Question

The most common and stable allotropic form of Sulfur is the one having the molecular formula S₈.

A. True
B. False

Answer 1

The most common and stable allotropic form of sulfur is S₈, with eight sulfur atoms bonded together in a molecule. This is represented by the structural formula, ball-and-stick model, and space-filling model as shown in Figure 2.17.

Step-by-step explanation:

The most common and stable allotropic form of sulfur is the one with the molecular formula S8. It consists of eight sulfur atoms bonded together in a molecule.

This is represented by the structural formula, ball-and-stick model, and space-filling model as shown in Figure 2.17.

Answer 2

The given statement regarding sulfur's most common and stable allotropic form being S8 is true; this eight-membered puckered ring structure of sulfur is the most stable and prevalent form at room temperature.

Step-by-step explanation:

The statement that the most common and stable allotropic form of sulfur has the molecular formula S₈ is True. Elemental sulfur is known to have several allotropes, which are different forms of the same element in the same physical state. The S₈ allotrope, which is composed of eight sulfur atoms arranged in a puckered ring, is the most prevalent and stable at room temperature. It turns into other allotropes at different temperatures, such as monoclinic sulfur above 95.3°C and orthorhombic sulfur below this temperature.

Sulfur can exist in other allotropes as well, particularly when it is vaporized at high temperatures, forming molecules such as S₂, S₆, and even longer chains at very high temperatures. Nonetheless, S₈ is recognized as the most stable form under normal atmospheric conditions, making it the predominant form encountered.