Electrons & Waves Test Review PDF

Name ______________________________________________________ Period ______ Date ________________________________ Electrons Test Review Matc...

Name ______________________________________________________ Period ______ Date ________________________________ Electrons Test Review Match each vocabulary word with its definition. ________ 1. hertz A. the number of waves that pass a given point per unit of time ________ 2. atomic orbital B. the SI unit of frequency ________ 3. spectrum C. lines of colored light obtained by passing the light emitted by an element through a prism ________ 4. emission spectrum D. the region around an atomic nucleus where an electron is likely to be moving ________ 5. quantum of energy E. a range of colors seen when light passes through a prism ________ 6. amplitude F. Electrons enter orbitals of lowest energy first. ________ 7. wavelength G. a region outside the nucleus where there is high probability of finding an electron ________ 8. energy level H. the lowest energy level for a given electron ________ 9. frequency I. When electrons occupy orbitals of equal energy, one electron enters each orbital before adding a second one. ________ 10. aufbau principle J. Each orbital holds a maximum of two electrons. ________ 11. Pauli exclusion K. the distance from one point on a wave to the same point principle on the next wave ________ 12. Hund’s rule L. the distance from the axis of a wave to the top of the crest ________ 13. ground state M. particle of light ________ 14. photons N. the amount of energy required to move an electron from one energy level to the next higher one 15. What formula represents the maximum number of electrons that can occupy an energy level? 16. What is the formula that represents the maximum number of orbitals that can occupy an energy level?  17. Compare the shapes and energies of the s, p, d, and f atomic orbitals. Orbital Type Orbital Shape Orbital Energy s p d f 18. As the frequency of light increases, the wavelength _________________________. Therefore, wavelength and frequency are _________________________ ( directly / inversely ) proportional to each other. 19. As the wavelength of light increases, the energy _________________________. Therefore, wavelength and energy are _________________________ ( directly / inversely ) proportional to each other. 20. As the energy of light increases, the frequency _________________________. Therefore, energy and frequency are _________________________ ( directly / inversely ) proportional to each other. 21. In the _________________________ state of an atom, the electrons are in the lowest energy level possible. When an atom absorbs a _________________________ of energy, the electron transitions from a _________________________ energy level to a _________________________ energy level. The atom is said to be in a(n) _________________________ state. The atom will _________________________ the same quantum of energy that was absorbed as it transitions back to a lower energy level. This energy is observed as _________________________, known as _________________________. Determine whether energy is absorbed or emitted in the following electronic transitions. 22. n = 1 to n = 2 Energy _________________________ 23. n = 5 to n = 2 Energy _________________________ 24. n = 4 to n = 1 Energy _________________________ 25. n = 2 to n = 5 Energy _________________________ 26. 1s to 2s Energy _________________________ 27. 2s to 2p Energy _________________________ 28. 4p to 4s Energy _________________________ 29. 3s to 2s Energy _________________________ 30. Compared with an electronic transition of n = 5 to n = 4, the amount of energy emitted by an electronic transition of n = 5 to n = 1 is __________________ ( higher / lower ). 31. Electrons and electromagnetic radiation exhibit properties of transverse waves. The motion of transverse waves is _________________________ to the axis. Determine the number of waves shown in the following figures. 32. 33. 34. 35. 36. If a light wave has low amplitude, it is ____________________ ( dull / bright ). If a light wave has high amplitude, it is ____________________ ( dull / bright ). 37. List the waves of the electromagnetic spectrum in order from longest wavelength to shortest wavelength. Label relative wavelengths, frequencies, and energies. Express each of the following numbers in scientific notation. 38. 819 41. 0.0275 39. 842,000,000 42. 1.38 40. 0.0000048 43. 0.203 Express each of the following numbers in standard notation. 44. 4.028 × 10–4 47. 3.244 × 105 45. 2.543 × 106 48. 8.179 × 100 46. 6.924 × 10–1 49. 9.370 × 10–4 For the following problems, show your work. Round your answer to the correct number of significant figures. 50. Calculate the frequency of a spectral line with wavelength of 4.6 × 10–7 m. 51. What is the wavelength of a photon that has a frequency of 6.2 × 1014 Hz? 52. What is the energy of an electromagnetic radiation with a wavelength of 6.8 × 10–7 m?  53. How many joules of energy does an electron lose when it emits a photon with a frequency of 6.55 × 1015 Hz? 54. What is the frequency of a photon that transfers 3.99 × 10−17 J of energy? ** Make sure you know where you can find the formulas and constants used for these calculations on the formula chart. 55. List the types of orbitals that occupy each energy level. n=1 ____________________ n=2 ____________________ n=3 ____________________ n=4 ____________________ n=5 ____________________ Write the full electron configurations for the following elements and ions. 56. Sodium (Na) ___________________________________________________________________ 57. Chlorine (Cl) ___________________________________________________________________ 58. Nickel (Ni) ___________________________________________________________________ 59. Ni2+ ___________________________________________________________________ 60. O2– ___________________________________________________________________ Write the condensed electron configurations for the following elements and ions. 61. Tin (Sn) ___________________________________________________________________ 62. Rubidium (Rb) ___________________________________________________________________ 63. Bromine (Br) ___________________________________________________________________ 64. Calcium (Ca) ___________________________________________________________________ 65. Sn4+ ___________________________________________________________________ 66. Ni2+ ___________________________________________________________________ 67. Mn2+ ___________________________________________________________________ Write the orbital diagram configuration for the following elements. 68. Nitrogen (N) 69. Silicon (Si) Determine whether the following electron configurations are that of an atom in the ground state or the excited state. 70. 1s2 2s2 2p5 3s1 71. 1s2 2s2 2p2 72. 1s2 2s1 2p4