* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download Chapter 5 Practice Section 5-1 Discuss the placement (if any) of
Molecular Hamiltonian wikipedia , lookup
Renormalization wikipedia , lookup
Bohr–Einstein debates wikipedia , lookup
Canonical quantization wikipedia , lookup
Quantum teleportation wikipedia , lookup
Ferromagnetism wikipedia , lookup
Bremsstrahlung wikipedia , lookup
Quantum state wikipedia , lookup
History of quantum field theory wikipedia , lookup
Chemical bond wikipedia , lookup
Hidden variable theory wikipedia , lookup
EPR paradox wikipedia , lookup
Double-slit experiment wikipedia , lookup
Particle in a box wikipedia , lookup
Auger electron spectroscopy wikipedia , lookup
Quantum electrodynamics wikipedia , lookup
Molecular orbital wikipedia , lookup
Tight binding wikipedia , lookup
X-ray photoelectron spectroscopy wikipedia , lookup
X-ray fluorescence wikipedia , lookup
Matter wave wikipedia , lookup
Hydrogen atom wikipedia , lookup
Theoretical and experimental justification for the Schrödinger equation wikipedia , lookup
Electron-beam lithography wikipedia , lookup
Wave–particle duality wikipedia , lookup
Atomic theory wikipedia , lookup
Chapter 5 Practice Section 5-1 1. 2. 3. 4. 5. 6. Discuss the placement (if any) of electrons in the following models of the atom: a. Dalton ____________________________________________________________________ b. Thompson _________________________________________________________________ c. Rutherford _________________________________________________________________ d. Bohr ______________________________________________________________________ e. Quantum Mechanical ________________________________________________________ __________________________________________________________________________ Which is a larger difference in energy? a. n = 1 to n = 2 b. n = 3 to n = 4 If a quantum of energy is added to an atom, an electron ________________________________ ________________________________________. An ________________ is where you will most probably find an electron. How many orbitals are in the following sublevels? a. 4 p sublevel b. 3d sublevel How do the px, py, and pz orbitals differ from each other? How are they similar? 7. What is the correlation between the energy level and the number of sublevels in that energy level? 8. From the given information, determine the pattern and fill in the missing values. Energy level # of sublevels # of orbitals # of electrons n=1 1 1 2 n=2 2 4 8 n=3 3 9 18 n=4 ? ? ? 9. Give the formula in terms of “n” for: a. # of orbitals b. # of electrons Section 5-2 Match the name of the rule to the rule itself. ______10. aufbau principle a. When electrons occupy orbitals of equal energy ______11. Pauli exclusion principle separately with parallel spin before pairing. ______12. Hund’s rule b. Electrons enter orbitals of lowest energy first. c. Every electron has a unique set of quantum numbers. Draw the orbital diagram for the following elements: 13. Magnesium 14. Oxygen 15. Argon 16. Scandium 17. Phosphorous Write out the electron configuration for the following elements: 18. Potassium 19. Cobalt 20. Silicon 21. Lithium 22. Selenium 23. Bismuth 24. Vanadium 25. Sulfur 26. Mercury Identify the following elements: 27. 1s22s22p63s23p64s2 28. 1s22s22p63s23p2 29. 1s22s22p63s23p64s23d3 30. 1s22s22p63s23p64s23d104p5 31. 1s22s22p6 32. 1s22s22p63s23p64s23d104p65s24d105p66s24f145d6 33. What elements are exceptions to the filling rule (Aufbau principle) For # 34-37, write the abbreviated electron configuration (kernel notation). 34. Iodine 35. Radium 36. Aluminum 37. Gallium 38. How do the 2p orbitals differ from each other? 39. How do the 2p and 3p orbitals differ from each other? Quantum Number Extension: NOT IN THE TEXTBOOK! 40. Which of the following sets of quantum numbers is allowed? Underline the parts that makes the others incorrect. a. n = 3, l = 2, ml = 2 b. n = 4, l = 3, ml = 4 c. n = 0, l = 0, ml = 0 d. n = 2, l = -1, ml = 1 41. How many electrons in an atom can have the designation: a. 1s b. 2p c. 3px d. 5f e 2dxy 42. How many orbitals in an atom can have the designation: a. 5p b. 4d c. n = 5 d. n = 4 43. What is the maximum number of electrons in an atom that can have these quantum numbers: a. n = 4 _____ b. n = 5, ml = +1 _____ c. n = 5, ms = + ½ _____ d. n = 3, l = 2 _____ e. n = 2, l =1 _____ 44. What is the maximum number of electrons in an atom that can have these quantum numbers: a. n = 0, l = 0, ml = 0 _____ b. n = 2, l = 1, ml = -1, ms = -½ _____ c. n = 3 _____ d. n = 3, l = 2 _____ e. n = 1, l = 0, ml = 0 _____ 45. Give a possible set of variables for the four quantum numbers for all the electrons in an atom of carbon. 46. What are the possible values of ml for a. l = 0 _________ b. l = 3 __________ c. n = 3 ___________ 47. Give the number of orbitals in a. n = 3 ________ b. a 4d sublevel _______ c. an f sublevel _______ 48. Given the following sets of quantum numbers, indicate those that could not occur a. 1, 1, 0, +½ b. 2, 1, 0, +½ c. 2, 0, 1, -½ d. 2, 1, 0, 0 49. Assign a set of four quantum numbers to a. the 4s electrons in Ca b. all the 3d electrons in Cr c. all the 3p electrons in Cd 50. Identify the specific element that has the following electron configuration: a. 1s22s22p4 b. [Ne]3s23p5 c. [Ar]4s1 d. [Ar]4s13d5 5-3 Practice The speed of light c = 2.998 x 108 m/s 51. 52. 53. 54. 55. 56. 57. 58. 59. 60. 61. 62. What is the wavelength of radiation with a frequency of 2.3 x 1014 Hz? What is the frequency of radiation with a wavelength of 1.8 x 10-9 m? Rank in order of increasing energy: Purple light, x-rays, Microwaves Rank the above in order of increasing frequency. Rank the above in order of increasing wavelength. Which of the following is in ground state? a. 1s22s22p63s13p1 b. 1s22s22p63s23p64s1 Which electron jump would result in energy being emitted? a. 3 → 4 b. 2 → 5 c. 2 → 1 d. 5 → 6 Which electron jump would absorb the most energy? a. 5→6 b. 6 →7 c. 3→ 4 d. 1 → 2 Which electron jump would release the most energy? a. 3→2 b. 4→2 c. 5→2 d. 7→6 Albert Einstein described light as having a particle nature as well as a wave nature. He called the light particles ________________. De Broglie thought that if light could have a particle nature, then particles could have ________________ nature. A neon light is really composed of a variety of colors of light. How are they produced?