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Chapter 5: Electrons in Atoms

Difficulty Level: At Grade Created by: CK-12

Chip Griffin. www.flickr.com/photos/chipgriffin/2210297177/. CC BY 2.0.

Chapter Overview

Rutherford’s gold foil experiment established the nucleus of the atom as the source of the positive charge and most of the mass. The nature of the electrons was still unknown. Experiments by Planck and Einstein led to the notion that light exhibits a wave-particle duality. The particle nature of light means that the energies that can be absorbed or released by atoms are quantized. The Bohr model of the atom explained the atomic emission spectrum of the hydrogen atom. Electrons also behave like both waves and particles. The quantum mechanical model of the atom is the modern accepted version of the atom, where electrons occupy orbitals of various shapes and energies, but their exact location is never known. An electron configuration is the specific arrangement of all the electrons in any atom.

Online Resources

See the following Web sites for appropriate activities:

Pacing the Lessons

Lesson Class Period(s) (60 min)
5.1 Light 2
5.2 The Quantum Mechanical Model 2
5.3 Electron Arrangement in Atoms 2-3

Chemistry Concepts

The table below matches each lesson from the FlexBook® student edition to the Chemistry Concepts.

FlexBook® Lesson Chemistry Concepts
5.1 Light 5.1 – 5.7
5.2 The Quantum Mechanical Model 5.8 – 5.13
5.3 Electron Arrangement in Atoms 5.14 – 5.19

Chapter Outline

Chapter Summary

Image Attributions


Difficulty Level:

At Grade

Date Created:

Jul 25, 2014

Last Modified:

May 07, 2015
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