Chapter 4 Electron Structure of the Atom

1. Chapter 4Electron Structure of the Atom

2. Review of Atomic Structure • The center of the atom is called the nucleus. • In it are the particles with mass: the protons and neutrons • Protons determine the identity of an atom • Electrons determine the properties of an atom • Where are the electrons?

3. Light • What is light, and what does it have to do with the electrons in an atom? • Light is electromagnetic radiation.

4. Electromagnetic Radiation (EMR) • Form of energy with wavelike behavior as it travels through space at the speed of light • Seven major types: • Gamma () Rays • X rays • Ultraviolet (UV) • Visible Light (ROYGBIV) • Infrared (IR) • Microwaves • Radio waves

5. Electromagnetic Spectrum(p. 98)

6. Wavelength (λ) • The distance between two corresponding points on a wave • Units are same as length - m, or commonly nm (10-9 m) Figure 7.5

7. Know the wavelengths for the visible spectrum R O Y G B IV 700 650 600 550 500 450 400 nm

8. Frequency • number of wave cycles that move through a point in space in 1 s • hertz (Hz) • same as inverse seconds (1/s) or (s-1)

9. Figure 7.7 • Which has the greater wavelength the red light or the green light? • Which has a greater frequency?

10. Frequency & Wavelength • inversely proportional • i.e. as one increases the other decreases c = λν c = speed of light (3.0 x 108 m/s) λ = wavelength (in meters) ν = frequency (in Hz)

11. Practice • What is the frequency and wave type of a wave with a wavelength of 5.2 x 10-7 m (5.2 x 102 nm)? wave type: green visible light

12. Practice • What is the frequency and wave type of a wave with a wavelength of 5.2 x 10-7 m (5.2 x 102 nm)? wave type: green visible light

13. What is the approximate frequency of blue light? • Wavelength = 475nm R O Y G B IV 400 700

14. Convert nm to m R O Y G B IV 400 700

15. What is the approximate frequency of blue light? R O Y G B IV 400 700

16. Homework • Calculate the frequency of light with a wavelength of 3.41 x 103 cm? • Calculate the wavelength of light with a frequency of 3.21 x 1016 Hz? What type of EMR is it? • What is the frequency of orange light?

17. Continuous spectrum all the wavelength of in the visible spectrum Produced by white light Line Spectrum distinct colored lines each a single wavelength of light Visible when an element has been heated “atomic fingerprint” Line Spectra

18. Energy is Quantized! Quantized = quantity = specific measured amount • Max Planck • energy produced by atoms can only have certain values • only distinct lines are seen in element line spectra • can only exist at certain wavelengths.

19. Max Planck • Proposed that objects emit energy in small packets called “quanta” • Quantum: min. quantity of energy lost or gained by an atom • This quantized energy is related to the frequency of the energy

20. Photons – waves and particles Energy of a photon • directly proportional to the frequency Ephoton = hν • inversely proportional to the wavelength Ephoton = hc/l Ephoton = (in Joules) h = Planck’s constant (6.626 x 10-34 Js) ν= frequency (in Hz) l = wavelength in meters

21. Low High Low E High Low High E

22. Which electromagnetic radiation has a higher energy? • microwaves • infrared 0% 0% Non-Response Grid 0 of 26

23. Which electromagnetic radiation has a longer wavelength? • X-ray • ultraviolet • microwave 0% 0% 0% Non-Response Grid 0 of 26

24. Which electromagnetic radiation has a lower frequency? • ultraviolet • visible light 0% 0% Non-Response Grid 0 of 26

25. Practice • What is the energy of a photon with a frequency of 1x1017Hz?

26. Practice • What is the energy of a photon with a wavelength of 8.1m?

27. Photoelectric Effect • Emission of electrons from a metal when light shines on it

28. This was explained by Einstein • Based on Planck's work, Einstein proposed that light also delivers its energy in chunks; light would then consist of little particles, or quanta, called photons, each with an energy of Planck's constant times its frequency • Electrons are only emitted if the photons have a high enough energy (high enough frequency)

29. Atomic Spectra • When visible light passes through a prism, its components separate into a spectrum. • White light, such as sun light or light from a regular light bulb, gives a continuous spectrum:

30. Atomic Spectra • Colored light gives only specific colors in a line spectrum:

31. What does this have to do with electrons? • Hydrogen atom: 1 proton, 1 electron • Passing electricity through a tube containing hydrogen gas gives off a pink light • Light is given off as electrons fall from an excited state to a ground state • The light can be separated into four frequencies

32. Spectra of other elements(spectral signatures applet)

33. Energy Level Transition • Excited State: higher energy state • Ground State: lowest energy state Ephoton Ephoton= Eexcited- Eground=h

34. Bohr Model links electron and emissions • Niels Bohr (Danish physicist) • planetary model • electron are in orbits • orbit 1 closest to the nucleus • increasing numbers as the orbits get further away from the nucleus.

35. Bohr Model • Orbits have a fixed radius. • Electrons cannot exist between orbits • lowest energy is closest to the nucleus • increases as the orbits get further away • Electrons absorb or emits energy when they change orbitals ∆E = Ef – Ei

36. Which transition results in the emission of light with the greatest photon energy? • A • B • C • D 0% 0% 0% 0% A B D C Non-Response Grid 0 of 26

37. Which transition results in the emission of light with the longest wavelength? • A • B • C • D 0% 0% 0% 0% A B D C Non-Response Grid 0 of 26

38. Which transition results in the emission of light with the highest frequency? • A • B • C • D 0% 0% 0% 0% A B D C Non-Response Grid 0 of 26

39. What type of ER has the longest wavelength? • red light • violet light • X-rays 0% 0% 0% Non-Response Grid 0 of 26

40. Who stated that matter when heated can emit energy in specific amounts called quanta? • Einstein • Bohr • Planck 0% 0% 0% Non-Response Grid 0 of 26

41. Light energy is delivered in specific amounts called photons. • True • False Non-Response Grid 0 of 26

42. An electron is emitted from metal when • Any beam of light hits the metal for enough time • Enough photons of light energy hit the metal • A photon with a sufficient amount of energy hits the metal • I have no idea 0% 0% 0% 0% Non-Response Grid 0 of 26

43. Bohr’s model of the atom • places electrons in orbits around the nucleus • each orbit has it’s own radius and energy • light is emitted when an electron moves to an excited state • both 1 and 2 are correct • both 2 and 3 are correct 0% 0% 0% 0% 0% Non-Response Grid 0 of 26

44. As an orbit’s distance from the nucleus increases, the amount of energy decreases • True • False Non-Response Grid 0 of 26

45. Deficiencies of Bohr Model • Did not work for other atoms • Doesn’t explain chemical behavior of atoms • More complex model needed • However, the Bohr model did give insight into the quantized behavior of the atom that was better understood in later days

46. Modern Models of the Atom • Bohr • deBroglie • Schrödinger (Wave Mechanical Model) • To view at home, click here. Click on Run Now!

47. Modern Model of the Atom(Quantum Mechanical Model) • electrons exist in orbitals. • Orbitals are 3-dimensional regions in space where an electron is likely to be found • not a circular pathway • The electron is thought of having wave properties

48. The exact location of the electron cannot be known. (Heisenberg Uncertainty Principle) • The location is described as a probability • This is a Probability Map for lowest-energy state of the electron in an H atom

49. A typical representation of an s-orbital

50. Principal Energy Levels • Orbitals of similar size exist in the same principal energy level (n=1, 2, 3…) • The principal energy levels correspond to Bohr’s energy levels and represent a distance from the nucleus