Oxidation Numbers and Chlorine Ions

The video tutorial explains how to find the oxidation number of chlorine in ClF4-. It begins by discussing the concept of oxidation numbers and the significance of the ion's charge. The tutorial then sets up an equation to determine the oxidation number of chlorine, considering the electronegativity of fluorine. By solving the equation, it concludes that the oxidation number of chlorine in ClF4- is +3. The video ends with a verification of the result.

What does the negative charge in ClF4- indicate about the ion?

• It has no charge.

• It is an ion with a negative charge.

• It has a positive charge.

• It is a neutral molecule.

When determining oxidation numbers, what should the sum of oxidation numbers in an ion equal?

• The charge of the ion

• The number of atoms

• Zero

• The atomic number of the central atom

Why is the oxidation number of fluorine always -1?

• Because it is a noble gas

• Because it is highly electronegative

• Because it is in group 17

• Because it forms diatomic molecules

What variable is used to represent the oxidation number of chlorine in the equation?

• a

• z

• y

• x

What is the equation set up to find the oxidation number of chlorine in ClF4-?

• x + 4 = -1

• x - 4 = -1

• x - 4 = 1

• x + 4 = 1

What is the oxidation number of chlorine in ClF4- after solving the equation?

• +3

• +2

• +4

• +1

How do you verify the oxidation number of chlorine in ClF4-?

• By checking if the sum equals the number of atoms

• By checking if the sum equals the charge of the ion

• By checking if the sum equals zero

• By checking if the sum equals the atomic number of chlorine

What is the final charge on the ClF4- ion after adding the oxidation numbers?

• +1

• 0

• -1

• -2