To determine the best information to fill the blanks in row 3, let's analyze the properties and types of bonds given in the table.
Row 1 indicates that the compound has an ionic bond, conducts electricity, and has a high melting point. Ionic bonds typically form between metals and non-metals, are good conductors of electricity in molten or aqueous states, and have high melting points due to strong electrostatic forces between ions.
Row 2, though incomplete, shows electrical conductivity which suggests the compound could either be metallic or ionic (since both can conduct electricity), but for ionic, it should show a high melting point as row 1 does. It also could not be covalent, as covalent substances typically do not conduct electricity.
For Row 3, we're told the compound does not conduct electricity. This suggests the compound is likely not ionic or metallic, as both typically conduct electricity in certain states.
Given this understanding, the compound that does not conduct electricity is likely covalent. Covalent bonds typically form between non-metal atoms and generally result in substances with low melting points due to weaker intermolecular forces compared to ionic and metallic bonds.
Thus, the information that best fits the blanks in row 3 would be:
- Bond: covalent bond
- Likely property: low melting point
Therefore, the answer is:
covalent bond and low melting point
