Oxidation Numbers in FeS Compounds

The video tutorial explains how to determine the oxidation numbers for elements in iron(II) sulfide (FeS). It begins by noting that FeS is a neutral compound, meaning the sum of oxidation numbers must equal zero. The tutorial highlights that iron, a transition metal, can have varying oxidation states depending on its bonding. A special rule is introduced, stating that the more electronegative element in a binary compound takes the oxidation number of its ion charge. For sulfur, this is -2. Consequently, iron must have an oxidation number of +2 to balance the compound. The video concludes with a summary of these calculations.

What is the significance of the compound FeS being neutral?

• It indicates that the oxidation numbers add up to zero.

• It suggests that sulfur has a positive oxidation number.

• It means the compound has a net positive charge.

• It implies that iron has a negative oxidation number.

Why is it challenging to determine the oxidation number of iron in FeS?

• Iron is not present in FeS.

• Iron is a non-metal.

• Iron is a transition metal and its oxidation number depends on what it is bonded to.

• Iron always has a fixed oxidation number.

What is the oxidation number of sulfur in FeS according to the special rule?

• +1

• -2

• +2

• 0

Which group does sulfur belong to, and what is its typical charge?

• Group 16, -2

• Group 2, +2

• Group 17, -1

• Group 1, +1

How do the oxidation numbers of iron and sulfur in FeS add up?

• They add up to zero.

• They add up to +1.

• They add up to -2.

• They add up to +2.

What is the oxidation number of iron in FeS?

• +2

• +3

• 0

• +1

Why does the sulfide ion have an oxidation number of -2?

• Because it is in Group 1 and typically has a charge of +1.

• Because it is in Group 16 and typically has a charge of -2.

• Because it is in Group 17 and typically has a charge of -1.

• Because it is in Group 2 and typically has a charge of +2.