Write Lewis structures and predict the molecular structures...

Write Lewis structures and predict the molecular structures of the following. (See Exercises 89 and $90 .$ ) a. $\mathrm{OCl}_{2}, \mathrm{KrF}_{2}, \mathrm{BeH}_{2}, \mathrm{SO}_{2}$ b. $\mathrm{SO}_{3}, \mathrm{NF}_{3}, \mathrm{IF}_{3}$ c. $\mathrm{CF}_{4}, \mathrm{SeF}_{4}, \mathrm{KrF}_{4}$ d. $\mathrm{IF}_{5}, \mathrm{AsF}_{5}$ Which of these compounds are polar?

Write Lewis structures and predict the molecular structures of the following. (See Exercises 89 and $90 .$ )
a. $\mathrm{OCl}_{2}, \mathrm{KrF}_{2}, \mathrm{BeH}_{2}, \mathrm{SO}_{2}$
b. $\mathrm{SO}_{3}, \mathrm{NF}_{3}, \mathrm{IF}_{3}$
c. $\mathrm{CF}_{4}, \mathrm{SeF}_{4}, \mathrm{KrF}_{4}$
d. $\mathrm{IF}_{5}, \mathrm{AsF}_{5}$
Which of these compounds are polar?

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Key Concepts

Polarity

Polarity in a molecule is determined by the distribution of electrical charges and the molecular geometry. A polar molecule has an uneven distribution of electrons leading to regions of partial positive and negative charges. This property affects intermolecular interactions, solubility, and overall molecular behavior.

Molecular Geometry

Molecular geometry describes the three-dimensional arrangement of atoms in a molecule, which is an outcome of the bonding pairs and lone pairs around the central atom. Understanding the geometry is critical for predicting physical and chemical properties such as reactivity and polarity.

Lewis Structures

Lewis structures are diagrams that represent the arrangement of electrons in molecules. They show how atoms are bonded together by denoting shared electron pairs as bonds and unshared, or lone, pairs as dots. This structural representation is essential for determining bonding patterns and predicting molecular geometry.

Valence Shell Electron Pair Repulsion (VSEPR) Theory

VSEPR theory is used to predict the three-dimensional shapes of molecules based on the repulsion between electron pairs in the valence shell of the central atom. It assumes that electron pairs will arrange themselves as far apart as possible to minimize repulsion, leading to specific molecular geometries.

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