Write the Lewis structure for each molecule. a. SF₂

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1. Determine the total number of valence electrons in the molecule. Sulfur (S) has 6 valence electrons, and each Fluorine (F) has 7 valence electrons. Therefore, SF₂ has a total of 6 + 2(7) = 20 valence electrons.
2. Identify the central atom. In SF₂, sulfur is less electronegative than fluorine, so sulfur will be the central atom.
3. Place the sulfur atom in the center and arrange the two fluorine atoms around it. Connect each fluorine atom to the sulfur atom with a single bond. Each single bond represents 2 electrons, so 4 electrons are used in total for the bonds.
4. Distribute the remaining electrons to satisfy the octet rule. Start by placing lone pairs on the fluorine atoms until each has 8 electrons (including the bonding electrons).
5. Place any remaining electrons on the central sulfur atom. Ensure that the sulfur atom also satisfies the octet rule, if possible. In this case, sulfur can have more than 8 electrons due to its ability to expand its octet.

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.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how atoms bond with each other. The number of valence electrons influences the molecule's reactivity and stability. For example, sulfur (S) has six valence electrons, which play a key role in forming bonds in SF2.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonding pairs and lone pairs of electrons around the central atom, which can affect the molecule's physical and chemical properties. In SF2, the molecular geometry is bent due to the presence of lone pairs on the sulfur atom.