Question

What is the oxidation number of \(\mathrm{O}\) in HFO?

Short answer

The oxidation number of O in HFO is 0.

Step-by-step solution

Understanding Oxidation Numbers

Oxidation numbers provide a way to keep track of electron transfers in compounds. They indicate the charge of an atom that has either gained or lost electrons. Common oxidation numbers include -1 for fluorine and +1 for hydrogen.

Assign Known Oxidation Numbers

In the compound HFO, we know the oxidation numbers of hydrogen ( ext{H}) is +1 and fluorine ( ext{F}) is -1 based on their common states in compounds.

Setting Up the Equation

The sum of the oxidation numbers in a neutral molecule must equal zero. Let's set up the equation: Let the oxidation number of oxygen ( ext{O}) be x. The equation will be: (+1) + (x) + (-1) = 0.

Solving for Oxidation Number of Oxygen

Solve the equation: (+1) + (x) + (-1) = 0 This simplifies to: x = 0.

Conclusion

The oxidation number of oxygen in the compound HFO is determined to be 0 based on balancing the sum of oxidation numbers to zero.

Key concepts

Electron Transfers in Compounds

In chemistry, understanding electron transfers is crucial to grasp how atoms interact and form compounds. Each atom tends to gain or lose electrons to achieve a more stable electronic configuration.
When atoms bond, the concept of oxidation numbers helps us track these changes in electron distribution.
Here's how it works:

• If an atom loses electrons, it results in a positive oxidation number.
• Conversely, if it gains electrons, the oxidation number becomes negative.

These numbers are essential to determine the oxidation state of elements within a compound and predict how they will react chemically. In any compound, the total of all oxidation numbers must sum to the overall charge of the compound. This principle is a fundamental rule used to balance chemical equations and explain oxidation-reduction reactions.

Oxidation State of Oxygen

Oxygen is a key element in numerous compounds, and its oxidation state is important for understanding chemical behaviors. Typically, oxygen has a common oxidation state of -2.
This is due to its electronegativity, meaning it tends to attract electrons towards itself.
However, there are exceptions to this rule:

• In peroxides, like hydrogen peroxide (H₂O₂), oxygen has an oxidation state of -1, due to equal sharing of electrons.
• In some complex molecules, such as the one encountered in the exercise (HFO), oxygen may have a different oxidation state, here determined to be 0.
• In compounds like OF₂, where a more electronegative element than oxygen is present, oxygen can have a positive oxidation state, such as +2.

Understanding these variations helps make predictions about the properties and reactions of oxygen-containing compounds.

Balancing Oxidation Numbers

Balancing oxidation numbers is essential to ensure the stability of chemical compounds. When dealing with a neutral compound such as HFO, the sum of all oxidation numbers must equal zero.
By doing this, we confirm the molecular integrity and charge balance.
Here's how it was achieved in the exercise:

• Assign the known oxidation numbers: +1 for hydrogen and -1 for fluorine.
• Set the equation for the compound's oxidation numbers, ensuring they add up to zero. In HFO, this was expressed as: \((+1) + x + (-1) = 0\).
• Solve for the unknown, here the oxidation number of oxygen, which came to be 0.

This method can be applied to any compound to ensure that it adheres to the laws of conservation of electric charge, a foundational concept in chemical reactions and stoichiometry.