How to write the correct formula for Iron (III) Nitride

Understanding Iron (III) Nitride

To determine the correct formula for Iron (III) Nitride, you need to understand the charges and the combining ratios of the ions involved.

Analyzing Iron (III)

Iron (III) refers to iron in its +3 oxidation state, which we denote as $\text{Fe}^{3+}$.

Analyzing Nitride

Nitride refers to nitrogen in its -3 oxidation state, denoted as $\text{N}^{3-}$.

Combining Ions

To write the correct formula, you need to balance the total positive and negative charges. Since Iron (III) and Nitride have charges of +3 and -3 respectively, one iron ion will balance with one nitride ion.

Correct Formula

The correct formula for Iron (III) Nitride is:

Where:

• $\text{Fe}^{3+}$ is the iron (III) ion
• $\text{N}^{3-}$ is the nitride ion

In summary, the subscript for each ion is 1 as the charges balance without any additional balancing requirements.

Understanding the Oxidation State of Iron (III) as +3

The term oxidation state refers to the degree of oxidation of an atom in a chemical compound. The oxidation state of an element in a particular compound provides insight into the distribution of electrons among the atoms.

Determining the Oxidation State

When we refer to the oxidation state of iron (III) as +3, we are indicating that iron in this compound has an oxidation number of +3. This is often indicated by the Roman numeral III in parentheses.

Example: Iron (III) Chloride

Consider iron (III) chloride, which is commonly represented by the formula $\text{FeCl}_3$. Here's how we determine the oxidation state:

1. Chlorine ($\text{Cl}$) typically has an oxidation state of $-1$.

2. Since there are three chlorine atoms, the total negative charge contributed by chlorine is:

   $$3 \times (-1) = -3$$

3. To balance this, iron ($\text{Fe}$) must have a positive oxidation state that counters the $-3$ from chlorine. Thus, the oxidation state of iron here is $+3$.

General Rule

In general:

• The sum of oxidation states of all atoms in a neutral compound must be zero.
• The sum for a polyatomic ion is equal to the charge of that ion.

Importance

Identifying the oxidation state of iron as $+3$ is crucial in various chemical processes, such as redox reactions, coordination chemistry, and industrial metallurgy. It plays a significant role in understanding the behavior and reactivity of iron in different chemical environments.

Example Reaction

An example reaction involving iron in the +3 oxidation state:

This reaction highlights the reduction of $\text{Fe}^{3+}$ (oxidation state +3) to elemental iron (oxidation state 0) through the gain of three electrons.

Conclusion

In summary, iron (III) in a compound signifies an oxidation state of +3, meaning that iron has lost three electrons. This oxidation state is essential for predicting and understanding the chemical behavior of iron in various compounds and reactions.

Explanation

In chemistry, the oxidation state (or oxidation number) of an element indicates the number of electrons lost or gained by an atom of that element in a compound. For nitride, we often refer to nitrogen in its most reduced form, which is when nitrogen gains electrons to achieve a stable configuration.

Understanding Oxidation State of Nitride

The nitride ion is represented as $\text{N}^{3-}$. This indicates that nitrogen has gained three electrons. In chemical terms, gaining electrons corresponds to a reduction in oxidation state. Therefore, the oxidation state of nitrogen in the nitride ion is $-3$.

Chemical Context

In compounds containing the nitride ion, nitrogen typically exists in an oxidation state of $-3$. For example:

1. Lithium Nitride (Li$_3$N)

   Lithium Nitride is composed of lithium and nitrogen. Lithium typically has an oxidation state of $+1$. The compound must be neutral overall, so the oxidation states must balance out.

   $$3 (\text{Li}^{+1}) + (\text{N}^{3-}) = 0$$ $$3 \cdot (+1) + (-3) = 0$$

   This confirms that nitrogen is in the $-3$ oxidation state.

2. Magnesium Nitride (Mg$_3$N$_2$)

   Similarly, in Magnesium Nitride, magnesium has an oxidation state of $+2$. To balance the two nitride ions in the formula, we have:

   $$3 (\text{Mg}^{+2}) + 2 (\text{N}^{3-}) = 0$$ $$3 \cdot (+2) + 2 \cdot (-3) = 0$$

   This also confirms that nitrogen is in the $-3$ oxidation state here.

Importance in Chemistry

The oxidation state of $-3$ for nitride is significant because it highlights nitrogen's ability to form stable ions by gaining electrons. This is the lowest oxidation state that nitrogen can achieve, representing its most reduced form. Understanding this helps in predicting the behavior of nitrogen in various chemical reactions and compounds.

Summary

The oxidation state of nitride as $-3$ indicates that nitrogen has gained three electrons. This is a key point in understanding nitrogen chemistry and its behavior in various compounds. The ability to hold a $-3$ oxidation state allows nitrogen to participate in the formation of numerous stable compounds.