Iron(II) Bromide and Oxidation States

The video tutorial explains how to determine the oxidation state of elements in the compound FeBr2, iron(II) bromide. It starts by noting that the compound is neutral, meaning the oxidation numbers must sum to zero. Bromine, being in group 17, typically has a -1 oxidation state. With two bromine atoms, the total is -2, requiring iron to have a +2 oxidation state to balance it out. This is why the compound is named iron(II) bromide, indicating the +2 state of iron.

What is the overall charge of the compound FeBr2?

• Positive

• Variable

• Negative

• Neutral

Which group does bromine belong to, and what is its typical oxidation state?

• Group 17, -1

• Group 1, +1

• Group 16, -2

• Group 18, 0

How many bromine atoms are present in FeBr2, and what is their combined oxidation state?

• Two bromine atoms, -2

• One bromine atom, -1

• Four bromine atoms, -4

• Three bromine atoms, -3

What must be the oxidation state of iron in FeBr2 to balance the compound?

• +1

• +2

• +3

• +4

Why is FeBr2 referred to as iron(II) bromide?

• Because iron has a +2 oxidation state

• Because iron has a +1 oxidation state

• Because bromine has a -2 oxidation state

• Because bromine has a -1 oxidation state

What is the significance of the Roman numeral in the name iron(II) bromide?

• It indicates the total charge of the compound

• It indicates the number of bromine atoms

• It indicates the oxidation state of iron

• It indicates the oxidation state of bromine