Oxidation Numbers and Peroxide Ions

The video tutorial explains the concept of oxidation numbers, focusing on the peroxide ion O2 2-. It details how oxidation numbers in ions add up to the ion's charge, using O2 2- as an example. The video also covers the conventions for writing oxidation numbers and highlights exceptions, such as peroxides, where oxygen has an oxidation number of -1 instead of the usual -2. The tutorial concludes with a brief thank you from Dr. B.

What is the oxidation number of each oxygen atom in the peroxide ion (O2 2-)?

• -1

• -2

• 0

• +1

In the context of ions, how do the oxidation numbers relate to the charge of the ion?

• They are always negative.

• They add up to the charge of the ion.

• They are equal to the number of atoms.

• They are always positive.

What is the total charge of the peroxide ion (O2 2-)?

• +2

• -2

• 0

• -1

Why is the oxidation number of oxygen in peroxides different from its usual state?

• Because it is bonded to hydrogen.

• Because it is in a different group.

• Because it is in a gaseous state.

• Because it forms a peroxide ion.

How is the notation for oxidation numbers different from that of charges?

• The negative sign comes before the number in oxidation numbers.

• Oxidation numbers use Roman numerals.

• Charges are always written in brackets.

• Oxidation numbers are always positive.

Which of the following is an exception to the typical oxidation state of oxygen?

• Oxygen in carbon dioxide

• Oxygen in water

• Oxygen in ozone

• Oxygen in peroxides