Final answer:
In H2O, the atoms are held together by strong covalent bonds, and individual water molecules interact with each other via weaker hydrogen bonds. The S2O molecule is also expected to have covalent bonds, as it involves nonmetals. However, S2O is less common and not as well characterized in its bonding properties.
Step-by-step explanation:
The compounds S₂O and H₂O involve different kinds of chemical bonds. In the case of water (H₂O), the molecules are held together by covalent bonds. This is a type of bond where electrons are shared between atoms to fill their outer electron shells, as oxygen wants to have eight electrons to be stable. Covalent bonds are strong and do not dissociate in water.
Additionally, between individual water molecules, hydrogen bonds occur. These are weaker interactions compared to covalent bonds and are a form of dipole-dipole interaction that happens when the positively charged hydrogen atom of one water molecule is attracted to the negatively charged oxygen atom of another water molecule. These bonds are indicated with a dotted line in molecular structures due to their relatively weak nature.
Regarding S₂O, which is less common, the bond within the molecule is also likely to be a covalent bond as it involves nonmetals. However, specific information on the bonding in S₂O is less readily available, so a detailed explanation is challenging without specific context or clarification on which sulfur oxide is being discussed, as several sulfur oxides exist with different molecular formulas (e.g., SO, SO₂, SO₃).