Draw the Lewis structures for each of the following molecules or ions. Identify instances where the octet rule is not obeyed; state which atom in each compound does not follow the octet rule; and state how many electrons surround these atoms: (a) PF₆^-, (b) BeCl₂, (c) NH₃, (d) XeF₂O (the Xe is the central atom), (e) SO₄^2- .

Key Concepts

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of molecules in chemical reactions.

Octet Rule

The octet rule is a chemical rule of thumb that states atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. However, there are exceptions to this rule, particularly for elements in the third period and beyond, which can accommodate more than eight electrons due to available d-orbitals.

Expanded Octet

An expanded octet occurs when an atom has more than eight electrons in its valence shell, which is common for elements in the third period and beyond, such as phosphorus, sulfur, and xenon. This phenomenon allows these atoms to form more bonds than would be predicted by the octet rule, leading to the formation of complex molecules and ions. Identifying atoms with expanded octets is crucial for accurately drawing Lewis structures.