Oxidation States and Chlorine Properties

The video tutorial explains how to determine the oxidation number of gold in the AuCl4- ion. It begins by discussing the concept of oxidation numbers and ions, then focuses on the specific case of AuCl4-. The tutorial explains that chlorine, being in group 17, typically has an oxidation state of -1. Using this information, the video demonstrates how to calculate the oxidation number of gold in the ion, which is found to be +3. The tutorial concludes with a summary of the process.

What is the total charge of the ion AuCl4-?

• -2

• +1

• 0

• -1

Which group does chlorine belong to, and what is its usual oxidation state?

• Group 15, -3

• Group 18, 0

• Group 17, -1

• Group 16, -2

Why can gold have different oxidation states?

• Because it is a transition metal

• Because it is a halogen

• Because it is an alkali metal

• Because it is a noble gas

How many chlorine atoms are present in AuCl4-?

• 3

• 2

• 4

• 5

What equation is set up to find the oxidation number of gold in AuCl4-?

• x + 4 = -1

• x - 4 = -1

• x + 1 = 4

• x - 1 = 4

What is the oxidation number of gold in AuCl4-?

• +1

• +2

• +3

• +4

What is the final step to solve for the oxidation number of gold in the equation x - 4 = -1?

• Add 4 to both sides

• Divide both sides by 4

• Subtract 4 from both sides

• Multiply both sides by 4