In its standard elemental form at $1 \mathrm{atm}$, what is the approximate normal boiling point of sulfur ($S$)?

• A. $115 °C$
• B. $445 °C$
• C. $100 °C$
• D. $212 °C$

Answer: (B)

Verified step by step guidance

1. Understand that the problem asks for the normal boiling point of elemental sulfur (S) at 1 atm pressure, which is a physical property related to the temperature at which sulfur transitions from liquid to gas under standard atmospheric pressure.
2. Recall that the normal boiling point is a characteristic property of a substance and can be found in standard reference tables or reliable chemistry data sources, as it is not calculated from first principles in typical general chemistry problems.
3. Recognize that sulfur exists in several allotropes, but the most common form at room temperature is rhombic sulfur, and its boiling point is significantly higher than its melting point (which is around 115 °C).
4. Use a standard chemistry reference (such as a textbook appendix or a trusted database) to look up the boiling point of sulfur at 1 atm, noting that it is much higher than 115 °C and well above the boiling point of water (100 °C).
5. Compare the given answer choices with the known boiling point from the reference to select the correct approximate boiling point of sulfur, which is around 445 °C.