Let's analyze the properties of the different types of bonds to determine the best information for the blanks in Row 3.
1. Ionic Bonds:
- Ionic compounds typically conduct electricity when melted or dissolved in water because their ions are free to move.
- Ionic compounds usually have high melting points due to the strong electrostatic forces between the ions.
2. Metallic Bonds:
- Metals conduct electricity in solid and liquid states because of the delocalized electrons that move freely throughout the structure.
- Metals generally have high melting points due to the strong bond between the atoms in the metallic lattice.
3. Covalent Bonds:
- Covalent compounds usually do not conduct electricity because they do not have free-moving charged particles. The electrons are shared between atoms and are not free to move.
- Covalent compounds typically have low melting points compared to ionic and metallic compounds because the forces holding the molecules together (intermolecular forces) are generally weaker than ionic or metallic bonds.
Given that Row 3 shows no electrical conductivity, this means the bond type in Row 3 cannot be metallic or ionic, as both of these types demonstrate conductivity in various states. This leaves covalent bonds as the credible option for the bond type in Row 3.
Among covalent compounds, the general physical property is a low melting point. Thus, the blank in the "Likely property" column should also reflect a low melting point.
Therefore, the most fitting information for the blanks in Row 3 would be "covalent bond and low melting point."
