For each of the following molecules or ions that contain...

For each of the following molecules or ions that contain sulfur, write the Lewis structure(s), predict the molecular structure (including bond angles), and give the expected hybrid orbitals for sulfur. a. $\mathrm{SO}_{2}$ b. $\mathrm{SO}_{3}$ e. $\mathrm{SO}_{3}^{2-}$ f. $\mathrm{SO}_{4}^{2-}$ g. $\mathrm{SF}_{2}$ h. $\mathrm{SF}_{4}$ i. $\mathrm{SF}_{6}$ j. $\mathrm{F}_{3} \mathrm{~S}-\mathrm{SF}$ k. $\mathrm{SF}_{5}{ }^{+}$

For each of the following molecules or ions that contain sulfur, write the Lewis structure(s), predict the molecular structure (including bond angles), and give the expected hybrid orbitals for sulfur.
a. $\mathrm{SO}_{2}$
b. $\mathrm{SO}_{3}$
e. $\mathrm{SO}_{3}^{2-}$
f. $\mathrm{SO}_{4}^{2-}$
g. $\mathrm{SF}_{2}$
h. $\mathrm{SF}_{4}$
i. $\mathrm{SF}_{6}$
j. $\mathrm{F}_{3} \mathrm{~S}-\mathrm{SF}$
k. $\mathrm{SF}_{5}{ }^{+}$

Key Concepts

Lewis Structures

Lewis structures are diagrams that show the arrangement of valence electrons among the atoms in a molecule. They are used to represent bonding between atoms as well as lone pairs of electrons, giving insight into the connectivity and electron distribution within the molecule. This is foundational for further predictions of molecular behavior and shape.

Molecular Geometry and VSEPR Theory

VSEPR (Valence Shell Electron Pair Repulsion) theory is used to predict the three-dimensional shape of a molecule based on the repulsions between electron pairs (both bonding and non-bonding) around the central atom. It provides a method to estimate bond angles and the overall geometry of a molecule, which is essential for understanding molecular structure and reactivity.

Hybridization

Hybridization is the concept that atomic orbitals mix to form new hybrid orbitals that can form bonds in specific geometries. It explains the observed bonding arrangements and shapes of molecules by describing how electrons are involved in forming sigma bonds and accommodating lone pairs, leading to designations such as sp, sp2, sp3, and beyond.

Octet Rule and Expanded Octet

The octet rule states that atoms tend to form bonds until they are surrounded by eight electrons in their valence shell, which is typical for second-period elements. However, elements in the third period and beyond, such as sulfur, can have expanded octets because they have available d-orbitals. This allows them to form more bonds than predicted by the octet rule, influencing the Lewis structures and hybridizations seen in these molecules.

Formal Charge and Resonance

Formal charge calculation is a tool used to determine the most plausible Lewis structure among several possibilities by showing the distribution of electrons as if all atoms had equal sharing. When multiple valid Lewis structures exist, resonance structures are used to represent the delocalization of electrons within a molecule, offering a more accurate depiction of the molecule's electron distribution and overall stability.

Transcript

Please give Ace some feedback