Draw Lewis structures for the following: (c) SF 2

Hello everyone. So in this video we're figuring out how to draw out the lewis structure for phosphorus Penta bromide. So first things first, let's go ahead and calculate the total number of valence electrons in this molecule. Starting off with our phosphorus that's in Group five A. So we have five valence electrons per atom in this molecule we have one atom. So one times 5 gives us five total valence electrons. Now for our bombing, that's a group seven A. We have five items of grooming each giving us seven electrons. So five times seven is 35. Now adding these two numbers up we get a total of advanced electrons that will be present in our molecule. So again we have phosphorus being our central atom because we have five means we'll go ahead and draw out the bonds to each browning adam. And of course remembering our architect rule will give each broken item three lone pairs. If we do that we can see if we have eight electrons per browning, Then we have five brewing. So five times eight is going to give us 40 advanced electrons. So we have used all that up. Therefore this molecule right here is going to be our final Lewis structure for our molecule.

Ch.8 - Basic Concepts of Chemical Bonding

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Brown 14th Edition

Ch.8 - Basic Concepts of Chemical Bonding

Problem 47c

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Chapter 8, Problem 47c

Draw Lewis structures for the following: (c) SF₂

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Determine the total number of valence electrons available. Sulfur (S) has 6 valence electrons, and each Fluorine (F) has 7 valence electrons. Therefore, SF<sub>2</sub> has a total of 6 + 2(7) = 20 valence electrons.

Place the least electronegative atom, which is Sulfur (S), in the center, and arrange the two Fluorine (F) atoms around it.

Form single bonds between the central Sulfur atom and each of the Fluorine atoms. Each single bond uses 2 electrons, so 2 bonds will use 4 electrons, leaving 16 electrons to be distributed.

Distribute the remaining electrons to satisfy the octet rule, starting with the outer atoms (Fluorine). Each Fluorine atom needs 8 electrons to complete its octet, including the electrons in the bond. Distribute 6 more electrons to each Fluorine atom.

Place any remaining electrons on the central Sulfur atom. After distributing electrons to the Fluorine atoms, place the remaining 4 electrons on the Sulfur atom to complete its octet.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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, while fluorine (F) has seven, which is important for constructing the Lewis structure of 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 polarity and reactivity. For SF2, the molecular geometry is bent due to the presence of lone pairs on the sulfur atom.