Ionic Compounds and Lewis Structures

This video tutorial explains how to write the Lewis structure for lithium oxide (Li2O). It begins by identifying lithium as a metal and oxygen as a non-metal, forming an ionic compound. The tutorial uses the periodic table to determine the valence electrons of lithium and oxygen. It then describes how lithium transfers its valence electrons to oxygen, resulting in a full outer shell for oxygen and a charge of two minus. The lithium atoms each lose a valence electron, gaining a one plus charge. The video concludes by discussing the concept of a formula unit and how it represents the repeating array in the crystal structure of Li2O.

What type of compound is formed when lithium and oxygen combine?

• Metallic compound

• Molecular compound

• Ionic compound

• Covalent compound

Where should oxygen be placed in the Lewis structure of Li2O?

• On the left side

• On the right side

• In the middle

• Above lithium

How many valence electrons does lithium have?

• One

• Two

• Three

• Four

What happens to the valence electrons of lithium in the formation of Li2O?

• They are shared with oxygen

• They are transferred to oxygen

• They remain with lithium

• They are lost to the environment

What charge does oxygen acquire after gaining electrons from lithium?

• 2-

• 1-

• 2+

• 1+

What is the charge on each lithium ion after electron transfer?

• 1-

• 2+

• 1+

• 2-

What is the purpose of placing brackets around ions in the Lewis structure?

• To show the ionic nature

• To indicate shared electrons

• To denote molecular geometry

• To highlight the central atom

What does the term 'formula unit' refer to in the context of Li2O?

• An isolated atom

• A covalent bond

• A repeating array in a crystal

• A single molecule