To determine the information that best fills the blanks in row 3, we need to match the properties of different bond types with the given electrical conductivity and likely property.
Here's a step-by-step approach:
1. Identify the Bond Type Based on Electrical Conductivity:
- Ionic Bonds: Typically conduct electricity when dissolved in water but not in solid form.
- Metallic Bonds: Conduct electricity in both solid and liquid form.
- Covalent Bonds: Generally do not conduct electricity because they do not have free-moving charged particles.
2. Analyze the Given Electrical Conductivity:
- Row 3 specifies "No" for electrical conductivity. This suggests that the compound does not conduct electricity in any form.
3. Determine the Likely Property:
- Melting Point: Can help further confirm the bond type.
- Ionic compounds typically have high melting points.
- Metallic compounds also have high melting points due to strong metallic bonds.
- Covalent compounds often have lower melting points compared to ionic and metallic bonds. This is because covalent bonds involve the sharing of electrons between atoms and usually result in structures that do not require as much energy to break apart.
Since Row 3 has "No" for electrical conductivity, we infer that the most likely type of bond present is a covalent bond because covalent compounds do not conduct electricity. Additionally, covalent bonds are usually associated with having lower melting points.
Therefore, the best information to fill in the blanks for row 3 is:
- Bond Type: Covalent Bond
- Likely Property: Low Melting Point
Thus, the answer is:
- Covalent bond and low melting point.
