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Ch.8 - Basic Concepts of Chemical Bonding
All textbooksBrown 15th EditionCh.8 - Basic Concepts of Chemical BondingProblem 49c
Chapter 8, Problem 49c

Draw Lewis structures that satisfy the octet rule for the following molecules and ions: c. SO32−

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Determine the total number of valence electrons in the molecule. Sulfur (S) has 6 valence electrons, each oxygen (O) has 6 valence electrons, and the 2− charge adds 2 more electrons.
Calculate the total number of valence electrons: 1 S (6 electrons) + 3 O (3 x 6 electrons) + 2 extra electrons from the charge = 26 valence electrons.
Place the least electronegative atom, sulfur, in the center, and arrange the three oxygen atoms around it.
Connect each oxygen atom to the sulfur atom with a single bond, using 2 electrons per bond, which accounts for 6 electrons.
Distribute the remaining 20 electrons to satisfy the octet rule for each oxygen atom first, and then place any remaining electrons on the sulfur atom.

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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 reactivity.
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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 helps predict the arrangement of electrons in molecules and is particularly useful in understanding the stability of ions and compounds.
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Formal Charge

Formal charge is a concept used to determine the distribution of electrons in a molecule or ion. It is calculated by taking the number of valence electrons of an atom, subtracting the number of non-bonding electrons, and half the number of bonding electrons. Minimizing formal charges in Lewis structures helps identify the most stable arrangement of atoms and electrons.
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Related Practice
Textbook Question

In the following pairs of binary compounds, determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances) to assign a name to each compound: (a) SiF4 and LaF3 (for ionic or molecular substances) to assign a name to each compound: (b) FeCl2 and ReCl6 (c) PbCl4 and RbCl.

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Textbook Question

In the following pairs of binary compounds, determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances) to assign a name to each compound: (a) TiCl4 and CaF2 (b) ClF3 and VF3

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Textbook Question

In the following pairs of binary compounds, determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances) to assign a name to each compound: (c) SbCl5 and AlF3.

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Textbook Question

Draw Lewis structures that satisfy the octet rule for the following molecules and ions: d. HCN (H and N are both bonded to C),

Textbook Question

Draw Lewis structures that satisfy the octet rule for the following molecules and ions: f. HOCl

Textbook Question

Write Lewis structures that satisfy the octet rule for the following molecules and ions: a. NH4+, b. C2F4 (the two C atoms are bonded to one another), c. COCl2 (the Cl atoms are bonded to C), d. HSO3− (H is bonded to one of the O atoms), e. HNC (H and C are both bonded to N), f. ClO3−.