Let's analyze the information given in the incomplete table, particularly focusing on row 3, where bond type and likely property are not specified, but electrical conductivity is stated to be "No."
To determine the correct bond type and property for row 3, we need to consider the characteristics of different types of bonds:
1. Ionic Bond:
- Typically exhibits high electrical conductivity when molten or dissolved in water.
- Tends to have high melting points.
2. Metallic Bond:
- Metals are generally good conductors of electricity due to free electrons.
- Metals usually have high melting points.
3. Covalent Bond:
- Compounds with covalent bonds usually have low electrical conductivity in all states (solid, liquid, or aqueous solution).
- These compounds often have low melting points, especially if they are simple molecular substances.
Given the characteristic that the compound in row 3 does not conduct electricity ("No" in electrical conductivity), we can eliminate both ionic and metallic bonds as possibilities because both types exhibit some electrical conductivity.
Therefore, the bond type in row 3 must be a covalent bond.
Next, we consider the likely property associated with covalent bonds. Covalent compounds generally have low melting points because the intermolecular forces between molecules are weak compared to ionic or metallic bonds.
Thus, the best information to fill in the blanks in row 3 is:
- Bond: Covalent bond
- Likely property: Low melting point
Hence, the information that best fills the blanks in row 3 is:
```
covalent bond and low melting point
```
