Oxidation Numbers in Iron Compounds

The video tutorial explains how to determine the oxidation number for each element in the ion FeO4 2-. It begins by introducing the concept of oxidation numbers and their role in ions. The tutorial then explains that the sum of oxidation numbers in an ion equals the ion's charge. Oxygen is identified as having a typical oxidation state of -2, except in certain compounds. An equation is set up to find the oxidation number of iron, resulting in a value of +6. The video concludes by summarizing the process and confirming the result.

What is the charge on the ion FeO4 2-?

• 2+

• 2-

• 4+

• 4-

What is the sum of the oxidation numbers in an ion equal to?

• The atomic number of the central atom

• Zero

• The number of atoms in the ion

• The charge on the ion

Which element in FeO4 2- typically has an oxidation number of -2?

• Hydrogen

• Iron

• Oxygen

• Fluorine

What is the oxidation number of each oxygen atom in FeO4 2-?

• +2

• +1

• -2

• -1

How do you set up the equation to find the oxidation number of iron in FeO4 2-?

• x - 4 = 0

• x + 8 = 2

• x + 2 = 0

• x - 8 = -2

What is the oxidation number of iron in FeO4 2-?

• +4

• +2

• +8

• +6

Why is the oxidation number of iron in FeO4 2- considered unusual?

• Iron usually has a negative oxidation number.

• Iron is typically found with an oxidation number of +2 or +3.

• Iron cannot have an oxidation number greater than +4.

• Iron is not a transition metal.