Write the Lewis structures for the following species, and...

Write the Lewis structures for the following species, and indicate whether each is an odd-electron species, an electron-deficient species, or an expanded valence shell species.
(a) $\mathrm{BI}_{3}$
(b) $\mathrm{IF}_{5}$
(c) $\mathrm{HN}_{2}$

Key Concepts

Lewis Structures

Lewis structures are diagrams showing the arrangement of valence electrons among the atoms in a molecule. They help predict the bonding, geometry, and reactivity of the molecule by depicting bonding pairs of electrons and lone pairs, and they are constructed by counting total valence electrons, assigning electron pairs to bonds and lone pairs, and then checking for octet fulfillment or other electron deficiencies.

Odd-Electron Species

Odd-electron species, also known as radicals, are molecules or ions that possess an unpaired electron. This unpaired electron typically results from an odd total number of valence electrons, giving rise to unique reactivity patterns and often making the species more reactive compared to molecules with paired electrons.

Electron-Deficient Species

Electron-deficient species are molecules or ions that have fewer electrons than necessary to form a conventional octet around the central atom, leading to incomplete electronic configuration. Such species often act as Lewis acids, seeking additional electrons to complete their octet, and their bonding cannot be accurately represented by the typical octet rule alone.

Expanded Valence Shell Species

Expanded valence shell species are molecules in which the central atom accommodates more than eight electrons in its valence shell. This is possible for elements in the third period and beyond, as they have access to d orbitals that allow them to form additional bonds, leading to structures that exceed the octet rule and often result in distinctive molecular geometries.

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