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Unit 2 Atomic Structure and Periodicity Evaluation Lab

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Unit 2 – Atomic Structure and Periodicity Evaluation 1. Calculate the wavelength (in nm) of the red light emitted by a barcode scanner that has a frequency of 4.62 × 1014 s–1. https://learning.hccs.edu/faculty/erika.bryant/chem1411/powerpoint-lecture/06-chapter-6-1 2. A laser dazzles the audience in a rock concert by emitting green light with a wavelength of 515 nm. Calculate the frequency of the light. 5.82×1014s−1 3. A nitrogen gas laser pulse with a wavelength of 337 nm contains 3.83 mJ of energy. How many photons does it contain? 6.49×1015 photons 4. Arrange the three types of electromagnetic radiation—visible light, X-rays, and microwaves—in order of increasing a. wavelength. b. frequency. c. energy per photon. 5. What are the quantum numbers and names (for example, 2s, 2p) of the orbitals in the n = 4 principal level? How many n = 4 orbitals exist? 6. These sets of quantum numbers are each supposed to specify an orbital. One set, however, is erroneous. Which one and why? a. n = 3; l = 0; ml = 0 b. n = 2; l = 1; ml = –1 c. n = 1; l = 0; ml = 0 d. n = 4; l = 1; ml = –2 7. Determine the wavelength of light emitted when an electron in a hydrogen atom makes a transition from an orbital in n = 6 to an orbital in n = 5. 8. Determine the wavelength of the light absorbed when an electron in a hydrogen atom makes a transition from an orbital in which n = 2 to an orbital in which n = 3 9. Two samples of carbon dioxide are decomposed into their constitue ...
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