**Streetlights and Sodium Emission**The soft yellow glow of many streetlights is produced by small amounts of sodium metal present in the bulbs. In the line spectrum of sodium, this light has a wavelength of 589 nm.**Image Description:**The image displays a row of streetlights glowing warmly along a wet, reflective street at dusk or nighttime. This illustrates the characteristic yellow glow emitted by sodium streetlights.**Graph/Diagram:**- **Graph (labeled b):** - The horizontal axis represents the wavelength in nanometers (nm), with markings at 400, 500, 600, and 700 nm. - A thick black bar spans the graph, and a thin yellow line is marked at 589 nm, indicating sodium’s emission wavelength.**Electron Behavior:**When sodium absorbs energy, its highest-energy electron jumps from the ground state to energy level 3p. When the electron relaxes back down, it releases this energy as 589-nm yellow light. Write the electron configuration for sodium in its ground state, and then write the electron configuration for the excited sodium atom. **Title: Understanding Electron Transitions in Sodium Atoms****Ground-State Electron Configuration:**[Enter configuration here]**Excited-State Electron Configuration:**[Enter configuration here]**Energy Difference in Electron Transitions:**Question: What is the energy difference in joules between the energy sublevels 3s and 3p in a sodium atom?**Energy Difference:**[Enter energy difference here] J**Photon Requirement for Energy Production:**Question: How many of these electronic transitions must occur to produce 2.25 kJ of light energy?**Electronic Transitions:**[Enter number of transitions here] photons---This resource provides a framework for students to explore the ground and excited states of electrons in sodium atoms, calculate the energy difference between sublevels, and determine the number of electronic transitions required for a specified energy output.

Since you have posted question with multiple subparts , as per the guidelines we can answer three.…

ground-state electron configuration: excited-state electron configuration: What is the energy difference in joules between energy sublevels 3s and 3p in a sodium atom? energy difference: How many of these electronic transitions must occur to produce 2.25 kJ of light energy? photons electronic transitions:

ground-state electron configuration: excited-state electron configuration: What is the energy difference in joules between energy sublevels 3s and 3p in a sodium atom? energy difference: How many of these electronic transitions must occur to produce 2.25 kJ of light energy? photons electronic transitions:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Spectroscopy, or the study of how light interacts with matter, is an extremely powerful tool scientists use to identify unknown substances. One branch of spectroscopy is the measurement of the interactions between gases and visible light. Sending a very high voltage through a gas adds energy to the system causing some of the electrons to enter a more unstable, or excited, state. To return to the stable state, the electron emits scme of that energy in the form of light. Using the fact that electrons can only exist in certain energy "shelves," we can predict what wavelengths of light, or colors, are emitted when we add energy to the system. The following equation shows the energy levels for a hydrogen atom with only one electron (when dealing with multiple electrons and protons the math becomes far more complex and is outside the scope of this activity). = R#) Where: A is the wavelength of light| RH is the Rydberg Constant for a Hydrogen atom, 1.0974 · 10’ /m n2 is the final energy level…
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