Write the Lewis formula of each member of each of the...

Write the Lewis formula of each member of each of the following pairs. Then use VSEPR theory to predict the geometry about each central atom, and describe any features that lead you to decide which member of each pair would have the lower boiling point. (a) $\mathrm{CH}_{3} \mathrm{COOH}$ and $\mathrm{HCOCH}_{3} ;$ (b) $\mathrm{NHF}_{2}$ and $\mathrm{BH}_{2} \mathrm{Cl} ;$ (c) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}$ and $\mathrm{CH}_{3} \mathrm{OCH}_{3}$

Key Concepts

Intermolecular Forces and Boiling Points

Intermolecular forces are the forces of attraction or repulsion between neighboring molecules, and they play a critical role in determining boiling points. Factors such as hydrogen bonding, dipole-dipole interactions, and dispersion forces contribute to the strength of these attractions. Generally, stronger intermolecular forces result in a higher boiling point, so comparing these forces among molecules allows one to predict relative boiling points.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of the atoms in a molecule, which is derived from the VSEPR theory. It describes the spatial orientation of bonds and lone pairs around the central atom, influencing many physical and chemical properties, including how molecules interact with each other.

Lewis Structures

Lewis structures are diagrams that represent the valence electrons of atoms within a molecule. They display how electrons are arranged in bonds between atoms and include non-bonding electron pairs. This representation is essential for understanding molecular connectivity, predicting reactivity, and providing the basis for further analysis such as geometry determination.

VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) theory is used to predict the geometry of a molecule by considering the repulsions between electron pairs (both bonding and lone pairs) in the valence shell of the central atom. According to this theory, electron pairs arrange themselves as far apart as possible to minimize repulsion, which in turn determines the molecular shape.

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