1. Electron Configuration CONFIGURED (GET IT??) BY MR. TARUSCIO

3. Clash of ideas! Is an electron a particle or a wave?

5. Schrödinger model quantifies electrons into ATOMIC ORBITALS rather than specific energy levels. Orbitals are described with 2 different numbers called Quantum Numbers 1)Principal Quantum Number (n) Integer values that describe the energy of the orbital Larger n means larger average distance of an electron from nucleus (thus larger orbital) 2)Angular Momentum Quantum Number (l) Tells us the “shape” of the orbitals l012345 Name of orbitalspdfgh

6. Orbital Diagrams

7. The s orbital has a spherical shape centered around the origin of the three axes in space. s orbital shape

8. Orbitals of the same shape (s, for instance) grow larger as n increases… Nodes are regions of low probability within an orbital. Sizes of s orbitals

9. 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

10. 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

11. Shape of f orbitals

12. Orbital filling table Label Your Periodic Table

13. Electron Configuration 1s11s1 row # shell # possibilities are 1-7 7 rows subshell possibilities are s, p, d, or f 4 subshells group # # valence e- possibilities are: s: 1 or 2 p: 1-6 d: 1-10 f: 1-14 Total e- should equal Atomic # What element has an electron configuration of 1s 1 ?

14. The Order of Orbitals  1s,  2s, 2p,  3s, 3p,  4s, 3d,4p,  5s, 4d, 5p,  6s, 4f, 5d, 6p,  7s, 5f, 6d, 7p,  (8s, 5g, 6f, 7d, 8p, and 9s)

15. PRACTICE!!!

16. RULES!! Memorize These!!  Three rules (To MEMORIZE)  Aufbau: Electrons fill orbitals starting in the lowest energy levels and moving out.  Pauli: No two electrons can have the same spin and occupy the same orbital.  Hunds: Electrons fill each orbital singly before any orbital get a second electron.

17. Details  Valence electrons- the electrons in the outermost energy levels (not d).  Core electrons- the inner electrons  Hund’s Rule- The lowest energy configuration for an atom is the one have the maximum number of unpaired electrons in the orbital.  C 1s 2 2s 2 2p 2

19. 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

20. Shorthand Notation  A way of abbreviating long electron configurations  Since we are only concerned about the outermost electrons, we can skip to places we know are completely full (noble gases), and then finish the configuration

21. Shorthand Notation  Step 1: Find the closest noble gas to the atom (or ion), WITHOUT GOING OVER the number of electrons in the atom (or ion). Write the noble gas in brackets [ ].  Step 2: Find where to resume by finding the next energy level.  Step 3: Resume the configuration until it’s finished.

22. Shorthand Notation  Chlorine  Longhand is 1s 2 2s 2 2p 6 3s 2 3p 5 You can abbreviate the first 10 electrons with a noble gas, Neon. [Ne] replaces 1s 2 2s 2 2p 6 The next energy level after Neon is 3 So you start at level 3 on the diagonal rule (all levels start with s) and finish the configuration by adding 7 more electrons to bring the total to 17 [Ne] 3s 2 3p 5

25. Electromagnetic Radiation

26. Properties of Waves All electromagnetic waves travel at the same speed The speed of light: 300,000 km/s trough crest

27. Properties of Waves Wavelength (length/cycle) Wavelength ( ): the length of one complete cycle trough crest

28. Properties of Waves Wavelength (length/cycle) Amplitude: 1/2 height between trough and crest Amplitude trough crest

29. Properties of Waves Wavelength (length/cycle) Frequency ( ): the number of cycles/second Amplitude trough crest

30. Speed = wavelength x frequency c = (length/second) = (length/cycle) x (cycle/second) Hence, = c / and = c /

31. Examples  What is the wavelength of light with a frequency 5.89 x 10 5 Hz?  What is the frequency of blue light with a wavelength of 484 nm?

32. Light  Made up of electromagnetic radiation  Waves of electric and magnetic fields at right angles to each other.

33. Copyright © Houghton Mifflin Company. All rights reserved. 7–33 Classification of Electromagnetic Radiation

35. Hydrogen spectrum  Emission spectrum because these are the colors it gives off or emits  Called a line spectrum.  There are just a few discrete lines showing 410 nm 434 nm 486 nm 656 nm Spectrum

36. The Bohr Ring Atom  He didn’t know why but only certain energies were allowed.  He called these allowed energies energy levels.  Putting energy into the atom moved the electron away from the nucleus  From ground state to excited state.  When it returns to ground state it gives off light of a certain energy

37. The Bohr Ring Atom n = 3 n = 4 n = 2 n = 1

38. An excited lithium atom emitting a photon of red light to drop to a lower energy state.

39. An excited H atom returns to a lower energy level.

40. Periodic Trends

41. Sizes of Atoms Difficult to define atomic radii for single atoms because the outside of the electron cloud.

42. Sizes of Atoms The non-bonding atomic radius is defined as one-half of the distance between two atoms when they collide.

43. Sizes of Atoms Bonding atomic radius tends to… …decrease from left to right across a row …increase from top to bottom of column

44. Sizes of Ions  Ionic size depends upon:  Nuclear charge.  Number of electrons.  Orbitals in which electrons reside.

45. Ionization Energy  Amount of energy required to remove an electron from the ground state of a gaseous atom or ion.  First ionization energy is that energy required to remove first electron.  Second ionization energy is that energy required to remove second electron, etc.

46. Ionization Energy  It requires more energy to remove each successive electron.  When all valence electrons have been removed, the ionization energy shows a HUGE increase.

47. Electronegatvity  Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons.  The Pauling scale is the most commonly used.  Fluorine (the most electronegative element) is assigned a value of 4.0  Values range down to cesium and francium which are the least electronegative at 0.7.

48. Electron Affinity  Electron affinity is defined as the change in energy of a neutral atom (in the gaseous phase) when an electron is added to the atom to form a negative ion.  The neutral atom's likelihood of gaining an electron

49. Do Now!  Define:  Electronegativity  Ionic Radius  Ionization energy  What appears to be the trend in atomic radius as you move from left to right in a row?  What appears to be the trend in atomic radius as you move down a column?