1. Four Quantum Numbers: –Specify the “address” (zip code) of each electron in an atom

2. First number…Principal Quantum Number ( n) Energy level (associated with the electron) Size if orbital –Lowest energy level is assigned principle quantum number of 1 (n=1) Ground state –What do you think happens as we increase n? Orbital becomes larger Electron spends more time farther away from the nucleus  atom’s energy increases

3. Principle energy levels contain… Energy Sublevels

4. Principle energy level 1  single sublevel Principle energy level 2  two sublevels Principle energy level 3  three sublevels What pattern do you see in the number of sublevels as we move further away from the nucleus? –They increase as n increases (the further we get from the nucleus) UPPER LEVEL

5. Electron’s are labeled according to n value In atom’s with more than one electron, two or more electron’s may have the same n value –They are in the same “electron shell”

6. Second quantum number Angular Momentum Quantum Number (l)

7. Each value of l corresponds to a different type of orbital with a different shape Value of n controls l (subshells possible) Angular momentum numbers can equal 0, 1, 2, 3… l=n-1 –When n=1, l=0  only one possible subshell –When n=2, l=0,1  two possible subshells

8. What the number of l means… Corresponds to the name of the subshell –L=0  subshell s –L=1  subshell p –L=2  subshell d –L=3  subshell f

9. S P D F: THE SUBLEVELS Each of these 4 sublevels has a unique shape Each orbital may contain at most, 2 electrons LETTERS ORIGINATED FROM DESCRIPTIONS OF THEIR SPECTRAL LINES –S  sharp…spherical –P  principal…dumbbell shaped –D  diffuse…not all the same shape –F  fundamental…not all the same shape

12. When principle energy level n=1, then l=0, which means there is only a single sublevel (one orbital) which is the small, spherical 1s When principle energy level n=2, then l can equal 0 or 1, which means that there are two sublevels (orbitals) 2s and 2p –2s sublevel  bigger than 1s, still sphere –2p sublevel  three dumbbell shaped p orbitals of equal energy called 2px, 2py, and 2pz The letters are just there to tell you what axis the electrons go on: x,y, or z axis When the principle energy level n=3, then l can equal 0,1, or 2, which means that there are 3 possible sublevels: –3s, sphere, bigger than 1s and 2s –3p, dumbbells –3d Each d sublevel consists 5 orbitals of equal energy Four d orbitals have same shape but different orientations Fifth d orbital, 3d z2 is shaped and oriented different from the other four When the principle energy level n=4, then 1 can equal 0,1,2, or 3 which means l=n-1=4 possible sublevels: –Seven f orbitals of equal energy ( 2 electrons in each orbital) –4s, sphere –4p, dumbbells –4d, –4f

13. n=# of sublevels per level n2=# of orbitals per level Sublevel sets: 1 s, 3 p, 5 d, 7 f

16. 2s 2p z 2p y 2p x Orbitals combine to form a spherical shape.

17. Remember… 1. Principal #  energy level 2. Ang. Mom. #  sublevel (s,p,d,f) There are two more quantum numbers (3 and 4) we will discuss next class

18. Third Quantum Number M l  specifies the orientation of the orbital in space containing the electron Tells us whether the orbital is on the x, y, or z axis

19. Fourth Quantum Number M s  related to the direction of the electron spin Tells us if electron has a clockwise spin or counter clockwise spin Specifies orientation of electrons spin axis

20. Recap… Bohr? –Orbits explained hydrogen’s quantized energy states De Broglie? –Dual particle and wave nature of electrons Schrodinger? –Wave equation predicted existence of atomic orbitals containing electrons

21. Electron Configuration Definition: arrangement of electrons in an atom Basic rules for filling up orbital's with electrons Which is more stable, low energy or high energy? –So which orbitals are going to be filled up first? –We are going to want an arrangement that gives us the lowest possible energy

22. Ground state electron configuration The most stable, lowest energy electron arrangement of an atom Each element has a ground-state electron configuration

23. Three Rules for Electron Arrangement Aufbau Principle Pauli Exclusion Principle Hund’s Rule

24. Aufbau Principle Each electron occupies the lowest energy orbital available In order to do this, you must learn the sequence of atomic orbitals from lowest to highest energy Aufbau Diagram –Each box represents an orbital –Each arrow represents an electron –Only two arrows per box… Only two electrons per orbital

27. Some important things to remember about Aufbau… All orbitals related to an energy sublevel are of equal energy –All three 2p orbitals have the same energy In a multi-electron atom, the energy sublevels within a principle energy level have different energies –All three 2p orbitals are of higher energy than the one 2s orbital

29. In order of increasing energies, the sequence of energy sublevels within a principle energy level is s, p, d, f Orbitals related to energy sublevels within one principle energy level can overlap orbitals related to energy sublevels within another principle level –Ex. An orbital related to the atoms 4s sublevel has a lower energy than the five orbitals related to 3d sublevel.

31. Pauli Exclusion Principle States that a maximum on 2 electrons can occupy a single atomic orbital but only if the electrons have opposite spins Wolfgang Pauli Austrian Physicist Observed atoms in excited states

32. Each electron has a spin Kinda like a spinning top It can only spin in one of 2 directions In order for electrons to be together in an orbital, they must have opposite spins

33. Hund’s Rule What kind of charge do electrons have? Do they attract or repel each other? So…….. Hund’s Rule states that single electrons with the same spin must occupy all each energy equal orbital before additional electrons with opposite spins can occupy the same orbital

34. 2p orbitals

35. Read section 5-3!