Understanding Manganese and Sulfate Ions

This video tutorial explains how to determine the oxidation numbers for elements in MnSO4, specifically focusing on manganese and sulfate ions. It begins by introducing the concept of oxidation numbers and their significance in neutral compounds. The tutorial then delves into the sulfate ion, explaining how its oxidation numbers add up to its ionic charge. Finally, it calculates the oxidation state of manganese in MnSO4, concluding with additional resources for further learning.

What does the absence of a charge on Mn(SO4)2 indicate about the compound?

• It is a positively charged compound.

• It is a negatively charged compound.

• It is a neutral compound.

• It is an unstable compound.

What is the total charge of the sulfate ion in Mn(SO4)2?

• -2

• -1

• -4

• 0

How many sulfate ions are present in Mn(SO4)2?

• 3

• 2

• 4

• 1

What must be the oxidation state of manganese in Mn(SO4)2 to balance the charges?

• +5

• +3

• +2

• +4

Why is manganese assigned an oxidation state of +4 in Mn(SO4)2?

• To balance the -4 charge from two sulfate ions.

• To balance the -2 charge from one sulfate ion.

• Because manganese always has an oxidation state of +4.

• To make the compound positively charged.

Where can you find more information on determining the oxidation state of sulfur in sulfate ions?

• In the video description.

• In the video comments.

• In the video title.

• In the video thumbnail.