1. Quantum Numbers: Much better than stupid cat jokes

2. How did your results compare to the probability plot? Mechanical Wave Lab results

3. The Quantum Numbers The principal quantum number is n It describes what energy level the electron is located in (n=1 is smallest (closest to nucleus). n also describes the number of sublevels contained in that energy level and the maximum number of electrons contained in that energy level Principal energy level (n) Number of sublevels (n) Number of orbitals present Total number of orbitals (n) 2 Maximum number of electrons ( 2n 2 ) 111 - - - 1 2 221 3 - - 4 8 331 3 5 - 9 18 441 3 5 7 16 32 s p d f The value of n is used to calculate the total number of orbitals and the maximum # of electrons

4. n # also tells # of subshells or orbitals e.g. n= 1 has 1 orbital (s) n= 2 has 2 orbitals (s, p) n= 3 has 3 orbitals (s,p,d) n= 4 has 4 orbitals (s,p,d,f) The quantum number l (The orbital quantum number) describes 3D shape of orbital also called subshell max. ℓ = n – 1 (ℓ = 0, 1, 2, 3,…..) orbitals identified by letters s, p, d, f,… n Sublevel types Value of ℓ 1 1 s ℓ = 0 2 2 s pℓ=0, ℓ =1 3 3 s p d ℓ =0, ℓ =1, ℓ =2 sublevels Fill this in

5. : The secondary quantum number If n can be thought of as shells, l can be thought of as “subshells” dividing each shell into subsections … (l = 0  n - 1) n = 1 = 0 (s) n = 2 = 0 (s) l = 1 (p) n = 3 = 0 (s) l = 1 (p) l = 2 (d) For more lessons, visit www.chalkbored.com www.chalkbored.com l l l l l llll l

6. The magnetic quantum number – m (m ℓ ) Describes the 3D orientation of the orbital and how many of that type orbital exist m ℓ = - ℓ, …, 0, … + ℓ Example: n = 2 m ℓ (for ℓ = 1) = -1, 0,+1 p x, p y, p z sublevel ℓ value # orbitals Shape of orbitals m ℓ value orbitals s ℓ = 0 1sphere m ℓ = 0 1 orientation p ℓ =1 3dumbells m ℓ = 3 orientations d ℓ =2 54 leaf m ℓ = 5 orientations f -1, 0,+1 FYI – its m ℓ = -ℓ to +ℓ -2, -1, 0, +1, +2 Fill in this

7. How many different ways are “s” orbitals oriented? How many different ways are“p “ orbitals oriented? How many different ways are “d” orbitals oriented? How many different ways are “f” orbitals oriented?

8. Spin Quantum number: m s (or s) –describes the spin of the electron on its own axis Clockwise spin is + ½, counterclockwise spin is -½ Orbital notation uses arrows to represent spin What “spins” do electrons have that share the same orbital?

9. Visualization of electron orbitals around a nucleus in an atom The nucleus is located somewhere in the center Slightly different diagram - 3d orbitals This is a computer designed image of over-lapping s and p orbitals in an atom of neon. The bright center portion is the approximate position of nucleus

10. It probably won’t be hard as this……. BUT.. NOT AS EASY AS THIS..

11. Electron Configurations 1. Electrons are located in a very specific place in the energy levels of atom 2. They will fill orbitals in sequential order –based on the energy value of that orbital. Which orbital has a higher energy 1s, 2s or 2p? 1s has the lowest energy 2p has a higher energy value FYI –electron orbitals in the same energy level are called degenerate

12. 2s How many electrons can a “s” orbital hold? Electron orbital Filling sequence What is the electron configuration of Li (lithium)? Li has an atomic number (Z=3) (Contains 3 electrons) 1s 2 How many electrons are left? 21 2 1 1s2s 21 Electron configuration of Li Practice: Z=7: 1s 2 2s 2 2p 3 Z=15: 1s 2 2s 2 2p 6 3s 2 3p 3 1s 2 2s 2 2p 6 3s 1 Z=11:

13. Orbital filling patterns of the Periodic Table

14. Including “f” orbitals in an electron configuration The configuration of: Lutetium Z= This is 4f block sublevel This is 5f block sublevel FYI- f blocks are filled with 14 electrons 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 5d 1 4f 14 3 4 5 6 1 1 3 2 5 4 7 6 Bismuth Z=1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 3 How many energy lvls? How many sublevels? How many valence electrons? 615 71 83 5 Abbreviated configuration of Bi:[Xe] 6s 2 4f 14 5d 10 6p 3

