Answer :
To determine the best information to fill the blanks in row 3 of the table, let’s analyze the properties given and infer the bond type and the likely property.
### Properties of Different Bond Types:
1. Ionic Bonds:
- Typically have high melting points.
- Conduct electricity when in molten state or dissolved in water.
2. Metallic Bonds:
- Conduct electricity in solid and liquid states because of the presence of free-moving electrons.
- Typically have high melting points due to the strong attraction between metal ions and delocalized electrons.
3. Covalent Bonds:
- Generally do not conduct electricity since there are no free ions or electrons to carry the charge.
- Usually have low melting points compared to ionic and metallic compounds, although some covalent network structures (like diamond) have high melting points.
### Given Information for Row 3:
- Electrical conductivity: No
- Likely property: ?
Since compounds with metallic bonds conduct electricity due to the presence of free-moving electrons, we can rule out metallic bonds for row 3 because its electrical conductivity is listed as "No."
Next, recognizing that ionic bonds typically conduct electricity when dissolved in water or in a molten state, we can also rule out ionic bonds as they would not fit the "No" for electrical conductivity.
This leaves us with covalent bonds. Covalent compounds generally do not conduct electricity because they do not have free ions or electrons. Additionally, covalent compounds typically have low melting points, although there are exceptions.
Based on these insights, the best information to fill the blanks in row 3 is:
- Bond: Covalent
- Likely property: Low melting point
Thus, the completed row 3 in the table should read:
[tex]\[ \begin{array}{|c|c|c|c|} \hline \text{Row} & \text{Bond} & \text{Electrical conductivity} & \text{Likely property} \\ \hline 3 & \text{Covalent} & \text{No} & \text{Low melting point} \\ \hline \end{array} \][/tex]
### Final Answer:
Covalent bond and low melting point
### Properties of Different Bond Types:
1. Ionic Bonds:
- Typically have high melting points.
- Conduct electricity when in molten state or dissolved in water.
2. Metallic Bonds:
- Conduct electricity in solid and liquid states because of the presence of free-moving electrons.
- Typically have high melting points due to the strong attraction between metal ions and delocalized electrons.
3. Covalent Bonds:
- Generally do not conduct electricity since there are no free ions or electrons to carry the charge.
- Usually have low melting points compared to ionic and metallic compounds, although some covalent network structures (like diamond) have high melting points.
### Given Information for Row 3:
- Electrical conductivity: No
- Likely property: ?
Since compounds with metallic bonds conduct electricity due to the presence of free-moving electrons, we can rule out metallic bonds for row 3 because its electrical conductivity is listed as "No."
Next, recognizing that ionic bonds typically conduct electricity when dissolved in water or in a molten state, we can also rule out ionic bonds as they would not fit the "No" for electrical conductivity.
This leaves us with covalent bonds. Covalent compounds generally do not conduct electricity because they do not have free ions or electrons. Additionally, covalent compounds typically have low melting points, although there are exceptions.
Based on these insights, the best information to fill the blanks in row 3 is:
- Bond: Covalent
- Likely property: Low melting point
Thus, the completed row 3 in the table should read:
[tex]\[ \begin{array}{|c|c|c|c|} \hline \text{Row} & \text{Bond} & \text{Electrical conductivity} & \text{Likely property} \\ \hline 3 & \text{Covalent} & \text{No} & \text{Low melting point} \\ \hline \end{array} \][/tex]
### Final Answer:
Covalent bond and low melting point
