**Energy Levels in Atomic Structure**This energy diagram represents the allowed energy levels of an electron in a certain atom or molecule. The diagram features horizontal lines labeled A, B, C, D, and E, representing different energy levels. The energy increases as you move from A to E.**Diagram Explanation:**- **Energy Levels:** Labeled from A (lowest energy) to E (highest energy).- **Transitions:** Possible electron transitions occur between these levels, impacting the emission or absorption of specific wavelengths of light.**Use this diagram to complete the table below:**| **Question** | **Answer** ||--------------------------------------------------------------|-------------|| Which is the ground state? | A || How many excited states are there? | 4 || How many lines are in the absorption line spectrum? | 4 || Which transition causes the emission line at the shortest wavelength? | E → A || Which transition causes the emission line at the longest wavelength? | B → A |These questions help understand electron transitions and their effects on spectral lines, useful in fields like spectroscopy.

Energy is given by formula E=hv We Where, h= planks constant v= frequency But v=c/λ Where c= speed…

This energy diagram shows the allowed energy levels of an electron in a certain atom or molecule: E energy D Which is the ground state? C B A Use this diagram to complete the table below. How many excited states are there? How many lines are in the absorption line spectrum? Which transition causes the emission line at the shortest wavelength? Which transition causes the emission line at the longest wavelength? (pick one) C 0 0 0→0 0→0

This energy diagram shows the allowed energy levels of an electron in a certain atom or molecule: E energy D Which is the ground state? C B A Use this diagram to complete the table below. How many excited states are there? How many lines are in the absorption line spectrum? Which transition causes the emission line at the shortest wavelength? Which transition causes the emission line at the longest wavelength? (pick one) C 0 0 0→0 0→0

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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Concept explainers

Electronic Transitions and Spectroscopy

The term “electronic” connotes electron, and the term “transition” implies transformation. In a molecule, the electrons move from a lower to a higher energy state due to excitation. The two energy states, the ground state and the excited state are the lowest and the highest energy states, respectively. An energy change is observed with this transition, which depicts the various data related to the molecule.

Photoelectron Spectroscopy

Photoelectron spectroscopy (PES) is a part of experimental chemistry. It is a technique used in laboratories that involves projecting intense beams of radiation on a sample element. In response, the element ejects electrons for which the relative energies are measured.

Question

**Energy Levels in Atomic Structure**

This energy diagram represents the allowed energy levels of an electron in a certain atom or molecule. The diagram features horizontal lines labeled A, B, C, D, and E, representing different energy levels. The energy increases as you move from A to E.

**Diagram Explanation:**
- **Energy Levels:** Labeled from A (lowest energy) to E (highest energy).
- **Transitions:** Possible electron transitions occur between these levels, impacting the emission or absorption of specific wavelengths of light.

**Use this diagram to complete the table below:**

| **Question** | **Answer** |
|--------------------------------------------------------------|-------------|
| Which is the ground state? | A |
| How many excited states are there? | 4 |
| How many lines are in the absorption line spectrum? | 4 |
| Which transition causes the emission line at the shortest wavelength? | E → A |
| Which transition causes the emission line at the longest wavelength? | B → A |

These questions help understand electron transitions and their effects on spectral lines, useful in fields like spectroscopy.

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