Oxidation Numbers and IO4- Ion

The video tutorial explains how to determine the oxidation numbers for elements in the IO4- ion, known as the periodate ion. It begins by introducing the concept of oxidation numbers and the rules for determining them, particularly focusing on oxygen and iodine. The tutorial highlights that oxygen typically has an oxidation number of -2, while iodine, despite being in group 17, can have exceptions when bonded to oxygen. The video then demonstrates the calculation process, showing that the sum of oxidation numbers equals the ion's charge, leading to the conclusion that iodine has an oxidation number of +7 in IO4-. The tutorial concludes with a recap of the steps taken to find the oxidation numbers.

What is the main focus of the video tutorial?

• Balancing chemical equations

• Finding oxidation numbers in IO4- ion

• Understanding molecular geometry

• Learning about ionic bonds

What is the typical oxidation state of oxygen in compounds?

• +2

• -1

• -2

• 0

How many oxygen atoms are present in the IO4- ion?

• 3

• 4

• 5

• 2

Why can't the usual rule for iodine's oxidation state be applied in IO4-?

• Iodine is in a gaseous state

• Iodine is bonded to oxygen

• Iodine is in a liquid state

• Iodine is bonded to a metal

What is the total oxidation number for the four oxygen atoms in IO4-?

• -10

• -8

• -6

• -4

What is the charge on the IO4- ion?

• +1

• -2

• 0

• -1

What is the oxidation number of iodine in the IO4- ion?

• +5

• +6

• +7

• +8

What is the final step in determining the oxidation number of iodine in IO4-?

• Multiplying the oxidation numbers of oxygen

• Adding the oxidation numbers of all elements

• Dividing the oxidation numbers of oxygen

• Subtracting the oxidation numbers of oxygen from the charge