Final answer:
Considering the properties of ionic and covalent compounds, the best match given the options is (c), which states that the compound does not dissolve in water, consistent with many covalent compounds. Options (a) and (b) are incorrect as they do not align with typical ionic properties, and option (d) does not provide a definitive clue.
Step-by-step explanation:
When trying to determine if an unknown compound has ionic or covalent bonds, one must consider its physical properties. Ionic compounds generally have high melting and boiling points, are good conductors of electricity when dissolved in water, and tend to be soluble in water. In contrast, covalent compounds typically have lower melting and boiling points, are poor conductors of electricity in any state, and many are not soluble in water. Therefore, based on these properties we can defect the following:
- a) Ionic bonds, because it melts at 100°C - This is incorrect since ionic compounds typically have much higher melting points.
- b) Ionic bonds, because it does not conduct electricity - This is incorrect since ionic compounds generally conduct electricity when molten or dissolved in water.
- c) Covalent bonds, because it does not dissolve in water - This could potentially be correct since many covalent compounds do not dissolve in water.
- d) Covalent bonds, because it is a white solid at room temperature - The color and state do not conclusively determine the bond type as both ionic and covalent compounds can be solids and various colors at room temperature.
Given the options, the one that aligns most closely with the properties of covalent compounds is option (c), as it highlights the typical property of covalent compounds being insoluble in water.