**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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