Oxidation Numbers in Bromate Ion

The video tutorial explains how to determine the oxidation number of bromine in the bromate ion (BrO3-). It begins by discussing the general rule that the sum of oxidation numbers in a compound equals the charge of the ion. The video then demonstrates the calculation process, showing that oxygen typically has an oxidation number of -2, leading to a total of -6 for three oxygens. To balance this with the ion's charge of -1, bromine must have an oxidation number of +5. An algebraic method is also presented to verify this result. The video concludes with a summary of the findings.

What is the main focus of the video tutorial?

• Calculating the oxidation number of bromine in the bromate ion

• Explaining the concept of reduction

• Determining the charge of the sulfate ion

• Finding the oxidation number of oxygen in water

What is the typical oxidation number assigned to oxygen in compounds?

• 0

• +1

• -1

• -2

How do the oxidation numbers of the elements in the bromate ion relate to the ion's charge?

• They add up to zero

• They add up to the ion's charge of -1

• They add up to +1

• They do not relate to the ion's charge

What is the oxidation number of bromine in the bromate ion?

• +3

• +5

• -1

• 0

In the algebraic method, what variable is used to represent the unknown oxidation number of bromine?

• b

• x

• z

• y

What is the result of adding the oxidation numbers of three oxygen atoms in the bromate ion?

• +6

• -6

• +3

• -3

What is the final step in solving for the oxidation number of bromine using algebra?

• Divide both sides by 3

• Multiply both sides by 2

• Add 6 to both sides

• Subtract 6 from both sides

What is the conclusion of the video regarding the oxidation number of bromine in the bromate ion?

• It is -1

• It is +3

• It is 0

• It is +5