1. Atomic Structure and Periodicity Mr. Guerrero, AP Chemistry

2. Electromagnetic Radiation Electromagentic Radiation(EM)- energy, in the form of photons, that moves in waves as it travels through space. Examples of EM Radiation are: 1 gamma rays6 microwaves 2 x-rays7 radar waves 3 ultraviolet radiation8 radio waves 4 visible light 5 infra-red radiation

3. Electromagnetic Spectrum

4. Electromagnetic Radiation Figure 7.1

5. Wave measurements Crest- highest point of a wave cycle. Trough – lowest point of a wave cycle. Wavelength ( )– distance between two consecutive points on a wave. Amplitude – height of the wave, from the axis. Frequency ( ) – the number of wave cycles per second.

6. Wave measurements

7. Photons All forms of Electromagnetic Radiation are made up of photons. Photon (quantum)- a tiny packet of light energy that travels through space in electric and magnetic waves. Photons behave as both waves and particles.(Duality of Light Theory)

8. Moving matter also has a wave-particle duality. Discovered by Louis De Broglie DeBroglie’s moving matter has a wavelength DeB = h = h p mv h = Planck’s Constant, p = momentum = mass(kg) x velocity(m/s)

9. Find the DeBroglie wavelength of: A 2.35 kg bowing ball moving at 7.00 m/s. An electron travelling at ½ the speed of light. A 75 Kg football player running at 8.55 m/s.

10. Visible Light All photons with a wavelength between 360 nm -740 nm. Ultra violet(UV) visible light Infra-red(IR) v i b g y o r 360 nm 740nm

11. Important Conversion 1 meter = 1 x 10 9 nanometers (memorize!) Make each conversion: 364 nm = ______ meter 9.88 x 10 - 8 meter = ______nm 2000 nm = ______meter 0.0045 m = ________nm

12. c = Practice Problems c = Find the wavelength of a photon(light) if it has a frequency of 8.1 x 10 12 Hz. Find the frequency of a photon of light with a wavelength of 350 nm. Find the wavelength of a 6 x 10 14 Hz photon and indicate its color. What is the frequency of a photon with a wavelength of 895 nm?

13. Calculating the energy in a photon E = h Energy = Planck’s Constant x frequency Find the energy in a 1.8 x 10 14 Hz photon. Find the frequency of a 5.05 x 10 -18 J photon. Find the energy of a 485 nm photon.

14. Photon calculations 1) Find the energy of a 3.50 x 10 14 Hz photon. 2) What is the frequency of a 6.13 x 10 -19 J photon? 3)A photon has a wavelength of 525 nm. What is the frequency? 4) What is the energy of this photon? 5)A photon has an energy of 1.05 x 10 -18 J. Is this photon visible? 6)Which line series does this light belong to?

15. How are photons produced?

17. Line Spectra(pre-AP) Each element has atoms with different numbers of electrons. As these electrons drop to lower energy levels, they emit photons of unique wavelengths. Each element emits its own set of colored lines, called an emission line spectrum. These spectra are used to identify elements in unknown samples or composition of stars.

18. Hydrogen atom spectra series n=2 n=3 n=4 n =2 n=6 n=5

19. Line spectra series Lyman Series- e - drops from n = X to n=1 lights are in Ultraviolet Region Balmer Series- e - drops from n = X to n =2 lights are in Visible Region Paschen Series- e - drops from n = X to n = 3 lights are in Infrared Region

20. Electron orbitals Orbital – a 3-dimensional space around the nucleus which can hold up to 2 electrons, with opposite spin. *electrons are found in their orbitals 99.9% of the time. Orbitals have different shapes: s, p, d, f

21. Orbitals have different shapes: Orbital shape sspherical pdumbbell dclover or dumbbell/donut ftoo complex

22. s-orbitals: spheres

23. p-orbitals: dumbbell

24. d-orbitals: clover (double dumbbell) or dumbbell/donut

25. f-orbitals: complex

26. Quantum Numbers The location of each electron in an atom can be determined by assigning each electron a four-number code called quantum numbers.

