Oxidation Numbers in OF2

The video tutorial explains how to determine the oxidation numbers of elements in the compound oxygen difluoride (OF2). It highlights the unique case where oxygen has a positive oxidation number due to fluorine's higher electronegativity. The tutorial demonstrates an algebraic approach to calculate these numbers, confirming that in OF2, fluorine has an oxidation number of -1, and oxygen has +2. The video concludes with a summary of these findings.

What is the total sum of oxidation numbers in a neutral molecule like OF2?

• It is always negative.

• It is always positive.

• It is zero.

• It depends on the elements present.

In most compounds, what is the typical oxidation number of oxygen?

• -1

• +2

• -2

• +1

Why does fluorine have a -1 oxidation number in OF2?

• Because it is less electronegative than oxygen.

• Because it shares electrons equally with oxygen.

• Because it is more electronegative than oxygen.

• Because it forms a positive ion.

What is the role of electronegativity in determining oxidation numbers in OF2?

• It has no role.

• It makes oxygen more electronegative.

• It makes fluorine more electronegative.

• It makes both elements equally electronegative.

How do you set up the equation to find the oxidation number of oxygen in OF2?

• x + 2 = 0

• x + (-2) = 0

• x - 2 = 0

• 2x + 1 = 0

What is the oxidation number of oxygen in OF2?

• +1

• +2

• -1

• -2

Which method can be used to determine the oxidation number of oxygen in OF2?

• Both algebraic method and visual inspection

• Only visual inspection

• Only algebraic method

• Neither method

What is unusual about the oxidation number of oxygen in OF2 compared to its usual state?

• It is zero.

• It is the same as usual.

• It is more positive than usual.

• It is more negative than usual.