Question:
What is the value of $\angle S\!-\!S\!-\!S$ in puckered $S_8$ rhombic sulfur?
What is the value of $\angle S\!-\!S\!-\!S$ in puckered $S_8$ rhombic sulfur?
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Chemistry Tip: The $S_8$ molecule is famous for its "crown" structure. Memorize its two key parameters: Bond Angle = $107^{\circ}$ and Bond Length = 204 pm.
Updated On: Apr 23, 2026
- $107^{\circ}$
- $120^{\circ}$
- $104.5^{\circ}$
- $60^{\circ}$
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The Correct Option is A
Solution and Explanation
Concept:
Chemistry (p-Block Elements) - Allotropes of Sulfur and Molecular Structure.
Step 1: Recall the allotropes of sulfur. Sulfur exists in several allotropic forms, the most common being rhombic sulfur ($\alpha$-sulfur) and monoclinic sulfur ($\beta$-sulfur). Both of these stable crystalline forms consist of $S_{8}$ molecules.
Step 2: Determine the molecular shape of the $S_{8}$ molecule. In an $S_{8}$ molecule, eight sulfur atoms are covalently bonded to each other to form a closed ring. However, to minimize steric hindrance and electronic repulsion, the ring is not planar. It adopts a puckered shape, commonly referred to as a "crown" shape.
Step 3: Identify the hybridization of the sulfur atoms. Each sulfur atom in the $S_{8}$ ring is bonded to two other adjacent sulfur atoms and has two lone pairs of electrons. This corresponds to an $sp^3$ hybridization state, which normally has a tetrahedral bond angle of $109.5^{\circ}$.
Step 4: Consider lone pair-lone pair repulsions. According to VSEPR theory, lone pair-lone pair repulsions are greater than bond pair-bond pair repulsions. The presence of two bulky lone pairs on every single sulfur atom pushes the S-S bonds slightly closer together, reducing the bond angle from the ideal $109.5^{\circ}$.
Step 5: State the experimentally determined bond angle. X-ray crystallography and structural studies have precisely measured the dimensions of the puckered $S_{8}$ crown ring. The uniform S-S bond length is exactly 204 pm, and the S-S-S bond angle is compressed to exactly $107^{\circ}$. Comparing this fixed structural property with the given options confirms that $107^{\circ}$ is the correct value. $$ \therefore \text{The value of the } \angle S-S-S \text{ in } S_{8} \text{ is } 107^{\circ}. $$
Step 1: Recall the allotropes of sulfur. Sulfur exists in several allotropic forms, the most common being rhombic sulfur ($\alpha$-sulfur) and monoclinic sulfur ($\beta$-sulfur). Both of these stable crystalline forms consist of $S_{8}$ molecules.
Step 2: Determine the molecular shape of the $S_{8}$ molecule. In an $S_{8}$ molecule, eight sulfur atoms are covalently bonded to each other to form a closed ring. However, to minimize steric hindrance and electronic repulsion, the ring is not planar. It adopts a puckered shape, commonly referred to as a "crown" shape.
Step 3: Identify the hybridization of the sulfur atoms. Each sulfur atom in the $S_{8}$ ring is bonded to two other adjacent sulfur atoms and has two lone pairs of electrons. This corresponds to an $sp^3$ hybridization state, which normally has a tetrahedral bond angle of $109.5^{\circ}$.
Step 4: Consider lone pair-lone pair repulsions. According to VSEPR theory, lone pair-lone pair repulsions are greater than bond pair-bond pair repulsions. The presence of two bulky lone pairs on every single sulfur atom pushes the S-S bonds slightly closer together, reducing the bond angle from the ideal $109.5^{\circ}$.
Step 5: State the experimentally determined bond angle. X-ray crystallography and structural studies have precisely measured the dimensions of the puckered $S_{8}$ crown ring. The uniform S-S bond length is exactly 204 pm, and the S-S-S bond angle is compressed to exactly $107^{\circ}$. Comparing this fixed structural property with the given options confirms that $107^{\circ}$ is the correct value. $$ \therefore \text{The value of the } \angle S-S-S \text{ in } S_{8} \text{ is } 107^{\circ}. $$
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