Question

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

Short answer

In HFO, O has an oxidation number of 0, and F has -1.

Step-by-step solution

Understanding Oxidation Number

The oxidation number is the charge that an atom would have if the compound was composed of ions. It provides an indication of the degree of oxidation of an element in a chemical compound.

Assign Known Oxidation Numbers

Fluorine ( F ) is the most electronegative element and always has an oxidation number of -1 in its compounds. Therefore, in HFO, the oxidation number of F is -1.

Assign Hydrogen's Oxidation Number

Hydrogen typically has an oxidation number of +1 when bonded to nonmetals. Thus in HFO, assign hydrogen an oxidation number of +1.

Calculate Oxygen's Oxidation Number

To find the oxidation number of oxygen, use the fact that the sum of oxidation numbers for all atoms in a neutral molecule is zero. Let x be the oxidation number of oxygen. The equation becomes: \[+1 (from\, H) + x (from\, O) - 1 (from\, F) = 0\]Solving for x: \[x = 0\]Therefore, the oxidation number of oxygen in HFO is 0.

Key concepts

Fluorine

Fluorine, symbolized as \( F \), is renowned for being the most electronegative element on the periodic table. This means it has a very strong tendency to attract electrons towards itself when forming chemical bonds. As a result, fluorine almost always carries an oxidation number of -1, especially in compounds with nonmetals.
Fluorine's high electronegativity dictates that it will aggressively pull electrons closer, giving it a more negative oxidation state. This is why in the compound HFO, the oxidation number assigned to fluorine is consistently -1.

• Most electronegative element
• Oxidation number usually -1
• Attracts electrons strongly

Understanding fluorine's behavior in chemical reactions is crucial for predicting how molecules will interact and what products they might form.

Hydrogen

Hydrogen is the simplest and most abundant element in the universe, represented by the symbol \( H \). It normally exists with an oxidation number of +1 when paired with nonmetals. This is due to its relatively higher electronegativity compared to metals, which allows it to often "donate" its single electron.
In the context of the compound HFO, hydrogen's oxidation state of +1 is used in balancing the overall charges of the molecule, maintaining the necessary condition where the sum of oxidation numbers in a neutral molecule equals zero.

• Typically +1 oxidation state with nonmetals
• Contributes to balancing charge
• Single electron donor

By assigning an oxidation number of +1 to hydrogen in compounds like HFO, it helps elucidate the overall chemical formula and stability of the molecule.

Oxygen

Oxygen, with the chemical symbol \( O \), is a common element that typically exhibits an oxidation number of -2 in most compounds due to its electronegativity. However, in some molecules like HFO, its oxidation number can deviate from this usual state.
For the molecule HFO, calculating the oxidation number of oxygen relies on the principle that the sum of oxidation numbers in a neutral molecule must equate to zero. Given hydrogen's +1 and fluorine's -1, oxygen assumes an oxidation number of 0 in this unique compound to satisfy the charge balance.

• Usually -2 oxidation state
• Variable in fluorine compounds
• Neutral molecule charge neutrality

This example underscores the importance of understanding oxidation numbers as adaptable parameters essential for accurately interpreting complex molecular interactions.

Electronegativity

Electronegativity is a foundational concept in chemistry, referring to an atom's ability to attract electrons toward itself. Fluorine holds the title of the most electronegative element, which greatly influences its behavior in chemical bonding. In contrast, hydrogen has a moderate electronegativity, positioning it usually just above many metals, which influences its typical oxidation number of +1.
The differences in electronegativity between the elements within a compound determine how atoms share or transfer electrons, thus resulting in particular oxidation numbers.

• Drives electron attraction
• Crucial for oxidation number assignment
• Fluorine: most electronegative

Understanding electronegativity helps clarify why elements prefer certain oxidation states and how compounds reach chemical stability.

Neutral Molecule

A neutral molecule is a chemical compound that has no overall charge. This is a balanced system where the sum of the oxidation numbers of all the atoms equals zero. For example, in the molecule HFO, the combined oxidation numbers of hydrogen (+1), fluorine (-1), and oxygen (0) lead to this balanced, neutral state.
This concept is critical in identifying the oxidation states of atoms because it provides a constraint that helps calculate unknown oxidation numbers.

• Overall charge is zero
• Sum of oxidation numbers equals zero
• Helpful in solving oxidation number problems

Recognizing the neutrality of a molecule aids in deducing the distribution of electrons among atoms and understanding chemical formulas more effectively.