Each of the following ionic compounds consists of a...

Each of the following ionic compounds consists of a combination of monatomic and polyatomic ions. Represent these compounds with Lewis structures. (a) $\mathrm{Al}(\mathrm{OH})_{3}$; (c) $\mathrm{NH}_{4} \mathrm{F}$; (d) $\mathrm{KClO}_{3}$; (b) $\mathrm{Ca}(\mathrm{CN})_{2}$; (e) $\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}$.

Each of the following ionic compounds consists of a combination of monatomic and polyatomic ions. Represent these compounds with Lewis structures.
(a) $\mathrm{Al}(\mathrm{OH})_{3}$;
(c) $\mathrm{NH}_{4} \mathrm{F}$;
(d) $\mathrm{KClO}_{3}$;
(b) $\mathrm{Ca}(\mathrm{CN})_{2}$;
(e) $\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}$.

Key Concepts

Lewis Structures

Lewis structures are schematic representations that show the distribution of valence electrons among the atoms in a molecule or ion. They are used to visualize bonding, lone pairs, and the arrangement of electrons, providing insight into molecular geometry and reactivity.

Ionic Compounds

Ionic compounds are formed by the electrostatic attraction between positively charged cations and negatively charged anions. In these compounds, electrons are transferred from one atom (or polyatomic group) to another, resulting in distinct charged species that combine in ratios that maintain overall charge neutrality.

Polyatomic Ions

Polyatomic ions are groups of atoms that are covalently bonded together and act as a single charged entity in a compound. Representing them with Lewis structures involves accounting for all valence electrons, determining bonding and lone pairs, and ensuring the overall charge matches the required ionic charge.

Valence Electrons

Valence electrons are the electrons in the outermost shell of an atom and are primarily involved in bonding. Counting valence electrons correctly is critical for drawing accurate Lewis structures, as it ensures that the drawn structures satisfy bonding requirements and the Octet Rule (or duet rule for hydrogen).

Octet Rule and Formal Charge

The Octet Rule is a guideline stating that atoms tend to form bonds so that they have eight electrons in their valence shell, leading to greater stability. Formal charge calculations are used in Lewis structures to assign electrons in bonds and lone pairs, helping to determine the most plausible structure for a molecule or ion by minimizing formal charges.

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