If an atom of sulfur (atomic number 16) were allowed to react with atoms of hydrogen (atomic number 1), which of the following molecules would be formed?

Question

Quizplus · Accepted Answer

Sulfur has six valence electrons and hydrogen has one. In order to form a molecule, the atoms must share electrons to fill their outermost energy levels. Sulfur needs two electrons to fill its outermost energy level, while hydrogen needs one.

Option A (S-H) would only share one electron between sulfur and hydrogen, leaving sulfur one electron short of a full outermost energy level.

Option C (no image provided) is unclear and cannot be determined.

Option D (two double bonds between sulfur and hydrogen) would require sulfur to use all of its valence electrons to bond with hydrogen, leaving sulfur with no electrons left to form bonds within the molecule.

Option E (H = S = H) would require sulfur to share six electrons with two hydrogen atoms, which is not possible given that sulfur only has six valence electrons available for bonding.

Therefore, the correct option is B (H-S-H), which would allow both sulfur and both hydrogen atoms to fill their outermost energy levels by sharing electrons in a covalent bond.

If an Atom of Sulfur (Atomic Number 16) Were Allowed