General Chemistry | Lewis Structures (Example #3)

The video tutorial explains how to draw the Lewis structure for chloroform (CHCl3). It begins with a brief history of chloroform's use as an anesthetic. The tutorial then guides viewers through the process of counting valence electrons, determining the central atom, and adding lone pairs to complete the Lewis structure. Key concepts include the calculation of valence electrons, the role of the central atom, and the importance of lone pairs in achieving a stable structure.

What was chloroform historically used for?

• As a cleaning agent

• As an anesthetic

• As a fuel

• As a food preservative

How many valence electrons does a carbon atom have?

• 8

• 6

• 4

• 2

Which group does chlorine belong to in the periodic table?

• Group 1

• Group 4

• Group 7

• Group 8

Why is hydrogen never the central atom in a Lewis structure?

• It is always bonded to oxygen

• It cannot have more than two electrons

• It is too small

• It can only form one bond

In chloroform, which atom is the central atom?

• Carbon

• Chlorine

• Hydrogen

• Oxygen

How many lone pairs are added to each chlorine atom in the Lewis structure of chloroform?

• Four

• One

• Two

• Three

What is the total number of valence electrons in chloroform?

• 30

• 26

• 24

• 28