Given the atoms involved and the number of valence electrons remaining, complete the Lewis structure by placing bonds between atoms such that each has a full octet.
(d)

Verified step by step guidance

1. Count the total number of valence electrons available for the molecule. In this case, you are given 12 valence electrons to work with.
2. Determine the central atom. Typically, the least electronegative atom (excluding hydrogen) is placed at the center of the structure.
3. Place single bonds (represented as lines) between the central atom and the surrounding atoms. Each single bond uses 2 electrons.
4. Distribute the remaining electrons as lone pairs around the outer atoms to satisfy their octet rule (8 electrons around each atom, except for hydrogen which only needs 2).
5. If there are still electrons left after satisfying the octet for the outer atoms, place the remaining electrons as lone pairs on the central atom. If the central atom does not have a full octet, consider forming double or triple bonds by sharing lone pairs from the outer atoms.

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.

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. This rule is fundamental in determining how atoms will bond and interact in a molecule, particularly in covalent bonding.

Valence Electrons

Valence electrons are the electrons in the outermost shell of an atom that are involved in forming bonds with other atoms. The number of valence electrons determines how an atom can bond and interact with others, influencing the structure and stability of molecules. In the context of the question, knowing the total number of valence electrons available is crucial for completing the Lewis structure correctly.