Which of the following bonds would be the most polar without being considered ionic?A) Mg-OB) C-OC) O-OD) Si-OE) N-O

To determine which bond would be the most polar without being considered ionic, we need to look at the difference in electronegativity between the two atoms in each bond. The greater the difference, the more polar the bond. However, if the difference is too great, the bond would be considered ionic rather than covalent.

Here are the electronegativity values for the relevant elements:

• Magnesium (Mg): 1.31
• Carbon (C): 2.55
• Oxygen (O): 3.44
• Silicon (Si): 1.90
• Nitrogen (N): 3.04

Now, let's calculate the difference in electronegativity for each bond:

A) Mg-O: 3.44 - 1.31 = 2.13 B) C-O: 3.44 - 2.55 = 0.89 C) O-O: 3.44 - 3.44 = 0 (this is a nonpolar bond because the electronegativity difference is zero) D) Si-O: 3.44 - 1.90 = 1.54 E) N-O: 3.44 - 3.04 = 0.40

From these calculations, we can see that the Mg-O bond has the greatest difference in electronegativity. However, this difference is so great that the bond would likely be considered ionic rather than covalent.

The Si-O bond has the next greatest difference in electronegativity, and this difference is not so great that the bond would be considered ionic. Therefore, the Si-O bond (D) would be the most polar without being considered ionic.