To determine the information that best fills the blanks in row 3, let's analyze the properties described:
Row 3:
- Bond: Unknown
- Electrical Conductivity: No
- Likely Property: Unknown
Given the electrical conductivity is "No," we can infer that the bond type is not metallic because metallic bonds typically have good electrical conductivity due to the free movement of electrons. Hence, metallic bonds are ruled out.
We are left with either ionic or covalent bonds. Given the general characteristics:
- Ionic bonds typically lead to compounds that do conduct electricity when dissolved in water or melted but not in solid form.
- Covalent bonds do not conduct electricity in any state since they do not have free-moving charged particles (ions or electrons).
Since row 3 specifies "No" electrical conductivity in any state, it aligns with the properties of covalent bonds.
Next, we consider the likely property. Covalent compounds typically have low melting points compared to ionic compounds, which have high melting points due to the strong electrostatic forces between ions.
Therefore, the information that best fills the blanks in row 3 is:
- Bond: Covalent bond
- Likely Property: Low melting point
The completed statement would be:
"Covalent bond and low melting point"