15. There are some “differences” in the sequential filling of orbitals in the “d” block “d” sublevel is full at 10 electrons, half full “d” orbital is more stable (at 5) Full d orbital (with 10 e - )is more stable than “almost full” d orbital (with 9e - ) Sc = [Ar] 4s 2 3d 1 Ti = [Ar] 4s 2 3d 2 V = [Ar] 4s 2 3d 3 Cr = [Ar] 4s 1 3d 5 Mn = [Ar] 4s 2 3d 5 Fe = [Ar] 4s 2 3d 6 Co= [Ar] 3d 7 4s 2 Ni= [Ar] 4s 2 3d 8 Cu = [Ar] 4s 1 3d 10 Zn= [Ar] 4s 2 3d 10 Remember half full Remember almost full Exceptions list: Cr = [Ar] 4s 1 3d 5 Cu = [Ar] 4s 1 3d 10 Mo = [Ar] 5s 1 4d 5 Ag = [Ar] 5s 1 4d 10 Au = [Ar] 6s 1 5d 10

16. Orbital notation diagrams 1. Each space represents a orbital, arrows are electrons. 2. Hund Rule: Every orbital in the SAME sublevel gets 1e- before any of them get 2 electrons Chlorine (Cl) 1s 2 2s 2 2p 6 3s 2 3p 5 ____ _____ _____ _____ ____ ____ _____ _____ _____ 1s 2s 2p 3s 3p Hint: circles can also be used to represent orbitals – just make sure to label, label, label

17. How to find an electron by it’s address-the 4 quantum numbers You don’t have to be a rocket scientist to do this – just remember to label-label-label! Chlorine (Cl) 1s 2 2s 2 2p 6 3s 2 3p 5 Each circle represents an orbital Arrows represent electrons. First arrow is always positive spin (pointing up). Remember Hunds Rule when filling in orbitals 1s 2s 2p 3s 3p m= 0 0 -1 0 +1 0 -1 0 +1 Energy levels and sublevels n= is energy level ℓ = is sublevel 0,1,2,3 (s,p,d,f) m = is the orbital in the sublevel S =is the spin of the electron or Remember: ___ ____ ____ ___ 1+1 2 + ½ n ℓ m s NOW: What are the addresses of the following electrons in Cl? 4 th 12 th 2 0 0 -½ This is the 7 th electron 3 0 0 -½ Last electron 3 1 0 -½ n ℓ m s

18. 1 0 0 +½ n= 1, it is in the 1 st energy level ℓ = 0, it is in the “s” sublevel (if ℓ =0, (m is also 0), s orbital +½ is the spin of the electron What’s that element ? These are the quantum numbers for the LAST ELECTRON n m s 1 s 1 First electron in H 2 1 1 -½ n m s N= 2, it is in the 2 nd energy level ℓ = 1, it is in the “p” sublevel (m is 1), 2p z orbital -½ is the spin of the electron second electron in 0 1s 2s 2p x 2p y 2p z -1 0 +1 1s 2 2s 2 2p 6 = Ne

19. 4 2 0 -½ N= 4, be careful! ℓ = is sublevel 0,1,2,3 (s,p,d,f) m=0 -½ is the spin of the electron What’s that element ? These are the quantum numbers –for the LAST electron n m s 2 nd electron in -2 -1 0 +1 +2 d sublevel N=4, 4d’s start in which period? ℓ = is sublevel 0,1,2,3 (s,p,d,f) m=0, go to the d orbital designated as zero Remember Hund’s Rule ! -½ is the spin of the electron - 2 nd electron in Where do 4d sublevels start? Last electron is in 4d 8 Element is Pd

20. 4 2 0 -½ N= 4, it is in the 4 th energy level ℓ = is sublevel 0,1,2,3 (s,p,d,f) m=0 -½ is the spin of the electron What’s that element ? These are the quantum numbers –for the LAST electron n m s 2 nd electron in 2 1 0 +½ n m s N= 2, it is in the 2nd energy level m ℓ = 1, it is in the “p” sublevel (if ℓ =1, ( but m is 0) +½ is the spin of the electron second electron in 1s 2 2s 2 2p 5 F _____ ______ ______ ______ _______ 1s 2s 2p x 2p y 2p z -1 0 +1 in p y d sublevel

21. http://www.youtube.com/watch?v=a4fklbnHTYY http://www.youtube.com/watch?v=A6DiVspoZ1E Some really good websites to peruse at your leisure concerning quantum numbers http://www.youtube.com/watch?v=yqzgYRBlslw