Question

must do: transition binary ionic
started: oct 28 at 9:17am
quiz instructions
question 1
name the following compound
fe₂s₃

Explanation:

Step1: Identify the elements

The compound \(Fe_2S_3\) contains iron (\(Fe\)) and sulfur (\(S\)).

Step2: Determine the oxidation state of iron

In \(Fe_2S_3\), sulfur has an oxidation state of \(- 2\). Let the oxidation state of \(Fe\) be \(x\). Using the formula for charge neutrality in a compound: \(2x+3\times(-2) = 0\). Solving for \(x\): \(2x-6 = 0\), so \(2x=6\) and \(x = + 3\).

Step3: Name the compound

For transition - metal ionic compounds, we use the Roman numeral for the oxidation state of the metal. The anion is sulfide (\(S^{2-}\)). So the name is iron(III) sulfide.

Answer:

iron(III) sulfide