Which is not correctly matched here? (a) XeO2 I2 See-saw (b) X c F6- Distorrct octahedtal (c) Xe

step 1 In this problem, I am writing the correctly matched geometry. As we own know that XCO2F2 is C -s

Which is not correctly matched here? (a) XeO2 I2 See-saw (b)...

Which is not correctly matched here?
(a) $\mathrm{XeO}_{2} \mathrm{I}_{2}$ See-saw
(b) $\mathrm{X} \mathrm{c} \mathrm{F}_{6}-$ Distorrct octahedtal
(c) $\mathrm{XeO}_{3}$ tetrahedral
(d) $\mathrm{XeF}_{4}-$ Planar

Key Concepts

Molecular Geometry

Molecular geometry refers to the three?dimensional arrangement of atoms in a molecule. It is determined by the number of bonding pairs and lone pairs around the central atom. Understanding molecular geometry is crucial because it affects the physical and chemical properties of the compound, including polarity, reactivity, and interactions with other molecules.

VSEPR Theory

The Valence Shell Electron Pair Repulsion (VSEPR) theory is a fundamental concept used to predict the shape of molecules. According to VSEPR theory, electron pairs around a central atom will repel each other and adopt an arrangement that minimizes this repulsion. This theory helps in predicting both the electron domain geometry and the actual molecular shape, particularly when lone pairs are present, which can lead to distortions from ideal geometries.

Electron Domain Geometry versus Molecular Shape

Electron domain geometry considers both bonding and nonbonding electron pairs, yielding an idealized three?dimensional arrangement. Molecular shape, on the other hand, describes the spatial arrangement of only the atoms (ignoring the lone pairs), which often results in forms that differ from the theoretical electron domain geometry. Distinguishing between these two is essential when interpreting molecular structures, especially in hypervalent molecules.

Effect of Lone Pairs on Molecular Geometry

Lone pairs of electrons occupy space and exert greater repulsive force than bonding pairs, leading to distortions in the observed molecular geometry. This effect is critical when determining the final shape of molecules since the presence of lone pairs can change a geometry from an ideal shape (like tetrahedral) to a different one (like trigonal pyramidal or see-saw). Recognizing these distortions is key in matching molecular formulas with their corresponding shapes.

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