Chlorate Ion and Oxidation States

The video tutorial explains how to determine the oxidation number of iron in iron(III) chlorate (Fe(ClO3)3). It begins by discussing the significance of the 'III' in iron(III) chlorate, indicating the oxidation state of iron. The tutorial then explains that since the compound is neutral, the sum of oxidation numbers must equal zero. It further elaborates on the chlorate ion, which has a charge of -1, and how this affects the overall oxidation state of the compound. The video concludes with a reminder to memorize the charge of the chlorate ion and offers additional resources for understanding the oxidation state of chlorine in the chlorate ion.

What is the oxidation number of iron in iron(III) chlorate?

• +1

• +2

• +4

• +3

Why must the oxidation numbers in a neutral compound add up to zero?

• Because the compound has no net charge

• To ensure the compound is stable

• To balance the chemical equation

• Because it is a rule of thumb

What is the ionic charge of the chlorate ion?

• 2+

• 1-

• 1+

• 2-

How does the charge of the chlorate ion affect the oxidation number of iron?

• It requires the oxidation number of iron to be positive

• It makes the oxidation number of iron negative

• It doubles the oxidation number of iron

• It has no effect on the oxidation number of iron

What is the total charge of three chlorate ions?

• 3+

• 3-

• 1-

• 2-

What should you memorize about the chlorate ion?

• Its ionic charge

• Its color

• Its molecular weight

• Its boiling point

Where can you find additional help for understanding the oxidation state of chlorine in chlorate?

• In a biology class

• In a physics lecture

• At the end of the video

• In a chemistry textbook