27. Important electron laws: Heisenberg Uncertainty Principle : the more accurately one knows the position of an electron the less accurately one can predict its momentum(speed) AND vice versa.

28. Important electron laws: Hund’s Rule: electrons fill empty orbitals first. Aufbau Principle: electrons occupy orbitals in a certain order: nearest to the nucleus first. Pauli Exclusion Principle: No two electrons in the same atom can have the same set of four quantum numbers.

29. 4 Quantum Numbers: 1 Principal Quantum Number (n), gives the energy level (aka shell) of the electron. 2 Orbital Quantum Number (l) = gives the shape of orbital of the electron. 3 Magnetic Quantum Number(m l ) = gives the orientation(direction) of the orbital. 4 Spin Quantum Number(m s ) = gives the direction of spin of the electron.

30. Allowable ranges for quantum numbers n (energy level) = 1  infinity l (type of orbital = 0  n-1 m l (direction) = -l  +l m s (spin) = -1/2 or +1/2

31. Determine whether each set of quantum numbers is valid or invalid: 1) 3, 2, -1, +1/2 2) 1, 2, 0, -1/2 3) 4, 3, -3, +1/4 4) 88, 67, -55, -1/2 5) -2, 1, -1, +1/2 6) 1, 0, 1, -1/2 7) 2, 0, 0, +1/2 8) 4, 2, -3, +1/2 9) 3, 1, 2, -1/2 10) 4, 2, -2, +1/2 Valid Invalid Valid Invalid Valid Invalid Valid

32. Energy sublevels around an atom energyelectron sublevels # of orbitalscapacity s1 2 p3 6 d5 10 f7 14 g*9 18 *orbitals exist, but not used most of the time.

33. Orbital Notation Aufbau Order: (Nucleus)1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f **This is the order in which electrons fill!!!!! You must learn the order!! Don’t worry there is always an easier way to memorize these things. For the Aufbau Order there are 2 ways: With arrows or with the periodic table! Smartboard activate!

34. Electron Configurations and the Periodic Table Figure 8.7

35. Electron Spin Quantum Number Diamagnetic : NOT attracted to a magnetic field all electrons are spin paired. Paramagnetic : substance is attracted to a magnetic field. Substance has unpaired electrons. Diamagnetic : NOT attracted to a magnetic field all electrons are spin paired. Paramagnetic : substance is attracted to a magnetic field. Substance has unpaired electrons.

36. Orbital Notation Write the orbital notation for each atom: Nitrogen, N(7 electrons) Sodium, Na(11 e - ) Iron, Fe(__ e - ) Antimony, Sb(__ e - ) Gold, Au(__ e - )

37. Write the orbital notation for each atom: Silver, Ag(__ e - ) Silver cations Aluminum cations Copper (I) & Copper (II) cations Zinc atoms & Zinc ions Iron(II) & Iron(III) ions

38. Electron Configurations Write the electron configurations for each atom: Nitrogen, N(7 electrons) Sodium, Na(11 e - ) Iron, Fe(__ e - ) Antimony, Sb(__ e - ) Gold, Au(__ e - )

39. Quantum Numbers Write the four quantum numbers for the last electron to fill each atom: Nitrogen, N(7 electrons) Sodium, Na(11 e - ) Iron, Fe(__ e - ) Antimony, Sb(__ e - ) Gold, Au(__ e - )

40. Valence electrons Give the number of valence electrons for each atom: Nitrogen, N(7 electrons) Sodium, Na(11 e - ) Iron, Fe(__ e - ) Antimony, Sb(__ e - ) Gold, Au(__ e - ) Silver, Ag(__ e - ) Aluminum cations Copper (I) & Copper (II) cations Zinc atoms & Zinc ions

41. Lewis Dot Structures Give the Lewis Dot Structure for each atom: Nitrogen, N(7 electrons) Sodium, Na(11 e - ) Iron, Fe(__ e - ) Antimony, Sb(__ e - ) Gold, Au(__ e - )