Oxidation States of Oxygen and Fluorine

The video tutorial explains the oxidation numbers for each element in the compound O2 F2, also known as dioxygen difluoride. It highlights the neutrality of the compound and the unique oxidation states of oxygen and fluorine. Oxygen, typically having an oxidation state of -2, is +1 in this compound due to fluorine's higher electronegativity. Fluorine always has an oxidation state of -1. The video concludes by summarizing these oxidation states and their implications.

What is another name for the compound O2 F2?

• Fluorine oxide

• Dioxygen difluoride

• Dioxygen monoxide

• Oxygen fluoride

Why do the oxidation numbers in O2 F2 add up to zero?

• Because it is a neutral compound

• Because it contains only fluorine

• Because it is a charged compound

• Because it contains only oxygen

What is the usual oxidation state of oxygen?

• -2

• -1

• +1

• 0

In O2 F2, what is the oxidation state of fluorine?

• -2

• -1

• 0

• +1

Why is fluorine's oxidation state always -1?

• Because it is less electronegative than oxygen

• Because it is more electronegative than oxygen

• Because it is neutral

• Because it is a metal

What is the oxidation state of oxygen in O2 F2?

• 0

• +1

• +2

• -1

Which element in O2 F2 has an unusual oxidation state compared to its typical state?

• Oxygen

• Fluorine

• Neither oxygen nor fluorine

• Both oxygen and fluorine