Column A
1.
Nitrogen (N) and Nitrogen (N) in N2.
:
e
Nitrogen (N) and Nitrogen (N) in N2.
2.
Sulfur (S) and Oxygen (O) in SO2.
:
Sulfur (S) and Oxygen (O) in SO2.
3.
Magnesium (Mg) and Chlorine (Cl). in MgCl2
:
Magnesium (Mg) and Chlorine (Cl). in MgCl2
Column B
Column B
a.
The electronegativity difference is 1.8. The bond will be ionic.
b.The electronegativity difference is 1. The bond will be polar covalent.
c.The electronegativity difference is 0. The bond will be ionic.
d.The electronegativity difference is 1. The bond will be nonpolar covalent.
e.The electronegativity difference is 0. The bond will be nonpolar covalent.
f.The electronegativity difference is 1.8. The bond will be polar covalent.
Based on the information provided in Column A, we can determine the types of chemical bonds for each compound:
1. Nitrogen (N2): Since both nitrogen atoms have the same element (N), there is no electronegativity difference. Therefore, the bond will be nonpolar covalent.
2. Sulfur Dioxide (SO2): Sulfur (S) has an electronegativity of 2.58, while oxygen (O) has an electronegativity of 3.44. The electronegativity difference is 0.86, which is considered significant. Therefore, the bond will be polar covalent.
3. Magnesium chloride (MgCl2): Magnesium (Mg) has an electronegativity of 1.31, while chlorine (Cl) has an electronegativity of 3.16. The electronegativity difference is 1.85, which is considered significant. Therefore, the bond will be ionic.
Matching the information from Column A to the types of chemical bonds in Column B, the correct pairs would be:
1. Nonpolar covalent
2. Polar covalent
3. Ionic