Phosphate Ions and Iron Compounds

This video tutorial explains how to determine the oxidation number of iron in the compound Fe3(PO4)2. It begins by noting that the compound is neutral, meaning all oxidation numbers must sum to zero. The video then identifies the phosphate ion (PO4) with a charge of 3-, and explains that two phosphate ions contribute a total charge of -6. To balance this, the oxidation number of iron must be +2, resulting in the compound being named iron(II) phosphate. Additional resources are provided for finding the oxidation number of phosphorus in the phosphate ion.

What is the overall charge of the compound Fe3(PO4)2?

• Depends on the environment

• Positive

• Negative

• Neutral

What is the charge of a single phosphate ion (PO4)?

• 2-

• 4-

• 3-

• 1-

How many phosphate ions are present in Fe3(PO4)2?

• One

• Two

• Three

• Four

What is the total negative charge contributed by the phosphate ions in Fe3(PO4)2?

• -3

• -6

• -12

• -9

What is the oxidation number of iron in Fe3(PO4)2?

• +1

• +2

• +4

• +3

Why is the oxidation number of iron in Fe3(PO4)2 important?

• It changes the compound's state of matter.

• It determines the color of the compound.

• It helps balance the overall charge to zero.

• It affects the solubility of the compound.

What is the compound Fe3(PO4)2 commonly referred to as?

• Iron(IV) phosphate

• Iron(III) phosphate

• Iron(I) phosphate

• Iron(II) phosphate

Where can you find more information on the oxidation number of phosphorus in the phosphate ion?

• In the video description

• In the video thumbnail

• In the video title

• In the video comments

Who is the presenter of the video?

• Dr. A

• Dr. B

• Dr. C

• Dr. D