Oxidation Numbers and Nitrate Ions

This video tutorial explains how to determine the oxidation number of manganese in Mn(NO3)2, also known as manganese(II) nitrate. It covers the rules for calculating oxidation numbers in neutral compounds and ions, emphasizing that the sum of oxidation numbers in a neutral compound is zero, while in an ion, it equals the ion's charge. The video provides a step-by-step calculation, showing that manganese must have a +2 oxidation number to balance the -2 from the nitrate ions. Additional resources are mentioned for further learning.

In a neutral compound, what should the sum of all oxidation numbers be?

• 0

• -1

• +1

• +2

What is the charge of the nitrate ion?

• +2

• -1

• 0

• +1

What is the oxidation number of manganese in Mn(NO3)2?

• +1

• +2

• +3

• +4

How many nitrate ions are present in Mn(NO3)2?

• 4

• 3

• 2

• 1

If the nitrate ion has a -1 charge, what is the total charge contributed by two nitrate ions?

• -1

• -2

• -3

• -4

What must the oxidation number of manganese be to balance the charges in Mn(NO3)2?

• +2

• +1

• +4

• +3

Where can you find additional help for finding oxidation numbers in the nitrate ion?

• In the video description

• In a separate video

• In a textbook

• In a card linked in the video