Sodium cyanide, empirical formula NaCN, is a solid which melts at 564 degrees C to give a liquid that conducts electricity. it also dissolves in water to give a conducting solution. Use these properties to deduce the type of bonding that holds this compound together.
It must be ionic or at least polar covalent
To deduce the type of bonding that holds sodium cyanide (NaCN) together, we can analyze the properties mentioned.
First, it's mentioned that sodium cyanide is a solid that melts at 564 degrees Celsius. This high melting point suggests strong bonds between the atoms in the compound. In general, compounds with high melting points tend to have either ionic or network covalent bonding.
Next, it's stated that when sodium cyanide melts, it forms a liquid that conducts electricity. This indicates that there are mobile charged particles present in the liquid. In ionic compounds, such as sodium chloride (NaCl), the ions separate and become mobile when the compound melts or dissolves in water, allowing it to conduct electricity. Covalent compounds, on the other hand, typically do not conduct electricity when they are in a liquid state.
Finally, it's mentioned that sodium cyanide dissolves in water to give a conducting solution. This further supports the idea that sodium cyanide is an ionic compound because it completely dissociates into ions when dissolved in water, allowing the solution to conduct electricity.
Based on these properties, we can conclude that sodium cyanide likely has an ionic or at least polar covalent bonding. However, since it forms a conducting liquid and conducting solution when melted or dissolved in water, it is more likely to be an ionic compound.