1. Electron Orbitals Cartoon courtesy of lab-initio.com

2. Quantum Mechanical Model of the Atom Mathematical laws can identify the regions outside of the nucleus where electrons are most likely to be found. These laws are beyond the scope of this class…

3. Heisenberg Uncertainty Principle The more certain you are about where the electron is, the less certain you can be about where it is going. The more certain you are about where the electron is going, the less certain you can be about where it is. “One cannot simultaneously determine both the position and momentum of an electron.” Werner Heisenberg

4. Quantum Numbers Each electron in an atom has a unique set of 4 quantum numbers which describe it.  Principal quantum number  Angular momentum quantum number  Magnetic quantum number  Spin quantum number

5. Electron Energy Level (Shell) Principle Quantum number Generally symbolized by n, it denotes the probable distance of the electron from the nucleus. “n” is also known as the Principle Quantum number Number of electrons that can fit in a shell: 2n 2

6. Orbital shapes are defined as the surface that contains 90% of the total electron probability. An orbital is a region within an energy level where there is a probability of finding an electron. Electron Orbitals The angular momentum quantum number, generally symbolized by l, denotes the orbital (subshell) in which the electron is located.

7. The s orbital ( l = 0) has a spherical shape centered around the origin of the three axes in space. s Orbital shape

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

9. Things get a bit more complicated with the five d orbitals ( l = 2) 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

10. Shape of f ( l = 3) orbitals

11. Energy Level (n) Sublevels in main energy level (n sublevels) Number of orbitals per sublevel Number of Electrons per sublevel Number of electrons per main energy level (2n 2 ) 1s122 2spsp 1313 2626 8 3spdspd 135135 2 6 10 18 4spdfspdf 13571357 2 6 10 14 32 Energy Levels, Sublevels, Electrons

12. Magnetic Quantum Number magnetic quantum number The magnetic quantum number, generally symbolized by m, denotes the orientation of the electron’s orbital with respect to the three axes in space.

13. Orbital filling table

14. Electron Spin The Spin Quantum Number The Spin Quantum Number describes the behavior (direction of spin) of an electron within a magnetic field. Possibilities for electron spin:

15. Pauli Exclusion Principle Two electrons occupying the same orbital must have opposite spins Wolfgang Pauli

16. Assigning the Numbers  The three quantum numbers (n, l, and m) are integers.  The principal quantum number (n) cannot be zero.  n must be 1, 2, 3, etc.  The angular momentum quantum number ( l ) can be any integer between 0 and n - 1.  For n = 3, l can be either 0, 1, or 2.  The magnetic quantum number (m l ) can be any integer between - l and + l.  For l = 2, m can be either -2, -1, 0, +1, +2.

17. Quantum numbers for the first four levels of orbitals in the hydrogen atom n l Orbital designation mlml # of orbitals 101s01 202s01 12p-1, 0, 13 303s01 13p-1, 0, 13 23d-2, -1, 0, 1, 25 404s01 14p-1, 0, 13 24d-2, -1, 0, 1, 25 34f-3, -2, -1, 0, 1, 2, 37

18. ElementConfiguration notation Orbital notationNoble gas notation Lithium1s 2 2s 1 ____ ____ ____ ____ ____ 1s 2s 2p [He]2s 1 Beryllium1s 2 2s 2 ____ ____ ____ ____ ____ 1s 2s 2p [He]2s 2 Boron1s 2 2s 2 p 1 ____ ____ ____ ____ ____ 1s 2s 2p [He]2s 2 p 1 Carbon1s 2 2s 2 p 2 ____ ____ ____ ____ ____ 1s 2s 2p [He]2s 2 p 2 Nitrogen1s 2 2s 2 p 3 ____ ____ ____ ____ ____ 1s 2s 2p [He]2s 2 p 3 Oxygen1s 2 2s 2 p 4 ____ ____ ____ ____ ____ 1s 2s 2p [He]2s 2 p 4 Fluorine1s 2 2s 2 p 5 ____ ____ ____ ____ ____ 1s 2s 2p [He]2s 2 p 5 Neon1s 2 2s 2 p 6 ____ ____ ____ ____ ____ 1s 2s 2p [He]2s 2 p 6