Question

A variety of chlorine oxide fluorides and related cations and anions are known. They tend to be powerful oxidizing and fluorinating agents. \(\mathrm{FClO}_{3}\) is the most stable of this group of compounds and has been studied as an oxidizing component in rocket propellants. Draw a Lewis structure for \(\mathrm{F}_{3} \mathrm{ClO}\) , \(\mathrm{F}_{2} \mathrm{ClO}_{2}^{+},\) and \(\mathrm{F}_{3} \mathrm{ClO}_{2}\) . What is the molecular structure for each species, and what is the expected hybridization of the central chlorine atom in each compound or ion?

Short answer

The molecular structures and expected hybridizations for the three species are as follows: 1. F₃ClO: Molecular structure: Tetrahedral (four electron groups) Expected hybridization: sp³ (four electron groups) 2. F₂ClO₂⁺: Molecular structure: Trigonal bipyramidal (five electron groups) Expected hybridization: sp³d (five electron groups) 3. F₃ClO₂: Molecular structure: Octahedral (six electron groups) Expected hybridization: sp³d² (six electron groups)

Step-by-step solution

Calculate the total number of valence electrons for each species

First, let's calculate the total number of valence electrons for each compound: - F₃ClO: 7 (Cl) + 3 * 7 (F) + 6 (O) = 34 valence electrons - F₂ClO₂⁺: 7 (Cl) + 2 * 7 (F) + 2 * 6 (O) - 1 (due to the positive charge) = 33 valence electrons - F₃ClO₂: 7 (Cl) + 3 * 7 (F) + 2 * 6 (O) = 40 valence electrons

Draw the Lewis structures for each species

We will draw the Lewis structures for three compounds: 1. F₃ClO: Put the Cl atom in the center, and surround it by F and O atoms. Form single bonds between the Cl and F atoms and the Cl and O atoms, using up 8 valence electrons. Fill in the F and O atoms with their remaining valence electrons, which will be 6 on each F atom and 4 on the O atom (18 electrons used). Lastly, place the remaining 8 valence electrons on the Cl atom. 2. F₂ClO₂⁺: Put the Cl atom in the center, and surround it by F and O atoms. Form single bonds between Cl and F atoms, and Cl and O atoms, using up 8 valence electrons. Fill in the F and O atoms with their remaining valence electrons, which will be 6 on each F atom and 4 on each O atom (16 electrons used). Lastly, place the remaining 9 valence electrons on the Cl atom. 3. F₃ClO₂: Put the Cl atom in the center, and surround it by F and O atoms. Form single bonds between Cl and F atoms, and Cl and O atoms, using up 10 valence electrons. Fill in the F and O atoms with their remaining valence electrons, which will be 6 on each F atom and 4 on each O atom (22 electrons used). Lastly, place the remaining 8 valence electrons on the Cl atom.

Determine the molecular structure and the expected hybridization for each species

1. F₃ClO: Molecular structure: Tetrahedral (four electron groups - three single bonds and one lone pair) Expected hybridization: sp³ (four electron groups) 2. F₂ClO₂⁺: Molecular structure: Trigonal bipyramidal (five electron groups - four single bonds and one lone pair) Expected hybridization: sp³d (five electron groups) 3. F₃ClO₂: Molecular structure: Octahedral (six electron groups - five single bonds and one lone pair) Expected hybridization: sp³d² (six electron groups)

Key concepts

Valence Electrons

Valence electrons are the outermost electrons of an atom, playing a crucial role in chemical bonding. They determine how atoms interact with each other and form molecules.
For example, when determining the Lewis structure of a molecule like \(\mathrm{F}_3 \mathrm{ClO}\), you calculate the total number of valence electrons.

• Chlorine (Cl) contributes 7 valence electrons.
• Each Fluorine (F) atom also contributes 7 valence electrons.
• Oxygen (O) provides 6 valence electrons.

Adding these up, remember to account for any charges. This step ensures we use the correct number of electrons when drawing Lewis structures
and helps predict the molecule's behavior.

Molecular Structure

The molecular structure describes the arrangement of atoms in a molecule. This layout is crucial to understanding the molecule's properties and behavior.
For instance, \(\mathrm{F}_3 \mathrm{ClO}\) has a tetrahedral structure.

• This means that there are four groups of electrons around the central Cl atom: three F atoms and one lone pair.

Understanding these structures helps predict reactions and interactions.
The molecular geometry can be deduced using the VSEPR (Valence Shell Electron Pair Repulsion) theory, which assumes that electron pairs will arrange themselves to minimize repulsion.

Hybridization

Hybridization explains the mixing of atomic orbitals to create new hybrid orbitals, which can have different shapes and angles than the original.
For \(\mathrm{F}_3 \mathrm{ClO}\), the expected hybridization is \(\mathrm{sp}^3\), meaning the chlorine atom forms four equivalent orbitals for bonding:

• Three are used for bonds with the fluorine atoms.
• One remains as a lone pair.

Hybridization informs us about molecular shapes and angles, crucial for understanding how molecules fit and work together.
For example, a \(\mathrm{sp}^3\) hybridization in \(\mathrm{F}_3 \mathrm{ClO}\) suggests a particular three-dimensional arrangement which matches a tetrahedral geometry.

Oxidizing Agents

Oxidizing agents are substances that can accept electrons during a chemical reaction, often 'oxidizing' another compound in the process.
In our example, compounds like \(\mathrm{FClO}_3\) and related ions are known for their strong oxidizing power, making them useful in applications like rocket propellants.

• They often contain elements with a high oxidation state, like chlorine in \(\mathrm{F}_3 \mathrm{ClO}_2\), to effectively pull electrons from other substances.

Understanding how these agents work is important in fields requiring controlled reactions, such as in energy storage or propulsion systems.
Their ability to alter the oxidation state of other elements makes them crucial in various chemical processes, impacting industries from manufacturing to energy production.