Question

Sketch the Lewis structures of \(\mathrm{C} 1 \mathrm{F}_{2}^{+}\) and \(\mathrm{C} \mathrm{AF}_{2}^{-} .\) What are the electron-pair and molecular geometrics of each ion? Do both have the same \(\mathbf{F}-\mathbf{C} \mathbf{7}-\mathbf{F}\) angle? What hybrid orbital set is used by \(\mathrm{G}\) in each ion?

Short answer

ClF2+ is linear with sp³d hybridization; CAF2− varies based on theoretical context. Angles differ with assumptions.

Step-by-step solution

Count Valence Electrons for ClF2+

Start by identifying the number of valence electrons for each atom in the ClF2+ ion. Chlorine (Cl) has 7 valence electrons, each fluorine (F) has 7, and with a positive charge, we lose one electron. Total is \(7 + 7 + 7 - 1 = 20\) valence electrons.

Draw the Lewis Structure for ClF2+

Place the chlorine atom in the center, as it is less electronegative than fluorine. Connect each fluorine atom to chlorine with a single bond. Distribute the remaining electrons to satisfy the octets, starting with the fluorine atoms. Two bonding pairs and three lone pairs on Cl yield a total of 10 pairs (or 20 electrons), which matches our count.

Identify the Geometry of ClF2+

With two bonding pairs and three lone pairs on chlorine, the electron-pair geometry is trigonal bipyramidal. Due to the lone pairs, the molecular geometry of ClF2+ is linear.

Determine the Hybridization of Cl in ClF2+

The chlorine atom in ClF2+ uses two bonding pairs and three lone pairs, requiring a total of five hybrid orbitals. Thus, the hybridization is sp³d.

Count Valence Electrons for CAF2−

For CAuF2−, let's assume 'CA' represents a central atom analogous to carbon (due to general convention, though this assumes a valid species). Begin with 4 valence electrons for a central atom like carbon and 7 for each fluorine. An additional electron comes from the negative charge. Total: \(4 + 7 + 7 + 1 = 19\) (normally not valid for typical elements, but this works for conceptual understanding).

Draw the Lewis Structure for CAF2−

If conceptualizing similar to carbon with four valence, draw the central atom as CA with two single bonds to fluorine atoms. Distribute available valence electrons to satisfy octet around fluorine. Due to formal charge considerations, a lone pair or structures with specific free radical nature might arise, suggesting typical options for conceptual understanding.

Identify the Geometry of CAF2−

If treating similar to a C-based analogy theoretically, the typical geometry could be bent, considering exploring with high-electron pairs or radical conditions. However, this is speculative without defining 'CA' in common elements.

Determine the Hybridization of CA in CAF2−

For conceptual understanding similar to a carbon-use analogy, potential hybridization can reflect sp³ or sp patterns depending on interaction. The exercise inherently lacks clarity without explicit identification, but typically sp might emerge through linear focus.

Compare F-C-F Angles

In ClF2+, the F–Cl–F angle is 180° as it is linear. For CAF2−, if pursued sp2 or sp analogies, it would potentially vary from linear precisely and depend on speculative bond context.

Key concepts

Valence electrons

Valence electrons play a crucial role in forming chemical bonds and defining the molecular structure of a compound. They are the electrons located in the outermost shell of an atom and are responsible for an atom's chemical properties. For the ion \(\text{ClF}_2^+\), we calculate the total number of valence electrons by considering the electrons brought by each atom:

• Chlorine (Cl) contributes 7 valence electrons.
• Each Fluorine (F) atom also contributes 7 valence electrons.
• The positive charge on the ion indicates a loss of one electron.

Performing the calculation gives us \(7 + 7 + 7 - 1 = 20\) valence electrons in total. These are spread out to form bonds and to satisfy the octet rule.
For \(\text{CAF}_2^-\), assuming 'CA' is a hypothetical element similar to Carbon:

• 'CA' would contribute 4 valence electrons (similar to Carbon).
• Each Fluorine atom contributes 7 electrons.
• The negative charge here means there is one extra electron.

That results in \(4 + 7 + 7 + 1 = 19\) valence electrons. While an odd number of valence electrons typically suggests a free radical or unconventional bonding, for conceptual purposes, thinking of achieving possible stable electron configurations is encouraged.

Molecular geometry

Molecular geometry refers to the 3D arrangement of atoms within a molecule and is determined by the number of bonds and lone pairs around the central atom. It greatly influences the molecule's physical properties and chemical reactivity.
For \(\text{ClF}_2^+\), the presence of two bonding pairs and three lone pairs on chlorine results in a molecular geometry that is **linear**. This is due to the symmetry and electronic repulsion pushing the fluorine atoms to opposite ends, making the \(\text{F-Cl-F}\) bond angle 180°. This linear shape minimizes electron pair repulsion.
In contrast, the geometry of \(\text{CAF}_2^-\) is more complex due to the assumptions and the unconventional 'central atom' used. If we consider an analogy with carbon, the expected geometry might be **bent** or **linear**, depending on electron pair distributions around the central atom and the specifics of interactions. With two bonding pairs and speculative electronic interactions, angles less than 180° could be hypothesized under certain structural conditions.

Hybridization

Hybridization is the concept of atomic orbitals mixing to form new hybrid orbitals, which can then form covalent bonds. This mixing helps explain the observed molecular shapes more accurately than simple orbital overlap would predict.
For \(\text{ClF}_2^+\), chlorine undergoes hybridization to accommodate its bonding and lone pairs. With five electron Agression coordinates (two bonding pairs and three lone pairs), chlorine undergoes **sp³d hybridization**. This hybrid orbital set helps to balance the repulsion between lone pairs and bonding pairs, resulting in a linear arrangement of fluorine atoms.
In the case of \(\text{CAF}_2^-\), assuming a simplistic analogy with carbon, potential hybridization is less straightforward due to assumptions and conceptualization. Normally, carbon structures with similar bonding can showcase **sp³ hybridization**. However, presence of unconventional bonding or lone pairs may invoke other hybridizations such as **sp²** or even **sp** based on specific interactions and electronic considerations. This emphasizes exploring the flexible nature of atomic interactions relying on context.

Electron-pair geometry

Electron-pair geometry describes the spatial arrangement of all electron pairs (bonding and lone pairs) around the central atom. Understanding this geometry is essential for predicting molecular shape and distribution of electrons in the compound.
In \(\text{ClF}_2^+\), the electron-pair geometry is **trigonal bipyramidal** due to its five regions of electron density around the central chlorine atom. This includes two bonding pairs and three lone pairs. Despite the complex overall electron-pair geometry, the structure's linear appearance reflects the absence of lone pairs affecting bond angles between the peripheral atoms.
When considering \(\text{CAF}_2^-\), if analogous to a carbon-centered model, the potential electron-pair geometry could be linear, bent, or even influenced by unique radical characteristics based on surrounding interactions. Conventional structures might suggest minimal coordination geometries like **tetrahedral** or **trigonal planar**, expanding explorations. Without a fixed electron configuration by definition, CAF2- offers a model to explore unconventional hypothetical electron pair arrangements.