Problem 68 - Chemistry

Question

What are the oxidation numbers of \(\mathrm{O}\) and \(\mathrm{F}\) in \(\mathrm{HFO} ?\)

Step-by-Step Solution

Answer

The oxidation number of Oxygen (O) is -2 and the oxidation number of Fluorine (F) is -1 in HFO.

Step 1: Identify Hydrogen Oxidation Number

The oxidation number of Hydrogen (H) is usually +1 in its compounds. So, \(H=+1\).

Step 2: Identify Fluorine Oxidation Number

Fluorine (F) always has an oxidation number of -1 in its compounds. So, \(F=-1\).

Step 3: Calculate Oxygen Oxidation Number

Add the oxidation numbers of H and F, and subtract from zero because the overall charge of the compound is 0 (since there are no charges indicated in HFO). For Oxygen (O): since The sum of oxidation numbers in neutral compound = 0, then \(O = 0 - (+1) - (-1) = -2\).

Key Concepts

Understanding Oxidation State

The oxidation state, or oxidation number, is a useful concept in chemistry to understand the distribution of electrons in chemical compounds. It helps us determine how electrons are shared or transferred between atoms. Generally, it represents the hypothetical charge that an atom would have if all bonds were 100% ionic, where atoms completely transfer electrons.

Each atom in a molecule generally has an assigned oxidation number, which varies based on the element's characteristics and the compound they are in. By knowing oxidation numbers, chemists can predict the reactivity and properties of molecules.

• Oxidation numbers help in balancing chemical equations.
• They assist in identifying the oxidizing and reducing agents in reactions.
• They are crucial for understanding redox reactions.

Hydrogen Oxidation Number

In most chemical compounds, hydrogen has an oxidation number of +1. This is due to hydrogen's tendency to lose its one electron, making it more positive. However, exceptions can occur such as in metal hydrides (e.g., \( \text{NaH} \)), where hydrogen's oxidation number is -1.

Examples of compounds where hydrogen is +1 include water (\( \text{H}_2\text{O} \)), acids, and organic molecules. Knowing hydrogen's typical oxidation state can greatly simplify the process of determining the overall oxidation states in a compound.

Fluorine Oxidation Number

Fluorine is the most electronegative element, meaning it strongly attracts electrons. As such, its oxidation number is always -1 in its compounds. This constant behavior makes it a strong agent in pulling electrons towards itself and stabilizing negative charges.

This tendency of fluorine helps us quickly establish its oxidation state in all compounds, which simplifies calculations involving oxidation, such as balancing redox reactions. In any given fluorine compound, you can safely assume fluorine is -1.

Oxygen Oxidation Number

Oxygen typically has an oxidation number of -2 in its compounds, with a few exceptions. This is because oxygen tends to attract electrons due to its high electronegativity. In peroxides (e.g., \( \text{H}_2\text{O}_2 \)), its oxidation number is -1, and in compounds with fluorine (like \( \text{OF}_2 \)), it can be positive.

In the compound \( \text{HFO} \), we determine oxygen's oxidation state by considering the overall charge of the compound, which we assume to be neutral. Given hydrogen's +1 and fluorine's -1 oxidation states, oxygen must be -2 to balance the overall equation. This common assignment helps predict a molecule's behavior in redox reactions and synthesis processes.