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Lesson 2.4 Slides: Exploring Valence Electrons and the Periodic Table

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Lesson 2.4 Slides: Exploring Valence Electrons and the Periodic Table

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Learn about valence electrons and how to locate elements by groups and periods.

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Eric D Norman
Eric D Norman
United States

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Lesson 2.4 Slides: Exploring Valence Electrons and the Periodic Table
 

Lesson 2.4 Slides: Exploring Valence Electrons and the Periodic TableOnline version

Learn about valence electrons and how to locate elements by groups and periods.

by Eric D Norman
1

Introduction to Valence Electrons

Valence electrons are the electrons located in the outermost shell of an atom. They play a crucial role in chemical bonding and reactions.

Key points:

  • Determine an element's reactivity.
  • Influence the formation of molecules.
  • Help predict the type of bonds an element can form.
2

Understanding the Periodic Table

The Periodic Table organizes elements based on their atomic number, electron configuration, and recurring chemical properties.

It consists of:

  • Groups: Vertical columns that share similar properties.
  • Periods: Horizontal rows that indicate the number of electron shells.
3

Identifying Groups in the Periodic Table

Elements in the same group have the same number of valence electrons, which leads to similar chemical behaviors.

Examples of groups:

  • Group 1: Alkali metals (1 valence electron)
  • Group 2: Alkaline earth metals (2 valence electrons)
  • Group 17: Halogens (7 valence electrons)
  • Group 18: Noble gases (8 valence electrons)
4

Understanding Periods in the Periodic Table

The periods indicate the number of electron shells an element has. As you move across a period, the number of valence electrons increases.

Characteristics of periods:

  • Elements in the same period have the same number of electron shells.
  • Properties change progressively across a period.
5

Trends in Valence Electrons

As you move across a period:

  • The number of valence electrons increases.
  • Elements become less metallic and more non-metallic.

As you move down a group:

  • The number of electron shells increases.
  • Valence electrons remain the same, but properties change.
 
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