QQuestionChemistry
QuestionChemistry
Draw the Lewis structure for the trisulfur $\left(\mathrm{S}_{3}\right)$ molecule. Be sure to include all resonance structures that satisfy the octet rule.
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Answer
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Step 1:: Identify the total number of valence electrons in the $\mathrm{S}_{3}$ molecule.
\text{Total valence electrons} = 3 \times 6 = 18 \ \text{electrons}
Sulfur is in the 16th group of the periodic table, so it has 6 valence electrons.
Step 2:: Determine the central atom and arrange the atoms in a linear shape.
\mathrm{S}-\mathrm{S}-\mathrm{S}
In this case, all three sulfur atoms are identical, so we can choose any of them as the central atom. Let's choose the leftmost sulfur atom as our central atom. The arrangement of atoms will be:
Step 3:: Distribute the valence electrons around the atoms.
: \mathrm{S} : \mathrm{S} : \mathrm{S} :
We will start by placing a pair of electrons between each pair of sulfur atoms to form single bonds. This will use up 6 electrons, leaving us with 12 electrons to distribute as lone pairs. (single bonds between sulfur atoms) Now, let's add the lone pairs to achieve an octet for each sulfur atom. We will add one lone pair to each terminal sulfur atom and two lone pairs to the central sulfur atom. (single bonds and lone pairs on each sulfur atom)
Step 4:: Check for resonance structures.
There are two possible resonance structures for the $\mathrm{S}_{3}$ molecule, one with a negative formal charge on the left terminal sulfur atom and another with a negative formal charge on the right terminal sulfur atom.
In this case, there is a formal charge separation in the molecule, as the central sulfur atom has 6 electrons in its valence shell, while the terminal sulfur atoms have 8 electrons. To satisfy the octet rule, we can consider resonance structures where the formal charges are redistributed.
Final Answer
The Lewis structure for the trisulfur $\left(\mathrm{S}_{3}\right)$ molecule, including all resonance structures that satisfy the octet rule, is shown below: : \mathrm{S}^{-} : \mathrm{S} : \mathrm{S}^{+} : \qquad \text{and} \qquad : \mathrm{S} : \mathrm{S}^{-} : \mathrm{S}^{+} :
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