolized by n, it denotes the shell (energy level) in which the electron is located. Number of electrons that can fit in a shell: 2n 2 Energy Level 1 can hold: 2e - Energy Level 2 can hold: 8e - Energy Level 3 can hold: 18e - Energy Level 4 can hold: 32e -

5. Energy Level 1 can hold: 2e - Energy Level 2 can hold: 8e - Energy Level 3 can hold: 18e - Energy Level 4 can hold: 32e - Things to remember: The element’s period # = the # of energy levels There can only be 2 e - in the first energy level When levels 2-7 are on the OUTSIDE, they can only hold a maximum of 8 e -.

6. Energy Level 1 can hold: 2e - Energy Level 2 can hold: 8e - Energy Level 3 can hold: 18e - Energy Level 4 can hold: 32e -

7. Sublevels There are 4 sublevels – s (has 1 orbital) – p (has 3 orbitals) – d (has 5 orbitals) – f (has 7 orbitals) Each orbital can hold 2 electrons How many electrons can each sublevel hold? Can hold 2 e - Can hold 6 e - Can hold 10 e - Can hold 14 e -

8. Orbital shapes are defined as the surface that contains 90% of the total electron probability. An orbital is a region within an atom where there is a probability of finding an electron. This is a probability diagram for the s orbital in the first energy level…

9. The s orbital has a spherical shape centered around the origin of the three axes in space. s orbital shape s sublevels have 1 orbital

10. There are three dumbbell-shaped p orbitals in each energy level above n = 1, each assigned to its own axis (x, y and z) in space. P orbital shape

12. Things get a bit more complicated with the five d orbitals that are found in the d sublevels beginning with n = 3. To remember the shapes, think of “double dumbells ” …and a “dumbell with a donut”! d orbital shapes

13. Shape of f orbitals

14. Click on the link below to see orbitals added one at a time: orbital shapes and positions, one at a time orbital shapes and positions, one at a time

15. Writing Electron Configurations 3p 4 Principal Energy Level Sublevel # of e - Describes e - location.

17. Electron configuration of the elements of the first three series

18. Orbital Notation Tell where electrons are arranged in s, p, d, and f sublevel orbitals in each level around the nuclei of atoms. Use boxes to represent orbitals Use  or  to represent e -

19. Aufbau Principle Electrons occupy lowest energy orbitals first

20. Like This Pauli Exclusion Principle Only two electrons can occupy one orbital… and they must have opposite spin. Wolfgang Pauli 

21. Like This p orbitals Hund’s Rule One electron enters each orbital until all the orbitals contain one electron with the same spin direction… …then they pair up. 

22. Orbital filling table

23. Irregular configurations of Cr and Cu Chromium steals a 4s electron to half fill its 3d sublevel. Copper steals a 4s electron to FILL its 3d sublevel

24. Wave-Particle Duality His son, George Thomson won the Nobel prize for describing the wave-like nature of the electron. The electron is an energy wave! The electron is a particle! JJ Thomson won the Nobel prize for describing the electron as a particle.

25. The Wave-like Electron Louis deBroglie The electron propagates through space as an energy wave. To understand the atom, one must understand the behavior of electromagnetic waves.